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Polarity of Bonds - Dipole Moment
The unit of dipolemoment is
1) Einstein
3.
3) Debye
4) Curie
One Debye (D) equal to
co
m
2.
2) Dalton
1) 1 × 10–4 esu.cm
2) 1 × 10–18 esu.cm
3) 1 × 10–10 esu.cm
4) 1 × 10–16 esu.cm
Carbon tetrachloride has no dipole moment because of
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1.
1) Its regular tetrahedral structure
2) Its planar structure
3) Similar sizes of carbon and chlorine atoms
4) Similar electron affinities of carbon and chlorine
4.
The unequal sharing of the bond pair of electons between two atoms in
a molecule causes,
1) Dipole
2) Radical Formation
6.
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1) e.s.u-cm
2) Coulomb-cm
3) Coulomb-meter
4) e.s.u – meter
Molecule with zero dipole moment is
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1) BCl3
1) CH2Cl2
8.
3) CCl4
4) All of these
2) SO3
3) NH3
4) H2O
Bent molecule having dipole moment among the following
1) F2O
9.
2) BeCl2
Which one of the following has = 0
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7.
4) Decomposition of molecule
S.I. unit for dipole moment is
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a
5.
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3) Covalent bond
2) H2O
3) Cl2O
4) All the above
Which of the following molecule has zero dipolemoment?
1) BeCl2
2) HCl
3) NH3
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4) H2O
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In which of the following pairs, both molecules possess dipole moment?
1)
11.
CO2 ,SO2
2)
2) CO2
H 2 O,SO2
4)
CO 2 ,CS2
3) CCl4
4) NF3
Molecule with dipole moment among the following
1) SF6
13.
3)
Which of the following has highest dipole moment?
1) BF3
12.
BCl3 ,PCl3
2) PCl5
3) CCl4
4) BF3
co
m
10.
(A): The dipolemoment value of NH3 is greater than zero.
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(R): In NH3 bond angle is approximately 104°.
1) Both (A) and (R) are true and (R) is the correct explanation of (A).
2) Both (A) and (R) are true and (R) is not the correct explanation of (A).
3) (A) is true but (R) is false.
4) (A) is false but (R) is true.
14.
(A): SiF4 is non polar even though fluorine is much more
electronegative than silicon.
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(R): The four bond dipoles cancel one another in SiF4 molecule.
1) Both (A) and (R) are true and (R) is the correct explanation of (A).
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2) Both (A) and (R) are true and (R) is not the correct explanation of (A).
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3) (A) is true but (R) is false.
4) (A) is false but (R) is true.
(A): SO2 molecule has unsymmetrical shape.
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15.
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(R): The dipole moment of SO2 molecule is not equal to zero.
1) Both (A) and (R) are true and (R) is the correct explanation of (A).
2) Both (A) and (R) are true and (R) is not the correct explanation of (A).
3) (A) is true but (R) is false.
4) (A) is false but (R) is true.
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16.
The following are some statements about dipole moment.
i) The dipole moment of a molecule in which the central atom has no lone–
pair, is zero.
ii) The dipole moment of a diatomic molecule having non–polar bonds is
zero.
co
m
iii) The dipole moment of a diatomic molecule having polar covalent bonds
is non–zero.
2) Only ii is correct.
3) Only ii and iii are correct.
4) Only i and iii correct.
In SF6 molecule
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17.
1) All the three statements are correct.
1) Bonds are polar but molecule is non polar.
2) Bonds are polar and molecule is also polar.
3) Bonds are non polar but molecule is polar.
4) Bonds are non polar and molecule is non polar.
18.
Dipolemoment is least in
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1) Para – dichlorobenzene
3) Ortho – dichlorobenzene
4) Mono chloro benzene
The dipole moment of HX molecule is 1.92D and bond distance is .2A0.
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19.
2) Meta – dichlorobenzene
.s
a
What is the percentage ionic character of HX?
1) 33%
3) 70%
Which of the following will have zero dipole moment?
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20.
2) 25%
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1) 1, 1– dichloroethylene
2) cis-1, 2-dichloroethylene
3) trans-1, 2-dichloroethylene
4) None of these
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4) 66%
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21.
The molecules BF3 and NF3 are covalent compounds. But BF3 is nonpolar and NF3 is polar. The reason is
1) Boron is a metal and nitrogen is a gas in uncombined state
2) BF bonds have no dipole moment where as NF bonds have dipole
3) Atomic size of boron is smaller than that of nitrogen
4) BF3 is planar but NF3 is pyramidal in shape
BeF2 has zero dipole moment where as H2O has a dipole moment
because
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co
m
moment
1) H2O is a linear molecule.
