Chemical Bonding and Molecular Structure Test

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Chemical Bonding and Molecular Structure Test - 1

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Weekly Quiz Competition

Question 1
4 / -1

The correct order of decreasing bond lengths of CO, CO₂and C0₃^2- is

A
CO > CO₂> CO^2-₃

B
CO^2-₃> CO₂> CO

C
CO₂ > CO >CO^2-₃

D
CO₂ > CO^2-₃ >CO

Solution

As the bond order increases, bond length
decreases.
Question 2
4 / -1

The correct sequence of bond length in single bond,double bond and triple bond of C 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

Solution
Question 3
4 / -1

Which of the following willbe the strongest bond?

A
F—O

B
O —Cl

C
N —H

D
O —H

Solution

Bond strength ∝ Difference in electronegativity
of atoms
Question 4
4 / -1

Arrange the following in increasing order of covalent character - NaCl, MgCl₂, AICI₃

A
NaCl < MgCl₂ < AICI₃

B
MgCl₂ 3

C
AICI₃ < MgCl₂ < NaCl

D
NaCl < AlCl₃< MgCl₂

Solution

Cation size is decreasing in the order:
Ne⁺ > Mg²⁺ > Al³⁺
Al³⁺ has maximum polarisation effect and Na⁺
has minimum polarisation effect.
The covalent nature is in the order : AlCl₃ > MgCl₂ > NaCl
Question 5
4 / -1

Match the bond enthalpies given in column II with the molecules given in column I and mark the appropriate choice.

A
(A)→(i), (B)→(ii), (C)→(iii)

B
(A)→(iii), (B)→(ii), (C)→(i)

C
(A)→(i), (B)→(iii), (C)→(ii)

D
(A)→(iii), (B)→(i), (C)→(ii)

Solution

The order of bond enthalpies of the bonds is
given as. Bond order ∝ Bond enthalpy
Hence, single bond enthalpy < double bond enthalpy < triple bond enthalpy
H − H < O = O < N ≡ N
Question 6
4 / -1

The given structures I, II and III of carbonate ion represent

A
hybrid structures

B
isomeric structures

C
canonical structures

D
dipole structures.

Solution

The structures represent canonical or resonating structures of carbonate ion.
Question 7
4 / -1

Which of the following molecules does not show any resonating structures?

A
NH₃

B
Co^2-₃

C
O₃

D
SO₃

Solution

NH₃ does not show any resonating structure due to the absence of double bond.
Question 8
4 / -1

The canonical or resonating structures of a molecule required to describe the structure of a molecule follow which of the following rules?

A
The relative position of all atoms can differ.

B
The same number of unpaired and paired electrons in all structures.

C
Theen ergyof each structure is different.

D
Like charges are present on adjacent atoms.

Solution

Canonical structures differonly in the position
of electrons not in number of paired and unpaired electrons.
Question 9
4 / -1

Arrange the following in order of increasing dipole moment: H₂O, H₂S,BF₃

A
BF₃ < H₂S < H₂O

B
H₂S < BF₃ < H₂O

C
H₂O < H₂S < BF₃

D
BF₃ < H₂O < H₂S

Solution

In BF₃, dipole moment is zero due to its
symmetrical structure. Summations of all dipoles is zero.
In H₂S and H₂O due to unsymmetrical structure net +ve dipole is there. H₂O has a higher dipole due to the higher electronegativity of oxygen than sulphur.
Question 10
4 / -1

Which of the following is non-polar?

A
SO₂

B
CO₂

C
H₂O

D
NH₃

Solution

Since the dipoles are in opposite directions, the net dipole moment is zero.
Question 11
4 / -1

Although F is more electronegative than H, the resultant dipole moment of NH₃is much more than that of NF₃. It can be explained as

A
the lone pair of nitrogen opposes the dipole moment of NF₃ while it is added to the dipole moment of NH₃

B
all the dipoles of NF₃ are in same direction

C
all the dipoles of NH₃ are in opposite direction

D
NH₃ has a regular geometry while NF₃ has irregular geometry which makes dipole moment of NH₃ more than NF₃.

Solution
Question 12
4 / -1

In a diatomic molecule the bond distance is 1X10^-8 cm. Its dipole moment is 1.2 D. What is the fractional electronic charge on each atom?

A
0.50

B
1.2 x 10^-10

C
0.25

D
1.2

Solution

(4.8 X10^-10 is a theoretical value of μ..)
Question 13
4 / -1

Which of the following are arranged in the decreasing order of dipole moment?

