Chemistry-2

+2 Chemistry (new syllabus) Inorganic Chemistry: I. Choose the correct answer 1. Atomic structure-II 1. Who discovered the atom a) Rutherford

b) Dalton

c) Neils Bohr

d) Goldstein

2. Who discovered the nucleus and proposed the first atomic model a) J.J.Thomson 3.

b) Max Plank

c) Rutherford

d) Julius Plucker

Who discovered the wave nature of the particle a) de-Broglie

b) Clark Maxwell

c) HGJ Mosely

d) Goldstein

4. Who introduced the concept of energy levels of atom based on spectra of hydrogen atom a) Dalton

b) Neils Bohr

c) Anderson

d) Pauli

5. The concept of quantum numbers introduced to distinguish the orbital on the basis of a) their size 6.

b) shape

c) orientation in space

d) all of them

Which rule followed for filling of electrons in various orbital a) Pauli exclusion

b) Aufbau principle

c) Hund's rule

d) all of them

7. En = - 313.6 / n2 if the value of Ei = - 34.84 to which value 'n' corresponds a) 4

b) 3

c) 2

d) 1

8. Dual property means a) material with wave character c) both of them

b) material with particle character d) none of them

9. Dual property of an electron was explained by a) Heisenberg

b) de-Broglie

c) Neils Bohr

d) Pauli

10. A grain of sand or a cricket ball is a particle because of a) it occupies space them 11.

b) do not interfere

c) total value is their sum d) all of

Sound from the speaker is called as wave because of

a) spread out in space b) it will interfere destructive d) all of them

c) interference may be constructive or

12. Wave character of electron proved by the experiment of a) Davisson and Germer b) de-Broglie c) GP Thomson

d) both a and c

13. In GP Thomson experiment the electrons are passed through a) Nickel crystal b) thin gold foil

c) thin Al foil

d) none of them

14.

When an electron strikes a zinc sulphide screen it produces a spot of light called a) diffraction

b) scintillation

c) illumination

d) none of them

15. Energy of a particle with wave character is a) E = hν

b) E = mc2

c) both a and b

d) none of them

16. In the equation E = hν, the value of ν is a) velocity of light 17.

b) Planck's constant

c) frequency of wave d) none of them

In the equation E = hν, the value of h is a) height

b) velocity

c) mass

d) Planck's constant

18. Energy of a particle with particle character is a) E = hν

b) E = mc2

c) both a and b

d) none of them

19. de-Broglie equation is a) λ = h/mv

b) λ = hmv

c) λ = hv/m

d) λ = mv/h

20. In the equation λ = h/mv, the λ is called as a) de-Broglie wave length them

b) Einstein constant

c) Planck's constant

d) none of

21. The value of the Planck's constant is a) 6.023 x 10-23

b) 6.626 x 10-34 Kg m2 s-1

c) 6.62 x 10-34 m

d) none of them

22. The value of the Bohr radius for hydrogen atom is a) 0.529 x 10-8 cm

b) 0.529 x 10-10 cm

c) 0.529 x 10-6 cm

d) 0.529 x 10-12 cm

23. Energy of electron in a given atom is given by En = 4π2me4 b) 2π2me2 c) 2π2me4 d) 2πme4 n2h2 n2h2 n2h2 n2h2 24. Which of the following particle having the same kinetic energy, would have the maximum de-Braglie wave length a)

a) α particle

b) β particle

c) proton

d) neutron

25. Which of the following particle having the same kinetic energy, would have the maximum de-Braglie wave length a) n

b) n + 1

c) n + 2

d) n - 1

26. If the energy of an electron in the second Bohr orbit of H-atom is E, what is the energy of the electron in Bohr's first orbit? a) 2E

b) - 4E

c) - 2E

d) 4E

27. The wave function ψ represents a) potential energy b) total energy d) the amplitude of the wave

c) probability of finding the electron

28. The wave function ψ2 represents a) probability of finding the electron b) potential energy them

c) both a & b d) none of

29. The size of s-orbital depends on the principal quantum number-n a) Greater the n value greater the size b) greater the n value smaller the size c) Lesser the n value greater is the size d) none of them 30. The number of nodes of s-orbitals of any energy level is a) n

