Answer to Question #248179 in Inorganic Chemistry for orange

Question

The common forms of nitrogen and phosphorus are N₂(g) and P₄(s) respectively. Account for the difference in terms of the single and multiple bond enthalpies.

I would like to know how to explain, thanks!!

Answer 1

In order for phosphorous to form a double bond with itself it requires more an ethalpy of N=N 418kJ/mol rather than P=P 489kJ/mol and is even more true for a double bond. So phosphorous would rather be in a P4 formation because P-P single bonds only require 197kJ/mol