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Chemistry
Chemical Bonding
238 questions · Click an option and press Check Answer to reveal the result
1
Which of the following is a planar species?
A
ClO3–
B
CO32–
C
AsO33–
D
SO32–
2
In a triple bond there is sharing of:
A
3 electrons
B
4 electrons
C
Several electrons
D
6 electrons
3
A sp³ hybrid orbital contains:
A
3/4 s-character
B
1/4 p-character
C
3/4 p-character
D
1/2 s-character
4
In the protonation of H₂O, change occurs in :
A
Hybridisation state of oxygen
B
Shape of molecule
C
Hybridisation and shape both
D
None
5
Correct order of polarising power is:
A
Cs⁺ < K⁺ < Mg²⁺ < Al³⁺
B
Al³⁺ < Mg²⁺ < K⁺ < Cs⁺
C
Mg⁺ < Al³⁺ < K⁺ < Cs⁺
D
K⁺ < Cs⁺ < Mg²⁺ < Al³⁺
6
Match List - I with List - II according to shape.
Choose the correct answer from the options given below
A
A-II, B-I, C-III, D-IV
B
A-II, B-III, C-I, D-IV
C
A-II, B-III, C-IV, D-I
D
A-III, B-II, C-IV, D-I
7
Most favourable conditions for electrovalent bonding are:
A
Low ionisation potential of one atom and high electron affinity of the other atom
B
High electron affinity and high ionisation potential of both the atoms
C
low electron affinity and low ionisation potential of both the atoms
D
High ionisation potential of one atom and low electrons affinity of the other atom
8
Among the following, covalent bond length is minimum for:
A
C – C
B
C – H
C
C – N
D
C = O
9
The lattice energies of KF, KCl, KBr and KI follow the order:
A
KF > KCl > KBr > KI
B
KI > KBr > KCl > KF
C
KF > KCl > KI > KBr
D
KI > KBr > KF > KCl
10
Which of the set of species have same hybridisation state but different shapes:
A
NO₂⁺, NO₂, NO₂⁻
B
ClO₄⁻, SF₄, XeF₄
C
NH₄⁺, H₃O⁺, OF₂
D
SO₄²⁻, PO₄³⁻, ClO₄⁻
11
Which of the following species will have the minimum bond energy:
A
N₂
B
N₂⁻
C
N₂⁺
D
N₂²⁻
12
The correct order of dipole moment is:
A
CH₄ < NF₃ < NH₃ < H₂O
B
NF₃ < CH₄ < NH₃ < H₂O
C
NH₃ < NF₃ < CH₄ < H₂O
D
H₂O < NH₃ < NF₃ < CH₄
13
A covalent bond is possible between:
A
Similar atoms
B
Dissimilar atoms
C
Similar and dissimilar atoms
D
Similar molecules
14
H₂O boils at higher temperature than H₂S, because it is capable of forming:
A
Ionic bonds
B
Covalent bonds
C
Hydrogen bonds
D
Metallic bonds
15
Which of the following statements is not correct?
A
Double bonds is shorter than a single bond
B
σ-bond is weaker than π bond
C
Double bond is stronger than a single bond
D
Covalent bond is stronger than a hydrogen bond
16
Which set of molecules is polar:
A
XeF₄, IF₇, SO₃
B
PCl₅, C₆H₆, SF₆
C
SnCl₂, SO₂, NO₂
D
CO₂, CS₂, C₂H₆
17
The bond order of CO molecule on the basis of molecular orbital theory is:
A
Zero
B
2
C
3
D
1
18
Match List-I with List-II. List-I List-II A. NH4+ I. Octahedral B. BF3 II. Tetrahedral C. HgCl2 III. Trigonal planar D. SF6 IV. Linear Choose the correct answer from the options given below:
A
A-III, B-II, C-IV, D-I
B
A-I, B-II, C-III, D-IV
C
A-II, B-III, C-IV, D-I
D
A-II, B-III, C-I, D-IV
19
Dipole moment is shown by :
A
1, 4-Dichlorobenzene
B
Cis 1, 2-dichloro ethene
C
Trans-1, 2-dichloro ethene
D
Benzene
20
The strength of bonds by 2s – 2s, 2p – 2p and 2p – 2s overlapping has the order:
A
s – s > p – p > s – p
B
s – s > s – p > p – p
C
p – p > s – p > s – s
D
p – p > s – s > s – p
21
What conclusion can be draw from the fact that BF₃ has no dipole moment but PF₃ does:
A
BF₃ is not symmetrical but PF₃ is symmetrical
B
BF₃ molecule must be linear
C
Atomic radius of P is larger than that of B
D
BF₃ molecule must be planar triangular
22
In terms of polar character, which of the following order is correct:
A
NH₃ < H₂O < HF < H₂S
B
H₂S < NH₃ < H₂O < HF
C
H₂O < NH₃ < H₂S < HF
D
HF < H₂O < NH₃ < H₂S
23
N2 and O2 are converted into monocations, N2+ and O2+ respectively. Which of the following statement is wrong?
A
In N2+, N–N bond weakens
B
In O2+, the O–O bond order increases
C
O2+ is paramagnetic
D
N2+ is diamagnetic
24
The type of bond formed between two electronegative atoms would be:
A
Covalent
B
Ionic
C
Metallic
D
All the above
25
Choose the molecules in which hybridisation occurs in the ground state: (1) BCl₃ (2) NH₃ (3) PCl₃ (4) BeF₂ The correct answer is:
A
1, 2, 4
B
1, 2, 3
C
2, 3
D
3, 4
26
What is not true about resonance:
A
The resonating structures are hypothetical
B
The unpaired electrons in various resonating structures are same
C
Hybrid structure is least stable
D
Hybrid structure is least energetic
27
Which of the following species are polar: (1) C₆H₆ (2) XeF₂ (3) SO₂ (4) SF₄ (5) SF₆ correct answer is:
A
(2) & (4)
B
(1), (2) & (5)
C
(1) & (5)
D
(3) & (4)
28
Which of the following statement is not correct -
A
CH₃⁺ shows sp²-hybridisation where as CH₃⁻ shows sp³-hybridisation
B
NH₄⁺ has a regular tetrahedral geometry
C
sp²-hybridised orbitals have equal s and p character
D
Hybridisation orbitals always form σ-bonds
29
In which compound coordinate bond is present:
A
NH₃
B
NH₄OH
C
H₂O
D
HCl
30
Which of the following elements can not exhibit sp³d hybridisation state: (1) C (2) P (3) Cl (4) B Correct answer is:
A
1, 3
B
1, 4
C
2, 3
D
2, 4
31
Which of the following having a square planner structure is:
A
NH₄⁺
B
BF₄⁻
C
XeF₄
D
CCl₄
32
Correct order of covalent character of alkaline earth metal chloride in:
A
BeCl₂ < MgCl₂ < CaCl₂ < SrCl₂
B
BeCl₂ < CaCl₂ < SrCl₂ < MgCl₂
C
BeCl₂ > MgCl₂ > CaCl₂ > SrCl₂
D
SrCl₂ > BeCl₂ > CaCl₂ > MgCl₂
33
Statement-1 : Dipole moment of NF3 is less than that of NH3.
