1. The property of a crystal, which is different in different directions, is called __________.
2. 0.00051 contains __________ significant figures.
3. The oxidation number of oxygen in OF2 is __________.
4. The volume of 1 gm of hydrogen gas at S.T.P is __________.
5. The oxidation number Mn in KMnO4 is __________.
6. The product of ionic concentration in a saturated solution is called __________.
7. 16 gm of oxygen at S.T.P occupies a volume of __________ dm3.
8. The shape of the orbital for which l = 0 is __________.
9. The radius of Cl-1 is __________ than the radius of Cl0.
10. Sp2 hybridization is also known as __________.
11. The value of 1 Debye is __________.
12. The reactions catalyzed by sunlight are called __________.
13. The blue colour of CuSO4 is due to the presence of __________.
14. The force of attraction between the liquid molecules and the surface of container is called __________.
15. The heat of neutralization of a strong acid and a strong base is __________.
16. C º C triple bond is __________. C = C double bond length.
17. The ions having the same electronic configuration are called iso electronic.
18. On heating, if a solid changes directly into vapours without changing into the liquid state, the phenomenon is called __________.
19. Each orbital in an atom can be completely described by __________.
20. In a molecule of alkene, __________ restricts the rotation of the group of atoms at either end of the molecule.
21. Density, refractive index and vapour pressure are __________ properties.
22. The addition of HCl to H2 solution __________ the ionization of H2S.
23. The reaction of cation or anion (or both) with water so as to change its __________ is known as Hydrolysis.
24. A reaction with higher activation energy will start at __________ temperature.
25. 6.02 x 1023 has __________ significant figures.
26. The internal resistance in the flow of liquid is called __________.
27. A catalyst increases the velocity of a reaction but decreases the __________.
Chapter 1
Introduction to Fundamental Concepts
1. 1 mole of a gas at S.T.P occupies a volume of __________.
2. A gas occupying a volume of 22.4 dm3 at S.T.P contains __________ molecules.
3. A formula, which gives the relative number of atoms in the molecule of a compound, is called __________.
4. A formula which gives the actual number of all kinds of atoms present in the molecule of compound is termed as __________.
5. The chemical formula that not only gives the actual number of atoms but also shows the arrangement of different atoms present in the molecule is called __________.
6. Atomic weight or molecular weight expressed in grams is known as __________.
7. 2 moles of H2O contain __________ grams and __________ number of molecules.
8. Any thing that occupies space and has __________ is called matter.
9. Volume of one __________ mole of a gas at S.T.P is 22.4 cubic feet.
10. A ton mole of iron is equal to __________ tons.
11. The force with which the earth attracts a body is called the __________ of the body.
12. A pure substance contains __________ kind of molecules.
13. The smallest indivisible particle of matter is called __________.
14. The atomic number is equal to the number of __________ in nucleus.
15. The atomic mass is the total number of protons and __________ in an atom of the element.
16. The average weight of atoms of an element as compared to the weight of one atom of __________ is called the atomic mass.
17. 1.0007 contains __________ significant figures.
18. The figure 24.75 will be rounded off to __________.
19. __________ means that the readings and measurements obtained in different experiments are very close to each other.
20. __________ means that the results obtained in different experiments are very close to the accepted values.
21. The degree of a measured quantity __________ with increasing number of significant figures in it.
22. The atomic mass of sodium is __________.
23. The symbolic representation of a molecule of a compound is called __________.
24. Molecular formula of CHCl3 and its Empirical formula is __________.
25. Molecular formula of benzene is C6H6 and its empirical formula is __________.
26. 58.5 is the __________ of NaCl.
27. 4.5 gms of nitrogen will have __________ molecules.
28. 28 gms of nitrogen will have __________ molecules.
29. 2 moles of SO2 is equal to __________ gms.
30. 1000 gms of H2O is equal to __________ moles.
31. The reactions, which proceed in both directions, are called __________.
32. The reactions, which proceed in forward directions only, are called __________ reactions.
33. The __________ reactions are completed after some time.
34. 0.0006 has __________ significant figures
35. 7.40 x 108 has __________ significant figures.
36. 7 x 108 has __________ significant figures.
37. Usually Molecular formula is simple multiple of the __________.
38. 0.1 mole of H2O contains __________ molecules of H2O.
39. Mass of 3.01 x 1022 molecules of CO2 is __________.
40. __________ is the branch of science which deals with the properties, composition and structure of matter.
41. None zero digits are all __________.
42. The integer part of logarithm is called __________.
43. The decimal fraction of logarithm is called __________.
44. __________ is the amount of substance, which contains as many number of particles as there are in 12 gms of Carbon.
45. 6.02 x 1023 is called the __________.
46. The accuracy of measurement depends on the number of __________.
47. __________ is the branch of chemistry that deals with quantitative relationships among the substances undergoing chemical changes.
48. The sum of atomic weights of all the elements present in molecular formula is called the __________.
49. __________ is the sum of atomic weights of the elements represented by the Empirical formula of the compound.
50. Very small and very large quantities are expressed in terms of __________.
51. In rounding off __________ figure is dropped.
52. Mole is the quantity, which has __________ particle of the substance.
53. For three significant figures, 25.55 is rounded off to __________.
54. The S.I unit of a mass is __________.
55. Mass of 6.02 x 1023 molecules of NaCl is __________ gm.
56. 1 mole of NaOH is __________ gm of NaOH.
57. Formula weight is used for __________ substances.
58. The word S.I stands for __________.
59. 4.5 gms of water will have __________ molecules.
60. 0.0087 has __________ significant figure.
Chapter 2
The Three States of Matter
1. The intermixing of gases or liquids in a container irrespective of their densities, is called __________.
2. At constant temperature, if the pressure of a given mass of a gas is decreased, its volume will __________.
3. A volume of __________ dm3 will hold 128 gms of SO2.
4. At constant temperature of a given mass of a gas, the product of its __________ and __________ is constant.
5. The rates of diffusion of gases are __________ proportional to the square root of their densities.
6. Gases deviate from ideal behaviour more markedly at high __________.
7. Liquid diffuse __________ than gases.
8. An imaginary line passing through the centre of a crystal is called __________.
9. The temperature at which more than one crystalline forms of a substance coexist in equilibrium is called __________.
10. Two or more substances crystallizing in the same form is called __________.
11. The existence of solid substances in more than one crystalline form is known as __________.
12. Rate of diffusion of gases is __________ as compared to liquids.
13. Boiling point of a liquid __________ with the pressure.
14. Mercury in a glass tube forms __________ curvature.
15. Gases can be compressed to __________ extent.
16. Viscosity of a liquid __________ with the increase of temperature.
17. Surface tension of water __________ by adding soap solution into it.
18. The internal resistance to the flow of a liquid is called __________.
19. The rise or the fall of a liquid in a capillary tube is called __________.
20. Matter exists in __________ states.
21. The freezing point of water in Fahrenheit scale is __________.
22. Boiling point of water is __________ °K.
23. SI unit for measurement of pressure is __________.
24. The value of gas law constant R = __________ dm3 atm/°K/mole.
25. The absolute Zero is equal to __________.
26. If P is plotted against 1/V at constant temperature a __________ is obtained.
27. Gases __________ in heating.
28. The pressure of air __________ at higher altitude.
29. Standard temperature means __________.
30. Standard pressure means __________.
31. Cooling is caused by __________ of gases.
32. Rate of diffusion of O2 is __________ times more than H2.
33. H2O has __________ viscosity than CH3OH.
34. Mercury does not wet the glass surface due to its higher __________.
35. Surface tension of mercury is __________ than water.
36. Viscosity can be easily measured by an instrument called __________.
37. The pressure exerted by the vapours when these vapours are in equilibrium with the liquid is called __________.
38. Vapour pressure __________ at high temperature.
39. Boyle’s Law and Charles Law can be combined into the mathematical expression __________.
40. Equal volumes of all gases at the same temperature and pressure contain __________ number of molecules.
41. The average Kinetic energy of a gas is proportional to its __________ temperature.
42. Kinetic equation may be mathematically written as __________.
43. The temperature at which two crystalline forms of a substance can coexist in equilibrium is called __________.
44. Lighter gases diffuse __________ than heavier gases.
45. Rain drops are __________ in shape.
46. Due to surface tension, the surface area of the liquid is __________.
47. Water __________ in the capillary tube.
48. Viscosity of a solution at 10°C is __________ than at 20°C.
49. Shape of NaCl crystal is __________.
50. Gases intermix to form a mixture.
51. Pressure of a dry gas is __________ than the pressure of a moist gas.
52. 22.4 dm3 of nitrogen at S.T.P will weigh equal to __________ gm.
53. 1 mole of any gas at S.T.P is equal to __________ dm3.
54. At -273°C, volume of all gases becomes __________.
55. The gases, which strictly follows the gas Laws are called __________ gas.
56. __________ is the property that determines the direction of flow of heat.
57. __________ is defined as force per unit area.
58. __________ viscosity is defined as the viscosity of a liquid as compared to the water.
Chapter 3
Structure of Atom
1. The maximum number of electrons in 2p orbital is __________.
2. 3d orbital has __________ energy than 4s orbital.
3. __________ rays are non-material in nature.
4. Charge to mass ratio of cathode rays resembles to that of __________.
5. __________ rays are most penetrating.
6. Neutrons have mass equal to that of __________.
7. Energy is __________ when an electron jumps from higher to lower orbit.
8. Second Ionization Potential has __________ value than the First Ionization Potential.
9. Electronegativity __________ from left to right in a period of Periodic Table.
10. __________ was discovered during the course of Artificial Radioactivity.
11. The velocity of alpha rays is nearly __________ of velocity of light.
12. Natural Radioactivity is confined in __________ elements.
13. The isotopes of an element differ in their __________.
14. Two electrons with the __________ spin, can never occupy the same atomic orbital.
15. ‘Al’ has electronic configuration, 1s2, 2s2, __________.
16. In a group of Periodic Table, the ionization potential __________ from top to bottom as the size of atom increases.
17. Ionization potential values __________ from left to right in a period.
18. The energy required to remove the most loosely bond electron from an atom in gaseous state is called __________.
19. The SI unit of Ionization Potential is __________.
20. An atom of sodium possesses 11 protons and __________ neutrons.
21. The particles of Cathode rays possess __________ charge.
22. The negatively charged particles found in Cathode rays are named as __________.
23. Positive rays are emitted from __________.
24. __________ rays are also known as Canal rays.
25. __________ consists of helium ions and are doubly positively charged.
26. __________ rays consists of negatively charged particles.
27. __________ rays are light waves of very short wavelength.
28. The phenomenon in which a stable element is made radioactive by artificial disintegration is called __________.
29. The electron move around the nucleus in different circular paths called __________.
30. The maximum number of electron in a shell is determined by the formula __________.
31. A particle whose mass is equal to that of electron but carries a positive charge is called __________.
32. 2p electrons are __________ in energy that 2s electrons in the same atom.
33. Number of protons of an element also indicates its __________.
34. According to __________ Principle electrons are fed in the order of increasing orbital energy.
35. According to __________ electrons are distributed among the orbitals of a sub shell to give maximum number of unpaired electron and have same spin.
36. The specific way in which the orbitals of an atom are occupied by electrons is called __________.
37. __________ rays are stream of doubly positively charged particles.
38. Electron in the outer most shell of an atom is called __________.
39. Protons are found in the __________ of an atom and bear __________ charge.
40. The atomic number of an atom is the sum of __________ inside the nucleus.
41. __________ limits the number of electron to different shell or orbits.
42. Sir William Crookes in 1878, discovered that the cathode in high vacuum tube emit radiations what he called __________.
43. X-rays were discovered in 1895 by __________.
44. The discovery of proton was done in 1886 by __________.
45. Neutrons were discovered by __________ in 1932 by the bombardment of beryllium with alpha particles.
46. Each atom has a __________, which contains all the positive charge and practically all the mass of atom.
47. Complete the reaction: 4Be9 + 2H4 ® __________ + __________.
48. __________ have higher ionization power as compared to b-rays.
49. No dark spaces between the colours are present in __________.
50. The symbol e+ represents __________.
51. p-orbitals are __________ shaped.
52. The energy released when an electron is added to an atom in the gaseous state is called __________.
53. The power of an atom to attract a shared pair of electrons towards itself is called __________.
54. Fluorine is __________ electronegative than chlorine.
55. Lyman series of spherical lines appear in the __________ portion of spectrum.
56. The electrons with __________ spin occupy the same orbital.
57. 3d orbital has __________ energy than 4s orbital.
58. Energy and frequency are __________ proportional to each other.
59. Ionic radii of cations are __________ than the atoms from which they are formed.
60. Ionic radii of anions are __________ than the atoms from which they are formed.
Chapter 4
Chemical Bonding
1. A bond formed due to transference of electron is called __________.
2. A bond formed due to sharing of electron is called __________.
3. Sigma bond is __________ than pi bond.
4. The shape of methane molecule is __________.
5. One s and 3p orbitals overlap to produce four __________ hybrid orbitals.
6. Ethene, C2H4 is an example of __________ hybridization.
7. Water molecule has __________ structure.
8. Water molecules are inter-linked with one another due to __________.
9. Polarity of the molecule is due to the difference of __________ between the two bonded atoms.
10. A chemical bond formed between to different atoms by mutual sharing of electron is termed as __________.
11. A chemical bond formed between two similar atoms by mutual sharing of electrons is known as __________.
12. The difference between the Electronegativity values of the two atoms forming covalent bond must be __________ than 1.7.
13. When two orbitals of different atoms by hybridize with each other having their axes in the same straight lines, the bond formed is termed as __________.
14. __________ bond is formed when p-orbitals of the two atoms with their axes parallel to each other overlap with each other.
15. Melting and boiling point of ionic compounds are usually __________ than that of covalent compounds.
16. Non polar compounds are usually __________ in non polar solvent.
17. The nitrogen in NH3 is __________ hybridized.
18. A hybrid orbital is called __________ orbital.
19. Since dipole moment of CS2 is zero, it is a __________ molecule.
20. A bond formed due to the electrostatic forces of attraction between the oppositely charged ions is called __________ bond.
