Question Bank For NEET
17
1 Question Bank For NEET CHEMISTRY (CHEMICAL BONDING AND MOLECULAR STRUCTURE) MCQ (1 to 234) ANSWER SHEET
Transcript of Question Bank For NEET
1
Question Bank For NEET
CHEMISTRY (CHEMICAL BONDING AND MOLECULAR STRUCTURE)
MCQ (1 to 234)
ANSWER SHEET
2
4
1. The octet rule is not obeyed in -
(1) CO2 (2) BCl3
(3) PCl5 (4) Both (2) and (3)
2. Weakest bond is
(1) ionic bond (2) covalent bond
(3) coordinate bond (4) hydrogen bond
3. The valency of sulphur in sulphuric acid is
(1) 2 (2) 4 (3) 6 (4) 8
4. The number of electrons involved in the bond
formation of N 2 molecule
(1) 2 (2) 4 (3) 6 (4) 10
5. The electronic configuration of four elements
are given in brackets
L (1s2 , 2s2 2 p1 ); M (1s2 , 2s2 2 p5) Q (1s2 , 2s2 2 p6 , 3s1 ) ; R( 1s2 , 2s2 2 p 2) The element that would most readily form a diatomic
molecule is
(1) Q (2) M (3) R (4) L
6. Which follows octet rule -
(1) FeCl2 (2) AgCl (3) CaCl2 (4) CuCl
7. The element completing its octet by transfer of elec-
trons is
(1) MgO (2) H2S (3) PH
3 (4) CCl
4
8. In covalency
(1) Electrons are transferred
(2) Electrons are equally shared
(3) The electron of one atom are shared between two
atoms
(4) None of the above
• • • •
11 Which condition favours the bond formation:
(1) Maximum attraction and maximum potential energy
(2) Minimum attraction and minimum potential energy
(3) Minimum potential energy and maximum attraction
(4) None of the above
12 Electrovalent compounds or ionic compounds do not
show stereoisomerism. The reason is:
(1) Presence of ions
(2) Strong electro static force of attraction
(3) Brittleness
(4) Non-directional nature of ionic bond
13 Which of the following is not a characteristic of a
covalent compound:
(1) It has low melting point and boiling point
(2) It is formed between two atoms having very
smallelectronegativity difference
(3) They have no definite geometry
(4) They are generally insoluble in water
14 For the formation of covalent bond, the difference
in the value of electronegativities should be
(1) Equal to or less than 1.7
(2) More than 1.7
(3) 1.7 or more
(4) None of these
15 In Co-ordinate bond, the acceptor atom must
essentially contain in its valency shell an orbital (ion
group):
(1) With paired electron (2) With single electron
(3) With no electron (4) With three electron
16 Four elements A (with one valence electron), B
(with three valence electrons), C (with five valence
electrons) and D (with seven valence electrons) are
lying in the second period in periodic table which of
the following is/are diatomic at room temperature :
(1) Only C2 (2) Only A2
(3) C2 and D2 (4) Only B2
17 Covalent compounds are generally ...... in water (1) Soluble (2) Insoluble
9. N• • N N
• • (3) Dissociated (4) Hydrolysed
(I) (II) (III)
Calculate the formal charge of each I, II and III nitrogen
atom respectively
18 Which one is the electron deficient compound
(1) ICl (2) NH 3
(1) +1, –1, 0 (2) –1, –1, +1
(3) –1, +1, –1 (4) 0, –1, –1 (3) BCl3 (4) PCl3
10. According to Lewis structure the number of lone pair
& bond pair of electrons in SO 2– ion.
(1) 12, 6 (2) 12, 4 (3) 10, 8 (4) 8, 8
19 Silicon has 4 electrons in the outermost orbit. In
forming the bonds
NEET-CHEMISTRY MCQ-230
3
(1) It gains electrons (2) It loses electrons
(3) It shares electrons (4) None of these
4
3 4 2 3
20. Which species has the maximum number of lone pair 31. The structure of orthophosphoric acid is
of electrons on the central atom? O H
(1) [ClO ]− (2) XeF (3) SF (4) [I ]−
|
3 4 4 3 ↑ H − O − P − O − H O ← P − O − H
21. A simple example of a coordinate covalent bond is
exhibited by
|
(1) O |
H
|
(2) O |
H
(1) C 2 H 2 (2) H 2 SO 4 (3) NH 3 (4) HCl
H
22. The bond that exists between
called
NH 3 and BF3 is
(3)
|
O ← P |
H
– O − H
(4)
O
↑ H − O − P = O
(2) Electrovalent (2) Covalent
(3) Coordinate (4) Hydrogen
23. Which of the following does not have a coordinate
bond
(1) SO 2 (2) HNO 3 (3) H 2 SO 3 (4) HNO 2
Coordinate Bond
24. Coordinate covalent compounds are formed by
(3) Transfer of electrons
(4) Sharing of electrons
(5) Donation of electrons
(6) None of these process
25. In the coordinate valency
(7) Electrons are equally shared by the atoms
(8) Electrons of one atom are shared with two atoms
(9) Hydrogen bond is formed
(10) None of the above
26. Which of the following contains a coordinate covalent
bond
32. What is the nature of the bond between B and O in
(C 2 H 5 )2 OBH 3
(1) Covalent (2) Co-ordinate covalent
(3) Ionic bond (4) Banana shaped bond
33. Sulphuric acid provides a example of
(1) Co-ordinate bonds
(2) Non-covalent compound
(3) Covalent and co-ordinate bond
(4) Non-covalent ion
34. The pair of compounds which can form a co-
ordinate bond is:
(1) (C2H5)3 B and (CH3)3N (2) HCl and HBr
(3) BF3 and NH3
(4) (1) and (3) both
VBT (overlapping and Hybridization)
35. The nature of bonding in graphite is
(1) Covalent (2) Ionic
(3) Metallic (4) Coordinate
(1) N 2 O 5 (2) BaCl 2 (3) HCl (4) H 2 O
36. Correct statement regarding this reaction
BF3 + NH3 ⎯→ [F3B ← NH3]
27. Which has a coordinate bond (1) Hybridisation of N is changed
(1) SO 2− (2) CH (3) CO (4) NH (2) Hybridisation of B is changed
(3) NH3 act as a lewis base (4) (2) & (3) both
28. The compound containing co-ordinate bond is
(1) O 3 (2) SO 3 (3) H 2 SO 4 (4) All of these 37. Triple bond in ethyne is formed from
(1) Three sigma bonds (2) Three pi bonds
29. The number of dative bonds in sulphuric acid
molecules is
(1) 0 (2)1 (3) 2 (4) 4
30. Which of the following compounds has coordinate
(dative) bond
(3) One sigma and two pi bonds
(4) Two sigma and one pi bond
38. The bond in the formation of fluorine molecule will
be
(1) Due to s − s overlapping (2) Due to s − p overlapping
(1) CH 3 NC (2) CH 3 OH (3) Due to p − p overlapping
(3) CH 3 Cl (4) NH 3 (4) Due to hybridization
5
39. Which type of overlapping results the formation of a
π bond
(1) Axial overlapping of s − s orbitals
(2) Lateral overlapping of p − p orbitals
(3) Axial overlapping of p − p orbitals
48. In a double bond connecting two atoms, there is a
sharing of
(1) 2 electrons (2) 1 electron
(3) 4 electrons (4) All electrons
49. Strongest bond is
(4) Axial overlapping of s − p orbitals
40. A sigma bond is formed by the overlap of atomic
(1) C − C
(3) C ≡ C
(2) C = C
(4) All are equally strong π
orbitals of atoms A and B. If the bond is formed along
the x-axis, which of the following overlaps is
acceptable?
