Structure of White Phosphorus

Phosphorus has the electronic configuration of [Ne]3s²3p³. It has five valence electrons in its outermost shell. In its elemental form, it exists in various allotropes, such as white, red, black, and violet phosphorus. White phosphorus is the most common allotrope of phosphorus.

The structure of white phosphorus is tetrahedral. Let's understand why.

Bonding in White Phosphorus

White phosphorus consists of P₄ molecules. Each P₄ molecule contains four phosphorus atoms bonded together by covalent bonds. Each phosphorus atom forms three single covalent bonds with the other three phosphorus atoms in the molecule. The fourth valence electron of each phosphorus atom does not participate in bonding and is called a lone pair.

The covalent bond in white phosphorus is formed by the overlapping of sp³ hybrid orbitals of the phosphorus atoms. The sp³ hybrid orbitals result from the hybridization of one s orbital and three p orbitals of each phosphorus atom. The hybridization of the orbitals allows the formation of four equivalent sp³ hybrid orbitals that are oriented in a tetrahedral arrangement.

Geometry of White Phosphorus

The tetrahedral arrangement of the sp³ hybrid orbitals leads to the tetrahedral geometry of the P₄ molecule. In the tetrahedral geometry, the four phosphorus atoms are located at the corners of a tetrahedron, and the lone pairs are situated in the center of the tetrahedron.

Therefore, the structure of white phosphorus is tetrahedral, with each P₄ molecule having a tetrahedral geometry.

Conclusion

In conclusion, the structure of white phosphorus is tetrahedral due to the tetrahedral geometry of the P₄ molecule. The tetrahedral arrangement of the sp³ hybrid orbitals of the phosphorus atoms leads to the formation of the tetrahedral geometry of the molecule.