A summary of topic 3, organised so the notes are easy to understand. The notes are on slides, so they can be printed out and used as revision cards or posters, for revision on the go. The notes cross-reference the specification so it is easy to see where each bit of information has come from. They ...
Oxidation & reduction Agents for change:
Ox = loss of e-, loss of H2 gain of O2, ox number ↑ Red agent = donates e-’s
Red = gain of e-, gain of H2, loss of O2, ox number ↓ - It is oxidised
Oxidation number = a measure of the e- density around each - Reduces something else
atom Ox agent = gains e-’s
- -ve number = e- density gained - It is reduced
- +ve number = e- density lost - Oxidises something else
Systematic names:
= tell you the +ve oxidation number
E.g. iron (ll) chloride: Fe = +2
iron (lll) chloride: Fe = +3
Potassium chlorate (V): Cl = +5
Ox numbers rules:
Group 1 = +1
Group 2 = +2
Al = +3
H = +1 (except metal hydrides → -1)
F = -1
O = -2 (except peroxides (H2O2) → -1 & compounds w/ F)
Cl = -1 (except w/ O & F)
Uncombined elements = 0
Half equations:
1. Balance non O/H
2. Balance O’s by adding H2O
3. Balance H’s by adding H+
4. Balance charge w/ e-’s
Disproportionation:
Redox = red & ox happening simultaneously
Disprop = 1 element simultaneously oxidised & reduced
e.g.
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