Statement-II : Polarity of N – F bond is less than that of N – H bond.
A
Statement-1 is true, statement-II is true and statement-II is correct explanation for statement-1.
B
Statement-1 is true, statement-II is true but statement-II is NOT the correct explanation for statement-1.
C
Statement-1 is true, statement-II is false.
D
Statement-1 is false, statement-II is true.
34
Which carbon is more electronegative:
A
sp³ hybridised carbon
B
sp hybridised carbon
C
sp² hybridised carbon
D
The electron attracting power of C is always same irrespective of its hybrid state
35
In which of the following pair the boiling point of first compound is not more than the second :
A
KCl, Cl₂
B
Ne, He
C
PH₃, AsH₃
D
HF, HCl
36
In SO42–, bond order of S–O is:
A
1.5
B
2
C
1.33
D
2.5
37
Assertion :- B2 is paramagnetic molecule.
Reason :- It has two unpaired electrons in π2p MO.
A
If both Assertion & Reason are True & Reason is a correct explanation of the Assertion.
B
If both Assertion & Reason are True but Reason is not a correct explanation of Assertion.
C
If Assertion is True but the Reason is False.
D
If both Assertion and Reason are False.
38
The bond-orders of the given species are such that -
A
O₂⁻ > O₂⁺ > O₂²⁻ > O₂
B
O₂⁺ > O₂ > O₂⁻ > O₂²⁻
C
O₂⁺ > O₂²⁻ > O₂⁻ > O₂
D
O₂²⁻ > O₂ > O₂⁺ > O₂⁻
39
Hydrogen bonding is different than the other three is shown by -
A
Aceto-acetic ester
B
Acetic acid
C
Ethyl alcohol
D
Ethyl amine
40
The shape of sulphate ion is:
A
Hexagonal
B
Square planar
C
Trigonal bipyramidal
D
Tetrahedral
41
The bond order of a molecule is given by:
A
the total number of electrons in bonding and antibonding orbitals.
B
the difference between the number of electrons in bonding and antibonding orbitals.
C
twice the difference between the number of electrons in bonding and antibonding orbitals.
D
half the difference between the number of electrons in bonding and antibonding orbitals.
42
The order of increasing bond length in F₂, N₂, Cl₂ and O₂ is:
A
N₂ < O₂ < Cl₂ < F₂
B
N₂ < O₂ < F₂ < Cl₂
C
O₂ < N₂ < Cl₂ < F₂
D
N₂ < Cl₂ < O₂ < F₂
43
Given below are two statements: Statements I: XeO3 is a planar molecule. Statements II: XeO3 is sp3 hybridised. In the light of the above statements, choose the most appropriate answer from the options given below:
A
Statement I is correct but Statement II is incorrect.
B
Statement I is incorrect but Statement II is correct.
C
Both Statement I and Statement II are correct.
D
Both Statement I and Statement II are incorrect.
44
Calcium reacts with an element (X) to form an ionic compound. If the ground state electronic configuration of (X) is 1s2 2s2 2p5 , the simplest formula for this compound is;
A
Ca2X3
B
CaX2
C
Ca2X
D
Ca3X2
45
The d-orbitals involved in sp³d hybridisation is :
A
d(x²−y²)
B
d(z²)
C
dxy
D
dxz
46
A sigma bond is formed by the overlapping of:
A
s-s orbital alone
B
s and p orbitals alone
C
s-s, s-p or p-p orbitals along internuclear axis
D
p-p orbital along the sides
47
Fluorine does not form any polyhalide as other halogens because:
A
It has maximum ionic character
B
It has low F-F bond energy (38.5 kcal mol⁻¹)
C
Of the absence of d-orbitals in the valence shell of fluorine
D
It brings about maximum coordination number in other elements
48
Which of the following statements regarding covalent bond is not true?
A
The electrons are shared between atoms
B
The bond is non-directional
C
The strength of the bond depends upon the extent of overlapping
D
The bond formed may or may not be polar
49
Choose the incorrect match.
A
HI – Linear
B
CCl4 – Tetrahedral
C
H2 – Bent
D
CO2 – Linear
50
The geometrical arrangement and shape of I₃⁻ are respectively:
A
Trigonal bipyramidal geometry, linear shape
B
Hexagonal geometry, T-shape
C
Triangular planar geometry, triangular shape
D
Tetrahedral geometry, pyramidal shape
51
Which of the following is not isostructural with SiCl4?
A
NH4+
B
SCl4
C
SO42–
D
PO43–
52
Which of the following is not a characteristic of a covalent compound:
A
It has low melting point and boiling point
B
It is formed between two atoms having not very small electronegativity difference
C
They have no definite geometry
D
They are generally insoluble in water
53
Maximum number of hydrogen bonds formed by a water molecule in ice are:
A
4
B
3
C
2
D
1
54
Identify the correct statement from the given alternatives:
A
Intra molecular hydrogen bonding is not found to occur in 2 hydroxy benzaldehyde
B
The boiling point of hydrogen iodide (HI) is more than hydrogen fluoride (HF)
C
The dipole moment of CH₃Cl is not equal to zero
D
CH₃F has a larger dipole moment that CH₃Cl
55
Which condition favours the bond formation:
A
Maximum attraction and maximum potential energy
B
Minimum attraction and minimum potential energy
C
Minimum potential energy and maximum attraction
D
None of the above
56
Three diatomic species are listed below in different sequences. Which of these presents the correct order of their increasing bond order?
