The linear molecule among the following is

1.  ${\mathrm{CO}}_2$

2.  ${\mathrm{NO}}_2$

3.  ${\mathrm{SO}}_2$

4.  ${\mathrm{ClO}}_2$

The molecule having the highest dipole moment is

1.  ${\mathrm{CO}}_2$

2.  ${\mathrm{CH}}_4$

3.  ${\mathrm{NH}}_3$

4.  ${\mathrm{NF}}_3$

The species which has triangular planar geometry is

1.  ${\mathrm{NF}}_3$

2.  ${{\mathrm{NO}}_3}^{-}$

3.  ${{\mathrm{BF}}_4}^{-}$

4.  ${\mathrm{SbH}}_3$

The correct sequence of stability for the given molecular species (from the given options) is:

1.  ${\mathrm{Li}}_2<mspace\; width="1em"></mspace><<mspace\; width="1em"></mspace>{{\mathrm{He}}_2}^{+}<mspace\; width="1em"></mspace><<mspace\; width="1em"></mspace>{{\mathrm{O}}_2}^{+}<mspace\; width="1em"></mspace><<mspace\; width="1em"></mspace>{\mathrm{C}}_2$

2.  ${\mathrm{C}}_2<mspace\; width="1em"></mspace><<mspace\; width="1em"></mspace>{{\mathrm{O}}_2}^{+}<mspace\; width="1em"></mspace><<mspace\; width="1em"></mspace>{\mathrm{Li}}_2<mspace\; width="1em"></mspace><<mspace\; width="1em"></mspace>{{\mathrm{He}}_2}^{+}$

3.  ${{\mathrm{He}}_2}^{+}<<mspace\; width="1em"></mspace>{\mathrm{Li}}_2<<mspace\; width="1em"></mspace>{\mathrm{C}}_2<mspace\; width="1em"></mspace><<mspace\; width="1em"></mspace>{{\mathrm{O}}_2}^{+}$

4.  ${{\mathrm{O}}_2}^{+}<mspace\; width="1em"></mspace><<mspace\; width="1em"></mspace>{\mathrm{C}}_2<mspace\; width="1em"></mspace><<mspace\; width="1em"></mspace>{\mathrm{Li}}_2<mspace\; width="1em"></mspace><<mspace\; width="1em"></mspace>{{\mathrm{He}}_2}^{+}$

From the given structures, the correct structure(s) of ${\mathrm{F}}_3{\mathrm{Cl}}_2$ is are

l.  

ll.  

lll.  

1.  Only l

2.  Only ll

3.  Only lll

4.  l, ll and lll

The pair that is isostructural (i.e. having the same shape and hybridization) is

1.  ${\mathrm{NH}}_3<mspace\; width="1em"></mspace>\mathrm{and}<mspace\; width="1em"></mspace>{\mathrm{BF}}_3$

2.  ${{\mathrm{BF}}_4}^{-}<mspace\; width="1em"></mspace>\mathrm{and}<mspace\; width="1em"></mspace>{{\mathrm{NH}}_4}^{+}$

3.  ${\mathrm{BCl}}_3<mspace\; width="1em"></mspace>\mathrm{and}<mspace\; width="1em"></mspace>{\mathrm{BrCl}}_3$

4.  ${\mathrm{NH}}_3<mspace\; width="1em"></mspace>\mathrm{and}<mspace\; width="1em"></mspace>{{\mathrm{NO}}_3}^{-}$

Which of the following represents the correct order of dipole moment?

1.  ${\mathrm{NH}}_3 > {\mathrm{NF}}_3 > {\mathrm{H}}_2\mathrm{O}$

2.  ${\mathrm{NH}}_3 > {\mathrm{H}}_2\mathrm{O} >{\mathrm{NF}}_3$

3.  ${\mathrm{H}}_2\mathrm{O} > {\mathrm{NH}}_3>{\mathrm{NF}}_3$

4.  ${\mathrm{H}}_2\mathrm{O} >{\mathrm{NF}}_3> {\mathrm{NH}}_3$

Which of the following has the shortest bond length?

1.  ${\mathrm{O}}_2$

2.  ${{\mathrm{O}}_2}^{-}$

3.  ${{\mathrm{O}}_2}^{+}$

4.  ${{\mathrm{O}}_2}^{-2}$

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