The incorrect statement among the following is:

1.	The sigma bond forms via head-on overlap and the pie bond forms via sidewise overlapping of orbitals.
2.	s and p orbitals combine to form a sigma bond as well as a pie bond.
3.	Hybrid orbitals form sigma bonds only.
4.	Sigma bonds are stronger than pie bonds.

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 :

The condition(s) required for the linear combination of atomic orbital is :

The following graph captures potential energy on the y-axis for hydrogen gas formation as a function of the internuclear distance on the x-axis:
        
The bond energy of H₂ can be represented by:

BF₃ is a planar and an electron deficient compound. Hybridization and number of electrons around the central atom, respectively are: 
1. sp² and 6
2. sp² and 8
3. sp³ and 4
4. sp³ and 6

Match List - I with List - II

Choose the correct answer from the options given below: