General Reaction Equations
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Reaction of acids with carbonates:
Acid + metal carbonate –> salt + water + carbon dioxide
Reaction of acids with reactive metals (e.g. magnesium, zinc):
Acid + metal –> salt + hydrogen
Reaction of acids with water (dissolving):
Production of hydrogen ions: E.g. HCl (aq) –> H+ (aq) + Cl- (aq)
Reaction of alkalis with water (dissolving):
Production of hydroxide ions (OH-): E.g. NaOH (aq) –> Na+ (aq) + OH- (aq)
Neutralisation reactions (acids + bases):
Acid + metal oxide –> salt + water Acid + metal hydroxide –> salt + water
Reaction of alkali metals with water
2M (s) + 2H2O –> 2MOH (aq) + H2 (g) • vigorous reaction • very exothermic • heat given off may ignite hydrogen, producing fire or explosions
Reaction of alkali metals with air:
4M (s) + O2 (g) –> 2M2O (s) • burns readily in air • loses metallic lustre
Reaction of alkali metals with chlorine:
2M (l) + Cl2 (g) –> 2MCl (s) • reaction becomes more vigorous down the group
Reaction of halogens with water
X2 (aq) + H2O (l) –> HX (aq) + HOCl (aq)
Reaction of halogens with alkali/base
X2 (aq) + 2NaOH (aq) –> NaX (aq) + NaOX (aq) + H2O (l)
Reaction of metal oxides with carbon
Carbon + metal oxide –> metal + CO2
Reaction of metal oxides with hydrogen
Metal oxide + hydrogen –> metal + water *only works for metals below zinc in reactivity
Thermal decomposition of metal carbonates (below sodium in reactivity series)
Metal carbonate –> metal oxide + carbon dioxide
Decomposition reaction of silver carbonate
Silver carbonate –> silver + oxygen + carbon dioxide
Thermal decomposition of potassium/sodium nitrates
Metal nitrate –> metal nitrate + O2
Thermal decomposition of all metals between sodium and silver in the reactivity series:
Metal nitrate –> metal oxide + oxygen + nitrate