A
C2 < He2 < NO
B
He2 < NO < C2
C
NO < C2 < He2
D
NO < He2 < C2
57
The hybrid state of B in BF₄⁻ is :
A
sp²
B
sp
C
sp³
D
No specific
58
Which overlapping is involved in HCl molecule:
A
s-s overlap
B
p-p overlap
C
s-d overlap
D
s-p overlap
59
The correct order of volatility is :
A
NH₃ < H₂O
B
p-nitro phenol < o-nitro phenol
C
CH₃OH > CH₃–O–CH₃
D
HF > HCl
60
In the following which of the two are paramagnetic: (1) N₂ (2) CO (3) B₂ (4) NO₂ correct answer is:
A
(1) & (3)
B
(2) & (3)
C
(3) & (4)
D
(2) & (4)
61
The order of increasing lattice energy of the following compound is:
A
NaCl < CaO < NaBr < BaO
B
NaBr < NaCl < BaO < CaO
C
NaCl < NaBr < BaO < CaO
D
NaBr < NaCl < CaO < BaO
62
The hybridization of N in N(SiH₃)₃ and the shape of N(SiH₃)₃ respectively are
A
sp² and bent
B
sp² and planar
C
sp³ and pyramidal
D
sp³ and tetrahedral
63
Intramolecular H-bonding is present in :
A
o-Nitrophenol
B
Salicylaldehyde
C
m-Nitrophenol
D
Both (A) and (B)
64
The correct order of increasing bond angles in the following triatomic species is;
A
NO2+ < NO2 < NO2–
B
NO2+ < NO2– < NO2
C
NO2– < NO2+ < NO2
D
NO2– < NO2 < NO2+
65
Select correct statement about hydrolysis of BCl₃ and NCl₃:
A
NCl₃ is hydrolysed and gives HClO but BCl₃ is not hydrolysed
B
Both NCl₃ and BCl₃ on hydrolysis gives HCl
C
NCl₃ on hydrolysis gives HClO but BCl₃ gives HCl
D
Both NCl₃ and BCl₃ on hydrolysis gives HOCl
66
Among LiCl, BeCl₂, BCl₃ and CCl₄, the covalent bond character follows the order:
A
LiCl < BeCl₂ > BCl₃ > CCl₄
B
LiCl > BeCl₂ < BCl₃ < CCl₄
C
LiCl < BeCl₂ < BCl₃ < CCl₄
D
LiCl > BeCl₂ > BCl₃ > CCl₄
67
The bond angle in H₂O is nearly 105° whereas bond angle in H₂S is nearly 90°. This is because:
A
Electronegativity of oxygen is greater than that of sulphur
B
Oxygen is a gas whereas sulphur is solid
C
Sulphur contains d-orbitals whereas oxygen does not
D
The number of lone pairs present on oxygen and sulphur is not equal
68
The Cl–C–Cl angle in 1,1,2,2-tetrachloroethene and tetrachloro methane respectively will be about:
A
120° and 109.5°
B
90° and 109.5°
C
109.5° and 90°
D
109.5° and 120°
69
Which of the following is correct molecular orbital representation of 2px-molecular orbital?
A
(1)
B
(2)
C
(3)
D
(4)
70
Which of the following has zero value of dipole moment:
A
Benzene
B
Naphthalene
C
p-dichlorobenzene
D
All the three
71
Which of the following species contains three bond pairs and one lone pair around the central atom?
A
NH2–
B
PCl3
C
H2O
D
BF3
72
Lattice enthalpy of an ionic compound depends upon;
A
Only charge on the ions
B
Only size of the ions
C
Only packing of the ions
D
Both charge and size of the ions
73
Identify which of the following has a see-saw shape?
A
CH4
B
CHCl3
C
PO43–
D
SF4
74
Weakest hydrogen bond is:
A
O–H .....N
B
S–H .....S
C
F–H .....F
D
N–H .....N
75
The combination of atoms occur because they want :
A
To decrease number of electrons in the outer most orbit
B
To attain an inert gas configuration
C
To increase number of electrons in the outer most orbit
D
To attain 18 electrons in the outermost orbit
76
Which of the following statements is correct :
A
HCl is covalent both in aqueous solution and in the gaseous state
B
HCl is covalent in the gaseous state but ionic in aqueous solution
C
HCl is ionic both in the gaseous state and in aqueous solution
D
None of the above
77
The shape of I₃⁻ is :
A
Tetrahedral
B
Linear
C
T-shape
D
Trigonal
78
Among CaH2, BeH2, BaH2, the order of ionic character is;
A
BeH2 > CaH2 > BaH2
B
CaH2 > BeH2 > BaH2
C
BeH2 > BaH2 > CaH2
D
BaH2 > BeH2 > CaH2
79
In the compound CH₂=CH–CH₂–CH₂–C≡CH, the C₂–C₃ bond formed by the overlapping of :
A
sp – sp²
B
sp³ – sp³
C
sp – sp³
D
sp² – sp³
80
Which of the following has strongest intra molecular hydrogen bonding:
A
(structure A)
B
(structure B)
C
(structure C)
D
(structure D)
81
Which is most ionic:
A
P₂O₅
B
MnO
C
CrO₃
D
Mn₂O₇
82
Predict the correct order of repulsion among the following;
A
lone pair – lone pair > lone pair – bond pair > bond pair – bond pair
B
lone pair – lone pair > bond pair – bond pair > lone pair – bond pair
C
bond pair – bond pair > lone pair – bond pair > lone pair – lone pair
D
lone pair – bond pair > bond pair – bond pair > lone pair – lone pair
83
Which of the following molecule have zero dipole moment:
A
BF₃
B
CH₂Cl₂
C
NF₃
D
SO₂
84
Which of the following is paramagnetic:
A
O₂⁻
B
CN⁻
C
CO
D
NO⁺
85
Shape of H2S is:
A
Linear
B
Trigonal pyramidal
C
Trigonal planar
D
Bent
86
The boiling point of a compound is raised by:
A
intermolecular hydrogen bonding
B
high volatility
C
intramolecular hydrogen bonding
D
non-polarity
87
Out of XeF₆, CH₄ and SF₄ the molecules having regular geometry are:
A
XeF₆ only
B
XeF₆ and SF₄
C
CH₄ only
D
CH₄ and SF₄
88
Density of ice is less than that of water because of :
A
presence of hydrogen bonding
B
crystal modification of ice
C
open porous structure of ice due to hydrogen bonding
D
different physical states of these
