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Metal Compounds - An Introduction to Inorganic Chemistry.

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Topic 1: Metal Compounds - An Introduction to Inorganic Chemistry Section 1.1 Types of Inorganic Reaction Thermal Decomposition Reactions * What sort of compounds decompose? 1. any Hydrated compound - gives off water easily 2. Metal carbonates - decompose variably easily giving CO2 + MO 3. Metal sulphates - decompose variably into MO + SOx 4. Metal nitrates - most give MO, NO2 + O2 reactive metal nitrates give MNO2 + O2 * How do we test for the gases liberated? 1. H2O vapour - condenses into water droplets. 2. CO2 - bubble through limewater; turns cloudy. 3. O2 - glowing splint relights. 4. SOx - colourless, strongly acidic (UI/litmus). 5. NO2 - brown acidic gas. Experiment 1.1a Heat small amounts of the following chemicals. Test for the gases you expect to be liberated: * CoCl2 hydrated * Cu(NO3)2 hydrated * FeSO4 hydrated * ZnCO3 * NaNO3 Note the safety notes on page 3. Put results into appropriate table, and answer questions on page 3. ...read more.


These reactions release considerable amounts of energy [equations and energy changes shown on page 9]. A reaction which releases energy [exothermic reaction] is given a negative value because the products contain less energy than the reactants [energy change = products energy - reactants energy]. Note that the Copper reaction is endothermic and, therefore, unlikely to 'go'. Much more about this later!! Thermit Reaction - read and make brief notes (page 9). But redox reactions are more than just loss or gain of oxygen - this would be rather limiting!! Iron forms two different series of compounds, each containing a different iron ion [Fe2+ and Fe3+]. Transition elements (of which iron is one) frequently contain more than one type of ion. If the charge on an ion becomes more positive (e.g. Fe2+ to Fe3+) then the ion is said to have been oxidised [i.e. it has undergone oxidation]. If the charge becomes more negative, then the ion has been reduced [i.e. it has undergone reduction].. ...read more.


+ H2O(l) See book for details. Expt. 1.2b Preparation of Mohr's salt, Ammonium Iron(II) Sulphate, (NH4)2SO4.FeSO4.6H2O Fe ? FeSO4 NH3 ? (NH4)2SO4 Mix, crystallise. See book for details. Section 1.3 Toolkit: Writing Formula & Balancing Equations Standard GCSE stuff - use GCSE notes where necessary. Section 1.4 Toolkit: The Mole, Molar Mass & Molar Volume Standard GCSE stuff - use GCSE notes where necessary. Section 1.5 Background Reading: A Golden Opportunity Answers to Questions: 1. Key Skills Communication [Background Reading] Number [Expts 1.2a&b] Topic Review 1. List the key words or terms in definitions. 2. Summarise key concepts as simply as possible. Review Questions 1. Name compounds of given formula. 2 Give formula and state of element. 3. Give formulae of given compounds. 4. Write and balance (simple) decomposition equations. 5. Write and balance precipitation ionic equations. 6. State type of reaction & reason. 7. Write balanced equations. 8*. Calculate molar masses of compounds. 9*. Calculate mass of x moles of substance. 10*. Calculate number of moles. 11*. Calculate masses or volumes. 12*. Preparation of hydrated magnesium chloride. Examination Questions 13. Preparation of hydrated zinc sulphate. 14. Preparation of vanadium alum. 15. Manganese - reactions and properties. 1 Topic 1 Metal Compounds ...read more.

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