(1) s orbital of A and pz orbital of B (2) px orbital of A and py orbital of B
(3) pz orbital of A and px orbital of B
(4) px orbital of A and s orbital of B
50. The double bond between the two carbon atoms in
ethylene consists of
(1) Two sigma bonds at right angles to each other
(2) One sigma bond and one pi bond
(3) Two pi bonds at right angles to each other
(4) Two pi bonds at an angle of 60 o to each other
51. In the series ethane, ethylene and acetylene, the
41. The strength of bonds by 2s – 2s, 2p – 2p and 2p – 2s C − H bond energy is
overlapping has the order:
(1) 2s – 2s > 2p – 2p > 2s – 2p
(2) 2s – 2s > 2p – 2s > 2p – 2p
(3) 2p – 2p > 2s – 2p > 2s – 2s
(4) 2p – 2p > 2s – 2s > 2p – 2s
42. n the following which species does not contain sp 3
hybridization
(1) NH 3 (2) CH 4 (3) H 2O (4) CO 2
43. Which of the following substances has giant
covalentucture
(1) Iodine crystal (2) Solid CO 2
(3) Silica (4) White phosphorus
44. With which of the given pairs CO2
resembles (2) HgCl
2, C
2H
2 (2) HgCl
2, SnCl
4
(3) C2H
2, NO
2 (4) N
2O and NO
2
45. A σ-bond is formed by two px orbitals each
containing one unpaired electron when they approach
each other along :
(3) x - axis (2) y - axis (3) z - axis (4) any direction
(1) The same in all the three compounds (2) Greatest in ethane
(3) Greatest in ethylene
(4) Greatest in acetylene
52. Which is not characteristic of π-bond:
(1) π-bond is formed when a sigma bond already formed
(2) π-bond are formed from hybrid orbitals
(3) π- bond may be formed by the overlapping of p-
orbitals
(4) π- bond results from lateral overlap of atomic orbital
53. Number of σ and π bonds present in
CH3 — CH == CH — C ≡≡ CH are:
(1) 10σ, 3π (2) 10σ, 2π (3) 9σ, 2π (4) 8σ, 3π
54. The correct order of bond length is
(1) C – C < C = C < C ≡ C
(2) C≡ C < C = C < C – C
(3) C = C < C ≡ C < C – C
(4) C = C < C – C < C ≡ C
55. In a sigma bond
(1) Sidewise as well as end to end overlap of orbitals
take place
(2) Sidewise overlap of orbitals takes place
(3) End to end overlap of orbitals takes place
(4) None of the above
46. Amongst ClF3 , BF3 and NH 3 molecules the one
with non-planar geometry is 56. Which of the following is not correct (1) A sigma bond is weaker than π bond
(1) ClF3
(3) BF3
(2) NH 3
(4) None of these
(2) A sigma bond is stronger than π bond (3) A double bond is stronger than a single bond
(4) A double bond is shorter than a single bond
47. The number and type of bonds between two carbon
atoms in calcium carbide are
(1) One sigma, one pi
(2) One sigma, two pi
(3) Two sigma, one pi
(4) Two singma, two pi
57. Strongest bond formed, when atomic orbitals
(1) Maximum overlap
(2) Minimum overlap
(3) Overlapping not done
(4) None of them
6
4
2 2 2
4 3 2
4 4 4
4 4 4
58. The p − p orbital overlapping is present in the 69 Which molecule is linear
following molecule
(1) Hydrogen (2) Hydrogen bromide (1) NO 2 (2) ClO2 (3) CO 2 (4) H 2S
(3) Hydrogen chloride (4) Chlorine
59. Which molecule is not linear
(1) BeF2 (2) BeH 2 (3) CO 2
(4) H 2O
70 Which of the following molecules has trigonal planer
geometry
(1) IF3 (2) PCl3 (3) NH 3 (4) BF3
60. The bond angle in water molecule is nearly or Directed
bonds in water forms an angle of
71. Structure of ammonia is
(1) Trigonal (2) Tetrahedral
(3) Pyramidal (4) Trigonal pyramidal
(1) 120 o (2) 180 o (3) 109 o 28 ' (4) 104 o 30 ' 72. Which of the following statement is not correct -
(1) CH + shows sp2-hybridisation whereas CH – shows 61. Cyanogen, (CN )2 , has a _ _ shape/structure :
(1) Linear (2) Zig-zag (3) V-shape (4) Cyclic
62. The d-orbitals involved in sp3d hybridisation in
trigonal bipyramidal geometry :
3 3
sp3-hybridisation
(2) NH + has a regular tetrahedral geometry
(3) sp2-hybridised orbitals have equal s and p character
(4) Hybrid orbitals always form σ-bonds
(1) dx2 −y2 (2) dz2 (3) dxy (4) dxz 73. Amongst NH3, BeCl2, CO2 and H2O, the non-linear
molecules are :
63. A sp3 hybrid orbital contains: (1) BeCl2 and H2O (2) BeCl2 and CO2
(3) NH3 and H2O (4) NH3 and CO2
(1)
(3)
3 s–character (2)
4
3 4
p–character (4)
