The axial bonds are longer as compared to equatorial bonds in PCl₅ because:

1.	Axial bond pairs suffer more repulsion from the equatorial bond pairs
2.	Equatorial bond pairs suffer more repulsion from the axial bond pairs
3.	Both 1, and 2
4.	None of the above

The relation between hydrogen bond and the van der Waals forces is:

If the main axis of a diatomic molecule is z, then the molecular orbital p_x and p_y overlap to form which of the following orbital:

1.  $\mathrm{\pi }$ molecular orbtial
2.  σ molecular orbital
3.  δ molecular orbtial
4.  No bond will form

The significance of the octet rule is:

1. To determine the stability of atoms.
2. To find the hybridization of elements.
3. To calculate the number of lone pairs.
4. None of the above.

The incorrect statement among the following is:

The correct Lewis structure of acetic acid is:

1.		2.
3.		4.	None of the above.

H₂ molecule on the basis of valence bond theory is formed due to:

1. Attractive forces being more than the repulsive forces.

2. Attractive forces being less than the repulsive forces.

3. No force of attraction.

4. Only repulsive force.

Hybridization of C₁ and C₂  in the structure given below are

1. ${\mathrm{C}}_1 = {\mathrm{sp}}^3 , {\mathrm{C}}_2= {\mathrm{sp}}^2$

2. ${\mathrm{C}}_1 = {\mathrm{sp}}^3 , {\mathrm{C}}_2= {\mathrm{sp}}^3$

3. ${\mathrm{C}}_1 = {\mathrm{sp}}^2 , {\mathrm{C}}_2= {\mathrm{sp}}^3$

4. ${\mathrm{C}}_1 = {\mathrm{sp}}^2 , {\mathrm{C}}_2= {\mathrm{sp}}^2$

Consider the following structure.

The hybridization of C₁, and C₂ carbon in the structure are -

1. $C_1$ = ${\mathrm{sp}}^2$ , ${\mathrm{C}}_2$ =  $s{p}^2$

2. $C_1$ = ${\mathrm{sp}}^3$ , ${\mathrm{C}}_2$ = ${\mathrm{sp}}^3$

3. $C_1$ = ${\mathrm{sp}}^3$ , ${\mathrm{C}}_2$ = ${\mathrm{sp}}^2$

4. None of the above

The number of resonating structures exhibited by \(CO^{2-}_3\) ion are :