Chapter 9, Problem 94AP

The stable allotropic form of phosphorus is ${\text{P}}_{\text{4}}$, in which each P atom is bonded to three other P atoms. Draw a Lewis structure of this molecule and describe its geometry. At high temperatures. ${\text{P}}_{\text{4}}$ dissociates to form ${\text{P}}_{\text{2}}$ molecules containing a $\text{P=P}$ bond. Explain why ${\text{P}}_{\text{4}}$ is more stable than ${\text{P}}_{\text{2}}$.