Question

In ${P_4}{O_{10}}$find the number of oxygen atoms bonded to each phosphorus atom.

Answer 1

In the question we know that the phosphorus is bonded to oxygen atoms. The number of oxygen atoms are ten, but it is not necessary that all are bonded to phosphorus. There are only four phosphorus in the given molecule ${P_4}{O_{10}}$.

Complete step by step answer:
To know how-many oxygen is bonded to phosphorus let's draw the structure. We have to know how it is formed.

The structure as shown in the above figure contains four phosphorus atoms and ten oxygen atoms. The${P_4}{O_{10}}$ is formed by the combustion reaction between tetra phosphorus in the presence of oxygen. The reaction is as follows: ${P_4}\; + {\rm{ }}5{O_2}\; \to {\rm{ }}{P_4}{O_{10}}$ here the phosphorus is white allotrope of phosphorus.
Another way of formation of ${P_4}{O_{10}}$is by combining the two molecules of ${P_2}{O_5}$. Hence, ${P_4}{O_{10}}$is also called a dimer of ${P_2}{O_5}$. The hexagonal cell of a molecule of phosphorus pentoxide is bonded together by weak van der Waals forces, known as the electrostatic attraction between molecules of ${P_2}{O_5}$. The Dimer of Phosphorus pentoxide contains $6{\rm{ }}P-O-P$ bonds and $4{\rm{ }}P = O$ bonds. The dipole-dipole interactions of the $P-O-P$ bonds are what keep the molecule together. $P-O-P$ bonds are polar with a negative valence on the oxygen atom. The empirical formula of ${P_4}{O_{10}}$ is ${P_2}{O_5}$. The relation between the empirical formula and molecular formula is molecular formula is n times empirical formula {P_4}{O_{10}}$$$$ = \;2({P_2}{O_5}). Same as the empirical formula of benzene and methane are carbon and hydrogen $CH$. It is also known as phosphorus pentoxide, phosphoric anhydride, and tetra phosphorus decaoxide, whereas phosphorus pentoxide is a common name.
Hence, the number of oxygen atoms bonded to each Phosphorus atom is four.

Note:
Do not get confused with the number of oxygen atoms that are bonded to two phosphorus atoms.