The oxidation state of N in NO2 is apparently +4 But in NH3 it's -3 (the N)
And in NO it's +2 (the N again)
Now Forgive me if I'm missing something, but the book has magically come up with these answers and I can't find where it's telling me this under this topic? This is way confusing.
How do they come up with these answers? Is there a quick way? What Am I missing?
you are wanting to calculate the charges on each atom on the molecule. Oxygen is -2. So in the case of NO2 you have to oxygens therefore you have 2 x -2 charges. making -4. You know that NO2 is a neutral molecule so to balance the charge nitrogen must = +4
The oxidation state of O is usually -2, and the oxidation state of H is usually +1. There's a couple of exceptions to each though: - If oxygen is attached to flourine it becomes a + - In peroxides, superoxies it's -1, -0.5 respectively (but you don't need to know that for A-levels) - Hydrogen is +1 except when bonded to more electropositive elements where it's -1
The molecule doesn't have a charge so it's oxidation states must balance for it to be equal to zero overall. If it had a charge of -1 for instance, the oxidation states would have to add to give -1.
And yeah there are 3 hydrogen's so you get: +1 +1 +1 = +3, so you need a -3 to balance it to make it 0.
why is it that in CaCl2 the oxidation state of Cl2 is -1? is it because Ca is +2 and to equate to zero Cl has to be -1 and not -2 because there are two Cl's?
Correct - Ca is in group 2 so it's oxidation state is +2. Also, halogen's have oxidation states of -1 (except when attached to oxygen, nitrogen or other halogens) so each is -1. Cl cannot be -2.
because it gives you the oxidation state of an individual Cl atom.......each atom of Cl has a charge of -1 so since there are two Cl their combined charge is -1x2= -2 and Ca is +2 and so +2-2=0......abracadabra :P
because it gives you the oxidation state of an individual Cl atom.......each atom of Cl has a charge of -1 so since there are two Cl their combined charge is -1x2= -2 and Ca is +2 and so +2-2=0......abracadabra :P
in Na2O2 it's O2 is apparently -1. When working out such element is it just knowing the rules? Because I was going all complex by working out the oxidation state of Na...btw for future reference when working out for example Na2 do I just do Na? Because I thought I times by two. Argh confusion settled in again.
That's an exception to the rule because it's a peroxide (here I've quoted it from the link I've given above):
Oxygen in peroxides
Peroxides include hydrogen peroxide, H2O2. This is an electrically neutral compound and so the sum of the oxidation states of the hydrogen and oxygen must be zero.
Since each hydrogen has an oxidation state of +1, each oxygen must have an oxidation state of -1 to balance it.
It's the same principle with oxygen, because Na has to have an oxidation state of +1, each oxygen has to have a state of -1 to balance it.
Yeah that's a metal hydride, another exception to the rule (quoted from the same article):
Hydrogen in the metal hydrides
Metal hydrides include compounds like sodium hydride, NaH. In this, the hydrogen is present as a hydride ion, H-. The oxidation state of a simple ion like hydride is equal to the charge on the ion - in this case, -1.
Alternatively, you can think of it that the sum of the oxidation states in a neutral compound is zero. Since Group 1 metals always have an oxidation state of +1 in their compounds, it follows that the hydrogen must have an oxidation state of -1 (+1 -1 = 0).
They've talked about group 1 metals above but it's the same principle for group 2. Group 2 metals always have oxidation states of +2, so in this case hydrogen has an oxidation state of -1. You have two hydrogens so you have -1 -1 to give -2. This balances the +2 charge on Mg.
No you're not! It's one of those things you either get it or you don't - nothing wrong with you at all if you don't! When you consider all the exceptions to the rules it can get a bit confusing. Also because the molecules you posted possess a charge it's easy to think "where are they getting that from" .
I'm trying to look up some examples for you to try atm.