The right order of increase in the ionic character of the molecules,
 LiF, K₂O, N₂, SO₂, ClF₃ is :

1. N₂ < SO₂ < ClF₃ < K₂O < LiF

2. N₂ > SO₂ > ClF₃ > K₂O < LiF

3. N₂ > SO₂ > ClF₃ > K₂O > LiF

4. LiF > K₂O < ClF₃ > SO₂ > N₂

The molecule among the following having the highest dipole moment is:

1. CO₂
2. HI
3. H₂O
4. SO₂

The correct order of the boiling points of \(\mathrm{H}_2 \mathrm{O}, \mathrm{HF}, \text{ and} \ \mathrm{NH}_3\) is: 

1. HF > H₂O > NH₃

2. H₂O > HF > NH₃

3. NH₃ > HF > H₂O

4. NH₃ > H₂O > HF

In ${\mathrm{NO}}_3^{-}$ ion, the number of bond pairs and lone pairs of electrons exhibited by nitrogen atom is:

1. 2, 2

2. 3, 1

3. 1, 3

4. 4, 0

The number of $\mathrm{\pi }$ bonds and $\mathrm{\sigma }$ bonds in the following structure is :

Hydrogen bond will be strongest in : 

1. HCl

2. H₂O

3. HI

4. H₂S

If the electronic configuration of an element is $1{\mathrm{s}}^{2}2{\mathrm{s}}^{2}2{\mathrm{p}}^{6}3{\mathrm{s}}^{2}3{\mathrm{p}}^{6}3{\mathrm{d}}^{2}4{\mathrm{s}}^2$, the four electrons that participate in the chemical bond formation will be from :

1. $3{\mathrm{p}}^6$

2. $3{\mathrm{p}}^6, 4{\mathrm{s}}^2$

3. $3{\mathrm{p}}^6, 3{\mathrm{d}}^2$

4. $3{\mathrm{d}}^2, 4{\mathrm{s}}^2$

The correct bond angle for \(\mathrm{sp}^2\) hybridization is:

The electronic configurations of the elements A, B, and C are given below.

$\mathrm{A} = 1{\mathrm{s}}^2 2{\mathrm{s}}^2 2{\mathrm{p}}^6$
$\mathrm{B} = 1{\mathrm{s}}^2 2{\mathrm{s}}^2 2{\mathrm{p}}^6 3{\mathrm{s}}^2 3{\mathrm{p}}^3$
$\mathrm{C} = 1{\mathrm{s}}^2 2{\mathrm{s}}^2 2{\mathrm{p}}^6 3{\mathrm{s}}^2 3{\mathrm{p}}^5$

The stable form of A may be represented by the formula: