Arrange the bonds in order of increasing ionic character in the molecules: LiF, K₂O , N₂, SO₂ and ClF₃ .

2

(a)

Arrange the following bonds in order of increasing ionic character giving reason. N-H, F-H, C-H and O-H

2

(a)

Arrange the following in order of decreasing bond angle, giving reason NO₂, \(NO_{ 2 }^{ + }\) and \(NO_{ 2 }^{ - }\)

2

(a)

Explain the shape of BrF₅

2

(a)

Why does formic acid exist as dimer? What is its one consequence?

2

(a)

Explain the formation of a chemical bond.

2

(a)

The skeletal structure of CH₃COOH as shown below is correct, but some of the bonds are shown incorrectly. Write the correct Lewis structure for acetic acid

2

(a)

Considering x-axis as the internuclear axis which out of the following will not form a sigma bond and why?
(a) 1s and 1s
(b) 1s and 2p_x ;
(c) 2p_y and 2p_y
(d) 1s and 2s.

2

(a)

How is bond order related to the stability of a molecule?

2

(a)

Write the type of hybridization involved in CH₄ C₂H₄ and C₂H_2.

2

(a)

Why B₂ is paramagnetic in nature while C₂ is not?

2

(a)

The molecular orbital electronic configuration of both B₂ and C₂ are.
B₂: [σ1s]² [σ*1s]² [σ2s]² [σ*2s]² [\(\pi\) 2px]¹ [\(\pi\)2y]¹
C₂: [σ1s]² [σ*1s]² [σ2s]² [σ*2s]² [\(\pi\) 2px]² [\(\pi\)2y]²
Since, B₂ has two unpaired electrons, B₂ is paramagnetic.
C₂ has no unpaired electron. Thus, C₂ is diamagnetic

What do you mean by Dipole moment? Draw the dipole diagram of H₂O.

2

(a)

Define bond order. How is it related to the stability of a molecule

2

(a)

Explain the diamagnetic behaviour of F₂ molecule on the basis of molecular orbital theory

2

(a)