b) n + 1

c) n + 2

d) n - 1

31. Molecular orbitals are formed by the combination of a) atomic orbitals of different energy b) atomic orbitals of equal energy c) or atomic orbitals of comparable energy d) both b and c 32. The bonding molecular orbitals are represented by a) π (pi)

b) δ (delta)

c) σ (sigma)

d) all of them

33. The molecular orbitals are filled in the order of orbitals of a) lowest energy b) same energy

c) higher energy

d) none of them

34. A molecular orbital can accommodate only a) one electron

b) two electron

c) four electron

d) eight electron

35. Energy level of the molecular orbitals determined experimentally by a) Ultroscopic

b) Microscopic

c) Spectroscopic

d) all of them

36. If the no. of electrons in bonding molecular orbitals, Nb = Na (antibonding mol. orbitals) then the molecule will be a) stable

b) unstable

c)

d)

37. Bond order is equal to a) ½ (Nb-Na)

b) ½ (Na-Nb)

c) Na-Nb

d) Nb-Na

c) 3

d) 2

c) sp3d

d) sp3d3

38. Bond order of Oxygen molecule is a) 2.5

b) 1

39. The hybridisation in SF6 molecule is a) sp3

b) sp3d2

40. The molecule or ion will be stable if the bond order is a) Positive

b) Zero

c) Negative

d)

41. Arrange the molecules in the order of increasing Bond order a) N2>Li2>O2

b) N2> O2>Li2

c) Li2> N2> O2

42. Arrange the molecules in the order of increasing Bond length

d) O2> N2> Li2

a) N2>Li2>O2

b) N2> O2>Li2

c) Li2> O2>N2

d) O2> N2> Li2

43. If all the electrons are paired then it is a) Paramagnetic b) Diamagnetic

c) Neutral

d) positive

44. Arrange in the order of relative stability a) O2> O2+>O22-> O2-

(b) O2+>O2>O2->O22-

(c) O22->O2-> O2>O2+

d)

45. Arrange in the order of bond dissociation energies a) O22->O2-> O2>O2+

b) O2> O2+>O22-> O2- c) O2+>O2>O2->O22-

d)

46. In metal atoms the bond is a) covalent bond b) Ionic bond

c) covalent-co-ordiante d) none of them

47. Arrange in the order of increase in electrical conductivity a) Tin>Germanium>Silicon>Carbon c) Germanium>Silicon>Carbon>Tin 48. A good conductor have the a) medium

b) Carbon>Silicon>Germanium> Tin d) Silicon>Carbon> Germanium> Tin

energy gap between conductor band and valence band

b) large

c) small

d)

49. Arrange in the order of decrease in intermolecular attraction (Vander Waals forces) a) Solids
b) Gas
c) Liquid<Solid
d)

50. For strong Hydrogen bond the molecule should have a) high electronegative

b) small atomic size

c) high electropositive d) both a & b

51. The bond strength of different bonds is in the order of a) covalent>hydrogen>ionic>dipole-dipole b) hydrogen>dipole-dipole> ionic>covalent c) dipole-dipole>hydrogen>ionic>covalent d) covalent>ionic>hydrogen> dipole-dipole 52. The dipole-dipole attraction is present in a) N2

b) H2

c) H2O

d) He

53. The dipole- induced dipole attraction is present in a) N2

b) He

c) H2O

d) both a & b

54. The inter molecular hydrogen bonding is present in a) H2O

b) o-nitro phenol

c) p-nitro phenol

d) both a & b

55. The intra molecular hydrogen bonding is present in a) m-nitro phenol b) o-nitro phenol

c) p-nitro phenol

2. Periodic classification-II: 56. On moving from top to bottom of a group the atomic radii will

d) None

a) increase

b) remains same

c) decrease

d) none

57. On moving from left to right across the period the atomic radii will a) decrease 58.

b) increase

c) remains same

d) none

On moving from top to bottom of a group the ionisation potential will a) remains same

