Pre-Electrochemistry Worksheet - (Chemistry 3)

Oxidation of any pure element

0

Oxidation number of a monatomic ion

Equals the charge on the ion

Oxidation number of fluorine in a compound

Always -1

Oxygen’s oxidation number

-2

Unless it’s combined with F, which makes it +1 or +2

And if it’s in a peroxide, it is -1

Hydrogen’s oxidation state

+1

Unless combined with a metal, it is -1

Group 1 and 2 elements and aluminum oxidation numbers

+1, +2, +3

Sum of the oxidation numbers in all atoms in a neutral compound

0

The sum of the oxidation numbers of all atoms in a polyatomic ion

Equals the charge of the ion

Oxidation in terms of electrons

Loss of electrons

Reduction in terms electrons

Gain of electrons

Why oxidation and reduction must always occur together

Electrons can’t be created or destroyed in a chemical reaction

Oxidation number of an element when it’s oxidized

Increases when oxidized

Oxidation number of an element when it’s reduced

Decreases when reduced

Why oxygen is involved in many oxidation reactions when no electrons are shown

Oxygen is very electronegative

One example of oxidation

Iron rusting