[NobleXenon]

Explain why NBr₅ does not exist.

[typhoon2028]

You should draw the lewis structure for nitrogen and bromine.

[NobleXenon]

Nitrogen could not bond to 5 Bromine because after the third bromine, nitrogen becomes full. succeeds octet.

[macman104]

Yup!

[typhoon2028]

Nitrogen could not bond to 5 Bromine because after the third bromine, nitrogen becomes full. succeeds octet.

This is probably a good enough answer for Grade 11 chemistry.  Nitrogen does have an oxidation state of 5+, as in (NO3)-, so it is capable of making five bonds.

In addition, NBr3 is not stable.  It does not exist any long period of time.

[macman104]

No, nitrogen makes 4 bonds in NO₃^-.  It is a 2nd row element, and for most purposes (only because there may be some exotic chemistry I'm unaware of), nitrogen is unable to become hypervalent and have more than 8 electrons.

[typhoon2028]

No, nitrogen makes 4 bonds in NO₃^-.  It is a 2nd row element, and for most purposes (only because there may be some exotic chemistry I'm unaware of), nitrogen is unable to become hypervalent and have more than 8 electrons.

My information comes from Creighton University website.  I wasn't implying nitrogen would have more than 8 electrons, but have an oxidation state of 5+ (thereby losing electrons).

http://mattson.creighton.edu/InorganicChemWeb/

[macman104]

Yes, but you are mixing oxidation state and bonds formed.  I understand that it has an oxidation state of +5, but that doesn't mean it has 5 bonds to it.