Unit
# 6…….. M.C.Qs on Chemical Bonding
1. The
shell of an atom with highest ‘n’ is known as:
|
(a)
|
Valance shell
|
(b)
|
Inner shell
|
|
(c)
|
Empty shell
|
(d)
|
Filled shell.
|
2. All
inert gases except Helium are characterized by a completion of the outer ………
|
(a)
|
s-orbital
|
(b)
|
p-orbital
|
|
(c)
|
d-orbital
|
(d)
|
f-orbital
|
3. Neutral
atoms of Neon have the same number of electrons as each of the following:
|
(a)
|
O2–
|
(b)
|
F1–
|
|
(c)
|
Na1+
|
(d)
|
Mg2+
|
4. The
attractive forces that holds an atom together in a molecule is termed as:
|
(a)
|
Covalent bond
|
(b)
|
Dative bond
|
|
(c)
|
Chemical bond.
|
(d)
|
Ionic bond
|
5. Chemical
bond formation takes place due to interaction of …………electrons.
|
(a)
|
Valance
|
(b)
|
Inner
|
|
(c)
|
Free
|
(d)
|
Paired
|
6. Lower
the energy…………. will be stability of molecules.
|
(a)
|
Lesser
|
(b)
|
Greater
|
|
(c)
|
Both a and b
|
(d)
|
None of the above
|
7. Inert
gases have ……………….valance electrons.
|
(a)
|
5
|
(b)
|
4
|
|
(c)
|
7
|
(d)
|
8
|
8. Which
of the compounds have the ionic bond?
|
(a)
|
NaCl
|
(b)
|
KCl
|
|
(c)
|
MgO
|
(d)
|
All of the above
|
9. The
mutual sharing of electrons pairs in atoms gives rise to:
|
(a)
|
Hydrogen bond
|
(b)
|
Ionic bond
|
|
(c)
|
Covalent bond
|
(d)
|
Dative bond
|
10. Which
molecule has covalent bond?
|
(a)
|
NaCl
|
(b)
|
CaCO3
|
|
(c)
|
MgO
|
(d)
|
HCl
|
11.
the bond formed by mutual sharing of one electron pair b/w two bonded
atoms is called…… bond:
|
(a)
|
Single covalent
|
(b)
|
Double covalent
|
|
(c)
|
Triple covalent
|
(d)
|
Ionic bond
|
12. Which
molecule has single covalent bond?
|
(a)
|
O2
|
(b)
|
N2
|
|
(c)
|
CO2
|
(d)
|
CH4
|
13. which molecule does not have single
covalent bond?
|
(a)
|
O2
|
(b)
|
N2
|
|
(c)
|
CCl4
|
(d)
|
HF
|
14. Which
molecule has double covalent bond?
|
(a)
|
O2
|
(b)
|
N2
|
|
(c)
|
CCl4
|
(d)
|
HF
|
15. Which
molecule has triple covalent bond?
|
(a)
|
O2
|
(b)
|
N2
|
|
(c)
|
CCl4 or CH4
|
(d)
|
H2
|
16. Bond
making is always:
|
(a)
|
Endothermic
|
(b)
|
Exothermic
|
|
(c)
|
Both
a and b
|
(d)
|
None
of the above
|
17. Bond breaking is always:
|
(a)
|
Endothermic
|
(b)
|
Exothermic
|
|
(c)
|
Both
a and b
|
(d)
|
None
of the above
|
18. The
formation of chemical bond is accomplished by:
|
(a)
|
Decrease in energy
|
(b)
|
Increase in energy
|
|
(c)
|
Neither decrease nor increase in energy
|
(d)
|
The repulsive forces overcoming the
attractive forces
|
19. chemical bond formation takes place
when:
|
(a)
|
Forces of
repulsions overcome forces of attractions.
|
(b)
|
Energy is absorbed
|
|
(c)
|
Forces of
attractions are equal to forces of repulsions
|
(d)
|
Forces of
attractions overcome forces of repulsions
|
20. Which one is correct reading ionic bond?
|
(a)
|
It
is formed by complete transference of electrons from one atom to another.
|
|
(b)
|
It
is an electrostatic force of attraction b/w two oppositely charged ions.
|
|
(c)
|
It
is formed b/w atoms of low IP and atoms of high EM
|
|
(d)
|
All
of the above
|
21. Generally an ionic bond is formed b/w:
|
(a)
|
Elements
of group IA an IIA and elements of group VIA and VIIA.