21. The ionic bond is formed between the atoms with low ionization potential and high __________.
22. A bond formed by the sharing of an electron pair contributed by one atom only is called a __________ bond.
23. A co-ordinate covalent bond is also known as __________ bond.
24. Polar covalent bond is __________ than a non polar covalent bond.
25. H-F bond is __________ than H-Br bond.
26. The SI unit of dipole moment is __________.
27. Commonly used unit of dipole moment is __________.
28. Dipole moment of non-polar compound is __________ D.
29. The reactions of ionic compounds are usually very __________.
30. Covalent compounds are generally __________ in nature.
31. Ionic compounds are generally __________ in nature.
32. A covalent bond is represented by a __________.
33. A co-ordinate covalent bond is represented by an __________.
34. The covalent bond between H-F is called __________ covalent bond.
35. The power of an atom to attract a shared pair of electron itself is called __________ of that atom.
36. m = d x e represents __________.
37. CO2 and SO2 molecules have __________ polar bonds.
38. NH3 molecule has __________ polar bonds.
39. A double bond has __________ bond energy than a single bond.
40. An orbital which surrounds a single nucleus is called __________ orbital.
41. An orbital which surrounds two or more atomic nuclei is called __________ orbital.
42. A molecular orbital, which is of lower energy than the atomic orbitals from which it is derived, is known as __________ orbital.
43. A molecular orbital, which has higher energy than the atomic orbitals from which it is derived, is known as __________ orbital.
44. Orbitals formed after hybridization are called __________ orbitals.
45. Bond angle in Sp3 hybridization is of __________.
46. Bond angle in Sp2 hybridization is of __________.
47. Bond angle in Sp hybridization is of __________.
48. Sp3 hybridization is also known as __________.
49. Sp2 hybridization is also known as __________.
50. Sp hybridization is also known as __________.
51. A pair of electrons residing on the central atom and which is not used in bonding is called a __________.
52. The sum of total number of electron pairs (bonding and lone pairs) is called __________ number.
53. __________ bond is usually expressed by dotted line.
54. Water molecule has dipole moment because of its __________ structure.
55. CO2 is non polar because of its __________ structure.
56. Overlapping in __________ bond is perfect.
57. Overlapping in __________ bond is not perfect.
58. H-H bond is __________ than H-Cl bond.
59. __________ hybrid orbitals are not co-planar.
60. Covalent bond is Cl2 molecule is __________.
Chapter 5
Energetics of Chemical Reaction
1. The branch of Chemistry, which deals with the heat changes that take place during chemical reaction, is called __________.
2. The branch of science which deals with energy changes accompanying physical and chemical transformation is called __________.
3. The amount of heat evolved or absorbed in a chemical reaction is called __________.
4. Such reactions in which heat is evolved are called __________ reactions.
5. Such reactions in which heat is absorbed are called __________ reactions.
6. In exothermic reactions, heat evolved is given by __________ sign of DH.
7. In endothermic reactions heat absorbed is given by __________ sign of DH.
8. The total heat change in a reaction is the same whether it takes place in one or several steps.
9. The first law of thermodynamics is also known as __________.
10. The part of universe under observation is called __________.
11. The system plus its surrounding is called __________.
12. Such properties, which give description of a system at a particular moment, is called __________.
13. The term E + PV is called __________.
14. DH represents change in __________.
15. The temperature of water is raised up when sulphuric acid is added to it. This is an __________ reaction.
16. The characteristic properties of a system which is independent of amount of material concerned is called __________ properties.
17. The characteristic properties of a system which depend on amount of substance present in it is called __________ properties.
18. Density, pressure and temperature are the examples of __________ properties.
19. Mole numbers and enthalpy are the examples of __________ properties.
20. A system, which exchange both energy and matter with its surrounding, is called __________ system.
21. A system, which only exchange energy with the surrounding but not matter is, called __________ system.
22. A system which neither exchange energy nor matter with its surrounding is called __________ system.
23. A system is __________ if it contains only one phase.
24. A system is __________ if it contains more than one phase.
25. 1 kilojoule is equal to __________ joules.
26. 1 Calorie is equal to __________ joules.
27. 1 kilo calorie is equal to __________ joules.
28. The work done (w) is mathematically denoted by __________.
29. The change in enthalpy is denoted by __________.
30. __________ law is used in calculating heat of reaction.
31. __________ is defined as the change in enthalpy when one gram mole of a compound is produced from its element.
32. Heat of formation is denoted by __________.
33. When the work is done on the system by the surrounding the sign of work done (w) is __________.
34. When the work is done by the system on surrounding the sign of work done is __________.
35. First law of Thermodynamics is mathematically represented as __________.
36. Standard enthalpies are measured at __________.
37. Hess’s Law is employed to calculate __________ of a chemical reaction.
38. Heat absorbed by the system at constant volume is completely utilize to increase the __________ of the system.
39. Heat change at constant pressure from initial to final state of the system is simply equal to the __________.
40. SI unit of measurement of heat change is __________.
Chapter 6
Chemical Equilibrium
1. The reactions, which proceed in both the directions, are called __________ reactions.
2. The reactions, which proceed to one direction only, are called __________ reactions.
3. Reversible reactions are __________ completed.
4. Irreversible reactions are __________ after some time.
5. A reversible reaction is said to be in __________ when the rate of forward reaction becomes equal to the rate of backward reaction.
6. The concentrations of reactants and products are __________ at equilibrium point.
7. The value of Kc depends upon the __________ of the reactants.
8. A increase of the value of Kc tends to move the reaction to the __________ direction.
9. A decrease of the value of Kc tends to move the reaction to the __________ direction.
10. An increase in the concentration of the reactants will move the reaction to the __________ direction.
11. A decrease in the concentration of the reactants will move the reaction to the __________ direction.
12. Equilibrium constant is denoted by __________.
13. When the equilibrium constant value is very __________, we can conclude that the forward reaction is almost completed.
14. When equilibrium constant value is very __________ we can conclude that forward reaction will occur to very little extent.
15. According to __________ principle, if system in equilibrium is subjected to a stress, the equilibrium shifts in a direction to minimize or undo the effect of the stress.
16. In exothermic reaction, the __________ of temperature favour the forward rate of reaction.
17. In endothermic reactions, the __________ of temperature favour the forward rate of reaction.
18. A __________ is a substance which effects the rate of reaction but remains unaltered at the end of the reaction.
19. A catalyst increases the velocity of the reaction by decreasing the __________.
20. The suppression of degree of ionization of a sparingly soluble weak electrolyte by the addition of a strong electrolyte containing an ion in common is called __________.
21. __________ is purified in industries by Common Ion Effect.
22. A reaction moves to the left when the concentrations of the products are __________.
23. A reaction moves to the right when the concentrations of the products are __________.
24. Increase in pressure will move the reaction in the direction of __________ volume.
25. Decrease in pressure will move the reaction in the direction of __________ volume.
26. An increase of temperature favours the formation of products in case of __________ reaction.
27. A decrease of temperature fovours the formation of products in case of __________ reaction.
28. Heating moves an endothermic reaction to the __________.
29. Cooling move an exothermic reaction to the __________.
30. The product of ionic concentration in a saturated solution is called __________ constant.
31. When HCl is added to NaCl, the concentration of __________ ion is increased.
32. Chemical reaction involving the substances in more than one phases are called __________.
33. The formation of NH3 is exothermic process hence __________ temperature will favour the formation of NH3.
34. The formation of NO from N2 and O2 is endothermic process hence __________ temperature will favour the formation of NO.
35. Chemical Equilibrium is __________ equilibrium.
36. Molar concentration is also called __________.
37. The rate at which a substance takes part in a chemical reaction depends upon its __________.
38. __________ principle is applied to all reversible reaction.
39. A common ion __________ the solubility of the salt.
40. Number of moles present per dm3 of a substance is called __________.
Chapter 7
Solutions and Electrolytes
1. A mixture of two or more substances, which are homogeneously mixed, is called a __________.
2. __________ is defined as the amount of solute dissolved in a given amount of solvent.
3. A solution is composed of two components __________ and __________.
4. A solution containing one mole of solute per dm3 of solution is called one __________ solution.
5. Molarity is denoted by __________.
6. 1M solution of NaOH contains __________ gms of it dissolved per dm3 of solution.
7. A solution containing one mole of solute dissolved by per kg of solvent is called __________ solution.
8. Molality is denoted by __________.
9. 1M solution of H2SO4 contains __________ gms of it per kg of solvent.
10. The process in which ions are surrounded by water molecules is called __________.
11. The water molecules attached with the hydrated substance are called __________.
12. Hydrated copper sulphate evolves __________ water molecules on heating.
13. The interaction between salt and water to produce acids and bases is called __________.
14. The products of ionic concentration in a saturated solution at a certain temperature are called the __________.
15. Solubility product constant expressed as __________.
16. The suppression of ionization by adding a common ion is called __________.
17. The process of dissociation of an electrolyte into ions is known as __________.
18. The chemical decomposition of a compound in a solution or in fused state brought about by a flow of electric current is known as __________.
19. Electrolysis is performed in an electrolytic cell, which is known as __________.
20. The positive electrode of a voltmeter is called __________ and negative as __________.
21. A solution, which tends to resist changes in pH is called a __________ solution.
22. A mixture of acetic acid and sodium acetate acts as a __________.
23. According to Sorenson __________ is defined as negative logarithm of the hydrogen ion concentration.
24. pH is mathematically expressed as __________.
25. The pH of a neutral solution is __________.
26. __________ substances have pH values lower than 7.
27. __________ solutions have pH values more than 7.
28. Oxidation is __________ of electron.
29. Reduction is the __________ of electron.
30. Such chemical reactions in which the oxidation number of atoms or ions is changed are called __________ reactions.
31. Oxidation number of a free element is __________.
32. Oxidation number of Oxygen in a compound is __________.
33. The sum of oxidation number of any formula of a compound is __________.
34. The oxidation number of any ion is equal to the __________ on the ion.
35. __________ is the reaction in which an acid reacts with a base to form salt and water.
36. __________ are organic compounds which change colour in accordance with the pH of the medium.
37. An indicator that changes from colourless to pink in the presence of an alkaline solution is called __________.
38. An indicator that changes from red to yellow in the presence of an alkaline solution is called __________.
39. Dissociation constant is denoted by __________.
40. According to Bronsted-Lowry Concept, __________ is the donor of proton and __________ is the acceptor of proton.
41. According to Arrhenius, acid is substance that produces __________ ions when dissolved in water.
42. According to Arrhenius, base is a substance that produces __________ ions when dissolved in water.
43. When ionic product is less than ksp, the solution will __________.
44. When ionic product is greater than ksp, the solution will __________.
45. The electrode at which oxidation takes place is called __________.
46. The electrode at which reduction takes place is called __________.
47. H3O+ ion is called __________ ion.
48. The logarithm of reciprocal of hydroxyl ion (OH)- is called __________.
49. Aqueous solution of NH4Cl is __________ while that of NaHCO3 is __________.
50. The ionic product of [H+] and [OH-] of pure water is __________.
51. An increase in the oxidation number of an element or ion during a chemical change is called __________.
52. A decrease in the oxidation number of an element or ion during a chemical change is called __________.
53. The degree of dissociation __________ with the increase in temperature.
54. The degree of dissociation __________ with the dilution of electrolytic solution.
55. A __________ consists of an electrode immersed in solution of its ion.
56. The potential difference between the electrode and the solution of its salt at equilibrium position is called __________ potential.
57. If the pH of a solution is 14, the solution is __________.
58. If the pH of a solution is 4, the solution is __________.
59. The oxidation number of Mn in KMnO4 is __________.
60. The oxidation number of Fe in FeCl3 is __________.
Chapter 8
Introduction to Chemical Kinetics
1. The branch of chemistry, which deals with the study of rates and mechanisms of chemical reactions, is known as __________.
2. Such reactions, which proceeds with very high velocities and are completed very quickly are called __________ reactions.
3. Such reactions, which take place very slowly, are called __________ reactions.
4. Reactions between silver nitrate and sodium chloride to form white precipitates of silver chloride are an example of __________ reaction.
5. Reactions of Organic compounds are slow and are called __________ reactions.
6. There are some reactions, which proceed slowly with a __________ speed.
7. The rate of __________ reaction can only be determined.
8. The amount of chemical change taking place in concentration of the per unit time is called __________ of reaction.
9. Rate of reaction is expressed in __________.
10. The rate of reaction between two specific interval of time is called __________.
11. The addition energy required to bring about a chemical reaction is called __________.
12. According to __________ theory for a chemical reaction to take place, the reacting molecules must come closed together.
13. The addition of __________ helps the reaction by lowering the energy of activation.
14. The rate of reaction __________ with the increase in concentration of the reacting molecules.
15. When the concentration of both the reacting molecules is double, the probability of collisions between them will be __________ times.
16. By __________ the surface area of the reactants, the rate of reaction is increased.
17. Rate of reaction generally __________ with the rise of temperature.
18. A __________ is a substance, which either accelerates or retards the rate of reaction without taking part in the reaction.
19. In the preparation of Oxygen from Potassium Chlorate, __________ is used as catalyst.
20. In the oxidation of SO2 to SO3 by the contact process for the manufacture of H2SO4 __________ is used as catalyst.
21. An unstable intermediate compound formed during a chemical reaction is called __________.
22. When a catalyst and the reactants are in the same phases, it is known as __________ catalyst.
23. When a catalyst and the reactants are in different phases, it is called __________.
24. When a catalyst increases the rate of reaction, it is called __________ catalyst.
25. When a catalyst retards the rate of reaction, it is called __________ catalyst.
26. A negative catalyst __________ the energy of activation, hence the rate of reaction is decreased.
27. The ratio between the rate of reaction and concentration of reactants is known as __________.
28. Velocity constant is independent of concentration but depends on __________.
29. Ionic reactions are __________ than molecular reactions.
30. The value of specific rates constant for a reaction __________ with time.
31. The sum of all exponents of concentration terms in the equation is called __________.
32. The sum of moles taking part in a chemical reaction is called __________ of the reactions.1. The property of a crystal, which is different in different directions, is called __________.