89
The phosphate of a metal has the formula MHPO₄. The formula of its chloride would be:
A
MCl
B
MCl₂
C
MCl₃
D
M₂Cl₃
90
The correct order of bond length is -
A
C–C < C=C < C≡C
B
C≡C < C=C < C–C
C
C=C < C≡C < C–C
D
C=C < C–C < C≡C
91
Which of the following statements is wrong:
A
Hybridisation is the mixing of atomic orbitals prior to their combining into molecular orbitals
B
sp² hybrid orbital are formed from two p atomic orbitals and one s atomic orbital
C
dsp² hybrid orbitals are all at 90° to one another
D
sp³d² hybrid orbitals are directed towards the corners of a regular tetrahedron
92
The correct statement for the reaction NH₃ + H⁺ → NH₄⁺
A
Hybridisation state is changed
B
Bond angle increases
C
NH₃ act as a Lewis acid
D
Regular geometry is changed
93
Which of the following compounds show intramolecular hydrogen bonding: (1) o-nitrophenol (2) p-nitrophenol (3) phenol (4) salicyl aldehyde
A
1 & 2
B
1 & 3
C
1 & 4
D
2 & 3
94
In which of the following species the angle around the central atom is exactly equal to 109°28′ :
A
SF₄
B
NH₃
C
NH₄⁺
D
None of the above
95
Correct Lewis representation of O3 molecule is;
A
(1)
B
(2)
C
(3)
D
(4)
96
Which is not characteristic of π-bond:
A
π-bond is formed when a sigma bond already formed
B
π-bond are formed from hybrid orbitals
C
π-bond may be formed by the overlapping of p-orbitals
D
π-bond results from lateral overlap of atomic orbital
97
In the electronic structure of acetic acid the number of electrons present are:
A
16 shared and 8 unshared
B
8 shared and 16 unshared
C
12 shared and 12 unshared
D
18 shared and 6 unshared
98
Given below are two statements: Statements I: AlCl3 is sp2 hybridised. Statements II: AlCl4– is sp3 hybridised. In the light of the above statements, choose the most appropriate answer from the options given below:
A
Statement I is correct but Statement II is incorrect.
B
Statement I is incorrect but Statement II is correct.
C
Both Statement I and Statement II are correct.
D
Both Statement I and Statement II are incorrect.
99
Which of the following has least polarity in bond?
A
H–F
B
H–Cl
C
H–O
D
H–S
100
The hybridization state of the central atom in I3– is;
A
sp2
B
sp3 d
C
sp3
D
sp3 d2
101
The formation of which of the following ions is not possible -
A
[SiF₆]²⁻
B
[AlF₆]³⁻
C
[BF₄]⁻
D
[BF₆]³⁻
102
Which of the following does not apply to metallic bond:
A
Overlapping valence orbital
B
Mobile valency electron
C
Delocalized electrons
D
None
103
The number of antibonding electron pairs in O₂²⁻ molecular ion on the basis of molecular orbital theory is (at no. O = 8):
A
2
B
3
C
4
D
5
104
Which of the following has fractional bond order?
A
O₂²⁺
B
O₂²⁻
C
F₂²⁻
D
H₂
105
Consider the molecules CH4, NH3 and H2O. Which of the given statements is false?
A
The H–C–H bond angle in CH4, the H–N–H bond angle in NH3 and the H–O–H bond angle in H2O are all greater than 90°.
B
The H–O–H bond angle in H2O is larger than the H–C–H bond angle in CH4.
C
The H–O–H bond angle in H2O is smaller than the H–N–H bond angle in NH3.
D
The H–C–H bond angle in CH4 is larger than the H–N–H bond angle in NH3.
106
Which of the following has maximum bond strength -
A
O₂
B
O₂⁺
C
O₂⁻
D
O₂²⁻
107
Intra molecular H-bond:
A
Decreases Volatility
B
Increases melting point
C
Increases viscosity
D
Increases vapour pressure
108
BeF₂ has zero dipole moment whereas H₂O has dipole moment because:
A
Water is linear
B
H₂O is bent
C
F is more electronegative than O
D
Hydrogen bonding is present in H₂O
109
Increasing order of bond length in NO, NO⁺ and NO⁻ is:
A
NO > NO⁻ > NO⁺
B
NO⁺ < NO < NO⁻
C
NO < NO⁺ < NO⁻
D
NO < NO⁺ = NO⁻
110
Maximum no. of hydrogen bonds formed by a water molecule in ice is:
A
4
B
3
C
2
D
1
111
The value of bond order in NO⁺ according to MOT is:
A
3
B
2
C
1
D
0
112
The correct increasing order of extent of hydrolysis is :
A
CCl₄ < MgCl₂ < AlCl₃ < SiCl₄ < PCl₅
B
CCl₄ < AlCl₃ < MgCl₂ < PCl₅ < SiCl₄
C
CCl₄ < SiCl₄ < PCl₅ < AlCl₃ < MgCl₂
D
CCl₄ < PCl₅ < SiCl₄ < AlCl₃ < MgCl₂
113
The M.P. of SnCl₄ is less than of SnCl₂, the suitable reason for the observed fact is:
A
There is more charge on Sn⁴⁺
B
The size of Sn⁴⁺ is small
C
Ionic potential (ϕ) of Sn⁴⁺ is high
D
The shape of SnCl₄ is tetrahedral
114
In a change from PCl₃ → PCl₅, The hybrid state of P change from:
A
sp² to sp³
B
sp³ to sp²
C
sp³ to sp³d
D
sp³ to dsp²
115
Number of valence electrons present in atoms of HClO₄, HClO₃, HClO₂ respectively are:
A
32, 26, 20
B
26, 20, 14
C
36, 30, 24
D
28, 22, 16
116
The bond angle in H₂O molecule is less than that of NH₃ molecule because:
A
The hybridisation of O in H₂O and N in NH₃ is different
B
The atomic radii of N and O are different
C
There is one lone pair of electrons on O and two lone pairs of electrons on N
D
There are two lone pairs of electrons on O and one lone pairs of electrons on N
117
Which of the given compounds contain ionic bond, covalent bond as well as co-ordinate bond?
