SASS Chem P3 Thermal Decomposition

Secondary 4 Chem Experiment 5.5: Thermal Decomposition 1 St Andrew’s Secondary School Department of Science, Chemistry Name: ________________________( ) Class: _______ Date: __________ Aim: To investigate the effect of heat on some common substances e.g. hydroxides, carbonates and nitrates. Theory of Thermal Decomposition Thermal decomposition is defined as a chemical reaction when a chemical substance breaks down into more than one simpler substances when heated. The reaction is usually endothermic as heat is required to break chemical bonds in the compound undergoing decomposition. The decomposition temperature of a substance is the temperature at which the substance decomposes into smaller substances or into its constituent atoms. Thermal Decomposition of metal carbonates The temperature of decomposition depends upon the reactivity of the metal. The more reactive metals, the more stable is the carbonate. Thus, the carbonates of sodium and potassium are stable at the highest temperatures of a Bunsen burner flame, whereas, the carbonates of silver and copper are easily decomposed. Common examples of the carbonate decomposition CuCO3(s) → CuO(s) + CO2(g) CaCO3(s) → CaO(s) + CO2(g) ∆ ∆

Secondary 4 Chem Experiment 5.5: Thermal Decomposition 2 St Andrew’s Secondary School Department of Science, Chemistry Thermal Decomposition of metal hydroxides On heating the Metal hydroxides, it decompose to form the metal oxide and water vapour. M(OH)2(s) → MO(s) + H2O(l) Thermal Decomposition of metal nitrates 1. The Group I Alkali Metal nitrates (NO3) decompose to form the nitrite (NO2-) salt and oxygen gas. 2MNO3(s) → 2MNO2(s) + O2(g) where M = Na or K so when M = Na: sodium nitrate ==> sodium nitrite + oxygen Nitrates are colourless crystals and nitrites are white solids and are all soluble in water giving neutral solutions. 2. The Group II, Lead, Aluminium and Transition Metal nitrates decompose to form the metal oxide, nasty brown nitrogen dioxide gas and oxygen gas when strongly heated. The nitrates are all water soluble neutral salts, all colourless crystals except Cu2+ is blue and Fe2+ is green. 2M(NO3)2(s) → 2MO(s) + 4NO2(g) + O2(g) 3. Aluminium and Iron(III) nitrates will decompose to form the metal oxide, nitrogen dioxide and oxygen gas too. 4M(NO3)3(s) ==> 2M2O3(s) + 12NO2(g) + 3O2(g) If M = Al, it gives white aluminium oxide, if M = Fe it gives give reddish-brown iron(II) oxide. Colours of the oxides Type of oxides Colour Most main group metal oxides White Zinc oxide Yellow when hot, white when cool Copper(II) oxide and iron(II) oxide Black Iron(III) oxide Reddish brown Lead(II) oxide Yellow ∆

Secondary 4 Chem Experiment 5.5: Thermal Decomposition 3 St Andrew’s Secondary School D