chemistry-2
TRANSCRIPT
+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 b) Max Plank c) Rutherford d) Julius Plucker
3. 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 b) shape c) orientation in space d) all of them
6. 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 b) material with particle character c) both of them 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 b) do not interfere c) total value is their sum d) all of them
11. Sound from the speaker is called as wave because of
a) spread out in space b) it will interfere c) interference may be constructive or destructive d) all of them
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 = h b) E = mc2 c) both a and b d) none of them
16. In the equation E = h, the value of is
a) velocity of light b) Planck's constant c) frequency of wave d) none of them
17. In the equation E = h, 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 = h 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 b) Einstein constant c) Planck's constant d) none of them
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 =
a) 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) 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 c) probability of finding the electrond) the amplitude of the wave
28. The wave function ψ2 represents
a) probability of finding the electron b) potential energy c) both a & b d) none of them
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 sizec) 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 energyc) 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
38. Bond order of Oxygen molecule is
a) 2.5 b) 1 c) 3 d) 2
39. The hybridisation in SF6 molecule is
a) sp3 b) sp3d2 c) sp3d d) sp3d3
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 d) O2> N2> Li2
42. Arrange the molecules in the order of increasing Bond length
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+>O2
2-> O2- (b) O2
+>O2>O2->O2
2- (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 b) Carbon>Silicon>Germanium> Tin
c) Germanium>Silicon>Carbon>Tin d) Silicon>Carbon> Germanium> Tin
48. A good conductor have the energy gap between conductor band and valence band
a) medium b) large c) small d)
49. Arrange in the order of decrease in intermolecular attraction (Vander Waals forces)
a) Solids<Liquids<Gases b) Gas<Liquid<solid c) Liquid<Solid<Gas 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 d) None
2. Periodic classification-II:
56. On moving from top to bottom of a group the atomic radii will
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 b) increase c) remains same d) none
58. 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-) b) r(C+) / r(A-) = Z*(A-) / Z*(C+) c) r(A-) / r(C+) = Z*(A-) / Z*(C+) d) both a and b
67. Ionisation energy is the energy required
a) to add an electron b) to remove an electron c) to attract the shared electrond) none
68. Second ionisation potential is related with the following equation
a) M2+(g) +IxM3+
(g) + e- b) M+(g) +IxM2+
(g) + e- c) M(g) +IxM+
(g) + e- d) 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 b) Li has lower nuclear charge than Be c) Be has higher nuclear charge than Li d) Be has lower nuclear charge than Li
71. The ionisation energy (IE) of 'Be' is more than 'B' because
a) B has higher nuclear charge than Be b) Be has lower nuclear charge than B c) B has unpaired electron than Be 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<p<d<f 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 electronsd) 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 b) inversely proportional to its sizec) independent of 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
90. The electron affinity is expressed in
a) kJ b) J c) kJ mol d) kJ mol-1
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 b) 1.44 c) 1.98 d) 2.28
94. Noble gases have electron affinity
a) High 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
96. When XA > XB, A - B bond is (H2O)
a) polar covalent b) non-polar covalent c) Ionic d) metallic
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 b) 3 - 12 c) 13 - 18 d) none
100.The general electronic configuration of p-block elements is
a) ns2np1-6 b) ns2np2 c) ns2np4 d) ns2np1
101.p-block elements consists of
a) metals only b) metals & non-metals c) non-metals only d) none
102.The familiar characteristic of p-block elements is
a) low I.E b) zero oxidation states c) inert pair effect d) none
103.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 b) Gallium c) Thallium d) Boron
105.Atomic radius and I.E of group 13 elements decreases from top to bottom except
a) Al b) Gallium c) Indium d) Thallium
106.The metallic character will increase in the order of
a) B, Al, Ga, In, Tl b) Tl,In,Ga,Al,B c) AL,B,In,Tl,Ga d) none
107.Among the group 13 elements the toxic element is
a) Al b) Gallium c) Indium d) Thallium
108.The atomic radii of Ga is slightly less than Al because of
a) higher atomic no. b) poor shielding effect of 3d electrons c) none d)
109.Group-13 elements generally have the oxidation no of
a) +3 b) +2 c) +1 d) none
110.Potash alum is
a) K2SO4.Al2(SO4)3.12H2O b) K2SO4.Al2(SO4)3.24H2Oc) K2SO4.Al2(SO4)3.42H2O d) K2SO4.Al2(SO4)3.2H2O
111.Potash ash is manufactured form
a) alunite or alum stone b) alumina c) both a & b d) none
112.Potash alum is crystallised by adding
a) Aluminium hydroxide b) Potassium sulphate c) Potassium sulphite d) none
113.Potash alum is
a) green crystal b) blue crystal c) silver crystal d) white crystal
114.Potash alum is insoluble in
a) water b) alcohol c) benzene d) acids
115.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 b) ns2np2 c) ns2np3 d) ns2np4