b) increase

c) decrease

d) none

59. On moving from top to bottom of a group electron gain enthalpy will a) decrease

b) increase

c) remains same

d) none

60. On moving from left to right across the period the electronegativity will a) increase

b) decrease

c) remains same

d) none

61. On moving from top to bottom of a group the electronegativity will a) increase

b) decrease

c) remains same

d) none

62. In case of homonuclear diatomic molecule, the radius, r(A) of a given atom is calculated by a)

d (A-A) b) 2 c) d (A-A) d) d (A-A) 1 d (A-A) 2 4 63. The Cl - Cl bond distance is 1.98Ǻ, the radius, r(Cl) of a Chlorine atom is a) 1.98 Ǻ

b) 3.96 Ǻ

c) 0.99 Ǻ

d) none

64. The value of C - C distance found experimentally in a saturated hydrocarbon is a) 1.34 Ǻ

b) 1.36 Ǻ

c) 1.54 Ǻ

d) 1.56 Ǻ

65. In case of heteronuclear diatomic molecule, the radius, r(A) of a given atom is calculated by a) d (B-A) - r(B) b) d (A-B) - r(A)

c) d (A+B) - r(B)

d) d (A-B) - r(B)

66. In case of ionic molecule, the radius, r(C+) or r(A-) of a given atom is calculated by a) r(C+) + r(A-)=d(C+ - A-) c) r(A-) / r(C+) = Z*(A-) / Z*(C+)

b) r(C+) / r(A-) = Z*(A-) / Z*(C+) d) both a and b

67. Ionisation energy is the energy required a) to add an electron d) none

b) to remove an electron

c) to attract the shared electron

68. Second ionisation potential is related with the following equation a) M2+(g) +Ix→M3+(g) + ec) M(g) +Ix→M+(g) + e-

b) M+(g) +Ix→M2+(g) + ed) None

69. Effective nuclear charge (Z*) can be calculated by using the formula a) Z* = Z - S

b) Z* = Z + S

c) Z* = S - Z

d) Z = Z* - S

70. The ionisation energy (IE) of 'Be' is more than 'Li' because a) Li has higher nuclear charge than Be c) Be has higher nuclear charge than Li than Li

b) Li has lower nuclear charge than Be d) Be has lower nuclear charge

71. The ionisation energy (IE) of 'Be' is more than 'B' because a) B has higher nuclear charge than Be c) B has unpaired electron than Be

b) Be has lower nuclear charge than B d) Be has paired electron than B

72. The ionisation energy (IE) of 'C' is more than 'B' because a) B has higher nuclear charge than C

b) B has lower nuclear charge than C

c) C has higher nuclear charge than B

d) C has lower nuclear charge than B

73. Comparing the ionisation energy (IE) of 'F' with 'C', F has a) lower ionisation energy

b) higher ionisation energy

c) same ionisation energy

d) none of these

74. The ionisation energy decreases while moving down a group is because of a) The valence shell experiences less attraction from the nucleus b) The electron to be removed is shielded from the nucleus by the electrons in the inner shell c) The attractive force of the nucleus is counterbalanced by the repulsive forces of electrons d) all the above 75. The ionisation energy decreases in the order of a) s>p>d>f

