Question

Please help. I am very confused.

For the following reaction, identify the substances being oxidized and reduced (including their oxidation numbers), the oxidizing agent, and reducing agent.

CH4 + (2)O2 → CO2 + (2)H2O

Answer 1

Please correct me if I'm wrong; I've been getting myself mixed up on this stuff all day.

Okay so I think the oxidization numbers for carbon go from -4 to +4
And the oxidization numbers for oxygen go from 0 to -2
The hydrogen oxidization numbers stay at +1 right? So it's just spectating and irrelevant.

Oxidization means that it lost its negative electrons right? So the carbon was oxidized.
Reduction means that it took in the negative electrons that were lost? So oxygen was reduced.

From there, can I conclude that carbon was the reducing agent and oxygen was the oxidizing agent?

Answer 2

Easiest way to remember Oxidation and Reduction is Oil Rig - Oxidation is loss of electrons. Reduction is gain of electrons. Carbon goes from having a -4 charge to a +4 charge. Therefore it is oxidized and the agent that did the oxidizing was oxygen. Oxygen went from 0 to -2. Therefore it was reduced because it gained electrons. The agent that reduced it was Carbon.

Answer 3

Its confusing and always will be. I had to delete and rewrite because I caught myself flipping them.