Just a chemistry question.

[Zzz]

Hey!

I just wanted to discuss a chemistry-related question with you guys and any response is appreciated!

So:
- Why does Nitrogen, such an inert gas, have so many oxidation states (-3, -2, -1, +1, +2, +3, +4 and +5)?

Thanks in advance!

 

[chopstickchakra]

My teacher said it's because do your own homework.

 

[Zzz]

My teacher said it's because do your own homework.

It's not homework.

 

[sage1999]

My teacher said it's because do your own homework.

my teacher said use google

 

[Joon]

Type it in google. Yahoo results. Does this come close to what you are looking for:

Oxides of Nitrogen
Nitrides use a variety of different oxidation numbers from +1 to +5 to 1- to -3 for oxide compounds. Almost all the oxides that form are gasses, and exist at 25 degrees Celsius. Oxides of nitrogen are acidic and easily attach protons.

N2O5 + H2O → 2HNO3 (aq)

The oxides play a large role in living organisms. They can be useful, yet dangerous.

Dinitrogen monoxide (N2O) is a anesthetic used at the dentist as a laughing gas.
Nitrogen dioxide (NO2) is harmful. It binds to hemoglobin molecules not allowing the molecule to release oxygen throughout the body. It is released from cars and is very harmful.
Nitrate (NO3-) is a polyatomic ion.
The more unstable nitrogen oxides allow for space travel.

Source:

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[fiend]

Nitrogen has an electronic config of 1s2 2s2 2p3.
It has 5 valence electrons 2s2 2p3
It has small size hence high electronegativity.
Hence more oxidation states.

In order to complete its octet Nitrogen can easily share 3 e- or form various ionic bonds a shown.

And OP nitrogen isn't inert, when existing as N2 it's very stable but nitrogen isn't inert.

I hope this helps.

 

[chopstickchakra]

It's not homework.

I was just screwing around.