b)f>d>p>s

c)s
d) both a and b

76. The ionisation energy (IE) of 'Mg' is more than 'Al' because a) Al has higher nuclear charge than Mg

b) Al has lower nuclear charge than Mg

c) Mg has higher nuclear charge than Al

d) Mg has lower nuclear charge than Al

77. The maximum ionisation energy is possessed by a) Alkali metals b) Halogen gases

c) Noble gases

d) Alkaline metals

78. The ionisation energy is expressed in a) kJ mol-1

b) kcal mol-1

c) eV / atom

d) all of them

79. Arrange the following elements in the order of increasing ionisation energy a) Li, B, Be

b) Be, B, Li

c) Be, Li, B

d) Li, Be, B

80. Arrange the following elements in the order of increasing ionisation energy a) C, N, O, F

b) N, C, O, F

c) F, O, N, C

d) Li, Be, B

81. The electron affinity of elements having d10s2 configuration is a) zero

b) positive

c) negative

d) both a and b

82. On moving from top to bottom of a group the electron affinity will a) increase

b) decrease

c) remains same

d) none

83. The electron affinity of noble gases are a) positive

b) negative

c) zero

d) none

84. The electron affinity of 'Be' and N2 are a) almost zero

b) positive

c) negative

d) none

85. The electron affinity of 'Au' is high due a) higher nuclear charge b) small size c) poor shielding of nucleus by electrons d) all of them 86. The electron affinity is directly proportional to a) size of the atom

b) nuclear charge

c) both a & b

d) shielding effect

87. The electron affinity of an atom a) directly proportional to its size c) independent of its size

b) inversely proportional to its size d) none of these

88. The electron affinity of F is less than Cl because a) small size

b) crowd of electrons around nucleus c) both a and b

d)

89. Among the following which has the higher electron affinity value a) F

b) Cl

c) Br

d) I

c) kJ mol

d) kJ mol-1

90. The electron affinity is expressed in a) kJ

b) J

91. The scale which is based on an empirical relation between the energy of a bond and the electronegativities bonded atoms is a) Pauling scale

b) Mulliken's scale

c) Sanderson's scale d)Alfred & Rochow's

92. Mulliken sacle to find the electronegativity is a) 0.208 ∆ = XA - XB

b) IE + EA /2

c) both

d) none

93. The bond length of Cl -Cl molecule is a) 0.74 94. Noble gases have a) High

b) 1.44

c) 1.98

d) 2.28

electron affinity b) zero

c) low

d) very low

95. When XA >> XB, A - B bond is (Na Cl) a) polar covalent b) non-polar covalent

c) Ionic

d) metallic

c) Ionic

d) metallic

96. When XA > XB, A - B bond is (H2O) a) polar covalent b) non-polar covalent

97. When XA = XB, A - B bond is (H-H) a) polar covalent b) non-polar covalent

c) Ionic

d) metallic

98. The bond length of Cl2 molecule is a) 0.74

b) 1.44

c) 1.98

d) 2.28

3. p. block elements: 99. p-block elements occupy the groups a) 1 - 2 100.

b) ns2np2

c) ns2np4

d) ns2np1

b) metals & non-metals

c) non-metals only

d) none

The familiar characteristic of p-block elements is a) low I.E

103.

d) none

p-block elements consists of a) metals only

102.

c) 13 - 18

The general electronic configuration of p-block elements is a) ns2np1-6

101.

b) 3 - 12

b) zero oxidation states

c) inert pair effect

d) none

p-block elements generally have the oxidation no of a) +ve

b) - ve

c) both a and b

d) none

Group-13 Elements 104.

Among the group 13 elements the rare element is a) Al

105.

d) Thallium

b) Tl,In,Ga,Al,B

c) AL,B,In,Tl,Ga

d) none

b) Gallium

c) Indium

d) Thallium

b) poor shielding effect of 3d electrons

c) none

Group-13 elements generally have the oxidation no of a) +3

110.

c) Indium

The atomic radii of Ga is slightly less than Al because of a) higher atomic no.

109.

b) Gallium

Among the group 13 elements the toxic element is a) Al

108.

d) Boron

The metallic character will increase in the order of a) B, Al, Ga, In, Tl

107.

c) Thallium

Atomic radius and I.E of group 13 elements decreases from top to bottom except a) Al

106.

b) Gallium

Potash alum is

b) +2

c) +1

d) none

d)

a) K2SO4.Al2(SO4)3.12H2O c) K2SO4.Al2(SO4)3.42H2O 111.

b) K2SO4.Al2(SO4)3.24H2O d) K2SO4.Al2(SO4)3.2H2O

Potash ash is manufactured form a) alunite or alum stone b) alumina

112.

c) both a & b

d) none

Potash alum is crystallised by adding a) Aluminium hydroxide b) Potassium sulphate c) Potassium sulphite

113.

