Oxidation and Reduction

Oxidation

a compound or partial loss of electrons
Na_(s) —> Na⁺ + 1e^- sodium is oxidized

Fe_(s) —> Fe²⁺ + 2e^- is a half reaction

Iron lose electrons and oxidation becomes positive

Reduction

a complete or partial gain of election

O₂ + 4e^- —> 2O^2- reduction - gains electrons becomes negative

oxygen is reduced

This is reaction 1. Fe_(s) —> Fe²⁺ + 2e^-

This is reaction 2. O₂ + 4e^- —> 2O^2-
2(1) +2

2(Fe_(s) —> Fe²⁺ + 2e^- -)
+ O₂ + 4e^- —> 2O^2- =

2Fe_(s)+O_2(g)+4e—>2Fe²⁺+4e^-+2O^2-

2Fe_(s)+O_2(g)—>2FeO_(s) Oxygen is reduced while Iron is oxidized. This is also a redox reaction.

Redox reaction

gaining and losing electrons from each other

LEO the lion goes GER

Lose electron oxidation
gain electron reduced

Oxidation numbers

A positive or negative number assigned to an atom to indicate its degree of oxidation or reduction

Monatomic ions have oxidation numbers equal to their charge

Na⁺ has a 1+
Fe³⁺ has a 3+
O^2- has a -2

The oxidation number for hydrogen in a compound is +1 except in metal hydrides when it is -1. It’s like a 2 in 1. A wombo combo. A dual element.

+1 -1

LiH

Lithium lose e^-

+1 -2
H₂O
Oxygen steals H’s electron

The oxidation number for oxygen in a compound is -2 except for peroxides, where it is -1, or if it is positive with fluorine

No example but one from chat gpt

Hydrogen peroxide

+1 -1

H₂O₂

The oxidation number of any atom is elemental form is 0.

0 0 0

O₂ H₂ Fe

A neutral compound should have oxidation numbers that add to zero

Yet another non example but example from your good friend Chat

A polyatomic ion should have an oxidation number that adds to the overall charge

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