Writing & Combining Half-equations - Redox (5.1)

Question 1

Define oxidation

Answer 1

The loss of electrons from any species

Question 2

Define reduction

Answer 2

The gain of electrons by any species

Question 3

Define redox reaction

Answer 3

A redox reaction is where one species is oxidised and another is simultaneously reduced

Question 4

What type of reaction is a redox reaction an example of?

Answer 4

A displacement reaction

Question 5

Where should electrons be in a reduction half equation?

Answer 5

Electrons are gained - on the left

Question 6

Where should electrons be in an oxidation half equation?

Answer 6

Electrons are lost - on the right

Question 7

Name the 3 steps for balancing a half equation

Answer 7

1. Check the atoms balance
2. Count the charges on both sides & make them equal
3. Add e-s to balance the charge

Question 8

When combining half equations, what should be removed from the overall equation?

Answer 8

Electrons

Question 9

When the amount of electrons are different in each half equation, how should you combine the half equations?

Answer 9

When electrons do not balance, find the lowest common multiple & multiply the whole equation to get this number of electrons - then you can combine the equations & remove the electrons