|
|
(b)
|
Elements
of group VA an VIIA.
|
|
(c)
|
Elements
of group IA an VIIA.
|
|
(d)
|
None
of the above.
|
22. In which one of the following does ionic
bonding occur between named atoms?
|
(a)
|
Aluminium
and chlorine in the tetrachloroaluminate ion.
|
|
(b)
|
Boron
and fluorine in boron trifluoride.
|
|
(c)
|
Hydrogen
and chlorine in hydrogen chloride.
|
|
(d)
|
Hydrogen
and sodium in sodium hydride.
|
23. Which one is correct reading ionic bond and
Ionic compounds?
|
(a)
|
Ionic
bond is non directional
|
|
(b)
|
Ionic
compounds are non-electrolytes and volatile
|
|
(c)
|
Ionic
compounds are hard and rigid solid
|
|
(d)
|
Ionic
compounds are soluble in polar solvent
|
24. Which one is correct reading covalent bond and
covalent compounds?
|
(a)
|
covalent
bond is directional.
|
|
(b)
|
Covalent
compounds are non-electrolytes and volatile.
|
|
(c)
|
covalent
compounds are soft and brittle.
|
|
(d)
|
Covalent
compounds are usually soluble in non-polar solvent.
|
25. Which
one is correct reading the effect of
ionic character of covalent bond on the properties of compounds?
|
(a)
|
Its
elevates m.p and b.p
|
|
(b)
|
It
increases the stability of compounds in polar solvent (H2O)
|
|
(c)
|
It
shorten the bond distance thereby enhancing bond energies
|
|
(d)
|
All
of the above.
|
26. Which one is incorrect reading bond energy?
|
(a)
|
It
is the amount of energy required to break one mole of bond to form isolated
natural atom.
|
|
(b)
|
It
measures the strength of covalent bond.
|
|
(c)
|
It
increases with the increase in polarity.
|
|
(d)
|
Bond
energy of non-polar molecule is greater then that of polar molecule.
|
27. Which one has highest bond energy?
|
(a)
|
Non-
Polar molecule
|
(c)
|
Polar
compounds having multiple bond
|
|
(b)
|
Polar
compounds having single bond
|
(d)
|
None
of the above.
|
28.
A covalent bond
in which the shared electron pair is attracted equally by the two atoms is
called:
|
(a)
|
Polar bond
|
(b)
|
Non- Polar bond
|
|
(c)
|
dative bond
|
(d)
|
hydrogen bond
|
29. Which one is correct reading the examples of
Non- Polar bond?
|
(a)
|
S=C=S
|
(b)
|
PH3
|
|
(c)
|
CH4
|
(d)
|
CH3Cl
|
30.
A covalent bond
in which the shared electron pair is attracted equally by the two atoms is
called:
|
(a)
|
Polar bond
|
(b)
|
Non- Polar bond
|
|
(c)
|
dative bond
|
(d)
|
hydrogen bond
|
31. Which
molecule has greater bond energy?
|
(a)
|
Polar molecule
|
(b)
|
Non- Polar molecule
|
|
(c)
|
None of the above
|
(d)
|
All of the above.
|
32. Greater
the difference in E N b/w bonded atoms _________will be polarity.
|
(a)
|
Lesser
|
(b)
|
Greater
|
|
(c)
|
None
of the above
|
(d)
|
All
of the above.
|
33. A bond
is said to be 100% covalent, if it exists b/w atoms of:
|
(a)
|
Same
elements
|
(b)
|
Different
elements
|
|
(c)
|
Same
group
|
(d)
|
Different
group
|
34. The
one sided sharing of electrons b/w two atoms produces which type of bond?
|
(a)
|
covalent bond
|
(b)
|
hydrogen bond
|
|
(c)
|
dative bond
|
(d)
|
Ionic bond
|
35. Which
of the following has co-ordinate covalent bond?
|
(a)
|
NH4+
|
(b)
|
H2O
|
|
(c)
|
H3O+
|
(d)
|
Both a and c
|
36. Which of the following has the shortest C─C
bond length?
|
(a)
|
C2H2
|
(b)
|
C2H4
|
|
(c)
|
C2H6
|
(d)
|
C2H5OH
|
37. Which
of the following has the highest bond energy?
|
(a)
|
C2H2
|
(b)
|
C2H4
|
|
(c)
|
C2H6
|
(d)
|
C2H5OH
|
38. Which
one of the following bond has the most polar character?
