Hi. I was just going over my notes for my chem half yearly and came across the oxidation states and their rules. I was wondering if someone could please explain it to me and give an example of how to solve it in a question??
Hey Gabby! Welcome to the forums!
Oxidations states is a useful tool we can use to decide whether a substance is oxidising or reducing. There are some pretty simple rules that we need to know before we can attack any question.
1. Oxygen has an oxidation state of -2Ever Oxygen we see will have an oxidation state of -2. So, if there are two oxygen atoms, we will say that the total state is -4!
Elements have an oxidation state of 0This is because it is 'neutral'
The oxidation state of each element will add up to the oxidation state of the moleculeThis is just sort of intuitive. Let's first look at an easy example.
Now, the initial oxidation state of Copper is 0 (as it is in elemental form). The final compound containing Copper has an overall charge of zero. However, we know that CO3 has an oxidation state of -1. Therefore, Copper must have a change of +1. So, as it has increased in oxidation state, it has oxidised.
The initial oxidation state of Silver is +1, as NO3 is -1. The final oxidation state of Silver is 0. Thus, the oxidation state has decrease, so Silver has reduced!
Let me know if you have a specific question you want us to work through, to help you better understand the theory!