Oxidation, Reduction, Redox
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What are reducing agents?
Electron donor substance that is oxidised, so loses electrons
What are oxidising agents?
Electron acceptor substance that is reduced, so gains electrons
Oxidation numbers of the following: Hydrogen Chlorine Oxygen Ions
Hydrogen: always +1, except in hydrides (metal and hydrogen), where it is -1 Chlorine: always -1, but in compounds with F or O, it is +1 Oxygen: -2, except in peroxides it’s -1 and when F is present it’s +2, as F takes priority Ions: same as charge on ion
What has happened to the substance if there is an increase in oxidation number? What is its role in the reaction?
Oxidation Reducing agent
What has happened to the substance if there is an decrease in oxidation number? What is its role in the reaction
Reduction Oxidising agent
Rules to balance half equations in redox
• Write down species before and after reaction • Balance any atoms apart from hydrogen/oxygen • Balance any oxygens with H2O • Balance hydrogens with H+ ions • Balance charges with electrons