A
Na2CO3
B
NaCl
C
NH4Cl
D
HCN
118
Consider the following statements. (A) PCl5 has an expanded octet. (B) PCl5 is a reactive molecule. (C) PCl5 is sp3 d hybridised. The correct statement(s) is/are:
A
Only A
B
Only C
C
Only A and B
D
A, B and C
119
The ratio σ bond π bond in tetracyano ethylene:
A
2 : 1
B
1 : 1
C
1 : 2
D
None of these
120
Identify which of the following has T-shape.
A
BrF5
B
XeF4
C
ClF3
D
H2O
121
The boiling point of methanol is greater than methyl thiol because:
A
There is intramolecular hydrogen bonding in methanol and intermolecular hydrogen bonding in methyl thiol
B
There is intermolecular hydrogen hydrogen bonding in methanol and no hydrogen bonding in methyl thiol
C
There is no hydrogen bonding in methanol and intermolecular hydrogen bonding in methyl thiol
D
There is intramolecular hydrogen bonding in methanol and no hydrogen bonding in methyl thiol
122
The pair of compounds which can form a co-ordinate bond is:
A
(C₂H₅)₃B and (CH₃)₃N
B
HCl and HBr
C
BF₃ and NH₃
D
(A) and (C) both
123
Which one of the following molecules has highest dipole moment:
A
H₂S
B
CO₂
C
CCl₄
D
BF₃
124
Given below are two statements.
Statement I: O₂⁺, O₂, O₂⁻ and O₂²⁻ are paramagnetic in nature with bond order 2.5, 2, 1.5 and 1 respectively.
Statement II: The lowest unoccupied molecular orbital (LUMO) for O₂ is σ*2pz.
In the light of above statements, choose the most appropriate answer from the options given below.
A
Statement I is correct but statement II is incorrect
B
Statement I is incorrect but statement II is correct
C
Both Statement I and statement II are correct
D
Both Statement I and statement II are incorrect
125
The hybridization of atomic orbitals of nitrogen in , and are
A
sp2, sp3 and sp2 respectively
B
sp, sp2 and sp3 respectively
C
sp2, sp and sp3 respectively
D
sp2, sp3 and sp respectively
126
In which of the following set, the value of bond order will be 2.5:
A
O₂⁺, NO, NO²⁺, CN
B
CN, NO²⁺, CN⁻, F₂
C
O₂⁺, NO²⁺, O₂²⁺, CN⁻
D
O₂²⁻, O₂⁻, O₂⁺, O₂
127
The type of hybrid orbitals used by chlorine atom in ClO⁻, ClO₂⁻, ClO₃⁻ and ClO₄⁻ is/are:
A
sp, sp², sp³ and sp³d
B
sp and sp³
C
Only sp³
D
Only sp
128
The hybridization of phosphorous in POCl₃ is the same as in:
A
P in PCl₃
B
S in SF₄
C
Cl in ClF₃
D
B in BCl₃
129
The correct decreasing order of lattice energy is;
A
KF KCl KBr KI
B
KCl KF KBr KI
C
KBr KCl KF KI
D
KI KBr KCl KF
130
Which of the following option w.r.t. increasing bond order is correct?
A
NO < C₂ < O₂⁻ < He₂⁺
B
C₂ < NO < He₂⁺ < O₂⁻
C
He₂⁺ < O₂⁻ < NO < C₂
D
He₂⁺ < O₂⁻ < C₂ < NO
131
Which of the following fluorides does not exists?
A
NF₅
B
PF₅
C
AsF₅
D
SbF₅
132
The bonds present in N₂O₅ are:
A
Only ionic
B
Covalent & coordinate
C
Only covalent
D
Covalent & ionic
133
In PO43–, the formal charge on each oxygen atom and the P–O bond order, respectively are;
A
–0.75 and 0.6
B
–0.75 and 1.0
C
–0.75 and 1.25
D
–3 and 1.25
134
The correct sequence of increasing covalent character is represented by:
A
BeCl₂ < NaCl < LiCl
B
NaCl < LiCl < BeCl₂
C
BeCl₂ < LiCl < NaCl
D
LiCl < NaCl < BeCl₂
135
The pair of molecules having identical geometry is:
A
BCl₃, PCl₃
B
BF₃, NF₃
C
CCl₄, CH₄
D
CH₄, SF₄
136
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 which of periodic table which of the following is/are diatomic at room temperature:
A
Only C₂
B
Only A₂
C
C₂ and D₂
D
Only B₂
137
Out of the two compounds shown below, the vapour pressure of (2) at a particular temperature is expected to be:
A
Higher than that of (1)
B
Lower than that of (1)
C
Same as that of (1)
D
Can be higher or lower depending upon the size of the vessel
138
Which of the following has the highest bond order?
A
O2+
B
O2
C
O2–
D
O22–
139
Molecular shapes of CF4 and XeF4 are;
A
The same, with 0 and 1 lone pair of electrons respectively.
B
The same, with 1 and 1 lone pair of electrons respectively.
C
Different, with 1 and 2 lone pair of electrons respectively.
D
Different, with 0 and 2 lone pair of electrons respectively.
