3.1.7 Oxidation, reduction and redox equations Flashcards
1
Q
What are redox reactions
A
Redox reactions involve a transfer of electrons from the reducing agent to the oxidising agent
2
Q
What is oxidation
A
Loss of electrons
3
Q
What is reduction
A
Gain of electrons
4
Q
What does an oxidising agent do
A
Accept electrons
5
Q
What does a reducing agent do
A
Donate electrons
6
Q
Oxidation state rules (7)
A
- An element is always 0
- A simple ion is its charge
- F in a compound is -1
- Cl is -1 except when in a compound with F
- O is -2 except when in a compound with F or in a peroxide where its -1
- H is +1 ecept when in a metal hydride where its -1
- Sum of oxidation states add up to charge
7
Q
How to write and combine half equations
A
- Balance half equations by:
- Balance any oxygen atoms by adding water
- Balance any hydrogen atoms by adding H+ ions
- Balance charges by adding electrons
- Combine two equations so number of electrons are balanced
8
Q
Oxidation state definition
A
Shows how many electrons have been added or removed from an element
