Elements - Zinc (Zn), Magnesium (Mg), Copper (Cu), Silver (Ag), Oxygen (O2)
Compounds - Sodium Bicarbonate (NaHCO3), Calcium Carbonate (CaCO3)
Solutions - Cupric Sulfate (CuSO4), Hydrochloric Acid (HCl), Sodium Hydroxide (NaOH), Zinc Chloride (ZnCl2), Silver Nitrate (AgNO3), Sodium Phosphate (Na3PO4)
Decomposition - a chemical reaction that occurs when a single compound breaks down into two or more elements or new compounds.
Decomposition - CaCO3(s) → CaO(s) + CO2(g)
Synthesis - a chemical reaction in which two or more substances react to create one product.
Synthesis - 2 Na(s) + Cl2(g) → 2 NaCl(s)
Single Replacement - a chemical reaction that occurs when the atoms of one element replace the atoms of another element in a compound.
Single Replacement - 2 AgNO3(aq) + Zn(s) → 2 Ag(s) + Zn(NO3)2(aq)
Double Replacement - a chemical reaction that involves the exchange of ions between two compounds and produces either a precipitate, a gas, or water.
Double Replacement - AgNO3 (aq) + NaCl (aq) → AgCl (s) + NaNO3 (aq)
Combustion - a chemical reaction that occurs when a substance reacts with oxygen, releasing energy in the form of heat and light.
Combustion - CH4 (g) + 2 O2 (g) → CO2 (g) + 2 H2O (g)
A single replacement reaction will produce new products when a metal is higher than the other metal on the activity series is when a single replacement will occur since the metal that is higher than the metal that is being replaced has a more active than the low one.
You can determine the precipitate in a double replacement by knowing the solubility rules. Such as all carbonates and phosphates except group I and ammonium, all hydroxides except Group I, Strontium, and Barium, all sulfides except group I, II, and ammonium, and all oxides except group I these are all insoluble.
A substance can be made to react with oxygen in the air from having a source of ignition. Which then oxygen can combine to form heat and light.