140
The high boiling point of water is due to the presence of:
A
Dative bond
B
Covalent bond
C
Hydrogen bond
D
Vander waals bond
141
In which of the following molecules S atom does not assume sp³ hybridisation:
A
SO₄²⁻
B
SF₄
C
SF₂
D
S₈
142
The compound formed by which of the following pair of ions will have lowest melting point :
A
Na⁺ and Cl⁻
B
Mg²⁺ and Cl⁻
C
Al³⁺ and Cl⁻
D
Sn⁴⁺ and Cl⁻
143
In which case hydrogen bond will not be observed -
A
H₃O₂⁻
B
H₂O
C
HF
D
H₃O⁺
144
According to Fajan’s rules necessary condition to form covalent bond is:
A
small cation and large anion
B
small cation and small anion
C
large cation and large anion
D
large cation and small anion
145
The electronegativity of cesium is 0.7 and fluorine is 4.0. The bond formed between the two is:
A
Covalent
B
Electrovalent/ionic
C
Coordinate
D
Metallic
146
XeF2 is isostructural with:-
A
BeCl2
B
CCl4
C
ICl2–
D
SbCl3
147
When two atoms combine to form a molecules:
A
Energy is released
B
Energy is absorbed
C
Energy is neither released nor absorbed
D
Energy may either released or absorbed
148
The ratio of σ to p bonds in mesitylene is
A
3
B
7
C
5
D
6
149
Amongst NH₃, BeCl₂, CO₂ and H₂O, the non-linear molecules are :
A
BeCl₂ and H₂O
B
BeCl₂ and CO₂
C
NH₃ and H₂O
D
NH₃ and CO₂
150
Ionic reactions occur in :
A
Aqueous solution and organic solvents of high polarity
B
Non-polar solvents of low polarity
C
Gaseous state
D
Solid state
151
The boiling point of ICl is nearly 40°C higher than that of Br₂ although the two substances have the same relative molecular mass. This is because:
A
ICl is ionic compound
B
I–Cl bond is stronger than Br–Br bond
C
ICl is polar covalent molecular while Br₂ is nonpolar
D
Ionization energy of iodine is less than that of Br
152
Which of the following is incorrect?
A
NO2 is sp hybridised
B
NH4+ is sp3 hybridised
C
CH3 is planar
D
BF3 is non-planar
153
The electron adds to which one of the following orbitals during change of N2 to N2– ?
A
σ orbital
B
σ* orbital
C
π* orbital
D
π orbital
154
Variable covalency is exhibited by:
A
P and S
B
N and O
C
N and P
D
F and Cl
155
The electronic configuration of a metal ‘M’ is 1s2 2s2 2p6 3s1 . The formula of its oxide will be;
A
MO
B
M2O
C
M2O3
D
MO2
156
Nitrogen does not form NF₅ because:
A
Nitrogen is member of V group
B
It contains no empty d-orbital
C
The bond energy of N≡N is very high
D
Inert pair effect exists in the molecule
157
Hydrogen bonding is formed in compounds containing hydrogen and:
A
Highly electro-negative atoms
B
Highly electro-positive atoms
C
Metal atoms with d-orbitals occupies
D
Metalloids
158
In which following set of compound/ion has linear geometry :
A
CH₄, NH₄⁺, BH₄⁻
B
CO₃²⁻, NO₃⁻, BF₃
C
NO₂⁺, CO₂, N₃⁻
D
BeCl₂, BCl₃, CH₄
159
The ion that is isoelectronic with CO and having same bond order is :
A
CN⁻
B
O₂⁺
C
O₂⁻
D
N₂⁺
160
p-p overlapping will be observed in the molecules of :
A
H₂
B
HBr
C
HCl
D
Cl₂
161
The intermolecular force in hydrogen fluoride is due to :
A
Dipole induced dipole interactions
B
Ion-dipole interactions
C
Hydrogen bond
D
None of these
162
π bond is formed:
A
By overlapping of hybridised orbital
B
Overlapping of co-axial p-p orbitals
C
Head on overlapping of s-s orbitals
D
By p-p collateral overlapping
163
Which of the following bonds will have directional character:
A
Ionic bond
B
Metallic bond
C
Covalent bond
D
Both covalent & metallic
164
Which of the following pairs of ions are isoelectronic and isostructural?
A
ClO3– , CO32–
B
SO32– , NO3–
C
ClO3– , SO32–
D
CO32– , SO32–
165
Which one of the following postulates is wrong about the electron gas theory of metallic bonding:
A
A metal consists of positively charged spheres called kernels and the loosely bound valence electrons.
B
The kernels remain fixed but the valence electrons are free to move throughout the metallic crystal
C
The strength of the metallic bond depends number of valence electrons
D
Metallic bond is stronger than a covalent bond
166
N₂ and O₂ are converted into monoanions, N₂⁻ and O₂⁻ respectively. Which of the following statements is wrong?
A
In N₂⁻, N-N bond weakens
B
In O₂⁻, O-O bond order increases
C
In O₂⁻, O-O bond order decreases
D
N₂⁻ becomes paramagnetic
167
Which is not correct:
A
Bond angle H–S–H < H–O–H
B
Bond angle F–O–F < Cl–O–Cl
C
Bond angle H–P–H < H–N–H
D
Bond angle Cl–Sn–Cl > Cl–Hg–Cl
168
The electronegativity of O,F,N, Cl and H are 3.5, 4.0, 3.0 and 2.1 respectively. The strongest bond will be :
A
F – O
B
O – Cl
C
N – H
D
O – H
169
The magnitude of the lattice energy of a solid increases if:
A
The ions are of large size
B
The ions are of small size
C
The ions are of equal size
D
Charges on the ions are small
170
Which of the following ion has not bond order of 2.5 ?
A
O₂⁻
B
O₂⁺
C
N₂⁺
D
N₂⁻
171
Which of the following orbitals can form bond, if internuclear axis is y-axis?
A
px dxy
B
pz dxz
C
dyz dxz
D
dxz dxz
172
How many σ and p bonds will be in allyisoyanide
A
9σ and 3p
B
9σ and 9p
C
3σ and 4p
D
5σ and 7p
173
Which molecule has the highest dipole moment?
A
CH4
B
CHCl3
C
CCl4
D
CHI3
174
Which of the following compounds is non-polar:
A
CH₃Cl
B
CH₂Cl₂
C
CHCl₃
D
CCl₄
175
Which of the following statement is not correct?
A
A sigma bond is weaker than bond.
B
A sigma bond is stronger than bond.