A
CH₃CI, CH₃Br. CH₃F

B
CH₃CI, CH₃F, CH₃Br

C
CH₃Br. CH₃CI, CH₃F

D
CH₃Br, CH₃F, CH₃CI

Solution

The values of dipole moments of methyl halides:
Question 14
4 / -1

In water molecule, the two O—H bonds are oriented at an angle of 104.5°. In BF₃, the tliree B—F bonds are oriented at an angle of 120°. In BeF₂, the two Be—F bonds are oriented at an angle of 180°. Which of the following will have highest dipole moment?

A
BeF₂

B
BF₃

C
H₂O

D
All have zero dipole moment

Solution

BeF2 : μ = 0
Question 15
4 / -1

What is the correct dipole moment of NH₃ and NF₃respectively?

A
4.90 x 10^-30 C m and 0.80 x10^-30 C m

B
0.80 X10^-30 C m and 4.90 x 10^-30 C m

C
4.90 x 10^-30C m and 4.90 x 10^-30 C m

D
0.80X10^-30 C m and 0.80 x 10^-30 C m

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Chemical Bonding and Molecular Structure Test - 1

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Question 1

CO > CO2 > CO2-3

CO2-3 > CO2 > CO

CO2 > CO >CO2-3

CO2 > CO2-3 >CO

Solution

Question 2

(C—C) = (C = C) = (C≡C)

C ≡ C< C = C< C—C

C—C < C = C < C ≡ C

C = C< C ≡ C < C — C

Solution

Question 3

F—O

O —Cl

N —H

O —H

Solution

Question 4

NaCl < MgCl2 < AICI3

MgCl2 3

AICI3 < MgCl2 < NaCl

NaCl < AlCl3 < MgCl2

Solution

Question 5

(A)→(i), (B)→(ii), (C)→(iii)

(A)→(iii), (B)→(ii), (C)→(i)

(A)→(i), (B)→(iii), (C)→(ii)

(A)→(iii), (B)→(i), (C)→(ii)

Solution

Question 6

hybrid structures

isomeric structures

canonical structures

dipole structures.

Solution

Question 7

NH3

Co2-3

O3

SO3

Solution

Question 8

The relative position of all atoms can differ.

The same number of unpaired and paired electrons in all structures.

Theen ergyof each structure is different.

Like charges are present on adjacent atoms.

Solution

Question 9

BF3 < H2S < H2O

H2S < BF3 < H2O

H2O < H2S < BF3

BF3 < H2O < H2S

Solution

Question 10

SO2

CO2

H2O

NH3

Solution

Question 11

the lone pair of nitrogen opposes the dipole moment of NF3 while it is added to the dipole moment of NH3

all the dipoles of NF3 are in same direction

all the dipoles of NH3 are in opposite direction

NH3 has a regular geometry while NF3 has irregular geometry which makes dipole moment of NH3 more than NF3.

Solution

Question 12

0.50

1.2 x 10-10

0.25

1.2

Solution

CO > CO₂> CO^2-₃

CO^2-₃> CO₂> CO

CO₂ > CO >CO^2-₃

CO₂ > CO^2-₃ >CO

NaCl < MgCl₂ < AICI₃

MgCl₂ 3

AICI₃ < MgCl₂ < NaCl

NaCl < AlCl₃< MgCl₂

NH₃

Co^2-₃

O₃

SO₃

BF₃ < H₂S < H₂O

H₂S < BF₃ < H₂O

H₂O < H₂S < BF₃

BF₃ < H₂O < H₂S

SO₂

CO₂

H₂O

NH₃

the lone pair of nitrogen opposes the dipole moment of NF₃ while it is added to the dipole moment of NH₃

all the dipoles of NF₃ are in same direction

all the dipoles of NH₃ are in opposite direction

NH₃ has a regular geometry while NF₃ has irregular geometry which makes dipole moment of NH₃ more than NF₃.

1.2 x 10^-10

CH₃CI, CH₃Br. CH₃F

CH₃CI, CH₃F, CH₃Br

CH₃Br. CH₃CI, CH₃F

CH₃Br, CH₃F, CH₃CI

BeF₂

BF₃

H₂O

4.90 x 10^-30 C m and 0.80 x10^-30 C m

0.80 X10^-30 C m and 4.90 x 10^-30 C m

4.90 x 10^-30C m and 4.90 x 10^-30 C m

0.80X10^-30 C m and 0.80 x 10^-30 C m