1
4 p–character
1
2 s – character
74 The cationic part of solid Cl2O6 is having the ___________shape.
(1) linear (2) angular
(3) Tetrahedron (4) undefined
64. Which of the set of species have same hybridisation
state but different shapes: 75 Molecular shapes of SF4, CF4 and XeF4 are:
(1) the same, with 2, 0 and 1 lone pair of electrons
(1) NO+, NO , NO−
(3) NH+, H O+, OF
(2) CIO−, SF , XeF
(4) SO−2, PO−3, ClO−
respectively
(2) the same, with 1, 1 and 1 lone pair of electrons
respectively
(3) different with 0, 1 and 2 lone pair of electrons
65. Among the following compounds the one that is planar
and has the central atom with sp2 hybridisation is:
respectively
(4) different with 1, 0 and 2 lone pair of electrons
(1) NH + (2) SiF (3) BF (4) ClO – respectively 4 4 3 4
66. In an octahedral structure, the pair of d orbitals
involved in sp3d2 hybridization is :
76. Compound formed by sp 3d hybridization will have
structure
(1) d , d (2) d 2 2 , d 2 (1) Planar (2) Pyramidal xy yz
(3) dxz , dx2 −y2
x −y z
(4) dz2 , dxz
(3) Angular (4) Trigonal bipyramidal
77. Which of the following formula does not correctly
epresent the bonding capacity of the atom involved
67. In a change from PCl3 →PCl5, The hybrid state of P
change from: (1) sp2 to sp3 (2) sp3 to sp2
⎡ H ⎤ ⎢ | ⎥
(1) ⎢ H − P − H ⎥
F F (2)
(3) sp3 to sp3d (4) sp3 to dsp2
68. The central atom in a molecule is in sp 2 hybrid state.
⎢ | ⎥ O
⎣ ⎢ H ⎥ ⎦
O O
The shape of molecule will be
(1) Pyramidal (2) Tetrahedral
(3) Octahedral (4) Trigonal planar
(3) O ← N O − H
(4) H − C = C
O − H
7
3 3
3
2
78. The mode of hybridisation of carbon in CO 2 is
(1) sp (2) sp 2
87. Which one in the following is not the resonance
structure of CO 2
(3) sp 3 (4) None of these (1) O = C = O
(3) + O ≡ C − O−
(2) − O − C ≡ O+
(4) O ≡ C = O
79. Which of the following molecules has a square
pyramidal structure :
88. Which of the following molecule contains one pair of
non-bonding electrons (1) XeO2F2 (2) XeOF2 (3) XeO3F2 (4) XeOF4 (1) CH 4 (2) NH 3 (3) H 2 O (4) HF
80. Which of the following hybridizations involves dxy
orbitals :
(1) sp3d (2) sp3d2 (3) dsp2 (4) sp3d3
81. The ratio between σ bond and π bond in tetracyano
ethylene :
(1) 2 : 1 (2) 1 : 1
(3) 1 : 2 (4) None of these
82. Choose the molecules in which same hybridisation
occurs in the ground state:
(i) BCl3 (ii) NH3 (iii) PCl3 (iv) BeF2
The correct answer is:
(1) i, ii, iv (2) i, ii, iii (3) ii, iii (4) iii, iv
83. In which of the following the central atom does not
89. Resonance is due to
(1) Delocalization of sigma electrons
(2) Delocalization of pi electrons
(3) Migration of H atoms
(4) Migration of protons
90. Resonating structures have different
(1) Atomic arrangements
(2) Electronic arrangements
(3) Functional groups
(4) Alkyl groups
91. In the cyanide ion, the formal negative charge is on
(1) C
(2) N
(3) Both C and N
(4) Resonate between C and N
use sp 3 hybrid orbitals in its bonding
(1) BeF − (2) OH + (3) NH − (4) NF3 92. The bond angle in H2O molecule is less than that of
NH3 molecule because: (5) The hybridisation of O in H2O and N in NH3 is
84. Which of the following hybridisation results in non-
planar orbitals
different
(6) The atomic radii of N and O are different
(1) sp 3 (2) dsp 2 (3) sp 2 (4) sp (3) There is one lone pair of electrons on O and two
lone pairs of electrons on N
(4) There are two lone pairs of electrons on O and one
85. Fluorine does not form any polyhalide as other
halogens because:
(1) It has maximum ionic character
(2) It has low F-F bond energy (38.5 kcl mol–1)
(3) Of the absence of d-orbitals in the valence shell
of fluorine
(4) It brings about maximum coordination number in
other elements
VSEPRT, Bond Angle, Bond Length, Bond Energy
86. Which of the following is true ?
lone pairs of electrons on N
93. The order of increasing adjacent bond angle in the
molecules BeCl2, BCl3, CCl4 and SF6 is:
(1) SF6 < CCl4 < BCl3 < BeCl2
(2) BeCl2 < BCl3 < CCl4 < SF6
(3) SF6 < CCl4 < BeCl2 < BCl3
(4) BCl3 < BeCl2 < SF6 < CCl4
94. Which does not show resonance
(1) Benzene (2) Aniline
(3) Ethyl amine (4) Toluene
(1) Bond order ∝ 1
bond length ∝ bond energy 95. The number of possible resonance structures for
CO 2− is
(2) Bond order ∝ bond length ∝
1
1
bond energy 1
(1) 2 (2) 3 (3) 6 (4) 9
96. The order of increasing bond length in F2, N2, Cl2
(3) Bond order ∝ ∝ bond length
bond energy and O2 is: (1) N2 < O2 < Cl2 < F2 (2) N2 < O2 < F2 < Cl2
(4) Bond order ∝ bond length ∝ bond energy (3) O2 < N2 < Cl2 < F2 (4) N2 < Cl2 < O2 < F2
8
4 4
97. In which of the following molecules/ions are all
the bonds not equal?