2. 0.00051 contains __________ significant figures.
3. The oxidation number of oxygen in OF2 is __________.
4. The volume of 1 gm of hydrogen gas at S.T.P is __________.
5. The oxidation number Mn in KMnO4 is __________.
6. The product of ionic concentration in a saturated solution is called __________.
7. 16 gm of oxygen at S.T.P occupies a volume of __________ dm3.
8. The shape of the orbital for which l = 0 is __________.
9. The radius of Cl-1 is __________ than the radius of Cl0.
10. Sp2 hybridization is also known as __________.
11. The value of 1 Debye is __________.
12. The reactions catalyzed by sunlight are called __________.
13. The blue colour of CuSO4 is due to the presence of __________.
14. The force of attraction between the liquid molecules and the surface of container is called __________.
15. The heat of neutralization of a strong acid and a strong base is __________.
16. C º C triple bond is __________. C = C double bond length.
17. The ions having the same electronic configuration are called iso electronic.
18. On heating, if a solid changes directly into vapours without changing into the liquid state, the phenomenon is called __________.
19. Each orbital in an atom can be completely described by __________.
20. In a molecule of alkene, __________ restricts the rotation of the group of atoms at either end of the molecule.
21. Density, refractive index and vapour pressure are __________ properties.
22. The addition of HCl to H2 solution __________ the ionization of H2S.
23. The reaction of cation or anion (or both) with water so as to change its __________ is known as Hydrolysis.
24. A reaction with higher activation energy will start at __________ temperature.
25. 6.02 x 1023 has __________ significant figures.
26. The internal resistance in the flow of liquid is called __________.
27. A catalyst increases the velocity of a reaction but decreases the __________.
Chapter 1
Introduction to Fundamental Concepts
1. 1 mole of a gas at S.T.P occupies a volume of __________.
2. A gas occupying a volume of 22.4 dm3 at S.T.P contains __________ molecules.
3. A formula, which gives the relative number of atoms in the molecule of a compound, is called __________.
4. A formula which gives the actual number of all kinds of atoms present in the molecule of compound is termed as __________.
5. The chemical formula that not only gives the actual number of atoms but also shows the arrangement of different atoms present in the molecule is called __________.
6. Atomic weight or molecular weight expressed in grams is known as __________.
7. 2 moles of H2O contain __________ grams and __________ number of molecules.
8. Any thing that occupies space and has __________ is called matter.
9. Volume of one __________ mole of a gas at S.T.P is 22.4 cubic feet.
10. A ton mole of iron is equal to __________ tons.
11. The force with which the earth attracts a body is called the __________ of the body.
12. A pure substance contains __________ kind of molecules.
13. The smallest indivisible particle of matter is called __________.
14. The atomic number is equal to the number of __________ in nucleus.
15. The atomic mass is the total number of protons and __________ in an atom of the element.
16. The average weight of atoms of an element as compared to the weight of one atom of __________ is called the atomic mass.
17. 1.0007 contains __________ significant figures.
18. The figure 24.75 will be rounded off to __________.
19. __________ means that the readings and measurements obtained in different experiments are very close to each other.
20. __________ means that the results obtained in different experiments are very close to the accepted values.
21. The degree of a measured quantity __________ with increasing number of significant figures in it.
22. The atomic mass of sodium is __________.
23. The symbolic representation of a molecule of a compound is called __________.
24. Molecular formula of CHCl3 and its Empirical formula is __________.
25. Molecular formula of benzene is C6H6 and its empirical formula is __________.
26. 58.5 is the __________ of NaCl.
27. 4.5 gms of nitrogen will have __________ molecules.
28. 28 gms of nitrogen will have __________ molecules.
29. 2 moles of SO2 is equal to __________ gms.
30. 1000 gms of H2O is equal to __________ moles.
31. The reactions, which proceed in both directions, are called __________.
32. The reactions, which proceed in forward directions only, are called __________ reactions.
33. The __________ reactions are completed after some time.
34. 0.0006 has __________ significant figures
35. 7.40 x 108 has __________ significant figures.
36. 7 x 108 has __________ significant figures.
37. Usually Molecular formula is simple multiple of the __________.
38. 0.1 mole of H2O contains __________ molecules of H2O.
39. Mass of 3.01 x 1022 molecules of CO2 is __________.
40. __________ is the branch of science which deals with the properties, composition and structure of matter.
41. None zero digits are all __________.
42. The integer part of logarithm is called __________.
43. The decimal fraction of logarithm is called __________.
44. __________ is the amount of substance, which contains as many number of particles as there are in 12 gms of Carbon.
45. 6.02 x 1023 is called the __________.
46. The accuracy of measurement depends on the number of __________.
47. __________ is the branch of chemistry that deals with quantitative relationships among the substances undergoing chemical changes.
48. The sum of atomic weights of all the elements present in molecular formula is called the __________.
49. __________ is the sum of atomic weights of the elements represented by the Empirical formula of the compound.
50. Very small and very large quantities are expressed in terms of __________.
51. In rounding off __________ figure is dropped.
52. Mole is the quantity, which has __________ particle of the substance.
53. For three significant figures, 25.55 is rounded off to __________.
54. The S.I unit of a mass is __________.
55. Mass of 6.02 x 1023 molecules of NaCl is __________ gm.
56. 1 mole of NaOH is __________ gm of NaOH.
57. Formula weight is used for __________ substances.
58. The word S.I stands for __________.
59. 4.5 gms of water will have __________ molecules.
60. 0.0087 has __________ significant figure.
Chapter 2
The Three States of Matter
1. The intermixing of gases or liquids in a container irrespective of their densities, is called __________.
2. At constant temperature, if the pressure of a given mass of a gas is decreased, its volume will __________.
3. A volume of __________ dm3 will hold 128 gms of SO2.
4. At constant temperature of a given mass of a gas, the product of its __________ and __________ is constant.
5. The rates of diffusion of gases are __________ proportional to the square root of their densities.
6. Gases deviate from ideal behaviour more markedly at high __________.
7. Liquid diffuse __________ than gases.
8. An imaginary line passing through the centre of a crystal is called __________.
9. The temperature at which more than one crystalline forms of a substance coexist in equilibrium is called __________.
10. Two or more substances crystallizing in the same form is called __________.
11. The existence of solid substances in more than one crystalline form is known as __________.
12. Rate of diffusion of gases is __________ as compared to liquids.
13. Boiling point of a liquid __________ with the pressure.
14. Mercury in a glass tube forms __________ curvature.
15. Gases can be compressed to __________ extent.
16. Viscosity of a liquid __________ with the increase of temperature.
17. Surface tension of water __________ by adding soap solution into it.
18. The internal resistance to the flow of a liquid is called __________.
19. The rise or the fall of a liquid in a capillary tube is called __________.
20. Matter exists in __________ states.
21. The freezing point of water in Fahrenheit scale is __________.
22. Boiling point of water is __________ °K.
23. SI unit for measurement of pressure is __________.
24. The value of gas law constant R = __________ dm3 atm/°K/mole.
25. The absolute Zero is equal to __________.
26. If P is plotted against 1/V at constant temperature a __________ is obtained.
27. Gases __________ in heating.
28. The pressure of air __________ at higher altitude.
29. Standard temperature means __________.
30. Standard pressure means __________.
31. Cooling is caused by __________ of gases.
32. Rate of diffusion of O2 is __________ times more than H2.
33. H2O has __________ viscosity than CH3OH.
34. Mercury does not wet the glass surface due to its higher __________.
35. Surface tension of mercury is __________ than water.
36. Viscosity can be easily measured by an instrument called __________.
37. The pressure exerted by the vapours when these vapours are in equilibrium with the liquid is called __________.
38. Vapour pressure __________ at high temperature.
39. Boyle’s Law and Charles Law can be combined into the mathematical expression __________.
40. Equal volumes of all gases at the same temperature and pressure contain __________ number of molecules.
41. The average Kinetic energy of a gas is proportional to its __________ temperature.
42. Kinetic equation may be mathematically written as __________.
43. The temperature at which two crystalline forms of a substance can coexist in equilibrium is called __________.
44. Lighter gases diffuse __________ than heavier gases.
45. Rain drops are __________ in shape.
46. Due to surface tension, the surface area of the liquid is __________.
47. Water __________ in the capillary tube.
48. Viscosity of a solution at 10°C is __________ than at 20°C.
49. Shape of NaCl crystal is __________.
50. Gases intermix to form a mixture.
51. Pressure of a dry gas is __________ than the pressure of a moist gas.
52. 22.4 dm3 of nitrogen at S.T.P will weigh equal to __________ gm.
53. 1 mole of any gas at S.T.P is equal to __________ dm3.
54. At -273°C, volume of all gases becomes __________.
55. The gases, which strictly follows the gas Laws are called __________ gas.
56. __________ is the property that determines the direction of flow of heat.
57. __________ is defined as force per unit area.
58. __________ viscosity is defined as the viscosity of a liquid as compared to the water.
Chapter 3
Structure of Atom
1. The maximum number of electrons in 2p orbital is __________.
2. 3d orbital has __________ energy than 4s orbital.
3. __________ rays are non-material in nature.
4. Charge to mass ratio of cathode rays resembles to that of __________.
5. __________ rays are most penetrating.
6. Neutrons have mass equal to that of __________.
7. Energy is __________ when an electron jumps from higher to lower orbit.
8. Second Ionization Potential has __________ value than the First Ionization Potential.
9. Electronegativity __________ from left to right in a period of Periodic Table.
10. __________ was discovered during the course of Artificial Radioactivity.
11. The velocity of alpha rays is nearly __________ of velocity of light.
12. Natural Radioactivity is confined in __________ elements.
13. The isotopes of an element differ in their __________.
14. Two electrons with the __________ spin, can never occupy the same atomic orbital.
15. ‘Al’ has electronic configuration, 1s2, 2s2, __________.
16. In a group of Periodic Table, the ionization potential __________ from top to bottom as the size of atom increases.
17. Ionization potential values __________ from left to right in a period.
18. The energy required to remove the most loosely bond electron from an atom in gaseous state is called __________.
19. The SI unit of Ionization Potential is __________.
20. An atom of sodium possesses 11 protons and __________ neutrons.
21. The particles of Cathode rays possess __________ charge.
22. The negatively charged particles found in Cathode rays are named as __________.
23. Positive rays are emitted from __________.
24. __________ rays are also known as Canal rays.
25. __________ consists of helium ions and are doubly positively charged.
26. __________ rays consists of negatively charged particles.
27. __________ rays are light waves of very short wavelength.
28. The phenomenon in which a stable element is made radioactive by artificial disintegration is called __________.
29. The electron move around the nucleus in different circular paths called __________.
30. The maximum number of electron in a shell is determined by the formula __________.
31. A particle whose mass is equal to that of electron but carries a positive charge is called __________.
32. 2p electrons are __________ in energy that 2s electrons in the same atom.
33. Number of protons of an element also indicates its __________.
34. According to __________ Principle electrons are fed in the order of increasing orbital energy.
35. According to __________ electrons are distributed among the orbitals of a sub shell to give maximum number of unpaired electron and have same spin.
36. The specific way in which the orbitals of an atom are occupied by electrons is called __________.
37. __________ rays are stream of doubly positively charged particles.
38. Electron in the outer most shell of an atom is called __________.
39. Protons are found in the __________ of an atom and bear __________ charge.
40. The atomic number of an atom is the sum of __________ inside the nucleus.
41. __________ limits the number of electron to different shell or orbits.
42. Sir William Crookes in 1878, discovered that the cathode in high vacuum tube emit radiations what he called __________.
43. X-rays were discovered in 1895 by __________.
44. The discovery of proton was done in 1886 by __________.
45. Neutrons were discovered by __________ in 1932 by the bombardment of beryllium with alpha particles.
46. Each atom has a __________, which contains all the positive charge and practically all the mass of atom.
47. Complete the reaction: 4Be9 + 2H4 ® __________ + __________.
48. __________ have higher ionization power as compared to b-rays.
49. No dark spaces between the colours are present in __________.
50. The symbol e+ represents __________.
51. p-orbitals are __________ shaped.
52. The energy released when an electron is added to an atom in the gaseous state is called __________.
53. The power of an atom to attract a shared pair of electrons towards itself is called __________.
54. Fluorine is __________ electronegative than chlorine.
55. Lyman series of spherical lines appear in the __________ portion of spectrum.
56. The electrons with __________ spin occupy the same orbital.
57. 3d orbital has __________ energy than 4s orbital.
58. Energy and frequency are __________ proportional to each other.
59. Ionic radii of cations are __________ than the atoms from which they are formed.
60. Ionic radii of anions are __________ than the atoms from which they are formed.
Chapter 4
Chemical Bonding
1. A bond formed due to transference of electron is called __________.
2. A bond formed due to sharing of electron is called __________.
3. Sigma bond is __________ than pi bond.
4. The shape of methane molecule is __________.
5. One s and 3p orbitals overlap to produce four __________ hybrid orbitals.
6. Ethene, C2H4 is an example of __________ hybridization.
7. Water molecule has __________ structure.
8. Water molecules are inter-linked with one another due to __________.
9. Polarity of the molecule is due to the difference of __________ between the two bonded atoms.
10. A chemical bond formed between to different atoms by mutual sharing of electron is termed as __________.
11. A chemical bond formed between two similar atoms by mutual sharing of electrons is known as __________.
12. The difference between the Electronegativity values of the two atoms forming covalent bond must be __________ than 1.7.
13. When two orbitals of different atoms by hybridize with each other having their axes in the same straight lines, the bond formed is termed as __________.
14. __________ bond is formed when p-orbitals of the two atoms with their axes parallel to each other overlap with each other.
15. Melting and boiling point of ionic compounds are usually __________ than that of covalent compounds.
16. Non polar compounds are usually __________ in non polar solvent.
17. The nitrogen in NH3 is __________ hybridized.
18. A hybrid orbital is called __________ orbital.
19. Since dipole moment of CS2 is zero, it is a __________ molecule.
20. A bond formed due to the electrostatic forces of attraction between the oppositely charged ions is called __________ bond.
