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.  ${\mathrm{Li}}_2 < {{\mathrm{He}}_2}^{+} < {{\mathrm{O}}_2}^{+} < {\mathrm{C}}_2$

2.  ${\mathrm{C}}_2 < {{\mathrm{O}}_2}^{+} < {\mathrm{Li}}_2 < {{\mathrm{He}}_2}^{+}$

3.  ${{\mathrm{He}}_2}^{+}< {\mathrm{Li}}_2< {\mathrm{C}}_2 < {{\mathrm{O}}_2}^{+}$

4.  ${{\mathrm{O}}_2}^{+} < {\mathrm{C}}_2 < {\mathrm{Li}}_2 < {{\mathrm{He}}_2}^{+}$

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.  ${\mathrm{NH}}_3 \mathrm{and} {\mathrm{BF}}_3$

2.  ${{\mathrm{BF}}_4}^{-} \mathrm{and} {{\mathrm{NH}}_4}^{+}$

3.  ${\mathrm{BCl}}_3 \mathrm{and} {\mathrm{BrCl}}_3$

4.  ${\mathrm{NH}}_3 \mathrm{and} {{\mathrm{NO}}_3}^{-}$

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.  ${{\mathrm{O}}_2}^{-2}$

Lattice energy for an ionic compound is calculated by using

1.  Kirchhoff's equation

2.  Markownikoff's rule

3.  Born Haber cycle

4.  Carnot cycle

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