The bond order for a species with the configuration $\sigma 1s^2<mspace\; width="1em"></mspace>\sigma *1s^2<mspace\; width="1em"></mspace>\sigma 2s^2<mspace\; width="1em"></mspace>\sigma *2s^2<mspace\; width="1em"></mspace>\sigma {{\rho }^1}_x$ will be

1.  1

2.  $\frac{1}{2}$

3.  Zero

4.  3/2

Which molecule is least likely to form hydrogen bonds? 

Which of the following compounds has zero dipole moment?

1.  ${\mathrm{NH}}_3$

2.  ${\mathrm{NF}}_3$

3.  ${\mathrm{BF}}_3$

4.  ${\mathrm{CHCl}}_3$

The bond order of ${\mathrm{NO}}^{+}$ ion is

1.  1

2.  2

3.  2.5

4.  3

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