|
(a)
|
C–O
|
(b)
|
C–Br
|
|
(c)
|
C–F
|
(d)
|
C–S
|
39. Which
one of the following bond has the least polar character?
|
(a)
|
C–H
|
(b)
|
C–Cl
|
|
(c)
|
C–O
|
(d)
|
C–N
|
40. the degree or extent of polarity of a
molecule is called:
|
(a)
|
Bond
energy
|
(b)
|
Moment arm
|
|
(c)
|
Dipole
moment
|
(d)
|
Ionic character
|
41. the product of magnitude of charge at
each pole and the internuclear distance b/w the two opposite charges
called:
|
(a)
|
debye
|
(b)
|
Moment arm
|
|
(c)
|
Dipole
moment
|
(d)
|
Bond length
|
42. Dipole moment is a:
|
(a)
|
Scalar quantity
|
(b)
|
Vector
quantity
|
|
(c)
|
Basic quantity
|
(d)
|
None
of the above
|
43. Dipole
moment is denoted by:
|
(a)
|
Double head arrow
|
(b)
|
Double arrow
|
|
(c)
|
Crossed tail arrow
|
(d)
|
None of the above
|
44. dipole moment is defined as
|
(a)
|
Charge
x Internuclear distance
|
(b)
|
Charge
x Charge
|
|
(c)
|
Charge
x Debye
|
(d)
|
Charge
x Bond energy
|
45. S.I
unit of dipole moment (µ) is
|
(a)
|
N-sec
|
(b)
|
N.m2
|
|
(c)
|
C.m
(coulomb x meter)
|
(d)
|
None
of the above
|
46. 1 coulomb is equal to:
|
(a)
|
2.99x10-9
e.s.u
|
(b)
|
2.99x1019
e.s.u
|
|
(c)
|
2.99x10-19
e.s.u
|
(d)
|
None
of the above
|
47. 1
debye (1D) is equal to:
|
(a)
|
10-30 coulomb-meter
|
(b)
|
10-18
e.s.u-cm
|
|
(c)
|
10-10 e.s.u-m
|
(d)
|
All
of the above
|
48.
the diatomic polar
molecules have dipole moment:
|
(a)
|
Equal to 0
|
(b)
|
Greater than 0
|
|
(c)
|
Equal to 1
|
(d)
|
None of the above
|
49.
Which one
has zero dipole moment?
|
(a)
|
CO2
|
(b)
|
CS2
|
|
(c)
|
HCl
|
(d)
|
Both a and b
|
50. CO2 and CS2 has no dipole moment due to:
|
(a)
|
Linear structure
|
(b)
|
Angular structure
|
|
(c)
|
Pyramidal structure
|
(d)
|
Both a and b
|
51. H2O and SO2 have dipole moment:
|
(a)
|
Equal to 0
|
(b)
|
Greater than 0
|
|
(c)
|
Equal to 1
|
(d)
|
None of the above
|
52. H2O and SO2 have same dipole moment due to
its:
|
(a)
|
Bent structure
|
(b)
|
Angular structure
|
|
(c)
|
Both a and b
|
(d)
|
None of the above
|
53.
the structure of
triatomic molecule whose dipole moment is zero will be:
|
(a)
|
Linear structure
|
(b)
|
Angular structure
|
|
(c)
|
Pyramidal structure
|
(d)
|
Tetrahedral
|
54. tetrahedral
molecules with symmetric structure have
|
(a)
|
Zero dipole moment
|
(b)
|
Some dipole moment
|
|
(c)
|
Both a and b
|
(d)
|
None of the above
|
55.
CH4
and CCl4 have zero dipole moment due to:
|
(a)
|
Symmetrical structure
|
(b)
|
Unsymmetrical structure
|
|
(c)
|
Both a and b
|
(d)
|
None of the above
|
56.
tetrahedral molecules with unsymmetrical structures
have
|
(a)
|
Zero dipole moment
|
(b)
|
Some dipole moment
|
|
(c)
|
Both a and b
|
(d)
|
None of the above
|
57.
CH3Cl,CH2Cl2
and CHCl3 have some dipole moment due to
|
(a)
|
Symmetrical structure
|
(b)
|
Unsymmetrical (or
Asymmetrical) structure
|
|
(c)
|
Both a and b
|
(d)
|
None of the above
|
58.
the bond energy of
hydrogen bond ranges
|
(a)
|
3 – 10 kcal
|
(b)
|
10 – 17 kcal
|
|
(c)
|
17 – 25 kcal
|
(d)
|
25-35 kcal
|
59.
water boils at higher
temperature than H2S due to
|
(a)
|
Ionic bonding
|
(b)
|
Covalent bonding
|
|
(c)
|
London forces
|
(d)
|
Hydrogen bonding
|
60.
hydrogen bond greatly ………………
the solubility of compound
|
(a)
|
Increase
|
(b)
|
Decrease
|
|
(c)
|
Has no effect
|
(d)
|
Both a and b
|
61.