Potash alum is a) green crystal

114.

b) blue crystal

c) silver crystal

d) white crystal

c) benzene

d) acids

Potash alum is insoluble in a) water

115.

d) none

b) alcohol

The burnt alum is a) heated potash ash

b) dissolved potash ash c) cooled potash ash

d) none

Group-14 Elements 116.

The general electronic configuration of G-14 elements is a) ns2np1

117.

b) ns2np2 b) +2

In group-14 elements, a) Carbon

119.

c) +1 c) Ge

b) SiO42-

c) SiO43-

d) SiO44-

The structure of SiO44- ion is c) tetrahedral

d) none

Silica is prepared by the complete hydrolysis of a) SiCl

122.

d) Pb

The basic chemical unit of silicate is

a) bi-pyramidal b) octahedral 121.

d) +4

element have high Catenation property

b) Si

a) SiO4 120.

d) ns2np4

Group-14 elements generally have the oxidation no of a) +3

118.

c) ns2np3

b) SiCl2

c) SiCl3

d) SiCl4

b) Cerrusite

c) Galena

d) all of them

b) bluish grey

c) reddish

d) none

Ores of Pb a) Anglesite

123.The colour of Lead is a) Greenish 124.

Red lead is a) Pb3O4

125.

b) PbO

Plumbo solvency is

c) Pb2O3

d) none

a) Pb(OH) 126.

b) Pb2(OH)

c) Pb(OH) 2

d) Pb(OH)3

Dilute H2SO4 reacts with Pb to give a) PbSO4

b) Pb2SO4

c) PbSO3

d) none

Group-15 Elements 127.

The general electronic configuration of group-15 elements is a) ns2np1

128.

b) ns2np2

129.

b) yellow or white P c) both a and b b) N b) Iodine b) CaOH

b) yellowish gas

b) H3PO4 b) H3PO4

d) none

c) HPO3

d) none

b) pleasant

c) garlic

d) none

b) HPO3

c) H3PO4

d) H3PO3

Phosphorous pentaoxide (P2O5) is a c) yellowish crystal

d) none

Metaphophoric acid is a) PH3

b) HPO3

c) H3PO4

d) H3PO3

Phosphorous pentaoxide (P2O5) is used as a a) reducing agent

140.

d) greenish solid

c) HPO3

a) white waxy substance b) white solid

139.

c) yellowish crystal

Phosphorous trioxide (P2O3) reacts with hot water to give a) PH3

138.

d) none

Phosphorous trioxide (P2O3) has a smell of a) rotton egg

137.

c) NaOH

With insufficient water PCl5 gives a) POCl3

136.

d) none

With excess water PCl5 gives a) POCl3

135.

c) Chlorine

PCl5 is a a) Colourless liquid

134.

d) Bi

Phosphine gas is produced by boiling white P with a) KOH

133.

c) As

White P can be converted into red P by heating in presence of a) Bromine

132.

d) none

Which element of Group-15 have allotropy character a) P

131.

d) ns2np6

Phosphorous (P) is present as a) red P

130.

c) ns2np3

b) oxidising agent

c) dehydrating agent d) none

Phosphorous acid (H3PO3) is used as a a) reducing agent

b) oxidising agent

c) dehydrating agent d) none

141.