C
A double bond is stronger than a single bond.
D
A double bond is shorter than a single bond.
176
Which of the following statement is incorrect of PCl₅:
A
Its all P-Cl bond lengths are equal
B
It involves sp³d hybridization
C
It has an regular geometry
D
Its shape is trigonal bipyramidal
177
Which one is paramagnetic and has the bond order 1/2
A
O2
B
N2
C
F2
D
H2+
178
Consider the following species: NO, H₂SO₄, O₃, NO₂, PCl₅, N₂O, CO₂ The number of species which do not follow octet rule is:
A
4
B
5
C
6
D
7
179
The order of increasing bond angle in the molecules BeCl₂, BCl₃, CCl₄ and SF₆ is:
A
SF₆ < CCl₄ < BCl₃ < BeCl₂
B
BeCl₂ < BCl₃ < CCl₄ < SF₆
C
SF₆ < CCl₄ < BeCl₂ < BCl₃
D
BCl₃ < BeCl₂ < SF₆ < CCl₄
180
Which of the following set contains species having same angle around the central atom:
A
SF₄, CH₄, NH₃
B
NF₃, BCl₃, NH₃
C
BF₃, NF₃, AlCl₃
D
BF₃, BCl₃, BBr₃
181
Which of the following group of molecules have 2½ bond order:
A
N₂²⁻, O₂²⁻, CO
B
N₂⁺, O₂⁺, NO
C
C₂²⁻, BN, O₂
D
CN⁻, NO⁺, O₂²⁺
182
Given below are two statements: one is labelled as Assertion (A) and the other is labelled as Reason (R): Assertion (A) : CO2 contains polar covalent bonds. Reason (R): CO2 is a linear molecule. In the light of the above statements, choose the correct answer from the options given below:
A
A is true but R is false.
B
A is false but R is true.
C
Both A and R are true and R is the correct explanation of A.
D
Both A and R are true but R is NOT the correct explanation of A.
183
Elements have electronegativities 1.5 and 3.0, bond formed between them would be :
A
Ionic
B
Covalent
C
Co-ordinate
D
Metallic
184
Element X is strongly electropositive and Y is strongly electronegative. Both are univalent. The compound formed would be:
A
X⁺Y⁻
B
X–Y
C
X⁻Y⁺
D
X →Y
185
A hybrid orbital formed from s-and p-orbital can contribute to:
A
A σ bond only
B
π bond only
C
Either σ or π bond
D
None of these
186
Which of the following statements is correct about N₂ molecule:
A
It has a bond order of 3
B
The number of unpaired electrons present in it is zero and hence it is diamagnetic
C
The order of filling of MO is [π(2px) = π(2py)] , σ(2pz)
D
All the above three statements are correct
187
Total number of lone pair present in XeF4 molecule is;
A
16
B
2
C
14
D
9
188
A : Tetracyanomethane, B : Carbondioxide, C : Benzene, D : 1, 3 butadiene ratio of σ and π bonds is in order:
A
A = B < C < D
B
A = B < D < C
C
A = B = C = D
D
C < D < A < B
189
The paramagnetic property of oxygen is well explained by:
A
Molecular orbital theory
B
Resonance theory
C
Valence bond theory
D
VSEPR theory
190
Electrovalent bond or ionic bond is formed by:
A
Sharing of electrons
B
Donation of electrons
C
Transfer of electrons
D
None of these
191
Electrovalent compounds or ionic compounds do not show stereoisomerism. The reason is:
A
Presence of ions
B
Strong electro static force of attraction
C
Brittleness
D
Non-directional nature of ionic bond
192
Polarity between two atoms is depend on:
A
Ionization potential of element
B
Electronegativity of element
C
Electronic configuration of element
D
No. of unpaired electrons
193
Which of the following diatomic molecular species has only π bonds according to Molecular Orbital Theory?
A
O2
B
N2
C
C2
D
Be2
194
In which molecule all atoms are coplanar
A
CH4
B
BF3
C
PF3
D
NH3
195
Species having zero dipole moment:
A
XeF₄
B
SO₂
C
SF₄
D
CH₂Cl₂
196
The correct decreasing order of dipole moment is given in:
A
HF > H2O > NH3 > NF3
B
NF3 > NH3 > HF > H2O
C
H2O > HF > NH3 > NF3
D
H2O > NH3 > HF > NF3
197
The correct order of dipole moment is :
A
CH3Cl < CH3F < CH3Br < CH3I
B
CH3Cl > CH3F > CH3Br > CH3I
C
CH3F > CH3Cl > CH3Br > CH3I
D
CH3F < CH3Cl < CH3Br < CH3I
198
The lattice energies of the oxides of Mg, Ca, Sr and Ba follow the order:
A
BaO > SrO > CaO > MgO
B
CaO > BaO > SrO > MgO
C
MgO > CaO > SrO > BaO
D
MgO > SrO > CaO > BaO
199
Solid NaCl is a bad conductor of electricity because:
A
In solid NaCl there are no ions
B
Solid NaCl is covalent
C
In solid NaCl there is no mobility of ions
D
In solid NaCl there are no electrons
200
Which of the following statement concerning a covalent bond is false :
A
The electrons are shared between atoms
B
The bond is non-directional
C
The strength of the bond depends upon the extent of overlapping
D
The bond formed may be polar or non-polar
201
Acetic acid exists as dimer in benzene due to :
A
Condensation reaction
B
Hydrogen bonding
C
Presence of carboxyl group
D
None of the above
202
Conditions for ionic bond formation is/are: (1) Small cation, large anion (2) low IP of cation, high electron affinity of anion (3) Large cation, small anion (4) Less lattice energy Correct answer is:
A
1, 4
B
2, 3 and 4
C
2 and 3
D
1, 2
203
Which of the following has been arranged in order of decreasing dipole moment:
A
CH₃Cl > CH₃F > CH₃Br > CH₃I
B
CH₃F > CH₃Cl > CH₃Br > CH₃I
C
CH₃Cl > CH₃Br > CH₃I > CH₃F
D
CH₃F > CH₃Cl > CH₃I > CH₃Br
204
Correct statement regarding this reaction BF₃ + NH₃ → [F₃B ← NH₃]
A
Hybridisation of N is changed
B
Hybridisation of B is changed
C
NH₃ act as a lewis base
D
(B) & (C) both
205
Which of the following has bond order 2?