Ethyl
alcohol is liquid while its isomer dimethyl ether is gas. This is b/c ethyl
alcohol has
|
(a)
|
Ionic bonding
|
(b)
|
Covalent bonding
|
|
(c)
|
Protonic Bridges
|
(d)
|
London forces
|
62.
hydrogen bond ……………. the
m.p and b.p of compounds.
|
(a)
|
Elevates
|
(b)
|
Reduces
|
|
(c)
|
Has no effect of
|
(d)
|
Both a and b
|
Modern
Concept of Covalent Bonding
63.
the modern theories of
covalent bond is
|
(a)
|
Valance Bond Theory (VBT)
|
(b)
|
Molecular Orbital theory(MOT)
|
|
(c)
|
Valance shell electron pair repulsion
(VSEPR) theory
|
(d)
|
All of the above.
|
64.
which theory explain the
chemical bonding in terms of overlapping of atomic orbitals which retain their identities and share electrons is mono centric
|
(a)
|
VBT
|
(b)
|
MOT
|
|
(c)
|
VSEPR
|
(d)
|
All of the above
|
65.
the molecular orbitals
which have lower energy then parent atomic orbital are called
|
(a)
|
Bonding molecular orbital(BMO)
|
(b)
|
Antibonding molecular orbital (AMO)
|
|
(c)
|
Both a and b
|
(d)
|
None
of the above
|
66.
the molecular orbitals
which have higher energy than parent atomic orbital are called
|
(a)
|
AMO
|
(b)
|
BMO
|
|
(c)
|
Hybrid orbital
|
(d)
|
All of the above
|
67.
a bond formed by the
pairing of electrons spin caused by the axial overlapping of half filled atoms
is called
|
(a)
|
Sigma bond
|
(b)
|
Pi bond
|
|
(c)
|
Ionic bond
|
(d)
|
None of the above
|
68. in a sigma
bond the region of …….. electron density is symmetrically distributed around
axis
|
(a)
|
Lowest
|
(b)
|
Intermediate
|
|
(c)
|
Highest
|
(d)
|
All of the above.
|
69. sigma bond
has
|
(a)
|
Lowest
|
(b)
|
Intermediate
|
|
(c)
|
Highest
|
(d)
|
All of the above.
|
70. which bond is
more stable?
|
(a)
|
Sigma bond
|
(b)
|
Pi bond
|
|
(c)
|
Both a and b
|
(d)
|
None of the above
|
71. How many sigma bonds can be predicted between two atoms?
|
(a)
|
4
|
(b)
|
3
|
|
(c)
|
2
|
(d)
|
1
|
72. in hydrogen
molecule sigma bond is formed by the head on overlapping of half filled
|
(a)
|
p-p orbitals
|
(b)
|
s-s orbitals
|
|
(c)
|
d-d orbitals
|
(d)
|
f-f orbitals
|
73. in F2
molecule sigma bond is formed by the end to end overlapping of half filled
|
(a)
|
p-p orbitals
|
(b)
|
s-s orbitals
|
|
(c)
|
d-d orbitals
|
(d)
|
f-f orbitals
|
74. in HCl
molecule sigma bond is formed by the axial overlapping of half filled
|
(a)
|
s-p orbitals
|
(b)
|
s-s orbitals
|
|
(c)
|
d-d orbitals
|
(d)
|
s-p3 orbitals
|
75. in CH4
molecule a sigma bond is formed by the axial overlapping half filled
|
(a)
|
p-p orbitals
|
(b)
|
s-s orbitals
|
|
(c)
|
d-d orbitals
|
(d)
|
s-sp3 orbitals
|
76. in C2H4
molecule a sigma bond between C to C is formed by the axial overlapping half
filled
|
(a)
|
s-p orbitals
|
(b)
|
s-s orbitals
|
|
(c)
|
s-p orbitals
|
(d)
|
sp2-sp2 orbitals
|
77. a bond formed
by pairing of electron spin caused by the parallel or side wise overlapping of two half filled coplanar
p-atomic orbitals already bonded through a sigma bond is called
|
(a)
|
Sigma bond
|
(b)
|
Pi bond
|
|
(c)
|
Hydrogen bond
|
(d)
|
None of the above
|
78. pi-bond is
formed by the overlap of
|
(a)
|
p-p orbitals
|
(b)
|
s-s orbitals
|
|
(c)
|
s-p orbitals
|
(d)
|
sp3-sp3 orbitals
|
79. the process
of mixing different atomic orbitals having small energy difference and
different shapes belonging to the
same atoms to form an equal no of new set of equivalent orbitals of the same energy, size and shape is
called
|
(a)
|
Overlapping
|
(b)
|
Hybridization
|
|
(c)
|
Blending
|
(d)
|
Delocalization
|
80. the hybrid orbitals
are …………orbitals.