108. As the s-character of hybridized orbital decreases, the
bond angle
(1) XeF (2) BF − (3) SF
(4) SiF (1) Decreases (2) Increases
4 4 4 4 (3) Does not change (4) Becomes zero
98. The bond angle in PH 3 would be expected to
be close to
(1) 90º (2) 105º (3) 109º (4) 120º
99. In which molecule are all atoms coplanar
109. XeF2 molecule is
(1) Linear
(2) Triangular planar
(3) Pyramidal
(4) Square planar
(1) CH 4 (2) BF3 (3) PF3 (4) NH 3 110. Of the following sets which one does NOT contain
100. Which has the least bond angle isoelectronic species
(1) NH 3 (2) BeF2 (3) H 2 O (4) CH 4 (1) PO 3 − , SO 2 −, ClO − (2) CN −, N , C 2 − 4 4 4 2 2
(3) SO 2− , CO 2 −, NO − (4) BO 3 −, CO 2− , NO − 101. In compound X , all the bond angles are exactly
109 o 28 ', X is
3 3 3
Dipole Moment
3 3 3
(1) Chloromethane (2) Iodoform
(3) Carbon tetrachloride (4) Chloroform 111. Which set of molecules is polar:
(1) XeF , IF , SO 4 7 3
102. The decreasing value of bond angles from NH3 (106)° (2) PCl5, C6H6, SF6 (3) SnCl2, SO2, NO–
to SbH3 (101)° down group-15 of the periodic table is 2 (4) CO , CS , C H
due to:
(1) decreasing lp – bp repulsion
(2) increasing electronegativity
(3) increasing bp – bp repulsion
(4) increasing p–orbital character in sp3
103. Of the following compounds, the one having a
linear structure is
(1) NH 2 (2) CH 4 (3) C 2 H 2 (4) H 2 O
104. XeF6 is
112.
2 2 2 6
BF3 and NF3 both molecules are covalent, but BF3 is
non-polar and NF3 is polar. Its reason is
(1) In uncombined state boron is metal and nitrogen
is gas
(2) B − F bond has no dipole moment whereas
N − F bond has dipole moment
(3) The size of boron atom is smaller than nitrogen
(4) BF3 is planar whereas NF3 is pyramidal
(1) Octahedral
(2) Distorted octahedral
113. Which of the following have both polar and non-polar
bonds
(3) Planar
(4) Tetrahedral (1) C 2 H 6 (2) NH 4 Cl (3) HCl (4) AlCl 3
105. Which has maximum bond angle
(1) CHF3
(2) CHCl 3
(3) CHBr 3
(4) All have maximum bond angle 106. Of the following species the one having a square planar
structure is
(1) NH + (2) BF − (3) XeF4 (4) SCl 4
107. In which of the following is the angle between the
two covalent bonds greatest
114.Which molecules has zero dipole movement
(1) H 2O (2) CO 2 (3) HF (4) HBr
115.In the following which one have zero dipole moment
(1) BF3 (2) CCl 4 (3) BeCl 2 (4) All of these
116. Which molecule has the largest dipole moment
(1) HCl (2) HI (3) HBr (4) HF
117. The unequal sharing of bonded pair of electrons
between two atoms in a molecule causes
(1) Dipole
(2) Radical formation
(3) Covalent bond
9
(1) CO 2 (2) CH 4 (3) NH 3 (4) H 2 O (4) Decomposition of molecule
10
118. BeF2 has zero dipole moment whereas H2O has dipole
moment because: 127. The molecule which has the largest dipole
moment amongst the following (1) Water is linear
(2) H2O is bent (3) F is more electronegative than O
(4) Hydrogen bonding is present in H2O
(1) CH 4 (2) CHCl 3 (3) CCl 4
128. Positive dipole moment is present in
(4) CHI 3
119. Which of the following molecules will show dipole (1) CCl 4 (2) C 6 H 6 (3) BF3 (4) HF
moment
(1) Methane (2) Carbon tetrachloride
(3) Chloroform (4) Carbon dioxide
120. Which of the following compounds possesses the
dipole moment
(1) Water (2) Boron trifluoride
(3) Benzene (4) Carbon tetrachloride
129 The polarity of a covalent bond between two atoms
depends upon
(1) Atomic size (2) Electronegativity
(3) Ionic size (4) None of the above
Cl
121. Which bond angle θ would result in the maximum
dipole moment for the triatomic molecule YXY
130 The dipole moment of is 1.5 D. The dipole
(1) θ = 90 o
(3) θ = 150 o
(2) θ = 120 o
(4) θ = 180 o
moment of is :
122. Which of the following would have a permanent dipole
moment
(1) BF3 (2) SiF4 (3) SF4 (4) XeF4 (1) 0 D (2) 1.5 D (3) 2.86 D (4) 2.25 D
123. Carbon tetrachloride has no net dipole moment because of
(1) Its planar structure
(2) Its regular tetrahedral structure
(3) Similar sizes of carbon and chlorine atoms
(4) Similar electron affinities of carbon and chlorine
131
H 2 O Pick out the molecule which has zero dipole
moment
(1) NH 3 (2) H 2 O (3) BCl 3 (4) SO 2
124. The correct oreder of dipole moment is:
(1) CH4 < NF3 < NH3 < H2O (2) NF3 < CH4 < NH3 < H2O
(3) NH3 < NF3 < CH4 < H2O
(4) H2O < NH3 < NF3 < CH4
125. Which one of the following molecules has highest
dipole moment:
(1) H2S (2) CO2 (3) CCl4 (4) BF3
126. Which of the following has more dipole moment :
132. Zero dipole moment is present in
(1) NH 3
(2) cis 1, 2-dichloroethene
(3) trans 1, 2-dichloroethene
(4) None of these
Hydrogen Bonding
133. The H bond in solid HF can be best represented as:
(1) H − F....H − F ... H − F
Cl
(1)
Cl
(2)
Cl
Cl
(2) H H H H
F F F
F F
(3) H H H H
F
(3) Cl Cl
Cl
H H
(4) F F F F
H (4) All has same dipole moment
11
134. In which of the following hydrogen bond is present 143. Out of the two compounds shown below, the vapour
