Important Objectives for Chemistry XI 2015

Important Objectives for Chemistry XI  2015

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

13.       No. of electrons in Mg²⁺ is 10 and in O²¯ is 10.

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 CH.  Its molecular formula will be C2H2 if its molecular mass is 26.

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.       P_{moist gas}  =  P_{dry gas}  +  P_{water 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/N_A represents an electronic charge.

112.     Ethyl alcohol is an ester.