1.7 Oxidation, reduction and redox reactions

Question 1

Oxidation definition

Answer 1

Loss of electrons
Oxidation state increases

Question 2

Reduction increases

Answer 2

Gain of electrons
Oxidation state decreases

Question 3

Reducing agent definition

Answer 3

Electron donor
The reducing agent is oxidised

Question 4

Oxidising agent definition

Answer 4

Electron acceptor
The oxidising agent is reduced

Question 5

Oxidation states order

Answer 5

Uncombined elements - 0
Metals
Fluorine - -1
Hydrogen - +1
Oxygen - -2
Chlorine - -1

Question 6

More positive oxidation number

Answer 6

Oxidised

Question 7

More negative oxidation number

Answer 7

Reduced

Question 8

Rules for balancing half equations

Answer 8

Balance main atom first
Balance O using h2o
Balance H using H+
Balance charge using electrons

Question 9

Steps to combine half equations

Answer 9

Multiple one or both half equations so they have the same no of electrons
Add the reactants from both half equations together
Add the products from both half equations together
Cancel out electrons

Question 10

Disproportionation definition

Answer 10

When one type of atom is reduced and oxidised in the same reaction