(1) H 2 (2) Ice pressure of (2) at a particular temperature is expected
(3) Sulphur (4) Hydrocarbon
135. In the following which has highest boiling point
(1) HI (2) HF (3) HBr (4) HCl
136. Which contains hydrogen bond
(1) HF (2) HCl (3) HBr (4) HI
to be:
NO2
(1)
OH
and
(2)
OH
NO2
137. Contrary to other hydrogen halides, hydrogen fluoride
is a liquid because
(1) Size of F atom is small
(2) HF is a weak acid
(3) HF molecule are hydrogen bonded
(4) Fluorine is highly reactive
138. Intramolecular H-bond:
(1) Decreases Volatility (2) Increases melting point
(3) Increases viscosity (4) Increases volatility
139. The hydrogen bond is strongest in:
(1) O – H - - - S (2) S – H - - - O
(3) F – H - - - F (4) O – H - - - O
140. Which of the following has strongest intramolecular
hydrogen bonding:
(1) Higher than that of (1)
(2) Lower than that of (1)
(3) Same as that of (1)
(4) Can be higher or lower depending upon the size of
the vessel
144. KF combines with HF to form KHF2. The compound
contains the species:
(1) K+, F– and H+ (2) K+, F– and HF
(3) K+ and [HF2]– (4) [KHF]+ and F2
145. The pairs of bases in DNA are held together by :
(1) Hydrogen bonds (2) Ionic bonds
(3) Phosphate groups (4) Deoxyribose groups
146. The reason for exceptionally high boiling point of water
OH
(1)
OH
(3)
COOH
(2)
(4)
OH
OCH3
COOH
is
(1) Its high specific heat
(2) Its high dielectric constant
(3) Low ionization of water molecules
(4) Hydrogen bonding in the molecules of water
147. Which concept best explains that o-nitrophenol is more
volatile than p-nitrophenol
(1) Resonance (2) Hyperconjugation
(3) Hydrogen bonding (4) Steric hinderence
COOH COOH 148. Which contains strongest
H − bond
141. As a result of sp hybridization, we get
(1) Two mutual perpendicular orbitals
(2) Two orbitals at 180 o
(1) O − H ..... S
(3) F − H ..... F
(2) S − H .... O
(4) F − H ..... O
(3) Four orbitals in tetrahedral directions
(4) Three orbitals in the same plane 149. Which of the following compound can form
hydrogen bonds
142. The boiling point of p-nitrophenol is higher than
that of o-nitrophenol because:
(1) CH 4 (2) NaCl (3) CHCl 3 (4) H 2 O
(1) NO2 group at p-position behaves in a different way
from that at o-position
(2) intramolecular hydrogen bonding exists in p-
nitrophenol
(3) there is intermolecular hydrogen bonding in p-
nitrophenol
(4) p-nitrophenol has a higher molecular weight than
o-nitrophenol
150. Of the following hydrides which has the lowest
boiling point
(1) NH 3 (2) PH 3 (3) SbH 3 (4) AsH 3
151. Water has high heat of vaporisation due to
(1) Covalent bonding (2) H − bonding
(3) Ionic bonding (4) None of the above
12
Weak Forces
152. The nature of intermolecular forces among benzene
(C6H6) molecules is:
(1) Dipole-dipole attraction
(2) London dispersion force
(3) Ion-dipole attraction
(4) Hydrogen bonding
153. In which molecule the Vander Waals force (dispersion
force) is likely to be the most important in determining
the m.pt. and b.pt. :
162. Which has weakest bond
(1) Diamond (2) Neon (Solid)
(3) KCl (4) Ice
163.Glycerol has strong intermolecular bonding therefore it is
(1) Sweet (2) Reactive
(3) Explosive (4) Viscous
164. Among the following the weakest one is
(1) Br2 (2) CO (3) H
2S (4) HCl (1) Metallic bond
(2) Ionic bond
154. In a crystal cations and anions are held together by
(1) Electrons (2) Electrostatic forces
(3) Nuclear forces (4) Covalent bonds
155. In the following metals which one has lowest probable
interatomic forces
(1) Copper (2) Silver (3) Zinc (4) Mercury
156. In solid argon, the atoms are held together by
(1) Ionic bonds
(2) Hydrogen bonds
(3) Vander Waals forces
(4) Hydrophobic forces
157. Covalent-molecules are usually held in a crystal struc-
ture by
(1) Dipole-dipole attraction
(2) Electrostatic attraction
(3) Hydrogen bond
(4) Van-der waal's attraction
158. Which one of the following substances consists of
small discrete molecules
(1) NaCl (2) Graphite (3) Copper (4) Dry ice
159. In melting lattice, structure of solid
(1) Remains unchanged (2) Changes
(3) Becomes compact (4) None of the above
(3) Van der Waal’s force
(4) Covalent bond
Back Bonding, Bridge bonding and odd electron
molecules
165. In BF3 :
(1) B-F bond has some double bond character and this
bond is delocalised
(2) All the B–F bonds are single covalent in nature
(3) Bond energy and bond-length of B–F bond indicate
its single bond character
(4) All of the above bonds are ionic
166. Which of the following is false statements :-
(1) Boranes are easily hydrolysed
(2) LiAlH4 reduces BCl
3 to borane
(3) BH3 is a Lewis acid
(4) All the B–H distances in diborane (B2H
6) are equal
167. When an inorganic compound (X) having 3c–2e as
well as 2c–2e bonds reacts with ammonia gas at a certain
temperature, gives a compound (Y), isostructural with
benzene. Compound (X) with ammonia at a high
temperature produces a substance (Z) :
Which of the following is/are correct statement?