A
NO
B
CN
C
CN–
D
CN+
206
Which of the compound is least soluble in water:
A
AgF
B
AgCl
C
AgBr
D
AgI
207
Carbon atoms in the compound (CN)₄C are:
A
sp hybridized
B
sp² hybridized
C
sp and sp² hybridized
D
sp, sp² and sp³ hybridized
208
How many σ and π bonds will be in allyl isocyanide:
A
9 σ and 3π
B
9 σ and 9π
C
3 σ and 4π
D
5 σ and 7π
209
The correct order of decreasing polarisable ions is:
A
Cl⁻ > Br⁻ > I⁻ > F⁻
B
F⁻ > I⁻ > Br⁻ > Cl⁻
C
F⁻ > Cl⁻ > Br⁻ > I⁻
D
I⁻ > Br⁻ > Cl⁻ > F⁻
210
The cyanide ion, CN⁻ and N₂ are isoelectronic. But in contrast to CN⁻, N₂ is chemically inert, because of:
A
Low bond energy
B
Absence of bond polarity
C
Unsymmetrical electron distribution
D
Presence of more number of electrons in bonding orbitals
211
Total number of canonical structures of CO32– is;
A
2
B
3
C
4
D
5
212
In which of the following molecules octet rule is violated?
A
NH3
B
CH4
C
CO2
D
BF3
213
In Co-ordinate bond, the acceptor atoms must essentially contain in its valency shell an orbital:
A
With paired electron
B
With single electron
C
With no electron
D
With three electron
214
Fluorine molecule is formed by:
A
the axial p-p orbital overlap
B
the sideways p-p orbital overlap
C
the s-s orbital overlap
D
the s-p orbital overlap
215
Among the following compounds the one that is polar and has the central atom with sp³ hybridisation is:
A
H₂CO₃
B
SiF₄
C
BF₃
D
HClO₂
216
In the series, ethane, ethylene & acetylene, the carbon-hydrogen bond length is:
A
Equal in all the three
B
Largest in ethane
C
Smallest in ethylene
D
Largest in acetylene
217
The correct order of increasing covalent character of the following is:
A
SiCl₄ < AlCl₃ < CaCl₂ < KCl
B
KCl < CaCl₂ < AlCl₃ < SiCl₄
C
AlCl₃ < CaCl₂ < KCl < SiCl₄
D
None of these
218
Higher is the bond order, greater is:
A
Bond dissociation energy
B
Covalent character
C
Bond length
D
Paramagnetism
219
which of the following configuration shows second excitation state of iodine:
A
(A)
B
(B)
C
(C)
D
(D)
220
Which of the following statement is not true about covalent compounds:
A
They may exhibit space isomerism
B
They have low melting and boiling points
C
They show ionic reactions
D
They show molecular reactions
221
Which of the following compound is formed in the second excitation state of sulphur atom :
A
SF₄
B
SF₆
C
SF₂
D
None
222
Which among the following molecules has bond order 3?
A
Cl2
B
NO
C
Ne2
D
N2
223
Element A has 3 electrons in the outermost orbit and element B has 6 electrons in the outermost orbit. The formula of the compound formed between A and B would be:
A
A₂B₃
B
A₂B₆
C
A₂B
D
A₃B₂
224
Which of the following will be octahedral:
A
SF₆
B
BF₄⁻
C
PCl₅
D
XeF₆
225
Ionic compounds in general possess both:
A
High melting points and non-directional bonds
B
High melting points and low boiling points
C
Directional bonds and low boiling points
D
High solubilities in polar and non-polar solvents
226
Which of the molecule is trigonal bipyramidal :
A
BF₃
B
CH₄
C
PCl₅
D
SF₆
227
Incorrect order of bond angle is given in;
A
NH NH 3 2
B
CCl CH 4 4
C
BF AlCl 3 3
D
NH NH 4 3
228
The bond angles of NH₂⁻, NH₃, and NH₄⁺ are in the order:
A
NH₂⁻ > NH₃ > NH₄⁺
B
NH₄⁺ > NH₃ > NH₂⁻
C
NH₃ > NH₂⁻ > NH₄⁺
D
NH₃ > NH₄⁺ > NH₂⁻
229
an electrovalent bond or ionic bond is formed between :
A
Two electronegative atoms
B
Two metals
C
Electropositive and electronegative atoms
D
Two electropositive atoms
230
Which of the following compound does not follow octet rule:
A
CO₂
B
PCl₃
C
ICl
D
ClF₃
231
Acetic acid is a dimer in benzene due to:
A
Condensation reaction
B
Hydrogen bonding
C
Presence of carboxylic group
D
Presence of hydrogen atom at α-carbon
232
The nature of intermolecular forces among benzene (C₆H₆) molecules is:
A
Dipole-dipole attraction
B
London dispersion force
C
Ion-dipole attraction
D
Hydrogen bonding
233
The correct order of volatility is;
A
NH3 < H2O
B
p–nitrophenol < o–nitrophenol
C
CH3OH > CH3 — O — CH3
D
HF > HCl
234
The pair of molecules forming strongest hydrogen bonds are :
A
SiH₄ and SiF₆
B
CH₃–CO–CH₃ and CHCl₃
C
HCOOH and CH₃COOH
D
H₂O and H₂
235
Which of the following match is not correct:
A
ICl₂⁻ — Linear ion
B
ICl₄⁻ — Square planar ion
C
XeF₂ — Linear molecule
D
SO₄²⁻ — Trigonal planar ion
236
In which of the excitation state of chlorine ClF₃ is formed:
A
In ground state
B
In third excitation state
C
In first excitation state
D
In second excitation state
237
All of the following are diamagnetic in nature, except:
A
N2
B
H2
C
Li2
D
O2
238
The type of bonds present in CuSO₄·5H₂O are:
A
Co-ordinate
B
Covalent and Co-ordinate
C
Covalent, co-ordinate, ionic and H-bonds
D
Only ionic
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