Question
Why is the $\mathrm{P}_{4}$ molecule unstable?
Step 1
This means that each phosphorus atom is bonded to three other phosphorus atoms. This can be represented as: \[ \begin{array}{ccc} & \mathrm{P} \\ & | \\ \mathrm{P}-\mathrm{P}-\mathrm{P} \end{array} \] Show more…
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The stable allotropic form of phosphorus is $P_{4},$ 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, $\mathrm{P}_{4}$ dissociates to form $\mathrm{P}_{2}$ molecules containing a $\mathrm{P}=\mathrm{P}$ bond. Explain why $\mathrm{P}_{4}$ is more stable than $\mathrm{P}_{2}$.
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