Question

(a) Account for the following :
(i) Interhalogens are more reactive than pure halogens.
(ii) $N_2$ is less reactive at room temperature.
(iii) Reducing character increases from $N{H}_3$ to $Bi{H}_3$.

(b) Draw the structures of the following :
$\left(i\right)H_4{P}_2{O}_7$ (Pyrophosphoric acid)
$\left(ii\right)Xe{F}_4$

Answer 1

(a) (i) This is because the bond in the interhalogen (X - X') is weaker than X -X and X' - X' bond in the halogens. This is due to less effective overlapping between orbitals of dissimilar atoms than those between similar atoms.

(ii) $N_2$ is less reactive at room temperature due to its high bond dissociation energy $(N\equiv N$ bond).

(iii) As we move from $N{H}_3$ to $Bi{H}_3$, the thermal stability of hydrides decreases and their tendency to liberate hydrogen increases. Hence, the reducing character increases from $N{H}_3$ to $Bi{H}_3$.