(1) (X) is B H 2 6
160. Which of the following has the highest melting point
(1) Pb (2) Diamond
(3) Fe (4) Na
161. In the formation of a molecule by an atom
(1) Attractive forces operate
(2) Repulsive forces operate
(2) (Z) is known as inorganic graphite
(3) (Y) is B3N
3H
6
(4) All of these
168. An oxide of chlorine which is an odd electron molecule
is :
(1) ClO2
(2) Cl2O
6
(3) Both attractive and repulsive forces operate (3) Cl O (4) Cl O
(4) None of these 2 7 2
13
169. Which of the following does not act as lewis acid ?
(1) BF3
(2) SnCl4
(3) CCl4
(4) SF4
170. Boron compounds behave as Lewis acids because of
their –
(1) Acidic nature
(2) Covalent nature
(3) Electron defficient character
(4) Ionising property
Molecules do not exist
171. An element X forms compounds of formula XCl3, X2O5
and Mg3X2 but does not form XCl5 then X is :
(1) Aluminium (2) Phosphorus
(3) Nitrogen (4) Boron
172. The formation of which of the following ions is not
possible -
(1) [SiF6]2– (2) [AlF6]3– (3) [BF4]– (4) [BF6]3–
Ionic Bond
173. Which forms a crystal of NaCl
(1) NaCl molecules (2) Na+ and Cl¯ ions
(3) Na and Cl atoms (4) None of the above
174. When sodium and chlorine reacts then
(1) Energy is released and ionic bond is formed
(2) Energy is released and a covalent bond is formed
(3) Energy is absorbed and ionic bond is formed
(4) Energy is absorbed and covalent bond is formed
175. Lattice energy of alkali metal chlorides follows the
order
(1) LiCl > NaCl > KCl > RbCl > CsCl
(2) CsCl > NaCl > KCl > RbCl > LiCl
(3) LiCl > CsCl > NaCl > KCl > RbCl (4) NaCl > LiCl > KCl > RbCl > CsCl
178. Electrovalent compound’s
(1) Melting points are low
(2) Boiling points are low
(3) Conduct current in fused state
(4) Insoluble in polar solvent
178. A electrovalent compound is made up of
(1) Electrically charged molecules
(2) Neutral molecules
(3) Neutral atoms
(4) Electrically charged atoms or group of atoms
179. Electrovalent bond formation depends on
(1) Ionization energy
(2) Electron affinity
(3) Lattice energy
(4) All the three above
180. In the following which substance will have highest
boiling point
(1) He (2) CsF (3) NH 3 (4) CHCl 3
181. Which compound is highest covalent
(1) LiCl (2) LiF (3) LiBr (4) LiI
182. Which among the following elements has the tendency to
form covalent compounds
(1) Ba (2) Be (3) Mg (4) Ca
183. An atom of sodium loses one electron and chlorine
atom accepts one electron. This result the formation
of sodium chloride molecule. This type of molecule
will be
(1) Coordinate (2) Covalent
(3) Electrovalent (4) Matallic bond
184. Formula of a metallic oxide is MO. The formula of its
phosphate will be
176. The electronic configuration of four elements L, P, Q
and R are given in brackets
(1) M 2 (PO4 )2
(3) M 2PO4
(2) M (PO4 )
(4) M3 (PO4 )2
L (1s2 , 2s2 2 p 4 ); Q (1s2, 2s2 2 p6 , 3 s2 3 p5 )
P (1s2 , 2s2 2 p6 , 3 s1 ); R (1s2 , 2s2 2 p6 , 3 s2 ) 177. The formulae of ionic compounds that can be formed
between these elements are
(1) L2 P, RL, PQ and R2Q
(2) LP, RL, PQ and RQ
(3) P2L, RL, PQ and RQ2
(4) LP, R2 L, P2Q and RQ
185. An ionic bond A+ B− is most likely to be formed when:
(1) the ionization energy of A is high and the electron
gain enthalpy of B is low
(2) the ionization energy of A is low and the electron
gain enthalpy of B is high
(3) the ionization energy of A and the electron gain
enthalpy of B both are high
(4) the ionization energy of A and the electron gain
enthalpy of B both are low
14
186. The compound which has the highest Lattice energy is
(1) LiF (2) LiCl
(3) NaCl (4) MgO
187. Compound of a metal ‘M’ is M2O3. The formula of its
nitride will be:
(1) M3N (2) MN
(3) M3N2 (4) M2N3
188. Ionic reactions occur in :
(1) Aqueous solution and organic solvents of high
polarity
(2) Non-polar or solvents of low polarity
(3) Gaseous state
(4) Solid state
189. Correct order of covalent character of alkaline earth
metal chloride in:
(1) BeCl2 < MgCl2 < CaCl2 < SrCl2
(2) BeCl2 < CaCl2 < SrCl2 < MgCl2
(3) BeCl2 > MgCl2 > CaCl2 > SrCl2
(4) SrCl2 > BeCl2 > CaCl2 > MgCl2
190. From the following which group of elements easily
forms cation
195. If the electron pair forming a bond between two
atoms A and B is not in the centre, then the bond is
(1) Single bond (2) Polar bond
(3) Non-polar bond (4) π bond
196. Which of the compound is least soluble in water:
(1) AgF (2) AgCl
(3) AgBr (4) Agl
197. Among LiCl, BeCl2, BCl3 and CCl4, the covalent bond
character follows the order:
(1) LiCl < BeCl2 > BCl3 > CCl4
(2) LiCl > BCl3 < BeCl2 < CCl4
(3) LiCl < BeCl2 < BCl3 < CCl4
(4) LiCl > BeCl2 > BCl3 > CCl4
198. Polarization of ions is governed by -
(1) Hybridization (2) VSEPR theory
(3) Fajan's rules (4) Pauling rule
199.The magnitude of the lattice energy of a solid increases if:
(1) The ions are of large size
(2) The ions are of small size
(3) The ions are of equal size
(4) Charges on the ions are small
(1) F, Cl, Br
(3) O, S , Se
(2) Li, Na, K
(4) N , P, As
200. The boiling point of ICl is nearly 40°C higher than that
of Br2 although the two subtances have the same relative molecular mass. This is bacause:
191. Which type of compounds show high melting and
boiling points
(1) Electrovalent compounds
(2) Covalent compounds
(3) Coordinate compounds
(4) All the three types of compounds have equal
melting and boiling points
192. Lattice energy of an ionic compound depends upon
(1) Charge on the ion only
(2) Size of the ion only
(3) Packing of ions only
(4) Charge on the ion and size of the ion