|
(a)
|
Atomic
|
(b)
|
Molecular
|
|
(c)
|
Both a and b
|
(d)
|
None of the above
|
81. the process
of mixing of one s and three p orbitals of the same atom to form four new equivalent hybrid orbital is called
|
(a)
|
sp hybridization
|
(b)
|
sp3 hybridization
|
|
(c)
|
sp2 hybridization
|
(d)
|
None of the above
|
82. in sp3 hybrid
orbitals the ratio of s and p orbitals is
|
(a)
|
1:2
|
(b)
|
1:3
|
|
(c)
|
1:4
|
(d)
|
1:1
|
83. the angel
between sp3 hybrid orbitals is
|
(a)
|
180o
|
(b)
|
120o
|
|
(c)
|
104.5o
|
(d)
|
109.5o
|
84. which of the
following hybrid orbitals has 25% s character and 75% p character
|
(a)
|
sp3
|
(b)
|
sp2
|
|
(c)
|
sp
|
(d)
|
None of the above
|
85. in which
molecule carbon atom is sp3 hybridized
|
(a)
|
C2H2
|
(b)
|
C2H4
|
|
(c)
|
CH4
|
(d)
|
C6H6
|
86. the process
of mixing of one s and two p orbitals of the same atom to form three new equivalent hybrid
orbital is called
|
(a)
|
sp3
|
(b)
|
sp2
|
|
(c)
|
sp
|
(d)
|
None of the above
|
87.
in sp2 hybrid
orbitals the ratio of s and p orbitals is
|
(a)
|
1:2
|
(b)
|
1:3
|
|
(c)
|
1:4
|
(d)
|
1:1
|
88. the angel
between sp2 hybrid orbitals is
|
(a)
|
180o
|
(b)
|
120o
|
|
(c)
|
104.5o
|
(d)
|
109.5o
|
89. which of the
following hybrid orbitals has 33.33% s character and 66.66% p character
|
(a)
|
sp3
|
(b)
|
sp2
|
|
(c)
|
sp
|
(d)
|
None of the above
|
90. in which
molecule carbon atom is sp2 hybridized
|
(a)
|
C2H4
|
(b)
|
C6H6
|
|
(c)
|
C2H6
|
(d)
|
Both a and b
|
91. the process
of mixing of one s and one p orbitals of
the same atom to form two new equivalent hybrid orbitals is called
|
(a)
|
sp3
|
(b)
|
sp2
|
|
(c)
|
sp
|
(d)
|
None of the above
|
92. in sp1
hybrid orbitals the ratio of s and p orbitals is
|
(a)
|
1:2
|
(b)
|
1:3
|
|
(c)
|
1:4
|
(d)
|
1:1
|
93. the angel
between sp3 hybrid orbitals is
|
(a)
|
180o
|
(b)
|
120o
|
|
(c)
|
104.5o
|
(d)
|
109.5o
|
94. which of the
following hybrid orbitals has 50% s character and 50% p character?
