Metals in Water
Reactive Metal + Liquid Water → Metal Hydroxide + Hydrogen Gas
E.g. Na(s) + H2O(l) → NaOH(aq) + H2(g)
Metal + Steam → Metal Oxide + Hydrogen Gas
E.g. Zn(s) + H2O(g) → ZnO(s) + H2(g)
Combustion of a Metal
Metal + Oxygen Gas → Metal Oxide
E.g. 2Mg(s) + O2(g) → MgO(s)
Combustion of a Carbon Compound
Hydrocarbon + Oxygen → Carbon Dioxide Gas + Liquid Water
E.g. 2C8H18(l) + 25O2(g) → 16CO2(g) + 18H2O(l)
Metals with Acids
Metal + Acid → Salt + Hydrogen gas
E.g. Zn(s) + 2HCl(aq) → ZnCl2(aq) + H2(g)
Carbonates with Acids
Carbonate + Acid → Salt + Carbon Dioxide Gas + Liquid Water
E.g. Na2CO3(aq) + 2HCl(aq) → 2NaCl(aq) + CO2(g) + H2O(l)
Oxidation
Metal → Metal Ion + Electron/s
E.g. Cu(s) → Cu2+(aq) + 2e–
Reduction
Metal Ion + Electron/s → Metal
E.g. Ag+(aq) + e– → Ag(s)
Redox (Reduction-Oxidation Reactions)
This reaction involves the transfer of electron/s from one reactant to another. This thus results in both a reduction and oxidation reaction occurring. To obtain the redox reaction, you can either write the net ionic equation for a displacement reaction (option 1) or add reduction and oxidation reactions together (option 2).
E.g. OPTION 1:
Cu(s) + 2AgNO3(aq) → Cu(NO3)2(aq) + 2Ag(s)
Cu(s) + 2Ag+(aq) + 2NO3– → Cu2+(aq) + 2NO3– + 2Ag(s)
Cu(s) + 2Ag+(aq) + 2NO3– → Cu2+(aq) + 2NO3– + 2Ag(s)
Cu(s) + 2Ag+(aq) → Cu2+(aq) + 2Ag(s)
E.g. OPTION 2
NOTE: BOTH THE CONSERVATION OF MASS AND CHARGE MUST BE SHOWN IN YOUR EQUATION!
Cu(s) → Cu2+(aq) + 2e–
+
2Ag+(aq) + 2e– → 2Ag(s)
__________________
Cu(s) + 2Ag+(aq) + 2e– → Cu2+(aq) + 2e– + 2Ag(s)
Cu(s) + 2Ag+(aq) → Cu2+(aq) + 2Ag(s)
Photosynthesis
Carbon Dioxide Gas + Liquid Water → Solid Glucose + Oxygen Gas
I.e. 6CO2(g) + 6H2O(l) → C6H12O6(s) + 6O2(g)
Respiration
Aqueous Glucose + Oxygen Gas → Carbon Dioxide Gas + Liquid Water
I.e. C6H12O6(s) + 6O2(g) → 6CO2(g) + 6H2O(l)
Lime Water Test (Lime Water and Carbon Dioxide)
Calcium hydroxide + Gaseous carbon dioxide → Solid calcium carbonate + liquid water
I.e. Ca(OH)2(aq) + CO2(g) → CaCO3(s) + H2O(l)
,