21. The ionic bond is formed between the atoms with low ionization potential and high __________.
22. A bond formed by the sharing of an electron pair contributed by one atom only is called a __________ bond.
23. A co-ordinate covalent bond is also known as __________ bond.
24. Polar covalent bond is __________ than a non polar covalent bond.
25. H-F bond is __________ than H-Br bond.
26. The SI unit of dipole moment is __________.
27. Commonly used unit of dipole moment is __________.
28. Dipole moment of non-polar compound is __________ D.
29. The reactions of ionic compounds are usually very __________.
30. Covalent compounds are generally __________ in nature.
31. Ionic compounds are generally __________ in nature.
32. A covalent bond is represented by a __________.
33. A co-ordinate covalent bond is represented by an __________.
34. The covalent bond between H-F is called __________ covalent bond.
35. The power of an atom to attract a shared pair of electron itself is called __________ of that atom.
36. m = d x e represents __________.
37. CO2 and SO2 molecules have __________ polar bonds.
38. NH3 molecule has __________ polar bonds.
39. A double bond has __________ bond energy than a single bond.
40. An orbital which surrounds a single nucleus is called __________ orbital.
41. An orbital which surrounds two or more atomic nuclei is called __________ orbital.
42. A molecular orbital, which is of lower energy than the atomic orbitals from which it is derived, is known as __________ orbital.
43. A molecular orbital, which has higher energy than the atomic orbitals from which it is derived, is known as __________ orbital.
44. Orbitals formed after hybridization are called __________ orbitals.
45. Bond angle in Sp3 hybridization is of __________.
46. Bond angle in Sp2 hybridization is of __________.
47. Bond angle in Sp hybridization is of __________.
48. Sp3 hybridization is also known as __________.
49. Sp2 hybridization is also known as __________.
50. Sp hybridization is also known as __________.
51. A pair of electrons residing on the central atom and which is not used in bonding is called a __________.
52. The sum of total number of electron pairs (bonding and lone pairs) is called __________ number.
53. __________ bond is usually expressed by dotted line.
54. Water molecule has dipole moment because of its __________ structure.
55. CO2 is non polar because of its __________ structure.
56. Overlapping in __________ bond is perfect.
57. Overlapping in __________ bond is not perfect.
58. H-H bond is __________ than H-Cl bond.
59. __________ hybrid orbitals are not co-planar.
60. Covalent bond is Cl2 molecule is __________.
Chapter 5
Energetics of Chemical Reaction
1. The branch of Chemistry, which deals with the heat changes that take place during chemical reaction, is called __________.
2. The branch of science which deals with energy changes accompanying physical and chemical transformation is called __________.
3. The amount of heat evolved or absorbed in a chemical reaction is called __________.
4. Such reactions in which heat is evolved are called __________ reactions.
5. Such reactions in which heat is absorbed are called __________ reactions.
6. In exothermic reactions, heat evolved is given by __________ sign of DH.
7. In endothermic reactions heat absorbed is given by __________ sign of DH.
8. The total heat change in a reaction is the same whether it takes place in one or several steps.
9. The first law of thermodynamics is also known as __________.
10. The part of universe under observation is called __________.
11. The system plus its surrounding is called __________.
12. Such properties, which give description of a system at a particular moment, is called __________.
13. The term E + PV is called __________.
14. DH represents change in __________.
15. The temperature of water is raised up when sulphuric acid is added to it. This is an __________ reaction.
16. The characteristic properties of a system which is independent of amount of material concerned is called __________ properties.
17. The characteristic properties of a system which depend on amount of substance present in it is called __________ properties.
18. Density, pressure and temperature are the examples of __________ properties.
19. Mole numbers and enthalpy are the examples of __________ properties.
20. A system, which exchange both energy and matter with its surrounding, is called __________ system.
21. A system, which only exchange energy with the surrounding but not matter is, called __________ system.
22. A system which neither exchange energy nor matter with its surrounding is called __________ system.
23. A system is __________ if it contains only one phase.
24. A system is __________ if it contains more than one phase.
25. 1 kilojoule is equal to __________ joules.
26. 1 Calorie is equal to __________ joules.
27. 1 kilo calorie is equal to __________ joules.
28. The work done (w) is mathematically denoted by __________.
29. The change in enthalpy is denoted by __________.
30. __________ law is used in calculating heat of reaction.
31. __________ is defined as the change in enthalpy when one gram mole of a compound is produced from its element.
32. Heat of formation is denoted by __________.
33. When the work is done on the system by the surrounding the sign of work done (w) is __________.
34. When the work is done by the system on surrounding the sign of work done is __________.
35. First law of Thermodynamics is mathematically represented as __________.
36. Standard enthalpies are measured at __________.
37. Hess’s Law is employed to calculate __________ of a chemical reaction.
38. Heat absorbed by the system at constant volume is completely utilize to increase the __________ of the system.
39. Heat change at constant pressure from initial to final state of the system is simply equal to the __________.
40. SI unit of measurement of heat change is __________.
Chapter 6
Chemical Equilibrium
1. The reactions, which proceed in both the directions, are called __________ reactions.
2. The reactions, which proceed to one direction only, are called __________ reactions.
3. Reversible reactions are __________ completed.
4. Irreversible reactions are __________ after some time.
5. A reversible reaction is said to be in __________ when the rate of forward reaction becomes equal to the rate of backward reaction.
6. The concentrations of reactants and products are __________ at equilibrium point.
7. The value of Kc depends upon the __________ of the reactants.
8. A increase of the value of Kc tends to move the reaction to the __________ direction.
9. A decrease of the value of Kc tends to move the reaction to the __________ direction.
10. An increase in the concentration of the reactants will move the reaction to the __________ direction.
11. A decrease in the concentration of the reactants will move the reaction to the __________ direction.
12. Equilibrium constant is denoted by __________.
13. When the equilibrium constant value is very __________, we can conclude that the forward reaction is almost completed.
14. When equilibrium constant value is very __________ we can conclude that forward reaction will occur to very little extent.
15. According to __________ principle, if system in equilibrium is subjected to a stress, the equilibrium shifts in a direction to minimize or undo the effect of the stress.
16. In exothermic reaction, the __________ of temperature favour the forward rate of reaction.
17. In endothermic reactions, the __________ of temperature favour the forward rate of reaction.
18. A __________ is a substance which effects the rate of reaction but remains unaltered at the end of the reaction.
19. A catalyst increases the velocity of the reaction by decreasing the __________.
20. The suppression of degree of ionization of a sparingly soluble weak electrolyte by the addition of a strong electrolyte containing an ion in common is called __________.
21. __________ is purified in industries by Common Ion Effect.
22. A reaction moves to the left when the concentrations of the products are __________.
23. A reaction moves to the right when the concentrations of the products are __________.
24. Increase in pressure will move the reaction in the direction of __________ volume.
25. Decrease in pressure will move the reaction in the direction of __________ volume.
26. An increase of temperature favours the formation of products in case of __________ reaction.
27. A decrease of temperature fovours the formation of products in case of __________ reaction.
28. Heating moves an endothermic reaction to the __________.
29. Cooling move an exothermic reaction to the __________.
30. The product of ionic concentration in a saturated solution is called __________ constant.
31. When HCl is added to NaCl, the concentration of __________ ion is increased.
32. Chemical reaction involving the substances in more than one phases are called __________.
33. The formation of NH3 is exothermic process hence __________ temperature will favour the formation of NH3.
34. The formation of NO from N2 and O2 is endothermic process hence __________ temperature will favour the formation of NO.
35. Chemical Equilibrium is __________ equilibrium.
36. Molar concentration is also called __________.
37. The rate at which a substance takes part in a chemical reaction depends upon its __________.
38. __________ principle is applied to all reversible reaction.
39. A common ion __________ the solubility of the salt.
40. Number of moles present per dm3 of a substance is called __________.
Chapter 7
Solutions and Electrolytes
1. A mixture of two or more substances, which are homogeneously mixed, is called a __________.
2. __________ is defined as the amount of solute dissolved in a given amount of solvent.
3. A solution is composed of two components __________ and __________.
4. A solution containing one mole of solute per dm3 of solution is called one __________ solution.
5. Molarity is denoted by __________.
6. 1M solution of NaOH contains __________ gms of it dissolved per dm3 of solution.
7. A solution containing one mole of solute dissolved by per kg of solvent is called __________ solution.
8. Molality is denoted by __________.
9. 1M solution of H2SO4 contains __________ gms of it per kg of solvent.
10. The process in which ions are surrounded by water molecules is called __________.
11. The water molecules attached with the hydrated substance are called __________.
12. Hydrated copper sulphate evolves __________ water molecules on heating.
13. The interaction between salt and water to produce acids and bases is called __________.
14. The products of ionic concentration in a saturated solution at a certain temperature are called the __________.
15. Solubility product constant expressed as __________.
16. The suppression of ionization by adding a common ion is called __________.
17. The process of dissociation of an electrolyte into ions is known as __________.
18. The chemical decomposition of a compound in a solution or in fused state brought about by a flow of electric current is known as __________.
19. Electrolysis is performed in an electrolytic cell, which is known as __________.
20. The positive electrode of a voltmeter is called __________ and negative as __________.
21. A solution, which tends to resist changes in pH is called a __________ solution.
22. A mixture of acetic acid and sodium acetate acts as a __________.
23. According to Sorenson __________ is defined as negative logarithm of the hydrogen ion concentration.
24. pH is mathematically expressed as __________.
25. The pH of a neutral solution is __________.
26. __________ substances have pH values lower than 7.
27. __________ solutions have pH values more than 7.
28. Oxidation is __________ of electron.
29. Reduction is the __________ of electron.
30. Such chemical reactions in which the oxidation number of atoms or ions is changed are called __________ reactions.
31. Oxidation number of a free element is __________.
32. Oxidation number of Oxygen in a compound is __________.
33. The sum of oxidation number of any formula of a compound is __________.
34. The oxidation number of any ion is equal to the __________ on the ion.
35. __________ is the reaction in which an acid reacts with a base to form salt and water.
36. __________ are organic compounds which change colour in accordance with the pH of the medium.
37. An indicator that changes from colourless to pink in the presence of an alkaline solution is called __________.
38. An indicator that changes from red to yellow in the presence of an alkaline solution is called __________.
39. Dissociation constant is denoted by __________.
40. According to Bronsted-Lowry Concept, __________ is the donor of proton and __________ is the acceptor of proton.
41. According to Arrhenius, acid is substance that produces __________ ions when dissolved in water.
42. According to Arrhenius, base is a substance that produces __________ ions when dissolved in water.
43. When ionic product is less than ksp, the solution will __________.
44. When ionic product is greater than ksp, the solution will __________.
45. The electrode at which oxidation takes place is called __________.
46. The electrode at which reduction takes place is called __________.
47. H3O+ ion is called __________ ion.
48. The logarithm of reciprocal of hydroxyl ion (OH)- is called __________.
49. Aqueous solution of NH4Cl is __________ while that of NaHCO3 is __________.
50. The ionic product of [H+] and [OH-] of pure water is __________.
51. An increase in the oxidation number of an element or ion during a chemical change is called __________.
52. A decrease in the oxidation number of an element or ion during a chemical change is called __________.
53. The degree of dissociation __________ with the increase in temperature.
54. The degree of dissociation __________ with the dilution of electrolytic solution.
55. A __________ consists of an electrode immersed in solution of its ion.
56. The potential difference between the electrode and the solution of its salt at equilibrium position is called __________ potential.
57. If the pH of a solution is 14, the solution is __________.
58. If the pH of a solution is 4, the solution is __________.
59. The oxidation number of Mn in KMnO4 is __________.
60. The oxidation number of Fe in FeCl3 is __________.
Chapter 8
Introduction to Chemical Kinetics
1. The branch of chemistry, which deals with the study of rates and mechanisms of chemical reactions, is known as __________.
2. Such reactions, which proceeds with very high velocities and are completed very quickly are called __________ reactions.
3. Such reactions, which take place very slowly, are called __________ reactions.
4. Reactions between silver nitrate and sodium chloride to form white precipitates of silver chloride are an example of __________ reaction.
5. Reactions of Organic compounds are slow and are called __________ reactions.
6. There are some reactions, which proceed slowly with a __________ speed.
7. The rate of __________ reaction can only be determined.
8. The amount of chemical change taking place in concentration of the per unit time is called __________ of reaction.
9. Rate of reaction is expressed in __________.
10. The rate of reaction between two specific interval of time is called __________.
11. The addition energy required to bring about a chemical reaction is called __________.
12. According to __________ theory for a chemical reaction to take place, the reacting molecules must come closed together.
13. The addition of __________ helps the reaction by lowering the energy of activation.
14. The rate of reaction __________ with the increase in concentration of the reacting molecules.
15. When the concentration of both the reacting molecules is double, the probability of collisions between them will be __________ times.
16. By __________ the surface area of the reactants, the rate of reaction is increased.
17. Rate of reaction generally __________ with the rise of temperature.
18. A __________ is a substance, which either accelerates or retards the rate of reaction without taking part in the reaction.
19. In the preparation of Oxygen from Potassium Chlorate, __________ is used as catalyst.
20. In the oxidation of SO2 to SO3 by the contact process for the manufacture of H2SO4 __________ is used as catalyst.
21. An unstable intermediate compound formed during a chemical reaction is called __________.
22. When a catalyst and the reactants are in the same phases, it is known as __________ catalyst.
23. When a catalyst and the reactants are in different phases, it is called __________.
24. When a catalyst increases the rate of reaction, it is called __________ catalyst.
25. When a catalyst retards the rate of reaction, it is called __________ catalyst.
26. A negative catalyst __________ the energy of activation, hence the rate of reaction is decreased.
27. The ratio between the rate of reaction and concentration of reactants is known as __________.
28. Velocity constant is independent of concentration but depends on __________.
29. Ionic reactions are __________ than molecular reactions.
30. The value of specific rates constant for a reaction __________ with time.
31. The sum of all exponents of concentration terms in the equation is called __________.
32. The sum of moles taking part in a chemical reaction is called __________ of the reactions.
2. 0.00051 contains __________ significant figures.
