## Oxidation Numbers

$\Delta G^{\circ} = -nFE_{cell}^{\circ}$

david_li3H
Posts: 16
Joined: Wed Sep 21, 2016 2:56 pm

### Oxidation Numbers

Hi!
I'm not sure if oxidation numbers is on the midterm (I don't remember Lavelle talking about it but I remember at discussion my TA asking a question about it so maybe I missed something?), but I'd like to ask a question on it anyways.

In a compound, is O always going to be -2, and H +1, or can it be different based on certain circumstances?
Thanks!

janavi_patel_2K
Posts: 20
Joined: Wed Sep 21, 2016 2:59 pm

### Re: Oxidation Numbers

Typically, O is always going to be -2 and H is always going to be +1. Based on those oxidation numbers, you can use those to determine the oxidation of the other atoms in the molecule.

samuelkharpatin2b
Posts: 55
Joined: Wed Sep 21, 2016 2:57 pm

### Re: Oxidation Numbers

The problems we are going to see in 14B will have Oxygen with an oxidation number of -2 (if in a compound) and Hydrogen with an oxidation number of +1. Using these known oxidation numbers you can find oxidation numbers of other elements in a compound, say Mn. There is an exception to the -2 rule for Oxygen, but the problems we have will have -2 as its oxidation number.

Jennifer Ho 1K
Posts: 31
Joined: Thu Jul 13, 2017 3:00 am

### Re: Oxidation Numbers

In most cases you'll see oxygen will have an oxidation state number of -2 (if not 0) and hydrogen will have an oxidation state of +1, so there is a point of reference to solve for the other ions that commonly have varying oxidation states. There are exceptions, but it's unlikely that you'll see them in 14B.

Yu Chong 2H
Posts: 30
Joined: Fri Sep 29, 2017 7:05 am

### Re: Oxidation Numbers

Oxidation numbers of O in a compound is most commonly -2, however, in peroxides like H2O2, the oxidation number of oxygen will be different. In this case, it is -1.