193. In the given bonds which one is most ionic
(1) Cs – Cl (2) Al – Cl
(3) C – Cl (4) H – Cl
194. Element X is strongly electropositive and Y is strongly
electronegative. Both element are univalent, the
compounds formed from their combination will be
(1) X+Y¯ (2) X¯ Y+
(3) X – Y (4) X → Y
(1) ICl is ionic compound
(2) I-Cl bond is stronger than Br-Br bond
(3) ICl is polar covalent molecule while Br2 is non polar (4) Ionization energy IP of Iodine is less than that of Br
201. Which of the following liquids is not deflected by a
non-uniform electrostatic field
(1) Water (2) Chloroform
(3) Nitrobenzene (4) Hexane
202. Which of the following is non-polar
(1) H2S (2) NaCl
(3) Cl2
(4) H2SO
4
203. Polarization is the distortion of the shape of an anion
by an adjacently placed cation. Which of the following
statements is correct
(1) Maximum polarization is brought about by a cation
of high charge
(2) Minimum polarization is brought about by a cation
of low radius
(3) Alarge cation is likely to bring about a large degree
of polarization
(4) A small anion is likely to undergo a large degree
of polarization
15
2 2
2
2 2 2
2
2
2
O 2
2 2
2 2
2 2 2 2
204. The bonds between P atoms and Cl atoms in PCl 5
are likely to be
(1) Ionic with no covalent character
(2) Covalent with some ionic character
(3) Covalent with no ionic character
(4) Ionic with some metallic character
205. In which of the following molecule the covalent bond
is most polar
(1) HI (2) HBr (3) HCl (4) H2
206. The lattice energies of KF, KCl, KBr and KI follow
the order:
(1) KF > KCl > KBr > KI
(2) KI > KBr > KCl > KF
(3) KF > KCl > KI > KBr (4) KI > KBr > KF > KCl
213. Bond order is a concept in the molecular orbital theory.
It depends on the number of electrons in the bonding
and antibonding orbitals. Which of the following
statements is true about it ? The bond order
(1) Can have a negative quantity
(2) Has always an integral value
(3) Can have any positive or integral or fractional value
including zero
(4) Is a non zero quantity
214. The bond order of NO molecule is
(1) 1 (2) 2 (3) 2.5 (4) 3
215. In which of the following set, the value of bond order
will be 2.5: (1) O +, NO, NO+2, N +
2 2
207. The order of increasing lattice energy of the following
compound is:
(1) NaCl < CaO < NaBr < BaO
(2) NaBr < NaCl < BaO < CaO
(3) NaCl < NaBr < BaO < CaO
(4) NaBr < NaCl < CaO < BaO
208. Which of the follwing statements is true?
(1) HF is less polar than HBr
(2) Water does not contain any ions
(3) Chemical bond formation takes place when forces
of attraction overcome the forces of repulsion
(4) In covalent cond, transfer of electrons takes place
(2) CN, NO+2, CN–, F2
(3) O +, NO2+, O 2+, CN–
(4) O 2–, O –, O +, O
216. How many unpaired electrons are present in N + :
(1) 1 (2) 2 (3) 3 (4) 4
217. When two atomic orbitals combine they form
(1) One molecular orbital
(2) Two molecular orbital
(3) Three molecular orbital
(4) Four molecular orbital
218. Which of the following species is the least stable
209. Which of the following has a high polarising power (1) O2 (2) O −2 (3) O +1 (4) O −1
(1) Mg 2+
(3) Na +
(2) Al 3+
(4) Ca 2+
219. The bond order is maximum in
210. Maximum covalent character is associated with the
compound
(1) O2
(3) O +1
(2) O −1
(4) O −2
(1) NaI (2) MgI2 220. Which of the following compounds of boron does not
MOT
(3) AlCl 3 (4) AlI3 exist in the free form
(1) BCl 3
(2) BF3
211. Which of the following is the correct order of bond-
orders of the given species are such that -
(3) BBr3 (4) BH 3
(1) O – > O + > O 2– > O 221. The bond order of a molecule is given by 2 2 2 2
(2) O + > O > O – > O 2– (1) The difference between the number of electrons in 2 2 2 2
(3) O + > O 2– > O – > O bonding and antibonding orbitals 2 2 2 2
(4) O 2– > O > O + > O –
212. The number of antibonding electron pairs in 2−
molecular ion on the basis of molecular orbital theory
is (at no. O = 8):
(1) 2 (2) 3 (3) 4 (4) 5
(2)Total number of electrons in bonding
and antibonding orbitals
(2) Twice the difference between the number of
electrons in bonding and antibonding electrons
(3) Half the difference between the number of
electrons in bonding and antibonding electrons
16
2
2 2
2
2
2 2
2
2
222. Oxygen molecule is paramagnetic because
(1) Bonding electrons are more than antibonding
electrons
(2) Contains unpaired electrons
(3) Bonding electrons are less than antibonding
228. Which of the following molecule is paramagnetic
(1) Chlorine (2) Nitrogen
(3) Oxygen (4) Hydrogen
229. Which molecule has the highest bond order
electrons
(4) Bonding electrons are equal to antibonding
electrons
(1) N 2 (2) Li 2 (3) He 2 (4) O 2
230. The molecular electronic configuration of H − ion is
223. Which one is paramagnetic from the following
(1) O − (2) NO (1) (σ 1s)2
(2) (σ 1s)2 (σ x 1s)2
(3) Both (a) and (b) (4) CN − (3) (σ 1s)2 (σ x 1s)1 (4) (σ 1s)3
224. Out of the following which has smallest bond length
(1) O (2) O +
231. The bond order in NO is 2.5 while that in NO+ is 3.
Which of the following statements is true for these 2
(3) O −
2
(4) O 2−
two species?
(1) Bond length in NO+ is equal to that in NO
(2) Bond length in NO is greater than in NO+
225. Pick out the incorrect statement?
(1) N2 has greater dissociation energy than N +
(3) Bond length in NO+ is greater than in NO
(4) Bond length is unpredictable
(2) O2 has lower dissociation energy than O + 2
(3) Bond length in N + is less than N2
(4) Bond length in NO+ is less than in NO.