3. The oxidation number of oxygen in OF2 is __________.
4. The volume of 1 gm of hydrogen gas at S.T.P is __________.
5. The oxidation number Mn in KMnO4 is __________.
6. The product of ionic concentration in a saturated solution is called __________.
7. 16 gm of oxygen at S.T.P occupies a volume of __________ dm3.
8. The shape of the orbital for which l = 0 is __________.
9. The radius of Cl-1 is __________ than the radius of Cl0.
10. Sp2 hybridization is also known as __________.
11. The value of 1 Debye is __________.
12. The reactions catalyzed by sunlight are called __________.
13. The blue colour of CuSO4 is due to the presence of __________.
14. The force of attraction between the liquid molecules and the surface of container is called __________.
15. The heat of neutralization of a strong acid and a strong base is __________.
16. C º C triple bond is __________. C = C double bond length.
17. The ions having the same electronic configuration are called iso electronic.
18. On heating, if a solid changes directly into vapours without changing into the liquid state, the phenomenon is called __________.
19. Each orbital in an atom can be completely described by __________.
20. In a molecule of alkene, __________ restricts the rotation of the group of atoms at either end of the molecule.
21. Density, refractive index and vapour pressure are __________ properties.
22. The addition of HCl to H2 solution __________ the ionization of H2S.
23. The reaction of cation or anion (or both) with water so as to change its __________ is known as Hydrolysis.
24. A reaction with higher activation energy will start at __________ temperature.
25. 6.02 x 1023 has __________ significant figures.
26. The internal resistance in the flow of liquid is called __________.
27. A catalyst increases the velocity of a reaction but decreases the __________.
Chapter 1
Introduction to Fundamental Concepts
1. 1 mole of a gas at S.T.P occupies a volume of __________.
2. A gas occupying a volume of 22.4 dm3 at S.T.P contains __________ molecules.
3. A formula, which gives the relative number of atoms in the molecule of a compound, is called __________.
4. A formula which gives the actual number of all kinds of atoms present in the molecule of compound is termed as __________.
5. The chemical formula that not only gives the actual number of atoms but also shows the arrangement of different atoms present in the molecule is called __________.
6. Atomic weight or molecular weight expressed in grams is known as __________.
7. 2 moles of H2O contain __________ grams and __________ number of molecules.
8. Any thing that occupies space and has __________ is called matter.
9. Volume of one __________ mole of a gas at S.T.P is 22.4 cubic feet.
10. A ton mole of iron is equal to __________ tons.
11. The force with which the earth attracts a body is called the __________ of the body.
12. A pure substance contains __________ kind of molecules.
13. The smallest indivisible particle of matter is called __________.
14. The atomic number is equal to the number of __________ in nucleus.
15. The atomic mass is the total number of protons and __________ in an atom of the element.
16. The average weight of atoms of an element as compared to the weight of one atom of __________ is called the atomic mass.
17. 1.0007 contains __________ significant figures.
18. The figure 24.75 will be rounded off to __________.
19. __________ means that the readings and measurements obtained in different experiments are very close to each other.
20. __________ means that the results obtained in different experiments are very close to the accepted values.
21. The degree of a measured quantity __________ with increasing number of significant figures in it.
22. The atomic mass of sodium is __________.
23. The symbolic representation of a molecule of a compound is called __________.
24. Molecular formula of CHCl3 and its Empirical formula is __________.
25. Molecular formula of benzene is C6H6 and its empirical formula is __________.
26. 58.5 is the __________ of NaCl.
27. 4.5 gms of nitrogen will have __________ molecules.
28. 28 gms of nitrogen will have __________ molecules.
29. 2 moles of SO2 is equal to __________ gms.
30. 1000 gms of H2O is equal to __________ moles.
31. The reactions, which proceed in both directions, are called __________.
32. The reactions, which proceed in forward directions only, are called __________ reactions.
33. The __________ reactions are completed after some time.
34. 0.0006 has __________ significant figures
35. 7.40 x 108 has __________ significant figures.
36. 7 x 108 has __________ significant figures.
37. Usually Molecular formula is simple multiple of the __________.
38. 0.1 mole of H2O contains __________ molecules of H2O.
39. Mass of 3.01 x 1022 molecules of CO2 is __________.
40. __________ is the branch of science which deals with the properties, composition and structure of matter.
41. None zero digits are all __________.
42. The integer part of logarithm is called __________.
43. The decimal fraction of logarithm is called __________.
44. __________ is the amount of substance, which contains as many number of particles as there are in 12 gms of Carbon.
45. 6.02 x 1023 is called the __________.
46. The accuracy of measurement depends on the number of __________.
47. __________ is the branch of chemistry that deals with quantitative relationships among the substances undergoing chemical changes.
48. The sum of atomic weights of all the elements present in molecular formula is called the __________.
49. __________ is the sum of atomic weights of the elements represented by the Empirical formula of the compound.
50. Very small and very large quantities are expressed in terms of __________.
51. In rounding off __________ figure is dropped.
52. Mole is the quantity, which has __________ particle of the substance.
53. For three significant figures, 25.55 is rounded off to __________.
54. The S.I unit of a mass is __________.
55. Mass of 6.02 x 1023 molecules of NaCl is __________ gm.
56. 1 mole of NaOH is __________ gm of NaOH.
57. Formula weight is used for __________ substances.
58. The word S.I stands for __________.
59. 4.5 gms of water will have __________ molecules.
60. 0.0087 has __________ significant figure.
Chapter 2
The Three States of Matter
1. The intermixing of gases or liquids in a container irrespective of their densities, is called __________.
2. At constant temperature, if the pressure of a given mass of a gas is decreased, its volume will __________.
3. A volume of __________ dm3 will hold 128 gms of SO2.
4. At constant temperature of a given mass of a gas, the product of its __________ and __________ is constant.
5. The rates of diffusion of gases are __________ proportional to the square root of their densities.
6. Gases deviate from ideal behaviour more markedly at high __________.
7. Liquid diffuse __________ than gases.
8. An imaginary line passing through the centre of a crystal is called __________.
9. The temperature at which more than one crystalline forms of a substance coexist in equilibrium is called __________.
10. Two or more substances crystallizing in the same form is called __________.
11. The existence of solid substances in more than one crystalline form is known as __________.
12. Rate of diffusion of gases is __________ as compared to liquids.
13. Boiling point of a liquid __________ with the pressure.
14. Mercury in a glass tube forms __________ curvature.
15. Gases can be compressed to __________ extent.
16. Viscosity of a liquid __________ with the increase of temperature.
17. Surface tension of water __________ by adding soap solution into it.
18. The internal resistance to the flow of a liquid is called __________.
19. The rise or the fall of a liquid in a capillary tube is called __________.
20. Matter exists in __________ states.
21. The freezing point of water in Fahrenheit scale is __________.
22. Boiling point of water is __________ °K.
23. SI unit for measurement of pressure is __________.
24. The value of gas law constant R = __________ dm3 atm/°K/mole.
25. The absolute Zero is equal to __________.
26. If P is plotted against 1/V at constant temperature a __________ is obtained.
27. Gases __________ in heating.
28. The pressure of air __________ at higher altitude.
29. Standard temperature means __________.
30. Standard pressure means __________.
31. Cooling is caused by __________ of gases.
32. Rate of diffusion of O2 is __________ times more than H2.
33. H2O has __________ viscosity than CH3OH.
34. Mercury does not wet the glass surface due to its higher __________.
35. Surface tension of mercury is __________ than water.
36. Viscosity can be easily measured by an instrument called __________.
37. The pressure exerted by the vapours when these vapours are in equilibrium with the liquid is called __________.
38. Vapour pressure __________ at high temperature.
39. Boyle’s Law and Charles Law can be combined into the mathematical expression __________.
40. Equal volumes of all gases at the same temperature and pressure contain __________ number of molecules.
41. The average Kinetic energy of a gas is proportional to its __________ temperature.
42. Kinetic equation may be mathematically written as __________.
43. The temperature at which two crystalline forms of a substance can coexist in equilibrium is called __________.
44. Lighter gases diffuse __________ than heavier gases.
45. Rain drops are __________ in shape.
46. Due to surface tension, the surface area of the liquid is __________.
47. Water __________ in the capillary tube.
48. Viscosity of a solution at 10°C is __________ than at 20°C.
49. Shape of NaCl crystal is __________.
50. Gases intermix to form a mixture.
51. Pressure of a dry gas is __________ than the pressure of a moist gas.
52. 22.4 dm3 of nitrogen at S.T.P will weigh equal to __________ gm.
53. 1 mole of any gas at S.T.P is equal to __________ dm3.
54. At -273°C, volume of all gases becomes __________.
55. The gases, which strictly follows the gas Laws are called __________ gas.
56. __________ is the property that determines the direction of flow of heat.
57. __________ is defined as force per unit area.
58. __________ viscosity is defined as the viscosity of a liquid as compared to the water.
Chapter 3
Structure of Atom
1. The maximum number of electrons in 2p orbital is __________.
2. 3d orbital has __________ energy than 4s orbital.
3. __________ rays are non-material in nature.
4. Charge to mass ratio of cathode rays resembles to that of __________.
5. __________ rays are most penetrating.
6. Neutrons have mass equal to that of __________.
7. Energy is __________ when an electron jumps from higher to lower orbit.
8. Second Ionization Potential has __________ value than the First Ionization Potential.
9. Electronegativity __________ from left to right in a period of Periodic Table.
10. __________ was discovered during the course of Artificial Radioactivity.
11. The velocity of alpha rays is nearly __________ of velocity of light.
12. Natural Radioactivity is confined in __________ elements.
13. The isotopes of an element differ in their __________.
14. Two electrons with the __________ spin, can never occupy the same atomic orbital.
15. ‘Al’ has electronic configuration, 1s2, 2s2, __________.
16. In a group of Periodic Table, the ionization potential __________ from top to bottom as the size of atom increases.
17. Ionization potential values __________ from left to right in a period.
18. The energy required to remove the most loosely bond electron from an atom in gaseous state is called __________.
19. The SI unit of Ionization Potential is __________.
20. An atom of sodium possesses 11 protons and __________ neutrons.
21. The particles of Cathode rays possess __________ charge.
22. The negatively charged particles found in Cathode rays are named as __________.
23. Positive rays are emitted from __________.
24. __________ rays are also known as Canal rays.
25. __________ consists of helium ions and are doubly positively charged.
26. __________ rays consists of negatively charged particles.
27. __________ rays are light waves of very short wavelength.
28. The phenomenon in which a stable element is made radioactive by artificial disintegration is called __________.
29. The electron move around the nucleus in different circular paths called __________.
30. The maximum number of electron in a shell is determined by the formula __________.
31. A particle whose mass is equal to that of electron but carries a positive charge is called __________.
32. 2p electrons are __________ in energy that 2s electrons in the same atom.
33. Number of protons of an element also indicates its __________.
34. According to __________ Principle electrons are fed in the order of increasing orbital energy.
35. According to __________ electrons are distributed among the orbitals of a sub shell to give maximum number of unpaired electron and have same spin.
36. The specific way in which the orbitals of an atom are occupied by electrons is called __________.
37. __________ rays are stream of doubly positively charged particles.
38. Electron in the outer most shell of an atom is called __________.
39. Protons are found in the __________ of an atom and bear __________ charge.
40. The atomic number of an atom is the sum of __________ inside the nucleus.
41. __________ limits the number of electron to different shell or orbits.
42. Sir William Crookes in 1878, discovered that the cathode in high vacuum tube emit radiations what he called __________.
43. X-rays were discovered in 1895 by __________.
44. The discovery of proton was done in 1886 by __________.
45. Neutrons were discovered by __________ in 1932 by the bombardment of beryllium with alpha particles.
46. Each atom has a __________, which contains all the positive charge and practically all the mass of atom.
47. Complete the reaction: 4Be9 + 2H4 ® __________ + __________.
48. __________ have higher ionization power as compared to b-rays.
49. No dark spaces between the colours are present in __________.
50. The symbol e+ represents __________.
51. p-orbitals are __________ shaped.
52. The energy released when an electron is added to an atom in the gaseous state is called __________.
53. The power of an atom to attract a shared pair of electrons towards itself is called __________.
54. Fluorine is __________ electronegative than chlorine.
55. Lyman series of spherical lines appear in the __________ portion of spectrum.
56. The electrons with __________ spin occupy the same orbital.
57. 3d orbital has __________ energy than 4s orbital.
58. Energy and frequency are __________ proportional to each other.
59. Ionic radii of cations are __________ than the atoms from which they are formed.
60. Ionic radii of anions are __________ than the atoms from which they are formed.
Chapter 4
Chemical Bonding
1. A bond formed due to transference of electron is called __________.
2. A bond formed due to sharing of electron is called __________.
3. Sigma bond is __________ than pi bond.
4. The shape of methane molecule is __________.
5. One s and 3p orbitals overlap to produce four __________ hybrid orbitals.
6. Ethene, C2H4 is an example of __________ hybridization.
7. Water molecule has __________ structure.
8. Water molecules are inter-linked with one another due to __________.
9. Polarity of the molecule is due to the difference of __________ between the two bonded atoms.
10. A chemical bond formed between to different atoms by mutual sharing of electron is termed as __________.
11. A chemical bond formed between two similar atoms by mutual sharing of electrons is known as __________.
12. The difference between the Electronegativity values of the two atoms forming covalent bond must be __________ than 1.7.
13. When two orbitals of different atoms by hybridize with each other having their axes in the same straight lines, the bond formed is termed as __________.
14. __________ bond is formed when p-orbitals of the two atoms with their axes parallel to each other overlap with each other.
15. Melting and boiling point of ionic compounds are usually __________ than that of covalent compounds.
16. Non polar compounds are usually __________ in non polar solvent.
17. The nitrogen in NH3 is __________ hybridized.
18. A hybrid orbital is called __________ orbital.
19. Since dipole moment of CS2 is zero, it is a __________ molecule.
20. A bond formed due to the electrostatic forces of attraction between the oppositely charged ions is called __________ bond.