H3PO4 is a) solid

142.

b) liquid

c) gas

H3PO4 reacts with AgNO3 to give a) red

143.

d) none

precipitate of silver phosphate

b) yellow

c) green

d) gold

H3PO4 reacts with AgNO3 to give a) Ag3PO4

144.

b) AgPO4

c) Ag2PO3

d) Ag4PO3

Phosphine (PH3) has a smell of a) rotton egg

145.

b) sweet

c) garlic

d) rotton fish

Which of the following is used as a smoke screen a) H3PO4

146.

b) HPO3

c) P2O5

d) PH3

PCl3 and PCl5 are chlorinating agents because they a) add Cl

147.

b) remove Cl

c) remove H

d) add O

PCl3 is a better chlorinating agents because it chlorinates a) only organic compounds

148.

b) metals also

c) non-metals

d) none

aaa a)

149.

b)

c)

d)

b)

c)

d)

aaa a)

Group-16 Elements 150.

elements O,S,Se,Te are CHALCOGENS because their ores are mainly a) sulphates

151. 152.

b) Se

d) sulphides

c) Te

d) Po

Which element is radioactive among the G-16 elements a) S

153.

b) Se

c) Te

d) Po

The general electronic configuration of group-16 elements is a) ns2np1

154.

b) ns2np2

c) ns2np4

d) ns2np6

Which element is having allotropy among the G-15 elements a) S

b) Se

c) Po

d) all of them

Which one is called as oil of vitriol a) H3PO3

156.

c) oxides & sulphides

Which element is called as Brim stone among the G-16 elements a) S

155.

b) oxides

b) H3PO4

c) H2SO4

Acid will be added to water to dilute the acid because

d) none

a) it precipitates b) it gets cooled 157.

c) it produces heat

d) none

c) red

d) white

c) red

d) gold

H2SO4 turns blue litmus paper to a) green

158.

b) no change

H2SO4 turns methyl orange to a) yellow

159.

b) pink

H2SO4 reacts with more electro+ve elements like Zn and Fe to give a) H2

160.

b) O2

c) S

d) both a & c

Dilute H2SO4 reacts with the metal a) Hg

b) Cu

c) Pb

d) none

Group-17 Elements 161.The general electronic configuration of G-17 elements is a) ns2np2 162.

b) ns2np4

c) ns2np6

Which element is radioactive among the G-16 elements a) Cl

163.

b) Br

c) I

164. 165.

b) Cl2

d) none

c) Br2

d) I2

b) O2

c) O3

d) all of them

Arrange in the decreasing order of halogens towards hydrogen a) F>Cl>Br>I

b) I>Br>Cl>F

c) Cl>F>Br>I

d) Br>Cl>F>I

c) HBr

d) HI

Which one the hydrogen halide is liquid a) HF

b) HCl

Arrange in the increasing order of hydrogen halides acidic character a) HF>HCl>HBr>HI

168.

c) solid

F2 reacts with water and gives a) HF

167.

b) liquid

Among the halogens which one is the strongest oxidising agent a) F2

168.

c) reddish brown gas d) yellowish green gas

Iodine (I2) is a a) gas

167.

d) At

Cl is a a) coulorless gas b) light yellow gas

166.

d) none

b) H I>HBr>HCl>HF

c) HCl>HF>HBr>HI

Which one the hydrogen halide is stored in wax bottle a) HF

b) HCl

c) HBr

d) HI

169.Which one the hydrogen halide is used for etching on glass a) HF

b) HCl

c) HBr

d) HI

d) none

170.

F2 has an odour of a) sweet

b) pungent

c) garlic

d) none

Group-18 Elements 171.

The general electronic configuration of G-18 elements is a) ns2np2

172.

b) ns2np4 b) liquids

d) none

b) reduction power

c) chemical inactivity

d) none

Group-18 elements can also be called as

a) halogen gases 175.

c) solids

All the elements of G-18 are called inert gases because of their

a) oxidation power 174.

d) none

All the elements of G-18 are a) gases

173.

c) ns2np6

b) noble gases

c) chalcogens

d) none

c) gases

d) none

Xenon fluorides are a) crystalline solids

b) liquids

176.Xenon fluorides will sublime at a) 273°K 176.

c) 3982K

d) 373°K

Aeroplane tyres are filled with a) H2

177.

