Which of the following reasons explains why nitrogen pentafluoride (NF 5 ) does not exist, whereas phosphorus pentafluoride (PF 5 ) is stable?

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Chemistry · Chemical Bonding

Verified Solution4 OptionsUpdated: October 2026👁️1 View

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Correct answer

Nitrogen lacks vacant d-orbitals in its valence shell to expand its octet.

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Answer 1

Nitrogen cannot form more than three covalent bonds under any conditions.

Answer 2

The N-F bond is too weak to support a pentafluoride structure.

Answer 3

Nitrogen is too electronegative to form a stable NF 5 molecule.

Answer 4

Nitrogen lacks vacant d-orbitals in its valence shell to expand its octet.

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