Between white & red phosphorus which one is more reactive & why?

Explanation

White phosphorus is a tetrahedral `(P_(4))` molecule in which the four P atoms are linked to each other by single covalent bonds. These `(P_(4))` molecules are held together by weak van der Waals forces of attraction. In each `(P_(4))` molecule, the P - P - P bond angle ( 60°) is less than that between two pure p -orbitals `(90^(@))` and hence, it suffers from internal angle strain. Due to weaker forces of attraction and considerable angle strain, white phosphorus is very reactive. On the other hand, in red phosphorus, these `P_(4)` tetrahedra are joined together through covalent: bonds to give a polymeric structure. ln this structure, the angle strain is relatively low (average P - P- P bond angle: `101^(@)`) and as a result, the P-P bonds become relatively stronger. Since greater amount of energy is required to convert these giant molecules into atoms by breaking relatively stronger covalent bonds, therefore white phosphorus is more reactive than red phosphorus.