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Nitrogen froms a trifluoride, NF3, but Nf5 does not exist. For phosphorous, both PF3 and PF5...

Nitrogen froms a trifluoride, NF3, but Nf5 does not exist. For phosphorous, both PF3 and PF5 are known. Write Lewis structures for NF3, PF3 and PF5 discuss possible explanations for the fact that PF5 is stable, whereas NF5 is not (keep periodic trends in mind when doing this).
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(NF3, PF3, PF5)uploaded image

 

NF5 cannot exist because nitrogen (N) is on the second period (row) of the periodic table. Any element on the second row CANNOT have more than 4 other atoms attached to it no matter what. For PF5 on the other hand, phosphorus (P) is on a higher period (row) within the periodic table. Hence, it has more valence shells to accept electrons from other atoms so it may sustain more than 4.

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