2.32 & 2.33: combined and oxidation reduction oxidising agent reducing agent in terms of gain or loss of oxygen and loss or gain of electrons. 4.5: becomes a practical statement 2.21 Practical: investigate reactions between dilute hydrochloric and sulfuric acids and metals (e.g. magnesium, zinc and iron) (e) Extraction and uses of metals New statement 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 5.1: becomes a bold 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 New statement: based on 5.1 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 5.2 5.4: statements deleted – 5.5: becomes a bold statement; 2.25C explain the uses of aluminium, copper, iron and in terms of their properties copper and steel added the types of steel will be limited to low-carbon (mild), high-carbon and stainless New statement 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 (f) Acids, alkalis and titrations 4.1 2.28 describe the use of litmus, phenolphthalein and methyl orange to distinguish between acidic and alkaline solutions 4.2 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) 4.3 2.30 describe the use of universal indicator to measure the approximate pH value of an aqueous solution 4.4 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
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
IGCSE-Chemistry-2017-mapping-document.docx