21. The ionic bond is formed between the atoms with low ionization potential and high __________.
22. A bond formed by the sharing of an electron pair contributed by one atom only is called a __________ bond.
23. A co-ordinate covalent bond is also known as __________ bond.
24. Polar covalent bond is __________ than a non polar covalent bond.
25. H-F bond is __________ than H-Br bond.
26. The SI unit of dipole moment is __________.
27. Commonly used unit of dipole moment is __________.
28. Dipole moment of non-polar compound is __________ D.
29. The reactions of ionic compounds are usually very __________.
30. Covalent compounds are generally __________ in nature.
31. Ionic compounds are generally __________ in nature.
32. A covalent bond is represented by a __________.
33. A co-ordinate covalent bond is represented by an __________.
34. The covalent bond between H-F is called __________ covalent bond.
35. The power of an atom to attract a shared pair of electron itself is called __________ of that atom.
36. m = d x e represents __________.
37. CO2 and SO2 molecules have __________ polar bonds.
38. NH3 molecule has __________ polar bonds.
39. A double bond has __________ bond energy than a single bond.
40. An orbital which surrounds a single nucleus is called __________ orbital.
41. An orbital which surrounds two or more atomic nuclei is called __________ orbital.
42. A molecular orbital, which is of lower energy than the atomic orbitals from which it is derived, is known as __________ orbital.
43. A molecular orbital, which has higher energy than the atomic orbitals from which it is derived, is known as __________ orbital.
44. Orbitals formed after hybridization are called __________ orbitals.
45. Bond angle in Sp3 hybridization is of __________.
46. Bond angle in Sp2 hybridization is of __________.
47. Bond angle in Sp hybridization is of __________.
48. Sp3 hybridization is also known as __________.
49. Sp2 hybridization is also known as __________.
50. Sp hybridization is also known as __________.
51. A pair of electrons residing on the central atom and which is not used in bonding is called a __________.
52. The sum of total number of electron pairs (bonding and lone pairs) is called __________ number.
53. __________ bond is usually expressed by dotted line.
54. Water molecule has dipole moment because of its __________ structure.
55. CO2 is non polar because of its __________ structure.
56. Overlapping in __________ bond is perfect.
57. Overlapping in __________ bond is not perfect.
58. H-H bond is __________ than H-Cl bond.
59. __________ hybrid orbitals are not co-planar.
60. Covalent bond is Cl2 molecule is __________.
Chapter 5
Energetics of Chemical Reaction
1. The branch of Chemistry, which deals with the heat changes that take place during chemical reaction, is called __________.
2. The branch of science which deals with energy changes accompanying physical and chemical transformation is called __________.
3. The amount of heat evolved or absorbed in a chemical reaction is called __________.
4. Such reactions in which heat is evolved are called __________ reactions.
5. Such reactions in which heat is absorbed are called __________ reactions.
6. In exothermic reactions, heat evolved is given by __________ sign of DH.
7. In endothermic reactions heat absorbed is given by __________ sign of DH.
8. The total heat change in a reaction is the same whether it takes place in one or several steps.
9. The first law of thermodynamics is also known as __________.
10. The part of universe under observation is called __________.
11. The system plus its surrounding is called __________.
12. Such properties, which give description of a system at a particular moment, is called __________.
13. The term E + PV is called __________.
14. DH represents change in __________.
15. The temperature of water is raised up when sulphuric acid is added to it. This is an __________ reaction.
16. The characteristic properties of a system which is independent of amount of material concerned is called __________ properties.
17. The characteristic properties of a system which depend on amount of substance present in it is called __________ properties.
18. Density, pressure and temperature are the examples of __________ properties.
19. Mole numbers and enthalpy are the examples of __________ properties.
20. A system, which exchange both energy and matter with its surrounding, is called __________ system.
21. A system, which only exchange energy with the surrounding but not matter is, called __________ system.
22. A system which neither exchange energy nor matter with its surrounding is called __________ system.
23. A system is __________ if it contains only one phase.
24. A system is __________ if it contains more than one phase.
25. 1 kilojoule is equal to __________ joules.
26. 1 Calorie is equal to __________ joules.
27. 1 kilo calorie is equal to __________ joules.
28. The work done (w) is mathematically denoted by __________.
29. The change in enthalpy is denoted by __________.
30. __________ law is used in calculating heat of reaction.
31. __________ is defined as the change in enthalpy when one gram mole of a compound is produced from its element.
32. Heat of formation is denoted by __________.
33. When the work is done on the system by the surrounding the sign of work done (w) is __________.
34. When the work is done by the system on surrounding the sign of work done is __________.
35. First law of Thermodynamics is mathematically represented as __________.
36. Standard enthalpies are measured at __________.
37. Hess’s Law is employed to calculate __________ of a chemical reaction.
38. Heat absorbed by the system at constant volume is completely utilize to increase the __________ of the system.
39. Heat change at constant pressure from initial to final state of the system is simply equal to the __________.
40. SI unit of measurement of heat change is __________.
Chapter 6
Chemical Equilibrium
1. The reactions, which proceed in both the directions, are called __________ reactions.
2. The reactions, which proceed to one direction only, are called __________ reactions.
3. Reversible reactions are __________ completed.
4. Irreversible reactions are __________ after some time.
5. A reversible reaction is said to be in __________ when the rate of forward reaction becomes equal to the rate of backward reaction.
6. The concentrations of reactants and products are __________ at equilibrium point.
7. The value of Kc depends upon the __________ of the reactants.
8. A increase of the value of Kc tends to move the reaction to the __________ direction.
9. A decrease of the value of Kc tends to move the reaction to the __________ direction.
10. An increase in the concentration of the reactants will move the reaction to the __________ direction.
11. A decrease in the concentration of the reactants will move the reaction to the __________ direction.
12. Equilibrium constant is denoted by __________.
13. When the equilibrium constant value is very __________, we can conclude that the forward reaction is almost completed.
14. When equilibrium constant value is very __________ we can conclude that forward reaction will occur to very little extent.
15. According to __________ principle, if system in equilibrium is subjected to a stress, the equilibrium shifts in a direction to minimize or undo the effect of the stress.
16. In exothermic reaction, the __________ of temperature favour the forward rate of reaction.
17. In endothermic reactions, the __________ of temperature favour the forward rate of reaction.
18. A __________ is a substance which effects the rate of reaction but remains unaltered at the end of the reaction.
19. A catalyst increases the velocity of the reaction by decreasing the __________.
20. The suppression of degree of ionization of a sparingly soluble weak electrolyte by the addition of a strong electrolyte containing an ion in common is called __________.
21. __________ is purified in industries by Common Ion Effect.
22. A reaction moves to the left when the concentrations of the products are __________.
23. A reaction moves to the right when the concentrations of the products are __________.
24. Increase in pressure will move the reaction in the direction of __________ volume.
25. Decrease in pressure will move the reaction in the direction of __________ volume.
26. An increase of temperature favours the formation of products in case of __________ reaction.
27. A decrease of temperature fovours the formation of products in case of __________ reaction.
28. Heating moves an endothermic reaction to the __________.
29. Cooling move an exothermic reaction to the __________.
30. The product of ionic concentration in a saturated solution is called __________ constant.
31. When HCl is added to NaCl, the concentration of __________ ion is increased.
32. Chemical reaction involving the substances in more than one phases are called __________.
33. The formation of NH3 is exothermic process hence __________ temperature will favour the formation of NH3.
34. The formation of NO from N2 and O2 is endothermic process hence __________ temperature will favour the formation of NO.
35. Chemical Equilibrium is __________ equilibrium.
36. Molar concentration is also called __________.
37. The rate at which a substance takes part in a chemical reaction depends upon its __________.
38. __________ principle is applied to all reversible reaction.
39. A common ion __________ the solubility of the salt.
40. Number of moles present per dm3 of a substance is called __________.
Chapter 7
Solutions and Electrolytes
1. A mixture of two or more substances, which are homogeneously mixed, is called a __________.
2. __________ is defined as the amount of solute dissolved in a given amount of solvent.
3. A solution is composed of two components __________ and __________.
4. A solution containing one mole of solute per dm3 of solution is called one __________ solution.
5. Molarity is denoted by __________.
6. 1M solution of NaOH contains __________ gms of it dissolved per dm3 of solution.
7. A solution containing one mole of solute dissolved by per kg of solvent is called __________ solution.
8. Molality is denoted by __________.
9. 1M solution of H2SO4 contains __________ gms of it per kg of solvent.
10. The process in which ions are surrounded by water molecules is called __________.
11. The water molecules attached with the hydrated substance are called __________.
12. Hydrated copper sulphate evolves __________ water molecules on heating.
13. The interaction between salt and water to produce acids and bases is called __________.
14. The products of ionic concentration in a saturated solution at a certain temperature are called the __________.
15. Solubility product constant expressed as __________.
16. The suppression of ionization by adding a common ion is called __________.
17. The process of dissociation of an electrolyte into ions is known as __________.
18. The chemical decomposition of a compound in a solution or in fused state brought about by a flow of electric current is known as __________.
19. Electrolysis is performed in an electrolytic cell, which is known as __________.
20. The positive electrode of a voltmeter is called __________ and negative as __________.
21. A solution, which tends to resist changes in pH is called a __________ solution.
22. A mixture of acetic acid and sodium acetate acts as a __________.
23. According to Sorenson __________ is defined as negative logarithm of the hydrogen ion concentration.
24. pH is mathematically expressed as __________.
25. The pH of a neutral solution is __________.
26. __________ substances have pH values lower than 7.
27. __________ solutions have pH values more than 7.
28. Oxidation is __________ of electron.
29. Reduction is the __________ of electron.
30. Such chemical reactions in which the oxidation number of atoms or ions is changed are called __________ reactions.
31. Oxidation number of a free element is __________.
32. Oxidation number of Oxygen in a compound is __________.
33. The sum of oxidation number of any formula of a compound is __________.
34. The oxidation number of any ion is equal to the __________ on the ion.
35. __________ is the reaction in which an acid reacts with a base to form salt and water.
36. __________ are organic compounds which change colour in accordance with the pH of the medium.
37. An indicator that changes from colourless to pink in the presence of an alkaline solution is called __________.
38. An indicator that changes from red to yellow in the presence of an alkaline solution is called __________.
39. Dissociation constant is denoted by __________.
40. According to Bronsted-Lowry Concept, __________ is the donor of proton and __________ is the acceptor of proton.
41. According to Arrhenius, acid is substance that produces __________ ions when dissolved in water.
42. According to Arrhenius, base is a substance that produces __________ ions when dissolved in water.
43. When ionic product is less than ksp, the solution will __________.
44. When ionic product is greater than ksp, the solution will __________.
45. The electrode at which oxidation takes place is called __________.
46. The electrode at which reduction takes place is called __________.
47. H3O+ ion is called __________ ion.
48. The logarithm of reciprocal of hydroxyl ion (OH)- is called __________.
49. Aqueous solution of NH4Cl is __________ while that of NaHCO3 is __________.
50. The ionic product of [H+] and [OH-] of pure water is __________.
51. An increase in the oxidation number of an element or ion during a chemical change is called __________.
52. A decrease in the oxidation number of an element or ion during a chemical change is called __________.
53. The degree of dissociation __________ with the increase in temperature.
54. The degree of dissociation __________ with the dilution of electrolytic solution.
55. A __________ consists of an electrode immersed in solution of its ion.
56. The potential difference between the electrode and the solution of its salt at equilibrium position is called __________ potential.
57. If the pH of a solution is 14, the solution is __________.
58. If the pH of a solution is 4, the solution is __________.
59. The oxidation number of Mn in KMnO4 is __________.
60. The oxidation number of Fe in FeCl3 is __________.
Chapter 8
Introduction to Chemical Kinetics
1. The branch of chemistry, which deals with the study of rates and mechanisms of chemical reactions, is known as __________.
2. Such reactions, which proceeds with very high velocities and are completed very quickly are called __________ reactions.
3. Such reactions, which take place very slowly, are called __________ reactions.
4. Reactions between silver nitrate and sodium chloride to form white precipitates of silver chloride are an example of __________ reaction.
5. Reactions of Organic compounds are slow and are called __________ reactions.
6. There are some reactions, which proceed slowly with a __________ speed.
7. The rate of __________ reaction can only be determined.
8. The amount of chemical change taking place in concentration of the per unit time is called __________ of reaction.
9. Rate of reaction is expressed in __________.
10. The rate of reaction between two specific interval of time is called __________.
11. The addition energy required to bring about a chemical reaction is called __________.
12. According to __________ theory for a chemical reaction to take place, the reacting molecules must come closed together.
13. The addition of __________ helps the reaction by lowering the energy of activation.
14. The rate of reaction __________ with the increase in concentration of the reacting molecules.
15. When the concentration of both the reacting molecules is double, the probability of collisions between them will be __________ times.
16. By __________ the surface area of the reactants, the rate of reaction is increased.
17. Rate of reaction generally __________ with the rise of temperature.
18. A __________ is a substance, which either accelerates or retards the rate of reaction without taking part in the reaction.
19. In the preparation of Oxygen from Potassium Chlorate, __________ is used as catalyst.
20. In the oxidation of SO2 to SO3 by the contact process for the manufacture of H2SO4 __________ is used as catalyst.
21. An unstable intermediate compound formed during a chemical reaction is called __________.
22. When a catalyst and the reactants are in the same phases, it is known as __________ catalyst.
23. When a catalyst and the reactants are in different phases, it is called __________.
24. When a catalyst increases the rate of reaction, it is called __________ catalyst.
25. When a catalyst retards the rate of reaction, it is called __________ catalyst.
26. A negative catalyst __________ the energy of activation, hence the rate of reaction is decreased.
27. The ratio between the rate of reaction and concentration of reactants is known as __________.
28. Velocity constant is independent of concentration but depends on __________.
29. Ionic reactions are __________ than molecular reactions.
30. The value of specific rates constant for a reaction __________ with time.
31. The sum of all exponents of concentration terms in the equation is called __________.
32. The sum of moles taking part in a chemical reaction is called __________ of the reactions.1. The property of a crystal, which is different in different directions, is called __________.
