Question

Explain the following
a. Bi(V) is a stronger oxidizing agent than Sb(V)
b. Unlike phosphorus, nitrogen shows little tendency for catenation?
c. Halogens have maximum negative electron gain enthalpy in the respective period why?

Answer 1

a. Due to the presence of orbital electrons in $Bi$, its $+3$ is more stable than $Sb(+3)$, since $Bi\left(V\right)$ is undergoing self reduction, hence it is a stronger oxidising agent then $Sb\left(V\right)$.

b. Since nitrogen atom is smaller, there is greater repulsion of electron density of two nitrogen atoms, thereby weakening the $N-N$ single bond. Catenation is much more common in phosphorous compounds than in nitrogen compounds.

C. This is due to their small size and higher effective nuclear charge. Due to these two parameters halogens easily gain one electron to complete their octet and attain Noble gas configuration.