1:39 write formulae for compounds formed between the ions listed in 1:38.1:38b know the charges of these ions: metals in Groups 1, 2 and 3, non-metals in Groups 5, 6 and 7, hydrogen (H⁺), hydroxide (OH⁻), ammonium (NH₄⁺), carbonate (CO₃²⁻), nitrate (NO₃⁻), sulfate (SO₄²⁻).1:38 know the charges of these ions: metals in Groups 1, 2 and 3, non-metals in Groups 5, 6 and 7, Ag⁺, Cu²⁺, Fe²⁺, Fe³⁺, Pb²⁺, Zn²⁺, hydrogen (H⁺), hydroxide (OH⁻), ammonium (NH₄⁺), carbonate (CO₃²⁻), nitrate (NO₃⁻), sulfate (SO₄²⁻).1:37 understand how ions are formed by electron loss or gain.1:36 practical: know how to determine the formula of a metal oxide by combustion (e.g.1:35 (Triple only) understand how to carry out calculations involving gas volumes and the molar volume of a gas (24dm³ and 24,000cm³ at room temperature and pressure (rtp)).1:34 (Triple only) understand how to carry out calculations involving amount of substance, volume and concentration (in mol/dm³) of solution.1:33 calculate empirical and molecular formulae from experimental data.1:32 know what is meant by the terms empirical formula and molecular formula.1:31 understand how the formulae of simple compounds can be obtained experimentally, including metal oxides, water and salts containing water of crystallisation.1:29 calculate reacting masses using experimental data and chemical equations.1:28 understand how to carry out calculations involving amount of substance, relative atomic mass (Aᵣ) and relative formula mass (Mᵣ).1:27 know that the mole (mol) is the unit for the amount of a substance.1:26 calculate relative formula masses (including relative molecular masses) (Mᵣ) from relative atomic masses (Aᵣ).1:25 write word equations and balanced chemical equations (including state symbols): for reactions studied in this specification and for unfamiliar reactions where suitable information is provided. (e) Chemical formulae, equations and calculations.1:24 understand why the noble gases (Group 0) do not readily react.1:23 Understand why elements in the same group of the Periodic Table have similar chemical properties. 1:22 understand how the electronic configuration of a main group element is related to its position in the Periodic Table.1:21 identify an element as a metal or a non-metal according to its position in the Periodic Table.1:20 understand how to use electrical conductivity and the acid-base character of oxides to classify elements as metals or non-metals.1:19 understand how to deduce the electronic configurations of the first 20 elements from their positions in the Periodic Table.1:18 understand how elements are arranged in the Periodic Table: in order of atomic number, in groups and periods.1:17 be able to calculate the relative atomic mass of an element (Aᵣ) from isotopic abundances.1:16 know what is meant by the terms atomic number, mass number, isotopes and relative atomic mass (Aᵣ).1:15 know the structure of an atom in terms of the positions, relative masses and relative charges of sub-atomic particles.1:14 know what is meant by the terms atom and molecule.1:13 practical: investigate paper chromatography using inks/food colourings.1:12 understand how to use the calculation of Rf values to identify the components of a mixture.1:11 understand how a chromatogram provides information about the composition of a mixture.1:10 describe these experimental techniques for the separation of mixtures: simple distillation, fractional distillation, filtration, crystallisation, paper chromatography.1:09 understand that a pure substance has a fixed melting and boiling point, but that a mixture may melt or boil over a range of temperatures.1:08 understand how to classify a substance as an element, a compound or a mixture.
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