Question

a) oxidation state of N in NH4N02
b) draw a lewis structure so both n's have a formal charge of +1

Answer 1

Find the charges of the other elements in the compound.

You'll notice that o2 is -4 and h4 must be -4 as well.

that's a charge of -8

for nitrogen to neutralize this, each nitrogen must have a oxidation state of +4

Answer 2

Isn't H +4?

Answer 3

One of the N has a charge of 1+ but the other doesn't.. I know N follows octet rule, so N attached to 5 things is not likely but when you break this compound up into its ions and do the individual lewis structres, n is attached to 4 H..