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Chapter 7: Redox

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Total cards: 7•Content version: v4•Public deck•Updated: 8/1/2026

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#1
Front (Question)

Common oxidation states

Back (Answer)

H +1 (except -1 in metal hydrides) Group 1 always +1 Group 2 always +2 Aluminium always +3 Oxygen -2 (except in peroxides, where it is -1 and with fluorine) Fluorine always -1 Cl, Br, I -1 unless combined with more reacive halogen or with oxygen

#2
Front (Question)

Uncombined elements

Back (Answer)

oxidation state is zero

#3
Front (Question)

Disproportionation

Back (Answer)

When an element is both oxidised and reduced in the same process. Cu2O –> Cu + CuO Cu2O: Cu = +1 Cu: Cu = 0 (reduced) CuO: Cu = +2 (oxidised)

#4
Front (Question)

O I L R I G

Back (Answer)

Oxidation Is Loss (of electrons) Reduction Is Gain (of electrons)

#5
Front (Question)

Oxidising agents…

Back (Answer)

… get reduced … accept electrons

#6
Front (Question)

Reducing agents…

Back (Answer)

…get oxidised …donate electrons

#7
Front (Question)

spectator ions

Back (Answer)

do not change state during a reaction. They are ignored in ionic equations; state symbols needed: AgNO3(aq) + KBr(aq) –> KNO3(aq) + AgBr(s) when ionic substances dissolve, the ions dissociate: Ag+(aq) + NO3-(aq) + K+(aq) + Br-(aq) –> K+(aq) + NO3-(aq) + AgBr(s) and then removing spectators to give the ionic equation: Ag+(aq) + Br-(aq) –> AgBr(s)