Question

Nitrogen is a gas at room temperature while phosphorous is a solid .Explain

Answer 1

$\huge\red{\underline{{\boxed{\textbf{ANSWER}}}}}$

The size of nitrogen is quite small. As a result two nitrogen atoms can be linked to each other by three covalent bonds in order to complete the octets of both the nitrogen atoms. This diatomic molecule N2 is very stable and has very negligible attraction towards other diatomic nitrogen molecules. Thus there is weak interaction between nitrogen molecules. So nitrogen exist as gas.

While phosphorus being large in size has less tendency to form three bonds. Therefore, P atoms completes octets by sharing its valence electrons with three other P atoms. As a result, it exist as tetratomic P4 molecule. In white phosphorous there is network which holds the phosphorous atoms together. This catenation tendency of phosphorus is reason why it exist as solid.

Answer 2

Answer:

The size of nitrogen is quite small. As a result two nitrogen atoms can be linked to each other by three covalent bonds in order to complete the octets of both the nitrogen atoms. This diatomic molecule N2 is very stable and has very negligible attraction towards other diatomic nitrogen molecules. Thus there is weak interaction between nitrogen molecules. So nitrogen exist as gas.

While phosphorus being large in size has less tendency to form three bonds. Therefore, P atoms completes octets by sharing its valence electrons with three other P atoms. As a result, it exist as tetratomic P4 molecule. In white phosphorous there is network which holds the phosphorous atoms together. This catenation tendency of phosphorus is reason why it exist as solid.