2. 0.00051 contains __________ significant figures.
3. The oxidation number of oxygen in OF2 is __________.
4. The volume of 1 gm of hydrogen gas at S.T.P is __________.
5. The oxidation number Mn in KMnO4 is __________.
6. The product of ionic concentration in a saturated solution is called __________.
7. 16 gm of oxygen at S.T.P occupies a volume of __________ dm3.
8. The shape of the orbital for which l = 0 is __________.
9. The radius of Cl-1 is __________ than the radius of Cl0.
10. Sp2 hybridization is also known as __________.
11. The value of 1 Debye is __________.
12. The reactions catalyzed by sunlight are called __________.
13. The blue colour of CuSO4 is due to the presence of __________.
14. The force of attraction between the liquid molecules and the surface of container is called __________.
15. The heat of neutralization of a strong acid and a strong base is __________.
16. C º C triple bond is __________. C = C double bond length.
17. The ions having the same electronic configuration are called iso electronic.
18. On heating, if a solid changes directly into vapours without changing into the liquid state, the phenomenon is called __________.
19. Each orbital in an atom can be completely described by __________.
20. In a molecule of alkene, __________ restricts the rotation of the group of atoms at either end of the molecule.
21. Density, refractive index and vapour pressure are __________ properties.
22. The addition of HCl to H2 solution __________ the ionization of H2S.
23. The reaction of cation or anion (or both) with water so as to change its __________ is known as Hydrolysis.
24. A reaction with higher activation energy will start at __________ temperature.
25. 6.02 x 1023 has __________ significant figures.
26. The internal resistance in the flow of liquid is called __________.
27. A catalyst increases the velocity of a reaction but decreases the __________.
Chapter 1
Introduction to Fundamental Concepts
1. 1 mole of a gas at S.T.P occupies a volume of __________.
2. A gas occupying a volume of 22.4 dm3 at S.T.P contains __________ molecules.
3. A formula, which gives the relative number of atoms in the molecule of a compound, is called __________.
4. A formula which gives the actual number of all kinds of atoms present in the molecule of compound is termed as __________.
5. The chemical formula that not only gives the actual number of atoms but also shows the arrangement of different atoms present in the molecule is called __________.
6. Atomic weight or molecular weight expressed in grams is known as __________.
7. 2 moles of H2O contain __________ grams and __________ number of molecules.
8. Any thing that occupies space and has __________ is called matter.
9. Volume of one __________ mole of a gas at S.T.P is 22.4 cubic feet.
10. A ton mole of iron is equal to __________ tons.
11. The force with which the earth attracts a body is called the __________ of the body.
12. A pure substance contains __________ kind of molecules.
13. The smallest indivisible particle of matter is called __________.
14. The atomic number is equal to the number of __________ in nucleus.
15. The atomic mass is the total number of protons and __________ in an atom of the element.
16. The average weight of atoms of an element as compared to the weight of one atom of __________ is called the atomic mass.
17. 1.0007 contains __________ significant figures.
18. The figure 24.75 will be rounded off to __________.
19. __________ means that the readings and measurements obtained in different experiments are very close to each other.
20. __________ means that the results obtained in different experiments are very close to the accepted values.
21. The degree of a measured quantity __________ with increasing number of significant figures in it.
22. The atomic mass of sodium is __________.
23. The symbolic representation of a molecule of a compound is called __________.
24. Molecular formula of CHCl3 and its Empirical formula is __________.
25. Molecular formula of benzene is C6H6 and its empirical formula is __________.
26. 58.5 is the __________ of NaCl.
27. 4.5 gms of nitrogen will have __________ molecules.
28. 28 gms of nitrogen will have __________ molecules.
29. 2 moles of SO2 is equal to __________ gms.
30. 1000 gms of H2O is equal to __________ moles.
31. The reactions, which proceed in both directions, are called __________.
32. The reactions, which proceed in forward directions only, are called __________ reactions.
33. The __________ reactions are completed after some time.
34. 0.0006 has __________ significant figures
35. 7.40 x 108 has __________ significant figures.
36. 7 x 108 has __________ significant figures.
37. Usually Molecular formula is simple multiple of the __________.
38. 0.1 mole of H2O contains __________ molecules of H2O.
39. Mass of 3.01 x 1022 molecules of CO2 is __________.
40. __________ is the branch of science which deals with the properties, composition and structure of matter.
41. None zero digits are all __________.
42. The integer part of logarithm is called __________.
43. The decimal fraction of logarithm is called __________.
44. __________ is the amount of substance, which contains as many number of particles as there are in 12 gms of Carbon.
45. 6.02 x 1023 is called the __________.
46. The accuracy of measurement depends on the number of __________.
47. __________ is the branch of chemistry that deals with quantitative relationships among the substances undergoing chemical changes.
48. The sum of atomic weights of all the elements present in molecular formula is called the __________.
49. __________ is the sum of atomic weights of the elements represented by the Empirical formula of the compound.
50. Very small and very large quantities are expressed in terms of __________.
51. In rounding off __________ figure is dropped.
52. Mole is the quantity, which has __________ particle of the substance.
53. For three significant figures, 25.55 is rounded off to __________.
54. The S.I unit of a mass is __________.
55. Mass of 6.02 x 1023 molecules of NaCl is __________ gm.
56. 1 mole of NaOH is __________ gm of NaOH.
57. Formula weight is used for __________ substances.
58. The word S.I stands for __________.
59. 4.5 gms of water will have __________ molecules.
60. 0.0087 has __________ significant figure.
Chapter 2
The Three States of Matter
1. The intermixing of gases or liquids in a container irrespective of their densities, is called __________.
2. At constant temperature, if the pressure of a given mass of a gas is decreased, its volume will __________.
3. A volume of __________ dm3 will hold 128 gms of SO2.
4. At constant temperature of a given mass of a gas, the product of its __________ and __________ is constant.
5. The rates of diffusion of gases are __________ proportional to the square root of their densities.
6. Gases deviate from ideal behaviour more markedly at high __________.
7. Liquid diffuse __________ than gases.
8. An imaginary line passing through the centre of a crystal is called __________.
9. The temperature at which more than one crystalline forms of a substance coexist in equilibrium is called __________.
10. Two or more substances crystallizing in the same form is called __________.
11. The existence of solid substances in more than one crystalline form is known as __________.
12. Rate of diffusion of gases is __________ as compared to liquids.
13. Boiling point of a liquid __________ with the pressure.
14. Mercury in a glass tube forms __________ curvature.
15. Gases can be compressed to __________ extent.
16. Viscosity of a liquid __________ with the increase of temperature.
17. Surface tension of water __________ by adding soap solution into it.
18. The internal resistance to the flow of a liquid is called __________.
19. The rise or the fall of a liquid in a capillary tube is called __________.
20. Matter exists in __________ states.
21. The freezing point of water in Fahrenheit scale is __________.
22. Boiling point of water is __________ °K.
23. SI unit for measurement of pressure is __________.
24. The value of gas law constant R = __________ dm3 atm/°K/mole.
25. The absolute Zero is equal to __________.
26. If P is plotted against 1/V at constant temperature a __________ is obtained.
27. Gases __________ in heating.
28. The pressure of air __________ at higher altitude.
29. Standard temperature means __________.
30. Standard pressure means __________.
31. Cooling is caused by __________ of gases.
32. Rate of diffusion of O2 is __________ times more than H2.
33. H2O has __________ viscosity than CH3OH.
34. Mercury does not wet the glass surface due to its higher __________.
35. Surface tension of mercury is __________ than water.
36. Viscosity can be easily measured by an instrument called __________.
37. The pressure exerted by the vapours when these vapours are in equilibrium with the liquid is called __________.
38. Vapour pressure __________ at high temperature.
39. Boyle’s Law and Charles Law can be combined into the mathematical expression __________.
40. Equal volumes of all gases at the same temperature and pressure contain __________ number of molecules.
41. The average Kinetic energy of a gas is proportional to its __________ temperature.
42. Kinetic equation may be mathematically written as __________.
43. The temperature at which two crystalline forms of a substance can coexist in equilibrium is called __________.
44. Lighter gases diffuse __________ than heavier gases.
45. Rain drops are __________ in shape.
46. Due to surface tension, the surface area of the liquid is __________.
47. Water __________ in the capillary tube.
48. Viscosity of a solution at 10°C is __________ than at 20°C.
49. Shape of NaCl crystal is __________.
50. Gases intermix to form a mixture.
51. Pressure of a dry gas is __________ than the pressure of a moist gas.
52. 22.4 dm3 of nitrogen at S.T.P will weigh equal to __________ gm.
53. 1 mole of any gas at S.T.P is equal to __________ dm3.
54. At -273°C, volume of all gases becomes __________.
55. The gases, which strictly follows the gas Laws are called __________ gas.
56. __________ is the property that determines the direction of flow of heat.
57. __________ is defined as force per unit area.
58. __________ viscosity is defined as the viscosity of a liquid as compared to the water.
Chapter 3
Structure of Atom
1. The maximum number of electrons in 2p orbital is __________.
2. 3d orbital has __________ energy than 4s orbital.
3. __________ rays are non-material in nature.
4. Charge to mass ratio of cathode rays resembles to that of __________.
5. __________ rays are most penetrating.
6. Neutrons have mass equal to that of __________.
7. Energy is __________ when an electron jumps from higher to lower orbit.
8. Second Ionization Potential has __________ value than the First Ionization Potential.
9. Electronegativity __________ from left to right in a period of Periodic Table.
10. __________ was discovered during the course of Artificial Radioactivity.
11. The velocity of alpha rays is nearly __________ of velocity of light.
12. Natural Radioactivity is confined in __________ elements.
13. The isotopes of an element differ in their __________.
14. Two electrons with the __________ spin, can never occupy the same atomic orbital.
15. ‘Al’ has electronic configuration, 1s2, 2s2, __________.
16. In a group of Periodic Table, the ionization potential __________ from top to bottom as the size of atom increases.
17. Ionization potential values __________ from left to right in a period.
18. The energy required to remove the most loosely bond electron from an atom in gaseous state is called __________.
19. The SI unit of Ionization Potential is __________.
20. An atom of sodium possesses 11 protons and __________ neutrons.
21. The particles of Cathode rays possess __________ charge.
22. The negatively charged particles found in Cathode rays are named as __________.
23. Positive rays are emitted from __________.
24. __________ rays are also known as Canal rays.
25. __________ consists of helium ions and are doubly positively charged.
26. __________ rays consists of negatively charged particles.
27. __________ rays are light waves of very short wavelength.
28. The phenomenon in which a stable element is made radioactive by artificial disintegration is called __________.
29. The electron move around the nucleus in different circular paths called __________.
30. The maximum number of electron in a shell is determined by the formula __________.
31. A particle whose mass is equal to that of electron but carries a positive charge is called __________.
32. 2p electrons are __________ in energy that 2s electrons in the same atom.
33. Number of protons of an element also indicates its __________.
34. According to __________ Principle electrons are fed in the order of increasing orbital energy.
35. According to __________ electrons are distributed among the orbitals of a sub shell to give maximum number of unpaired electron and have same spin.
36. The specific way in which the orbitals of an atom are occupied by electrons is called __________.
37. __________ rays are stream of doubly positively charged particles.
38. Electron in the outer most shell of an atom is called __________.
39. Protons are found in the __________ of an atom and bear __________ charge.
40. The atomic number of an atom is the sum of __________ inside the nucleus.
41. __________ limits the number of electron to different shell or orbits.
42. Sir William Crookes in 1878, discovered that the cathode in high vacuum tube emit radiations what he called __________.
43. X-rays were discovered in 1895 by __________.
44. The discovery of proton was done in 1886 by __________.
45. Neutrons were discovered by __________ in 1932 by the bombardment of beryllium with alpha particles.
46. Each atom has a __________, which contains all the positive charge and practically all the mass of atom.
47. Complete the reaction: 4Be9 + 2H4 ® __________ + __________.
48. __________ have higher ionization power as compared to b-rays.
49. No dark spaces between the colours are present in __________.
50. The symbol e+ represents __________.
51. p-orbitals are __________ shaped.
52. The energy released when an electron is added to an atom in the gaseous state is called __________.
53. The power of an atom to attract a shared pair of electrons towards itself is called __________.
54. Fluorine is __________ electronegative than chlorine.
55. Lyman series of spherical lines appear in the __________ portion of spectrum.
56. The electrons with __________ spin occupy the same orbital.
57. 3d orbital has __________ energy than 4s orbital.
58. Energy and frequency are __________ proportional to each other.
59. Ionic radii of cations are __________ than the atoms from which they are formed.
60. Ionic radii of anions are __________ than the atoms from which they are formed.
Chapter 4
Chemical Bonding
1. A bond formed due to transference of electron is called __________.
2. A bond formed due to sharing of electron is called __________.
3. Sigma bond is __________ than pi bond.
4. The shape of methane molecule is __________.
5. One s and 3p orbitals overlap to produce four __________ hybrid orbitals.
6. Ethene, C2H4 is an example of __________ hybridization.
7. Water molecule has __________ structure.
8. Water molecules are inter-linked with one another due to __________.
9. Polarity of the molecule is due to the difference of __________ between the two bonded atoms.
10. A chemical bond formed between to different atoms by mutual sharing of electron is termed as __________.
11. A chemical bond formed between two similar atoms by mutual sharing of electrons is known as __________.
12. The difference between the Electronegativity values of the two atoms forming covalent bond must be __________ than 1.7.
13. When two orbitals of different atoms by hybridize with each other having their axes in the same straight lines, the bond formed is termed as __________.
14. __________ bond is formed when p-orbitals of the two atoms with their axes parallel to each other overlap with each other.
15. Melting and boiling point of ionic compounds are usually __________ than that of covalent compounds.
16. Non polar compounds are usually __________ in non polar solvent.
17. The nitrogen in NH3 is __________ hybridized.
18. A hybrid orbital is called __________ orbital.
19. Since dipole moment of CS2 is zero, it is a __________ molecule.
20. A bond formed due to the electrostatic forces of attraction between the oppositely charged ions is called __________ bond.
