Chemical Bonding & Molecular Structure Test

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Chemical Bonding & Molecular Structure Test - 2

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Weekly Quiz Competition

Question 1
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Which of the following sets represents molecules with linear geometry only?

A
SO₂, NO₂^-, H₂O, I₃^-

B
CO₂, NO₂^-, SO₂, IF₂^-

C
CO₂, NH₂^-, I₃^-, IF₂^-

D
CO₂, BeCl₂, I₃^-, IF₂^-

Solution

CO₂, BeCl₂, I₃^-, IF₂^-: All have linear geometry
Question 2
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Which of the following sets represents molecules with trigonal planar geometry only?

A
BF₃, NH₃, IF₃, SO₃^2-

B
BF₃, SO₃, GaF₃, NO₃^-

C
NH₃, SO₃^2-, GaF₃, NO₃^-

D
BF₃, SO₃, GaF₃, IF₃

Solution

BF₃, SO₃, GaF₃, NO₃^-: All have trigonal planar geometry.
Question 3
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Which of the following statements is true?

A
Linear overlapping of p-orbitals forms a pi bond.

B
All molecules with polar bonds have a dipole moment.

C
The sp³ hybrid orbitals have equal s and p characters.

D
The dipole moment of CH₃Cl is greater than that of CH₃F.

Solution

F is more electronegative than Cl, but due to the greater bond length of the C-Cl bond as compared to the C-F bond, the dipole moment of CH₃Cl is more than that of CH₃F.
Question 4
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Which of the following sets is correct with respect to molecule/ion, hybridisation of central atom and shape of the molecule/ion?

A
H₂S, sp³, linear

B
AsH₃, sp³, trigonal pyramidal

C
NH₄⁺, dsp², tetrahedral

D
BeCl₂, sp², linear

Solution

AsH₃: sp³ hybridization, trigonal pyramidal shape
Question 5
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Geometry of the conjugate base of NH₄⁺ ion is _________.

A
tetrahedral

B
square planar

C
trigonal pyramidal

D
linear

Solution

Conjugate base of NH₄⁺ ion is NH₃. NH₃hastrigonal pyramidal shape (sp3 hybridization; 3 shared pairs and one lone pair)
Question 6
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Which of the following statements is TRUE?

A
B-F bond is larger in BF₄^- than in BF₃.

B
FCl₃ exists whereas ClF₃ does not.

C
BF₃ is a stronger lewis acid than BBr₃.

D
NF₃ acts as donor molecule, while PF₃ shows little tendency to act as donor.

Solution

B-F bond is larger in BF₄^- than in BF₃. This is due to the fact that in BF₄^-, boron atom is sp³ hybridised, while in BF₃, boron atom is sp² hybridised and bond length decreases with increase in s-character, since s-orbital is smaller than p-orbital.
Question 7
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Which of the following sets represents molecules with zero dipole moment only?

A
BeCl₂, AlCl₃, H₂O, NH₃, CCl₄

B
HCl, BF₃, AlCl₃, SO₂, CH₄

C
BeCl₂, BF₃, AlCl₃, CO₂, CCl₄

D
CH₄, PCl₃, BF₃, CO₂, CH₄

Solution

BeCl₂, BF₃, AlCl₃, CO₂, CCl₄: All are non-polar molecules with zero dipole moment.

The dipole moment of the individual bonds is cancelled out due to the regular molecular geometry.

BeCl₂ and CO₂ have linear geometry; BF₃ and AlCl₃ have a trigonal planar geometry and CCl₄ has tetrahedral geometry.
Question 8
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Which of the following combinations of 'molecule : shape' is incorrect?

A
XeO₃: Trigonal pyramidal

B
XeOF₄: Trigonal bipyramidal

C
XeO₃F₂: Trigonal bipyramidal

D
XeO₆^4-: Octahedral

Solution

XeOF₄has square pyramidal shape.

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Re-Attempt Weekly Quiz Competition

Chemical Bonding & Molecular Structure Test - 2

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Chemical Bonding & Molecular Structure Test - 2

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Question 1

SO2, NO2-, H2O, I3-

CO2, NO2-, SO2, IF2-

CO2, NH2-, I3-, IF2-

CO2, BeCl2, I3-, IF2-

Solution

Question 2

BF3, NH3, IF3, SO32-

BF3, SO3, GaF3, NO3-

NH3, SO32-, GaF3, NO3-

BF3, SO3, GaF3, IF3

Solution

Question 3

Linear overlapping of p-orbitals forms a pi bond.

All molecules with polar bonds have a dipole moment.

The sp3 hybrid orbitals have equal s and p characters.

The dipole moment of CH3Cl is greater than that of CH3F.

Solution

Question 4

H2S, sp3, linear

AsH3, sp3, trigonal pyramidal

NH4+, dsp2, tetrahedral

BeCl2, sp2, linear

Solution

Question 5

tetrahedral

square planar

trigonal pyramidal

linear

Solution

Question 6

B-F bond is larger in BF4- than in BF3.

FCl3 exists whereas ClF3 does not.

BF3 is a stronger lewis acid than BBr3.

NF3 acts as donor molecule, while PF3 shows little tendency to act as donor.

Solution

Question 7

BeCl2, AlCl3, H2O, NH3, CCl4

HCl, BF3, AlCl3, SO2, CH4

BeCl2, BF3, AlCl3, CO2, CCl4

CH4, PCl3, BF3, CO2, CH4

Solution

Question 8

XeO3 : Trigonal pyramidal

XeOF4 : Trigonal bipyramidal

XeO3F2 : Trigonal bipyramidal

XeO64- : Octahedral

Solution

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SO₂, NO₂^-, H₂O, I₃^-

CO₂, NO₂^-, SO₂, IF₂^-

CO₂, NH₂^-, I₃^-, IF₂^-

CO₂, BeCl₂, I₃^-, IF₂^-

BF₃, NH₃, IF₃, SO₃^2-

BF₃, SO₃, GaF₃, NO₃^-

NH₃, SO₃^2-, GaF₃, NO₃^-

BF₃, SO₃, GaF₃, IF₃

The sp³ hybrid orbitals have equal s and p characters.

The dipole moment of CH₃Cl is greater than that of CH₃F.

H₂S, sp³, linear

AsH₃, sp³, trigonal pyramidal

NH₄⁺, dsp², tetrahedral

BeCl₂, sp², linear

B-F bond is larger in BF₄^- than in BF₃.

FCl₃ exists whereas ClF₃ does not.

BF₃ is a stronger lewis acid than BBr₃.

NF₃ acts as donor molecule, while PF₃ shows little tendency to act as donor.

BeCl₂, AlCl₃, H₂O, NH₃, CCl₄

HCl, BF₃, AlCl₃, SO₂, CH₄

BeCl₂, BF₃, AlCl₃, CO₂, CCl₄

CH₄, PCl₃, BF₃, CO₂, CH₄

XeO₃: Trigonal pyramidal

XeOF₄: Trigonal bipyramidal

XeO₃F₂: Trigonal bipyramidal

XeO₆^4-: Octahedral