b) 298°K b) N2

c) He

d) O2

c) O2 & He

d) only O2

Divers will use the mixture of a) H2 & O2

b) N2 & O2

177.Electrical bulbs were filled with a) N2 178.

c) Ar

d) both b & C

Which of the following is most abundant in earth's crust? a) C

179.

b) Ne

b) Si

c) Ge

d) Sn

c) Ge

d) Sn

The metalloid among the following is a) Si

b) P

178.Which of the following does not exhibit allotropy a) C 180.

c) Sn

d) Pb

Which one of the following is three-dimensional silicate?

a) talc 181.

b) Si b) beryl

c) quartz

d) kaoline

c) spodumena

d) forsterite

An example of an amphibole is a) beryl

b) tremolite

182.Which one shows most pronounced inert pair effect? a) Si

b) Sn

c) Pb

d) C

183.Phosphorous is manufactured by heating electric furnace a mixture of a) bone ash and coke alone

b) bone ash & silica c) bone ash, coke, sand d) bone ash

184.Which element is kept in water? a) P

b) Na

c) S

d) Si

185.An element when burnt in limited supply of air gives an oxide A which on treatment with water gives an acid B. Acid B on heating gives an acid C which gives yellow ppt. with AgNO3 solution, A is a) SO2

b) NO2

c) P2O3

d) SO3

186.The compound with garlic odour? a) P2O3

b) P2O5

c) H3PO4

d) H3PO3

184.The shape of PCl5 is a) pyramidal

b) linear

c) trigonal bipyramidal d) tetrahedral

184.The member of chalcogen family which can exhibit an oxidation state of +2 as well as -2 a) O2 only

b) S only

c) S and O2

d) Se only

185.

II. Very short answers: 1. Atomic structure-II: 1. What is dual character? 2. What is a matter wave? 3. Write de-Brolie equation 4. Define uses of de-Broglie's concept 5. Write Schrodinger's wave equation 6. Write the formula to calculate the energy of the electron by applying Schrodinger's equation 7. What is a node or nodal surface?

8. Draw the molecular orbital energy level for first and second period (except O2 and F2) 9. Expalin about diamagnetic and paramagnetic nature of molecules. 10. Explain why N2- is a paramagnetic ion. 11. Expalin about the metallic bond 12. Calculate the type of hybridisation of SF6 2. Atomic structure: 13. aa 14. aaa 15. aa 16. aa 17. aa 18. aa 19. aa 20. aa 3. Atomic structure: 21. aa 22. aaa 23. aa 24. aa 4. Atomic structure: 25. aa 26. aaa 27. aa 28. aa 5. Atomic structure: 29. aa 30. aaa 31. aa 32. aa 6. Atomic structure: 33. aa 34. aaa

35. aa 36. aa 7. Atomic structure: 37. aa 38. aaa 39. aa 40. aa 8. Atomic structure: 41. aa 42. aaa 43. aa 44. aa 9. Atomic structure: 45. aa 46. aaa 47. aa 48. aa 49. aa 50. aa III. Short answers: Section-A 1. Explain about the dual properties of light. 2. Explain about the difference between a particle and a wave. 3. Explain about the wave character of electron. 4. Explain about the particle character of electron. 5. Explain about de-Broglie equation 6. Explain how the energy of the electrons acquire negative value 7. Explain why the s-orbitals are spherically symmetrical in size? 8. Prove that He2 molecule does not exist. (based on bond order) 9. Give molecular orbital energy level of N2 molecule. 10. Expalin about the differences between metallic bond and covalent bond. 11. Expalin about the differences between metallic bond and ionic bond.

12. Expalin why rubber and glass are not electrical conductors. 13. Define hybridisation. 14. Section-B 51. aaa OR 52. IV. Long / Elaborate answers: Section-A 15. Explain about the experiments to prove the wave and particle character of electron. 16. aa 17. aa 18. aa 19. aaa Section-B 53. aaa OR 54.