GCSE Chemistry Year 9 Spec Points - TutorMyself Chemistry

1:01 understand the three states of matter in terms of the arrangement, movement and energy of the particles

1:02 understand the interconversions between the three states of matter in terms of: the names of the interconversions, how they are achieved and the changes in arrangement, movement and energy of the particles

1:03 understand how the results of experiments involving the dilution of coloured solutions and diffusion of gases can be explained

1:04 know what is meant by the terms: solvent, solute, solution, saturated solution

1:05 (Triple only) know what is meant by the term solubility in the units g per 100g of solvent

1:06 (Triple only) understand how to plot and interpret solubility curves

1:07 (Triple only) practical: investigate the solubility of a solid in water at a specific temperature

1:08 understand how to classify a substance as an element, a compound or a mixture

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

1:10 describe these experimental techniques for the separation of mixtures: simple distillation, fractional distillation, filtration, crystallisation, paper chromatography

1:11 understand how a chromatogram provides information about the composition of a mixture

1:12 understand how to use the calculation of Rf values to identify the components of a mixture

1:13 practical: investigate paper chromatography using inks/food colourings

1:14a know what is meant by the terms atom

1:14 know what is meant by the terms atom and molecule

1:15 know the structure of an atom in terms of the positions, relative masses and relative charges of sub-atomic particles

1:16a know what is meant by the terms atomic number, mass number and relative atomic mass (Aᵣ)

1:18 understand how elements are arranged in the Periodic Table: in order of atomic number, in groups and periods

1:19 understand how to deduce the electronic configurations of the first 20 elements from their positions in the Periodic Table

1:20a understand how to use electrical conductivity to classify elements as metals or non-metals

1:20 understand how to use electrical conductivity and the acid-base character of oxides to classify elements as metals or non-metals

1:21 identify an element as a metal or a non-metal according to its position in the Periodic Table

1:22 understand how the electronic configuration of a main group element is related to its position in the Periodic Table

1:23 Understand why elements in the same group of the Periodic Table have similar chemical properties

1:24 understand why the noble gases (Group 0) do not readily react

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

1:26 calculate relative formula masses (including relative molecular masses) (Mᵣ) from relative atomic masses (Aᵣ)

1:37 understand how ions are formed by electron loss or gain

1:38a understand how to use the charges of these ions in ionic formulae: 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⁻)

1:39 write formulae for compounds formed between the ions listed in 1:38

1:40 draw dot-and-cross diagrams to show the formation of ionic compounds by electron transfer, limited to combinations of elements from Groups 1, 2, 3 and 5, 6, 7 only outer electrons need be shown

1:41 understand ionic bonding in terms of electrostatic attractions

1:42 understand why compounds with giant ionic lattices have high melting and boiling points

1:44 know that a covalent bond is formed between atoms by the sharing of a pair of electrons

1:45 understand covalent bonds in terms of electrostatic attractions

1:46 understand how to use dot-and-cross diagrams to represent covalent bonds in: diatomic molecules, including hydrogen, oxygen, nitrogen, halogens and hydrogen halides, inorganic molecules including water, ammonia and carbon dioxide, organic molecules containing up to two carbon atoms, including methane, ethane, ethene and those containing halogen atoms

1:47 explain why substances with a simple molecular structures are gases or liquids, or solids with low melting and boiling points. The term intermolecular forces of attraction can be used to represent all forces between molecules

1:48 explain why the melting and boiling points of substances with simple molecular structures increase, in general, with increasing relative molecular mass

2:09 know the approximate percentages by volume of the four most abundant gases in dry air

2:10 understand how to determine the percentage by volume of oxygen in air using experiments involving the reactions of metals (e.g. iron) and non-metals (e.g. phosphorus) with air

2:11 describe the combustion of elements in oxygen, including magnesium, hydrogen and sulfur

2:12 describe the formation of carbon dioxide from the thermal decomposition of metal carbonates, including copper(II) carbonate

2:13 know that carbon dioxide is a greenhouse gas and that increasing amounts in the atmosphere may contribute to climate change

2:14 Practical: determine the approximate percentage by volume of oxygen in air using a metal or a non-metal

2:28a describe the use of litmus to distinguish between acidic and alkaline solutions

2:28 describe the use of litmus, phenolphthalein and methyl orange to distinguish between acidic and alkaline solutions

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)

2:30 describe the use of Universal Indicator to measure the approximate pH value of an aqueous solution

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

2:32 know that bases can neutralise acids

2:37 describe the reactions of hydrochloric acid, sulfuric acid and nitric acid with metals, bases and metal carbonates (excluding the reactions between nitric acid and metals) to form salts

2:38 know that metal oxides, metal hydroxides and ammonia can act as bases, and that alkalis are bases that are soluble in water

2:42 practical: prepare a sample of pure, dry hydrated copper(II) sulfate crystals starting from copper(II) oxide

2:44a describe tests for these gases: hydrogen, carbon dioxide

2:44 describe tests for these gases: hydrogen, oxygen, carbon dioxide, ammonia, chlorine

2:49 describe a test for the presence of water using anhydrous copper(II) sulfate

2:50 describe a physical test to show whether a sample of water is pure

3:01 know that chemical reactions in which heat energy is given out are described as exothermic, and those in which heat energy is taken in are described as endothermic

4:01 know that a hydrocarbon is a compound of hydrogen and carbon only

4:02a understand how to represent organic molecules using molecular formulae, general formulae, structural formulae and displayed formulae

4:02 understand how to represent organic molecules using empirical formulae, molecular formulae, general formulae, structural formulae and displayed formulae

4:03a know what is meant by the term isomerism

4:04 understand how to name compounds relevant to this specification using the rules of International Union of Pure and Applied Chemistry (IUPAC) nomenclature. Students will be expected to name compounds containing up to six carbon atoms

4:05 understand how to write the possible structural and displayed formulae of an organic molecule given its molecular formula

4:07 know that crude oil is a mixture of hydrocarbons

4:08 describe how the industrial process of fractional distillation separates crude oil into fractions

4:09 know the names and uses of the main fractions obtained from crude oil: refinery gases, gasoline, kerosene, diesel, fuel oil and bitumen

4:10 know the trend in colour, boiling point and viscosity of the main fractions

4:11 know that a fuel is a substance that, when burned, releases heat energy

4:12 know the possible products of complete and incomplete combustion of hydrocarbons with oxygen in the air

4:13 understand why carbon monoxide is poisonous, in terms of its effect on the capacity of blood to transport oxygen references to haemoglobin are not required

4:14 know that, in car engines, the temperature reached is high enough to allow nitrogen and oxygen from air to react, forming oxides of nitrogen

4:15 explain how the combustion of some impurities in hydrocarbon fuels results in the formation of sulfur dioxide

4:16 understand how sulfur dioxide and oxides of nitrogen oxides contribute to acid rain

4:19 know the general formula for alkanes

4:20 explain why alkanes are classified as saturated hydrocarbons

4:21 understand how to draw the structural and displayed formulae for alkanes with up to five carbon atoms in the molecule, and to name the unbranched-chain isomers