What happens when $\mathrm{Phosphorous}$ burns in $\mathrm{Oxygen}$ ?

• The non-metal $\mathrm{Phopsphorous}\left(\mathrm{P}\right)$ burns in $\mathrm{Oxygen}$ with intense flame and produces white fumes of oxide.
• The reaction between $\mathrm{Phopsphorous}\left(\mathrm{P}\right)$ and $\mathrm{Oxygen}\left({\mathrm{O}}_2\right)$ is an example of an oxidation reaction, because the reaction involves the formation of$\mathrm{Phosphorous}\mathrm{pentoxide}\left({\mathrm{P}}_2{\mathrm{O}}_5\right)$.
• These proprieties of combustion $\mathrm{Phopsphorous}\left(\mathrm{P}\right)$ have led to its use in bombs and crackles.

Chemical equation

$\underset{\mathrm{Phosphorous}}{{\mathrm{P}}_4\left(\mathrm{s}\right)}+\underset{\mathrm{Oxygen}}{5{\mathrm{O}}_2\left(\mathrm{g}\right)}\to \underset{\mathrm{Phosphorous}\mathrm{pentoxide}}{2{\mathrm{P}}_2{\mathrm{O}}_5\left(\mathrm{g}\right)}$