232. Which of the following molecules\ions does not
contain unpaired electrons?
(1) N+ (2) O2 (3) O2− (4) B2 226. Which of the following represents correctly the order
of filling of the molecular orbitals of B2, C2, N2
233. In which of the following ionizion processes, the bond
(1) π2px
(2) σ2pz
= π2py
< π2px
< σ2pz
= π2py
* 2py
* 2px
* 2pz
* 2py
* 2pz
* 2pz
order has increased and the magnetic behaviour has
changed
(1) NO → NO+ (2) O2 → O+ (3) N2 → N + (4) C → C+
(3) σ
π
2pz
2px
= π2px
< π2py
= π2py
< σ2pz
* 2px
* 2py
* 2py
* 2pz
* 2pz
* 2pz
2 2 2
234.Which one of the following pairs of species
have the same bond order :
(1) CN– and NO+ (2) CN– and CN+
227. Which one of the following pairs of molecules will
have permanent dipole moments for both members:
(1) NO2 and CO2 (2) NO2 and O3
(3) SiF4 and CO2 (4) SiF4 and NO2
(3) O – and CN– (4) NO+ and CN+
2
< π = π < σ
< π =< π < σ
< π =< π < σ
> π < π = σ
17
NEET CHEMISTRY MCQ -230 ANSWERSHEET
Q.1 (4) Q.2 (4) Q.3 (3) Q.4 (3) Q.5 (2) Q.6 (3) Q.7 (1) Q.8 (2) Q.9 (3) Q.10 (2)
Q.11 (3) Q.12 (4) Q.13 (3) Q.14 (1) Q.15 (3) Q.16 (3) Q.17 (2) Q.18 (3) Q.19 (3) Q.20 (4)
Q.21 (2) Q.22 (3) Q.23 (4) Q.24 (3) Q.25 (2) Q.26 (1) Q.27 (1) Q.28 (4) Q.29 (3) Q.30 (1)
Q.31 (1) Q.32 (2) Q.33 (3) Q.34 (4) Q.35 (1) Q.36 (4) Q.37 (3) Q.38 (3) Q.39 (2) Q.40 (4)
Q.41 (3) Q.42 (4) Q.43 (3) Q.44 (1) Q.45 (1) Q.46 (2) Q.47 (2) Q.48 (3) Q.49 (3) Q.50 (2)
Q.51 (4) Q.52 (2) Q.53 (1) Q.54 (2) Q.55 (3) Q.56 (1) Q.57 (1) Q.58 (4) Q.59 (4) Q.60 (4)
Q.61 (1) Q.62 (2) Q.63 (3) Q.64 (3) Q.65 (3) Q.66 (2) Q.67 (3) Q.68 (4) Q.69 (3) Q.70 (4)
Q.71 (3) Q.72 (3) Q.73 (3) Q.74 (2) Q.75 (4) Q.76 (4) Q.77 (4) Q.78 (1) Q.79 (4) Q.80 (4)
Q.81 (2) Q.82 (3) Q.83 (1) Q.84 (1) Q.85 (3) Q.86 (1) Q.87 (4) Q.88 (2) Q.89 (2) Q.90 (2)
Q.91 (2) Q.92 (4) Q.93 (1) Q.94 (3) Q.95 (2) Q.96 (2) Q.97 (3) Q.98 (1) Q.99 (2) Q.100 (3)
Q.101 (3) Q.102 (4) Q.103 (3) Q.104 (2) Q.105 (1) Q.106 (3) Q.107 (1) Q.108 (1) Q.109 (1) Q.110 (3)
Q.111 (3) Q.112 (4) Q.113 (2) Q.114 (2) Q.115 (4) Q.116 (4) Q.117 (1) Q.118 (2) Q.119 (3) Q.120 (1)
Q.121 (1) Q.122 (3) Q.123 (2) Q.124 (1) Q.125 (1) Q.126 (4) Q.127 (2) Q.128 (4) Q.129 (2) Q.130 (1)
Q.131 (3) Q.132 (4) Q.133 (3) Q.134 (2) Q.135 (2) Q.136 (1) Q.137 (3) Q.138 (4) Q.139 (3) Q.140 (1)
Q.141 (2) Q.142 (3) Q.143 (1) Q.144 (3) Q.145 (1) Q.146 (4) Q.147 (3) Q.148 (3) Q.149 (4) Q.150 (2)
Q.151 (2) Q.152 (2) Q.153 (1) Q.154 (2) Q.155 (4) Q.156 (3) Q.157 (4) Q.158 (4) Q.159 (2) Q.160 (2)
Q.161 (3) Q.162 (4) Q.163 (4) Q.164 (3) Q.165 (1) Q.166 (4) Q.167 (4) Q.168 (1) Q.169 (3) Q.170 (3)
Q.171 (3) Q.172 (4) Q.173 (2) Q.174 (1) Q.175 (1) Q.176 (3) Q.177 (3) Q.178 (4) Q.179 (4) Q.180 (2)
Q.181 (4) Q.182 (2) Q.183 (3) Q.184 (4) Q.185 (2) Q.186 (4) Q.187 (2) Q.188 (1) Q.189 (3) Q.190 (2)
Q.191 (1) Q.192 (4) Q.193 (1) Q.194 (1) Q.195 (2) Q.196 (4) Q.197 (3) Q.198 (3) Q.199 (2) Q.200 (3)
Q.201 (4) Q.202 (3) Q.203 (1) Q.204 (2) Q.205 (3) Q.206 (1) Q.207 (2) Q.208 (3) Q.209 (2) Q.210 (4)
Q.211 (2) Q.212 (3) Q.213 (3) Q.214 (3) Q.215 (1) Q.216 (1) Q.217 (2) Q.218 (2) Q.219 (3) Q.220 (4)
Q.221 (4) Q.231 (2)
Q.222 (2) Q.232 (3)
Q.223 (3) Q.233 (1)
Q.224 (2) Q.234 (1)
Q.225 (3) Q.226 (1) Q.227 (2) Q.228 (3) Q.229 (1) Q.230 (3)
