101The extent of overlapping of d orbital of Phosphorus and 1s orbital of H is very less becoz the energy difference between them is too high for favourable bond formation so at the most 1s of H can interact considerably with p orbitals that is why PH3 exists whereas u don't see PH5 as d-s overlapping is less so it dissociates into PH3 and H2...
101because it does not have a d-orbital !!
since it has its last configuration 3p3 soo.. it can only form 3 bonds! :)
Jeet Sen Sharma phosphorus has a d orbital !!!!!!!!101okkk im srry..i just thot abt nitrogen thr... PH5 is possible..!!
as it has 3d orbitals..!!
101noppee.. studied today in details abt yy PH5 is not possi..
Jeet Sen Sharma yyyy
41Phosphorus can form bonds to five ligands, as in PF5 or PCl5, by using its d-orbitals. However, this becomes much stable if you involve pi-overlap with p-orbitals on the ligands. F and Cl have p-orbitals and that's why they form stable PF5 or PCl5. On the other side H do not have p-orbital, instead it has only s-orbitals and that's why it forms much less stable s-d bonds.
So, PH5 can exist but it won't be stable, because PH5 splits too easily into the more stable PH3 and H2.