Bond Hybridization?

Question

I don't understand hybridization really and i have to explain why nitrogen trifluoride and phosphoruos pentafluoride are stable molecules and how nitrogen pentafluoride does not exist.

Can someone explain how hybridization works by explaining them?

Answer 1

Hybridisation or hybridization (see also spelling differences) is the concept of mixing atomic orbitals to form new hybrid orbitals suitable for the qualitative description of atomic bonding properties. Hybridised orbitals are very useful in the explanation of the shape of molecular orbitals for molecules. It is an integral part of valence bond theory.
Remember: nitrogen is in the second period where only S and P orbits are allowed. Phospher is in the third period where S, P, and D orbits are allowed. Therefore, nitrogen may have SP3 hybridization, but not SP3D2 hybridization, while phospher has 5 valence shell electrons and it can have SP3D2 hybridization to form 5 bonds with 5 fluorine atoms. Nitrogen can have SP3 hybridization, form three bonds with fluorine atoms thus a total 8 electrons in the valence shell.