21. The ionic bond is formed between the atoms with low ionization potential and high __________.
22. A bond formed by the sharing of an electron pair contributed by one atom only is called a __________ bond.
23. A co-ordinate covalent bond is also known as __________ bond.
24. Polar covalent bond is __________ than a non polar covalent bond.
25. H-F bond is __________ than H-Br bond.
26. The SI unit of dipole moment is __________.
27. Commonly used unit of dipole moment is __________.
28. Dipole moment of non-polar compound is __________ D.
29. The reactions of ionic compounds are usually very __________.
30. Covalent compounds are generally __________ in nature.
31. Ionic compounds are generally __________ in nature.
32. A covalent bond is represented by a __________.
33. A co-ordinate covalent bond is represented by an __________.
34. The covalent bond between H-F is called __________ covalent bond.
35. The power of an atom to attract a shared pair of electron itself is called __________ of that atom.
36. m = d x e represents __________.
37. CO2 and SO2 molecules have __________ polar bonds.
38. NH3 molecule has __________ polar bonds.
39. A double bond has __________ bond energy than a single bond.
40. An orbital which surrounds a single nucleus is called __________ orbital.
41. An orbital which surrounds two or more atomic nuclei is called __________ orbital.
42. A molecular orbital, which is of lower energy than the atomic orbitals from which it is derived, is known as __________ orbital.
43. A molecular orbital, which has higher energy than the atomic orbitals from which it is derived, is known as __________ orbital.
44. Orbitals formed after hybridization are called __________ orbitals.
45. Bond angle in Sp3 hybridization is of __________.
46. Bond angle in Sp2 hybridization is of __________.
47. Bond angle in Sp hybridization is of __________.
48. Sp3 hybridization is also known as __________.
49. Sp2 hybridization is also known as __________.
50. Sp hybridization is also known as __________.
51. A pair of electrons residing on the central atom and which is not used in bonding is called a __________.
52. The sum of total number of electron pairs (bonding and lone pairs) is called __________ number.
53. __________ bond is usually expressed by dotted line.
54. Water molecule has dipole moment because of its __________ structure.
55. CO2 is non polar because of its __________ structure.
56. Overlapping in __________ bond is perfect.
57. Overlapping in __________ bond is not perfect.
58. H-H bond is __________ than H-Cl bond.
59. __________ hybrid orbitals are not co-planar.
60. Covalent bond is Cl2 molecule is __________.
Chapter 5
Energetics of Chemical Reaction
1. The branch of Chemistry, which deals with the heat changes that take place during chemical reaction, is called __________.
2. The branch of science which deals with energy changes accompanying physical and chemical transformation is called __________.
3. The amount of heat evolved or absorbed in a chemical reaction is called __________.
4. Such reactions in which heat is evolved are called __________ reactions.
5. Such reactions in which heat is absorbed are called __________ reactions.
6. In exothermic reactions, heat evolved is given by __________ sign of DH.
7. In endothermic reactions heat absorbed is given by __________ sign of DH.
8. The total heat change in a reaction is the same whether it takes place in one or several steps.
9. The first law of thermodynamics is also known as __________.
10. The part of universe under observation is called __________.
11. The system plus its surrounding is called __________.
12. Such properties, which give description of a system at a particular moment, is called __________.
13. The term E + PV is called __________.
14. DH represents change in __________.
15. The temperature of water is raised up when sulphuric acid is added to it. This is an __________ reaction.
16. The characteristic properties of a system which is independent of amount of material concerned is called __________ properties.
17. The characteristic properties of a system which depend on amount of substance present in it is called __________ properties.
18. Density, pressure and temperature are the examples of __________ properties.
19. Mole numbers and enthalpy are the examples of __________ properties.
20. A system, which exchange both energy and matter with its surrounding, is called __________ system.
21. A system, which only exchange energy with the surrounding but not matter is, called __________ system.
22. A system which neither exchange energy nor matter with its surrounding is called __________ system.
23. A system is __________ if it contains only one phase.
24. A system is __________ if it contains more than one phase.
25. 1 kilojoule is equal to __________ joules.
26. 1 Calorie is equal to __________ joules.
27. 1 kilo calorie is equal to __________ joules.
28. The work done (w) is mathematically denoted by __________.
29. The change in enthalpy is denoted by __________.
30. __________ law is used in calculating heat of reaction.
31. __________ is defined as the change in enthalpy when one gram mole of a compound is produced from its element.
32. Heat of formation is denoted by __________.
33. When the work is done on the system by the surrounding the sign of work done (w) is __________.
34. When the work is done by the system on surrounding the sign of work done is __________.
35. First law of Thermodynamics is mathematically represented as __________.
36. Standard enthalpies are measured at __________.
37. Hess’s Law is employed to calculate __________ of a chemical reaction.
38. Heat absorbed by the system at constant volume is completely utilize to increase the __________ of the system.
39. Heat change at constant pressure from initial to final state of the system is simply equal to the __________.
40. SI unit of measurement of heat change is __________.
Chapter 6
Chemical Equilibrium
1. The reactions, which proceed in both the directions, are called __________ reactions.
2. The reactions, which proceed to one direction only, are called __________ reactions.
3. Reversible reactions are __________ completed.
4. Irreversible reactions are __________ after some time.
5. A reversible reaction is said to be in __________ when the rate of forward reaction becomes equal to the rate of backward reaction.
6. The concentrations of reactants and products are __________ at equilibrium point.
7. The value of Kc depends upon the __________ of the reactants.
8. A increase of the value of Kc tends to move the reaction to the __________ direction.
9. A decrease of the value of Kc tends to move the reaction to the __________ direction.
10. An increase in the concentration of the reactants will move the reaction to the __________ direction.
11. A decrease in the concentration of the reactants will move the reaction to the __________ direction.
12. Equilibrium constant is denoted by __________.
13. When the equilibrium constant value is very __________, we can conclude that the forward reaction is almost completed.
14. When equilibrium constant value is very __________ we can conclude that forward reaction will occur to very little extent.
15. According to __________ principle, if system in equilibrium is subjected to a stress, the equilibrium shifts in a direction to minimize or undo the effect of the stress.
16. In exothermic reaction, the __________ of temperature favour the forward rate of reaction.
17. In endothermic reactions, the __________ of temperature favour the forward rate of reaction.
18. A __________ is a substance which effects the rate of reaction but remains unaltered at the end of the reaction.
19. A catalyst increases the velocity of the reaction by decreasing the __________.
20. The suppression of degree of ionization of a sparingly soluble weak electrolyte by the addition of a strong electrolyte containing an ion in common is called __________.
21. __________ is purified in industries by Common Ion Effect.
22. A reaction moves to the left when the concentrations of the products are __________.
23. A reaction moves to the right when the concentrations of the products are __________.
24. Increase in pressure will move the reaction in the direction of __________ volume.
25. Decrease in pressure will move the reaction in the direction of __________ volume.
26. An increase of temperature favours the formation of products in case of __________ reaction.
27. A decrease of temperature fovours the formation of products in case of __________ reaction.
28. Heating moves an endothermic reaction to the __________.
29. Cooling move an exothermic reaction to the __________.
30. The product of ionic concentration in a saturated solution is called __________ constant.
31. When HCl is added to NaCl, the concentration of __________ ion is increased.
32. Chemical reaction involving the substances in more than one phases are called __________.
33. The formation of NH3 is exothermic process hence __________ temperature will favour the formation of NH3.
34. The formation of NO from N2 and O2 is endothermic process hence __________ temperature will favour the formation of NO.
35. Chemical Equilibrium is __________ equilibrium.
36. Molar concentration is also called __________.
37. The rate at which a substance takes part in a chemical reaction depends upon its __________.
38. __________ principle is applied to all reversible reaction.
39. A common ion __________ the solubility of the salt.
40. Number of moles present per dm3 of a substance is called __________.
Chapter 7
Solutions and Electrolytes
1. A mixture of two or more substances, which are homogeneously mixed, is called a __________.
2. __________ is defined as the amount of solute dissolved in a given amount of solvent.
3. A solution is composed of two components __________ and __________.
4. A solution containing one mole of solute per dm3 of solution is called one __________ solution.
5. Molarity is denoted by __________.
6. 1M solution of NaOH contains __________ gms of it dissolved per dm3 of solution.
7. A solution containing one mole of solute dissolved by per kg of solvent is called __________ solution.
8. Molality is denoted by __________.
9. 1M solution of H2SO4 contains __________ gms of it per kg of solvent.
10. The process in which ions are surrounded by water molecules is called __________.
11. The water molecules attached with the hydrated substance are called __________.
12. Hydrated copper sulphate evolves __________ water molecules on heating.
13. The interaction between salt and water to produce acids and bases is called __________.
14. The products of ionic concentration in a saturated solution at a certain temperature are called the __________.
15. Solubility product constant expressed as __________.
16. The suppression of ionization by adding a common ion is called __________.
17. The process of dissociation of an electrolyte into ions is known as __________.
18. The chemical decomposition of a compound in a solution or in fused state brought about by a flow of electric current is known as __________.
19. Electrolysis is performed in an electrolytic cell, which is known as __________.
20. The positive electrode of a voltmeter is called __________ and negative as __________.
21. A solution, which tends to resist changes in pH is called a __________ solution.
22. A mixture of acetic acid and sodium acetate acts as a __________.
23. According to Sorenson __________ is defined as negative logarithm of the hydrogen ion concentration.
24. pH is mathematically expressed as __________.
25. The pH of a neutral solution is __________.
26. __________ substances have pH values lower than 7.
27. __________ solutions have pH values more than 7.
28. Oxidation is __________ of electron.
29. Reduction is the __________ of electron.
30. Such chemical reactions in which the oxidation number of atoms or ions is changed are called __________ reactions.
31. Oxidation number of a free element is __________.
32. Oxidation number of Oxygen in a compound is __________.
33. The sum of oxidation number of any formula of a compound is __________.
34. The oxidation number of any ion is equal to the __________ on the ion.
35. __________ is the reaction in which an acid reacts with a base to form salt and water.
36. __________ are organic compounds which change colour in accordance with the pH of the medium.
37. An indicator that changes from colourless to pink in the presence of an alkaline solution is called __________.
38. An indicator that changes from red to yellow in the presence of an alkaline solution is called __________.
39. Dissociation constant is denoted by __________.
40. According to Bronsted-Lowry Concept, __________ is the donor of proton and __________ is the acceptor of proton.
41. According to Arrhenius, acid is substance that produces __________ ions when dissolved in water.
42. According to Arrhenius, base is a substance that produces __________ ions when dissolved in water.
43. When ionic product is less than ksp, the solution will __________.
44. When ionic product is greater than ksp, the solution will __________.
45. The electrode at which oxidation takes place is called __________.
46. The electrode at which reduction takes place is called __________.
47. H3O+ ion is called __________ ion.
48. The logarithm of reciprocal of hydroxyl ion (OH)- is called __________.
49. Aqueous solution of NH4Cl is __________ while that of NaHCO3 is __________.
50. The ionic product of [H+] and [OH-] of pure water is __________.
51. An increase in the oxidation number of an element or ion during a chemical change is called __________.
52. A decrease in the oxidation number of an element or ion during a chemical change is called __________.
53. The degree of dissociation __________ with the increase in temperature.
54. The degree of dissociation __________ with the dilution of electrolytic solution.
55. A __________ consists of an electrode immersed in solution of its ion.
56. The potential difference between the electrode and the solution of its salt at equilibrium position is called __________ potential.
57. If the pH of a solution is 14, the solution is __________.
58. If the pH of a solution is 4, the solution is __________.
59. The oxidation number of Mn in KMnO4 is __________.
60. The oxidation number of Fe in FeCl3 is __________.
Chapter 8
Introduction to Chemical Kinetics
1. The branch of chemistry, which deals with the study of rates and mechanisms of chemical reactions, is known as __________.
2. Such reactions, which proceeds with very high velocities and are completed very quickly are called __________ reactions.
3. Such reactions, which take place very slowly, are called __________ reactions.
4. Reactions between silver nitrate and sodium chloride to form white precipitates of silver chloride are an example of __________ reaction.
5. Reactions of Organic compounds are slow and are called __________ reactions.
6. There are some reactions, which proceed slowly with a __________ speed.
7. The rate of __________ reaction can only be determined.
8. The amount of chemical change taking place in concentration of the per unit time is called __________ of reaction.
9. Rate of reaction is expressed in __________.
10. The rate of reaction between two specific interval of time is called __________.
11. The addition energy required to bring about a chemical reaction is called __________.
12. According to __________ theory for a chemical reaction to take place, the reacting molecules must come closed together.
13. The addition of __________ helps the reaction by lowering the energy of activation.
14. The rate of reaction __________ with the increase in concentration of the reacting molecules.
15. When the concentration of both the reacting molecules is double, the probability of collisions between them will be __________ times.
16. By __________ the surface area of the reactants, the rate of reaction is increased.
17. Rate of reaction generally __________ with the rise of temperature.
18. A __________ is a substance, which either accelerates or retards the rate of reaction without taking part in the reaction.
19. In the preparation of Oxygen from Potassium Chlorate, __________ is used as catalyst.
20. In the oxidation of SO2 to SO3 by the contact process for the manufacture of H2SO4 __________ is used as catalyst.
21. An unstable intermediate compound formed during a chemical reaction is called __________.
22. When a catalyst and the reactants are in the same phases, it is known as __________ catalyst.
23. When a catalyst and the reactants are in different phases, it is called __________.
24. When a catalyst increases the rate of reaction, it is called __________ catalyst.
25. When a catalyst retards the rate of reaction, it is called __________ catalyst.
26. A negative catalyst __________ the energy of activation, hence the rate of reaction is decreased.
27. The ratio between the rate of reaction and concentration of reactants is known as __________.
28. Velocity constant is independent of concentration but depends on __________.
29. Ionic reactions are __________ than molecular reactions.
30. The value of specific rates constant for a reaction __________ with time.
31. The sum of all exponents of concentration terms in the equation is called __________.
32. The sum of moles taking part in a chemical reaction is called __________ of the reactions.
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