|
(a)
|
sp3
|
(b)
|
sp2
|
|
(c)
|
sp
|
(d)
|
None of the above
|
95. in which
molecule carbon atom is sp hybridized
|
(a)
|
C2H4
|
(b)
|
C6H6
|
|
(c)
|
C2H6
|
(d)
|
C2H2
|
96. a molecule of
ethylene (C2H4) contains total
|
(a)
|
2 σ and 1 π bond
|
(b)
|
5 σ and 1 π bond
|
|
(c)
|
4 σ and 2 π bond
|
(d)
|
3 σ and 3 1π bond
|
97. a molecule of
acetylene (C2H2) contains total
|
(a)
|
3 σ and 2 π bond
|
(b)
|
2 σ and 3 π bond
|
|
(c)
|
4 σ and 1 π bond
|
(d)
|
5 σ and no π bond
|
98. a molecule of
ethane (C2H6) contains total
|
(a)
|
7 σ and 1 π bond
|
(b)
|
6 σ and no π bond
|
|
(c)
|
5 σ and no π bond
|
(d)
|
7 σ and no π bond
|
99. The active electrons pair around the central atom are arranged in
space in such a way that they keep as far a part as possible so that there is minimum inter-electronic
repulsion. This is the basic assumption of
|
(a)
|
MOT
|
(b)
|
VBT
|
|
(c)
|
VSLPR theory
|
(d)
|
H.O.M
|
100. inter-electronic repulsion forces decrease sharply with increasing
|
(a)
|
Bond length
|
(b)
|
Bond energy
|
|
(c)
|
Bond angle
|
(d)
|
All of the above.
|
101. the presence of lone pair on the central atom ………… bond angle
|
(a)
|
Expend
|
(b)
|
Contract
|
|
(c)
|
Has no effect on
|
(d)
|
All of the above.
|
102. two active pairs of electron in valance shell around the central atom will
give
|
(a)
|
Linear shape
|
(b)
|
Angular
|
|
(c)
|
Trigonal
|
(d)
|
Pyramidal
|
103. which one has linear structure?
|
(a)
|
BeCl2
|
(b)
|
CO2 or CS2
|
|
(c)
|
C2H2
|
(d)
|
All of the above.
|
104. three active pairs of electron in valance shell around the central atom will
give shape
|
(a)
|
Linear shape
|
(b)
|
Angular
|
|
(c)
|
Trigonal
|
(d)
|
Pyramidal
|
105. which of the following has trigonal shape?
|
(a)
|
BCl3
|
(b)
|
C2H4
|
|
(c)
|
SO3 or CO42–
|
(d)
|
All of the above
|
106. four active pairs of electron in valance shell around the central atom with
no non-bonding (lone pair) electrons will give …………….shape
|
(a)
|
Tetrahedral
|
(b)
|
Angular
|
|
(c)
|
Trigonal
|
(d)
|
Pyramidal
|
107. which of the following
has tetrahedral shape?
|
(a)
|
CH4
|
(b)
|
CCl4
|
|
(c)
|
C2H6
|
(d)
|
SO42–
|
108. Four active pairs of electron in valance shell around the
central atom with one non-bonding (lone pair) electrons will give …………….. shape
|
(a)
|
Tetrahedral
|
(b)
|
Angular
|
|
(c)
|
Trigonal
|
(d)
|
Pyramidal
|
109. which of the following has pyramidal shape?
|
(a)
|
NH3 or PH3
|
(b)
|
CO
|
|
(c)
|
H2O
|
(d)
|
Both a and b
|
110. four active pairs of electron in valance shell around the central atom with
two non-bonding (lone pair) electrons will give …………… shape
|
(a)
|
Tetrahedral
|
(b)
|
Angular
|
|
(c)
|
Trigonal
|
(d)
|
Pyramidal
|
111. which of the following has angular shape?
|
(a)
|
H2O or H2S
|
(b)
|
SO2
|
|
(c)
|
SCl2
|
(d)
|
All of the above.
|
112. the bond angle in NH3 (Pyramidal molecule) is
|
(a)
|
180o
|
(b)
|
120o
|
|
(c)
|
107o
|
(d)
|
109.5o
|
113. the bond angle in H2O (Angular molecule) is
|
(a)
|
180o
|
(b)
|
120o
|
|
(c)
|
107o
|
(d)
|
104.5o
|
114. all diatomic molecules are _____________ in shape
|
(a)
|
Tetrahedral
|
(b)
|
Angular
|
|
(c)
|
Planar Trigonal
|
(d)
|
Linear
|
115. the shape of HCl, HBr, HF and HI are
|
(a)
|
Tetrahedral
|
(b)
|
Angular
|
|
(c)
|
Planar Trigonal
|
(d)
|
Linear
|
116. the shape of NH2Cl2 molecule is
|
(a)
|
Tetrahedral
|
(b)
|
Angular
|
|
(c)
|
Planar Trigonal
|
(d)
|
Linear
|
117. the shape of NHCl3 molecule is
|
(a)
|
Tetrahedral
|
(b)
|
Angular
|
|
(c)
|
Planar Trigonal
|
(d)
|
Linear
|
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