INTERNATIONAL GCSE CHEMISTRY Principles of chemistry The following sub-topics are covered in this section. States of matter Elements, compounds and mixtures Atomic structure The Periodic Chemical formulae, equations and calculations Ionic bonding Covalent bonding Metallic bonding Electrolysis (a) States of matter 2011 specification reference 1.1 understand the three states of matter in terms of the arrangement, movement and energy of the particles 1.1 1.2 understand the interconversions between the three states of matter in terms of: the of the interconversions how they are achieved the changes in arrangement, movement and energy of the particles. 1.2 & 1.3: combined and slightly 1.3 understand how the results of experiments involving the dilution of coloured solutions and diffusion of gases can be explained 1.4 1.4 know what is meant by the terms: solvent solute solution saturated solution New statement
in general, with increasing relative molecular mass 1.49 explain why substances with giant covalent structures are solids with high melting and boiling points 1.43 1.44 & 1.45: statements deleted 1.50 explain how the structures of diamond, graphite and C60 fullerene influence physical properties, including electrical conductivity and hardness New statement 1.51 know that covalent compounds do not usually conduct electricity 1.49 (h) Metallic bonding 1.52C know how to represent a metallic lattice by a 2-D diagram New statement, on 1.46 1.53C understand metallic bonding in terms of electrostatic attractions 1.46: becomes a bold statement 1.54C explain typical physical properties of metals, including electrical conductivity and malleability 1.47: becomes a bold statement (i) Electrolysis 1.48: statement deleted 1.55C understand why covalent compounds do not conduct electricity 1.49: becomes a bold statement 1.56C understand why compounds conduct electricity only when molten or in aqueous solution 1.50: becomes a bold statement 1.51 – 1.52: statement deleted 1.57C know that anion and cation are terms used to refer to negative and positive ions respectively New statement 1.58C describe experiments to investigate electrolysis, using inert electrodes, of molten compounds (including lead(II) bromide) and aqueous solutions (including sodium chloride, dilute sulfuric acid and copper(II) sulfate) and to predict the products 1.53: becomes a bold statement & 1.54 1.59C write ionic half-equations representing the reactions at the electrodes during electrolysis and understand why these reactions are classified as oxidation or reduction 1.55: becomes a bold statement & 1.29: becomes a bold statement 1.60C Practical: investigate the electrolysis of aqueous solutions 1.54: becomes a practical statement 1.56 & 1.57: statements deleted
oxidation reduction oxidising agent reducing agent in terms of gain or loss of oxygen and loss or gain of electrons. 2.32 & 2.33: combined and 2.21 Practical: investigate reactions between dilute hydrochloric and sulfuric acids and metals (e.g. magnesium, zinc and iron) 4.5: becomes a practical statement (e) Extraction and uses of metals 2.22C know that most metals are extracted from ores found in the Earth’s crust and that unreactive metals are often found as the uncombined element New statement 2.23C explain how the method of extraction of a metal is related to its position in the reactivity series, illustrated by carbon extraction for iron and electrolysis for aluminium 5.1: becomes a bold statement 2.24C be able to comment on a extraction process, given appropriate information detailed knowledge of the processes used in the extraction of a specific is not required New statement: based on 5.1 5.2 – 5.4: statements deleted 2.25C explain the uses of aluminium, copper, iron and in terms of their properties the types of steel will be limited to low-carbon (mild), high-carbon and stainless 5.5: becomes a bold statement; copper and steel added 2.26C know that an alloy is a mixture of a metal and one or more elements, usually other metals or carbon New statement 2.27C explain why alloys are harder than pure metals New statement (f) Acids, alkalis and titrations 2.28 describe the use of litmus, phenolphthalein and methyl orange to distinguish between acidic and alkaline solutions 4.1 2.29 understand how to use the pH scale, from 0–14, can be used to classify solutions as strongly acidic (0–3), weakly acidic (4–6), neutral (7), weakly alkaline (8–10) and strongly alkaline (11–14) 4.2 2.30 describe the use of universal indicator to measure the approximate pH value of an aqueous solution 4.3 2.31 know that acids in aqueous solution are a source of hydrogen ions and alkalis in a aqueous solution are a source of hydroxide ions 4.4
hydrochloric acid 3.16 Practical: investigate the effect of different solids on the catalytic decomposition of hydrogen peroxide solution 4.17: becomes a practical statement (c) Reversible reactions and equilibria 3.17 know that some reactions are reversible and this is indicated by the symbol ⇌ in equations 4.22 3.18 describe reversible reactions such as the dehydration of hydrated copper(II) sulfate and the effect of heat on ammonium chloride 4.23 3.19C know that a reversible reaction can reach dynamic equilibrium in a sealed container 4.24: re-worded; also becomes a bold statement 3.20C know that the characteristics of a reaction at dynamic equilibrium are: the forward and reverse reactions at the same rate the concentrations of reactants and products remain constant. 4.24: re-worded; also becomes a bold statement 3.21C understand why a catalyst does not affect the position of equilibrium in a reversible reaction New statement 3.22C know the effect of changing either temperature or pressure on the position of equilibrium in a reversible reaction: an increase (or decrease) in temperature shifts the position of equilibrium in the direction of the endothermic (or exothermic) reaction an increase (or decrease) in pressure shifts the position of equilibrium in the direction that produces fewer (or more) moles of gas References to Le Chatelier's principle are not required 4.25: re-worded; also becomes a bold statement 5.22 – 5.25: statements deleted & 5.26 – 5.31: statements deleted Organic chemistry The following sub-topics are covered in this section. Introduction oil Alkanes Alkenes