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  • Why can't Nitrogen (N) form five-coordinate compounds using  hybridization?

Why can't Nitrogen (N) form five-coordinate compounds using \mathrm{sp^{3}d} hybridization?

Option: 1

Nitrogen lacks available d orbitals in its outermost shell.


Option: 2

Nitrogen is too large to accommodate five substituents without crowding.


Option: 3

Nitrogen has too many electrons in its outermost shell.


Option: 4

Nitrogen forms stable compounds with only four covalent bonds.


Answers (1)

best_answer

As there are no d-orbitals available in the Nitrogen valence shell, for which there is no way to arrange five pairs of bonding electrons around a nitrogen atom, and formation of five bonds.

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Rishabh

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