The order of electronegativity of carbon in sp, ${\mathrm{sp}}^2 \mathrm{and} {\mathrm{sp}}^3$ hybridized states follows:

1. $\mathrm{sp}>{\mathrm{sp}}^2>{\mathrm{sp}}^3$

2. ${\mathrm{sp}}^3>{\mathrm{sp}}^2>\mathrm{sp}$

3. $\mathrm{sp}>{\mathrm{sp}}^3>{\mathrm{sp}}^2$

4. ${\mathrm{sp}}^2>\mathrm{sp}>{\mathrm{sp}}^3$

The diamagnetic species among the following is:

1. NO

2. ${\mathrm{NO}}_2$

3. ${\mathrm{O}}_2$

4. ${\mathrm{CO}}_2$

Among the following atomic orbital overlaps, the non-bonding overlap is:
 

1.		2.
3.		4.

The correct structure of $PC{l}_3{F}_2$ is

1. 

2. 

3. 

4.   

The compounds containing sp hybridized carbon atoms are: 

i.		ii.
iii.	${\mathrm{H}}_3\mathrm{C}-\mathrm{CN}$	iv.	${\mathrm{H}}_2\mathrm{C}=\mathrm{C}={\mathrm{CHCH}}_3$

1. i and ii

2. iii and iv

3. ii and iii

4. i and iv

The hybridization of the central atom and the shape of ${\left[{\mathrm{lO}}_2{\mathrm{F}}_5\right]}^{2-}$ ion, respectively, are

1.  $s{p}^3{d}^3$

2.  $s{p}^2{d}^4$

3.  $s{p}^2{d}^4$

4.  $s{p}^3{d}^3$

Which of the following contain a maximum number of electrons in the antibonding molecular orbitals?

Which of the following compounds has the least tendency to form hydrogen bonds between molecules?

1.  ${\mathrm{NH}}_3$

2.  ${\mathrm{H}}_2\mathrm{NOH}$

3.  HF

4.  ${\mathrm{CH}}_3\mathrm{F}$

Assuming that Hund's rule is violated by the diatomic molecule $B_2$, its bond order and magnetic nature will be respectively

1.  1, diamagnetic

2.  1, paramagnetic

3.  2, diamagnetic

4.  2, paramagnetic

In the Lewis structure of ozone $\left({\mathrm{O}}_3\right)$ the formal charge on the central oxygen atom is:  

1.  +1

2.  -1

3.  0

4.  -2