1. The oxidation potential of hydrogen electrode is 0.00
volt.
2. The pH of 0.01M HCl solution is 2.
3. The oxidation number of oxygen in H2O2
is –1 and in OF2 is +2.
4. The volume of 1 gm of H2 gas at STP is 11.2 dm3.
5. The oxidation number of ‘N’ in NO21¯
and NO31¯ are +3 and +5 respectively.
6. Volume of 1 mole of chlorine gas at STP is 22.4 dm3.
7. Shorter the bond length, higher will be bond energy.
8. pH + pOH = 14.
9. Oxidation takes place at anode while reduction at cathode.
10. Evaporation is a cooling process.
11. The blue colour of CuSO4 is due to the water of crystallization, [Cu(H2O)4]2+.
12. 4Be9 + 2He4 ¾¾¾¾® 6C12 + 0n1
14. 1s2, 2s2 2px1 is the electronic configuration of Boron.
15. Cations have smaller radii than its neutral atom.
16. Anions are larger in size than its parent atom.
17. The shape of orbital for which l = 1 is dumb-bell.
18. A solution which tends to resist changes in its pH is called Buffer.
19. Shape of sp-hybrid orbital is Linear.
20. Shape of sp2-hybrid orbital is Trigonal.
21. Shape of sp3-hybrid orbital is Tetrahedral.
22. There are 2 significant figures in 0.0021.
23. The oxidation number of ‘Cr’ in K2Cr2O7 is +6.
24. The substances undergoing decrease in oxidation no. is called Oxidizing Agent.
25. The substances undergoing increase in oxidation no. is called Reducing Agent.
26. Water rises in capillary tube due to Capillary Action (Surface Tension).
27. CO2 has zero dipole moment due to its linear structure.
28. The oxidation no. of Cl in HOCl is +1 and in HClO4 is +7.
29. KMnO4 is an example of Oxidizing Agent.
30. 1 M solution of KMnO4 contains 158 gm/litre.
31. 1 N solution of KMnO4 contains 31.6 gm/litre.
32. The shape of CH4 is Tetrahedral.
33. The shape of C2H4 is Trigonal.
34. The shape of C2H2 is Linear.
35. 3.2 gm of O2 gas at STP has a volume 2.24 dm3.
36. pH is the negative logarithm of Hydrogen Ion Concentration, [H+].
37. The oxidation No. of ‘Mn’ in KMnO4, K2MnO4, MnO2 and MnSO4 are +7, +6, +4 and +2 respectively.
38. The shape of H2O is Angular.
39. 7.3 is the pH of human blood.
40. 35.5 g of Cl2 gas at STP has a volume 11.2 dm3.
41. 1 N solution of oxalic acid contains 63 g/litre.
42. The empirical formula of acetylene is
43. During electrolytic conduction, cations are attracted towards cathode while anions are attracted towards anode.
44. A graph of volume with 1/P is straight line.
45. Reaction between an acid and alcohol is called Esterification.
46. Aqueous solution of Na2CO3 is basic in nature.
47. Aqueous solution of NH4Cl is acidic in nature.
48. The oxidation number of N in NCl3 is +3.
49. The oxidation number of C in C2H6O is –2.
50. Universal indicator turns green in neutral solution.
51. Universal indicator turns yellow at pH 6.
52. Universal indicator turns blue at pH 8.
53. The amount of heat of neutralization for strong acid and strong base is about 13700 calories.
54. Fast reactions possess low energy of activation.
55. Slow reactions have high energy of activation.
56. Each orbital in an atom can be completely described by Quantum Numbers.
57. The addition of HCl to H2S solution decreases the ionization of H2S.
58. A catalyst increases the velocity of a reaction but decreases Ea.
59. The reactions catalysed by sunlight are called Photochemical Reactions.
60. The e/m ratio of canal rays is the lowest when hydrogen is taken in the discharge tube.
61. The negative ion tends to expand with the increase of negative charge on it.
62. I.P. decreases in a group from top to bottom.
63. I.P. increases along each period.
64. Cesium is the most electropositive element.
65. Fluorine is the most electronegative element.
66. Atomic radii increases down each group.
67. Atomic radii decreases along each period.
68. Dipole moment = Charge x distance between the charges.
69. 1st I.P. is always less than 2nd I.P.
70. It is easier to remove electron from Mg than to Mg+.
71.H If DE.N. between bonding atoms is greater than 1.7 than the bond between them will be ionic.
72. If DE.N. < 1.7, than the bond will be covalent.
73. Water forms concave meniscus in glass tube due to greater adhesive forces.
74. Mercury forms convex meniscus in a glass tube due to greater cohesive forces.
75. Wetting liquids always form concave meniscus.
76. Non-wetting liquids always form convex meniscus.
77. Surface tension is inversely proportional to the temperature.
78. Viscosity of liquid decreases with the rise of temperature (2% per degree).
79. Viscosity of gases increases with the rise of temperature.
80. Pmoist gas = Pdry gas + Pwater vapours.
81. Partial pressure of a gas = Mole fraction x Total pressure.
82. Rate of diffusion of a gas is inversely proportional to the square root of the density (Molecular wt) of the gas.
83. Value of ‘R’ in dm3-atm is 0.0821.
84. Value of ‘R’ in N-m or Joule is 8.3143.
85. 6.02 x 1023 molecules of N2 gas at STP has a volume 22.4 dm3.
86. 0°C = 273.16 K.
87. K = °C + 273.
88. The lowest possible temperature at which all molecular motion ceases to exist is called Absolute Zero.
89. 1 atm = 14.7 lb/inch2 (Psi).
90. 1 atm = 101325 (1.01325 x 105) N/m2.
91. 1 a.m.u. = 1.67 x 10¯24 gm = 1.67 x 10¯27 Kg.
92. The value of ‘h’ in J.S. is 6.627 x 10¯34.
93. 92U238 ¾¾¾¾® 90Th234 + 2He4
94. The radius of Bohr’s orbit is found out to be 0.529 °A.
95. 1°A = 10¯10 m = 10¯8 cm.
96. As the multiple bonds are shorter, they have greater bond energies than single bond.
97. s-p sigma bond is stronger than s-s sigma bonds.
98. p-p sigma bond is stronger than s-p or s-s sigma bonds.
99. s-orbitals do not take part in p-bond formation.
100. The bond angle in CH4 is 109. 28° while in C2H4 is 120°.
101. Alpha rays have higher ionizing power than b and g rays.
102. Density, Pressure, M.P, B.P and Refractive Index are Intensive Properties.
103. Enthalpy, Internal Energy, Mass, Volume and Mole are Extensive Properties.
104. W is + when work is done on system.
105. W is – when work is done by the system.
106. The difference of potential, create between a metal and solution of its salt is called Electrode Potential of the metal.
107. Potential associated with oxidation is called Oxidation Potential.
108. Potential associated with reduction is called Reduction Potential.
109. Metals placed in the electro chemical series above hydrogen act as anode (they are oxidised) while below hydrogen acts as cathode (they are reduced).
110. If the sign of electrode potential is positive, then the reaction is spontaneous, and the electrode acts as anode whereas if the sign is negative then the electrode act as cathode.
111. The ratio F/NA represents an electronic charge.
112. Ethyl alcohol is an ester.