117.Group-14 elements generally have the oxidation no of
a) +3 b) +2 c) +1 d) +4
118.In group-14 elements, element have high Catenation property
a) Carbon b) Si c) Ge d) Pb
119.The basic chemical unit of silicate is
a) SiO4 b) SiO42- c) SiO4
3- d) SiO44-
120.The structure of SiO44- ion is
a) bi-pyramidal b) octahedral c) tetrahedral d) none
121.Silica is prepared by the complete hydrolysis of
a) SiCl b) SiCl2 c) SiCl3 d) SiCl4
122.Ores of Pb
a) Anglesite b) Cerrusite c) Galena d) all of them
123.The colour of Lead is
a) Greenish b) bluish grey c) reddish d) none
124.Red lead is
a) Pb3O4 b) PbO c) Pb2O3 d) none
125.Plumbo solvency is
a) Pb(OH) b) Pb2(OH) c) Pb(OH) 2 d) Pb(OH)3
126.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 b) ns2np2 c) ns2np3 d) ns2np6
128.Phosphorous (P) is present as
a) red P b) yellow or white P c) both a and b d) none
129.Which element of Group-15 have allotropy character
a) P b) N c) As d) Bi
130.White P can be converted into red P by heating in presence of
a) Bromine b) Iodine c) Chlorine d) none
131.Phosphine gas is produced by boiling white P with
a) KOH b) CaOH c) NaOH d) none
132.PCl5 is a
a) Colourless liquid b) yellowish gas c) yellowish crystal d) greenish solid
133.With excess water PCl5 gives
a) POCl3 b) H3PO4 c) HPO3 d) none
134.With insufficient water PCl5 gives
a) POCl3 b) H3PO4 c) HPO3 d) none
135.Phosphorous trioxide (P2O3) has a smell of
a) rotton egg b) pleasant c) garlic d) none
136.Phosphorous trioxide (P2O3) reacts with hot water to give
a) PH3 b) HPO3 c) H3PO4 d) H3PO3
137.Phosphorous pentaoxide (P2O5) is a
a) white waxy substance b) white solid c) yellowish crystal d) none
138.Metaphophoric acid is
a) PH3 b) HPO3 c) H3PO4 d) H3PO3
139.Phosphorous pentaoxide (P2O5) is used as a
a) reducing agent b) oxidising agent c) dehydrating agent d) none
140.Phosphorous acid (H3PO3) is used as a
a) reducing agent b) oxidising agent c) dehydrating agent d) none
141.H3PO4 is
a) solid b) liquid c) gas d) none
142.H3PO4 reacts with AgNO3 to give precipitate of silver phosphate
a) red b) yellow c) green d) gold
143.H3PO4 reacts with AgNO3 to give
a) Ag3PO4 b) AgPO4 c) Ag2PO3 d) Ag4PO3
144.Phosphine (PH3) has a smell of
a) rotton egg b) sweet c) garlic d) rotton fish
145.Which of the following is used as a smoke screen
a) H3PO4 b) HPO3 c) P2O5 d) PH3
146.PCl3 and PCl5 are chlorinating agents because they
a) add Cl b) remove Cl c) remove H d) add O
147.PCl3 is a better chlorinating agents because it chlorinates
a) only organic compounds b) metals also c) non-metals d) none
148.aaa
a) b) c) d)
149.aaa
a) b) c) d)
Group-16 Elements
150.elements O,S,Se,Te are CHALCOGENS because their ores are mainly
a) sulphates b) oxides c) oxides & sulphides d) sulphides
151.Which element is called as Brim stone among the G-16 elements
a) S b) Se c) Te d) Po
152.Which element is radioactive among the G-16 elements
a) S b) Se c) Te d) Po
153.The general electronic configuration of group-16 elements is
a) ns2np1 b) ns2np2 c) ns2np4 d) ns2np6
154.Which element is having allotropy among the G-15 elements
a) S b) Se c) Po d) all of them
155.Which one is called as oil of vitriol
a) H3PO3 b) H3PO4 c) H2SO4 d) none
156.Acid will be added to water to dilute the acid because
a) it precipitates b) it gets cooled c) it produces heat d) none
157.H2SO4 turns blue litmus paper to
a) green b) no change c) red d) white
158.H2SO4 turns methyl orange to
a) yellow b) pink c) red d) gold
159.H2SO4 reacts with more electro+ve elements like Zn and Fe to give
a) H2 b) O2 c) S d) both a & c
160.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 b) ns2np4 c) ns2np6 d) none
162.Which element is radioactive among the G-16 elements
a) Cl b) Br c) I d) At
163.Cl is a
a) coulorless gas b) light yellow gas c) reddish brown gas d) yellowish green gas
164.Iodine (I2) is a
a) gas b) liquid c) solid d) none
165.Among the halogens which one is the strongest oxidising agent
a) F2 b) Cl2 c) Br2 d) I2
166.F2 reacts with water and gives
a) HF b) O2 c) O3 d) all of them
167.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
168.Which one the hydrogen halide is liquid
a) HF b) HCl c) HBr d) HI
167.Arrange in the increasing order of hydrogen halides acidic character
a) HF>HCl>HBr>HI b) H I>HBr>HCl>HF c) HCl>HF>HBr>HI d) none
168.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
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 b) ns2np4 c) ns2np6 d) none
172.All the elements of G-18 are
a) gases b) liquids c) solids d) none
173.All the elements of G-18 are called inert gases because of their
a) oxidation power b) reduction power c) chemical inactivity d) none
174.Group-18 elements can also be called as
a) halogen gases b) noble gases c) chalcogens d) none
175.Xenon fluorides are
a) crystalline solids b) liquids c) gases d) none
176. Xenon fluorides will sublime at
a) 273°K b) 298°K c) 3982K d) 373°K
176.Aeroplane tyres are filled with
a) H2 b) N2 c) He d) O2
177.Divers will use the mixture of
a) H2 & O2 b) N2 & O2 c) O2 & He d) only O2
177. Electrical bulbs were filled with
a) N2 b) Ne c) Ar d) both b & C
178.Which of the following is most abundant in earth's crust?
a) C b) Si c) Ge d) Sn
179.The metalloid among the following is
a) Si b) P c) Ge d) Sn
178. Which of the following does not exhibit allotropy
a) C b) Si c) Sn d) Pb
180.Which one of the following is three-dimensional silicate?
a) talc b) beryl c) quartz d) kaoline
181.An example of an amphibole is
a) beryl b) tremolite c) spodumena d) forsterite
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 b) bone ash & silica c) bone ash, coke, sand d) bone ash alone
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.