One last reaction question?

Question

2 O²⁻_(aq)  →  O_2(g)  

The reaction above is an example of:

 

Question 1 options:

a.	oxidation
b.	reduction

This one I believe it to be a oxidation as the 2O lost the 2-? Please correct me if I'm wrong

Answer 1

You are correct , but as further input...

I see that you’ve asked several of these question before. Lauren has given you some excellent answeres. Yet, some how you still don’t seem to get it. So let’s try another approach to see if we can help you.

What is the oxidation number of oxygen on the left side of the equation? It is 2- if you don’t see why that is the case, then you must go back and review the concept of oxidation states. Now, on the right side of the equation, the oxidation number for oxygen is zero. How did it go from 2- to zero. It must have lost electrons (2 electrons). Since it lost electrons, it has been oxidized. So this is an OXIDATION half reaction.

It may help you to recall that electrons have a - (minus) charge. If oxygen goes from 2- to 1- or to zero, it is becoming more positive so it must be LOSING negative charges (electrons). If something loses electrons, it is oxidized and is the reducing agent. Just memorize that, or go with what Lauren to.d you originally. Tha is OIL RIG, which means Oxidation Is Loss and Reduction Is Gain of electrons.

Answer 2

Hi Michael,

Yes, this would be oxidation. Each O^2- has 8 electrons each (16 electrons total). O₂ only has 12 electrons. Remember that Losing Electrons is Oxidation (16 ->12). Therefore, this is oxidation.

You can remember this using LEO the lion says GER.

LEO = Losing Electrons is Oxidation

GER = Gaining Electrons is Reduction

Hope this Helps!