I read that diphosphorus has 2 phosphorus atoms joined by a triple bond (ie) it has one sigma bond and 2 pi bonds with 2 lone pairs ( 1 lone pair on each atom). I'm confused about the hybridization of the orbitals. Phosphorus in excited state has one 3s orbital, three 3p orbitals and one d orbital .
If sp2 hybridization takes place, it will form one sigma bond and what about the other 2 hybridized orbitals what would become of them? I'm confused on the lone pair part :/
If the above even took place, would the unhybridized p orbital form pi bond with the unhybridized p orbital of the other phosphorus. And the same would go for the 2 d orbitals. Am I correct on this??
Here it says that "Diatomic molecules don't need hybridisation that is phosphorus would be using p pi p pi bonding which it could never do cuz of large diffuse orbitals !!