2) H2O is a bent molecule.
3) F is more electronegative than O.
4) Hydrogen bonding is present in H2O.
23.
From the following given statements of the order of dipolemoments.
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i) HF > H2O > NH3
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ii) CH2Cl2 > CHCl3>CCl4
Cl
Cl
Cl
.s
a
>
>
Cl
iii)
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The correct combination is
2) i, ii are correct
3) Only iii is correct
4) Only i is correct
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1) All are correct
24.
A molecule MX3 has zero dipole moment. The % of’s’ character in the
hybridized orbitals of M is
1) 25%
2) 33.3%
3) 50%
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4) 75%
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25.
Dipole moment of H2X is 1.0D. If the bond angle is 90 o, the
approximate bond moment of H-X bond is (Cos 45o= 0.7)
1) 0.4D
26.
2) 0.5D
3) 0.7D
4) 0.6D
The dipolemoment of HX is 1.2D. If the ionic character of the bond is
1) 10A0
27.
2) 10–10m
co
m
25%, then its bond length is
3) 10–8m
4) 10–6m
Which bond angle would result in the maximum dipole moment for the
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tri-atomic molecule XY2?
1)  =90
28.
2)  =120
3)  =150
4)  =180
If the bond length and dipolemoment of a diatomic molecule are 1.25Ao
and 1.0D respectively, what is the percent ionic charcter of the bond?
1) 10.66
29.
2) 12.33
3) CO2
4) CH3F
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2) CH3OH
The compound having highest dipole moment is
H
CH 3
|
|
C = C
|
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CH3 H
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Cl
CH3
|
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C = C
|
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CH3 Cl
H
2)
H
.s
a
1)
31.
4) 19.33
The highest dipolemoment is of
1) CF4
30.
3) 16.66
C=O
3)
4)
CH3 H
|
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C = C
|
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CH3 H
Dipole moment of is zero which implies that
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1) Carbon and oxygen have equal electro negativities
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2) Carbon has no polar bond
3) Is a linear molecule
4) Carbon has bond moments of zero value
32.
In which of the following bond is polar but molecule is non-polar
1) H2O
2) NH3
3) SO
4) CO
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The molecule having non-zero dipole moment is
1) H 2O2
2) ClF3
2) CH4
3) 1 C m = 3.3356 D
C 2 H 5C  CC2 H 5
3) CO
4) XeF4
2) 1D= 3.3356 10
30
Cm
4)1Cm= 3.3356 1030 D
Bond - length of HCl is; 1.275 Ao (e  4.8 1010 esu ).If   1.02 D
Then, HCl is
1) 100% ionic
38.
4)
Which of the following unit conversion of dipole moment is correct?
1) 1D = 3.3356 C m
37.
3) XeF4
BF4-
In which of the following bond is polar and molecule also polar
1) H2S
36.
4)
Dipolemoment is not zero for
1) PCl5
35.
3) C2H6
co
m
34.
2) CH4
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33.
2) 83% covalent
3) 50% covalent
4) 40% ionic
The dipole moment of HBr is esu cm. The bond length of HBr is 1.41A0
The ionic character of HBr is
3) 15
4) 27
The electronegativity difference between N and F is greater than N and
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39.
2) 11.52
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1) 7.5
H, yet the dipole moment is greater than that of This is because
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a
1) In as well as, the atomic dipole and bond dipole are in opposite direction.
2) In, the atomic dipole and bond dipole are in the opposite direction; where
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as in these are in same direction.
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3) In, as well as in the atomic dipole and bond dipole is in same direction.
4) In, the atomic dipole and bond dipole are in same direction where as in
these are in opposite direction.
40.
A diatomic molecule has a dipole moment of 1.2 D, if the bond distance
is 1, what percentage of electronic charge exists on each atom.
1) 25% of e
2) 29% of e
3) 19% of e
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4) 12 % of e
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KEY
3) 1
4) 1
5) 3
6) 4
7) 2
8) 4
9) 1
10) 3
11) 4 12) 2 13) 3 14) 1 15) 1
16) 3
17) 1 18) 1 19) 1 20) 3
21) 4 22) 2 23) 2 24) 2 25) 3
26) 2
27) 1 28) 3 29) 2 30) 3
31) 3 32) 4 33) 1 34) 2 35) 1
36) 2
37) 2 38) 2
co
m
2) 2
39)4
40)1
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1) 3
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