Science 4XSD1 — specification explorer

1. States of matter

• 1.1understand the three states of matter in terms of the arrangement, movement and energy of the particlesUnit 3
• 1.2

  understand the interconversions between the three states of matter in terms of:

  • the names of the interconversions
  • how they are achieved
  • the changes in arrangement, movement and energy of the particles
  Unit 3
• 1.3understand how the results of experiments involving the dilution of coloured solutions and diffusion of gases can be explainedUnit 3
• 1.4

  know what is meant by the terms:

  • solvent
  • solute
  • solution
  • saturated solution
  Unit 3

2. Elements, compounds and mixtures

• 1.8understand how to classify a substance as an element, compound or mixtureUnit 3
• 1.9understand that a pure substance has a fixed melting and boiling point, but that a mixture may melt or boil over a range of temperaturesUnit 3
• 1.10

  describe these experimental techniques for the separation of mixtures:

  • simple distillation
  • fractional distillation
  • filtration
  • crystallisation
  • paper chromatography
  Unit 3
• 1.11understand how a chromatogram provides information about the composition of a mixtureUnit 3
• 1.12understand how to use the calculation of Rfvalues to identify the components of a mixtureUnit 3
• 1.13practical: investigate paper chromatography using inks/food colouringsUnit 3

3. Atomic structure

• 1.14know what is meant by the terms ‘atom’ and ‘molecule’Unit 3
• 1.15know the structure of an atom in terms of the positions, relative masses and relative charges of sub-atomic particlesUnit 3
• 1.16know what is meant by the terms: atomic number, mass number, isotopes and relative atomic mass (Ar)Unit 3
• 1.17be able to calculate the relative atomic mass of an element (Ar) from isotopic abundancesUnit 3

4. The Periodic Table

• 1.18

  understand how elements are arranged in the Periodic Table:

  • in order of atomic number
  • in groups and periods
  Unit 3
• 1.19understand how to deduce the electronic configurations of the first 20 elements from their positions in the Periodic TableUnit 3
• 1.20understand how to use electrical conductivity and the acid-base character of oxides to classify elements as metals or non-metalsUnit 3
• 1.21identify an element as a metal or a non-metal according to its position in the Periodic TableUnit 3
• 1.22understand how the electronic configuration of a main group element is related to its position in the Periodic TableUnit 3
• 1.23understand why elements in the same group of the Periodic Table have similar chemical propertiesUnit 3
• 1.24understand why the noble gases (Group 0) do not readily reactUnit 3

5. Chemical formulae, equations and calculations

• 1.25

  write word equations and balanced chemical equations (including state symbols):

  • for reactions studied in this specification
  • for unfamiliar reactions where suitable information is provided
  Unit 3
• 1.26calculate relative formula masses (including relative molecular masses) (Mr) from relative atomic masses (Ar)Unit 3
• 1.27know that the mole (mol) is the unit for the amount of a substanceUnit 3
• 1.28understand how to carry out calculations involving amount of substance, relative atomic mass (Ar) and relative formula mass (Mr)Unit 3
• 1.29calculate reacting masses using experimental data and chemical equationsUnit 3
• 1.30calculate percentage yieldUnit 3
• 1.31understand how the formulae of simple compounds can be obtained experimentally, including metal oxides, water and salts containing water of crystallisationUnit 3
• 1.32know what is meant by the terms ‘empirical formula’ and ‘molecular formula’Unit 3
• 1.33calculate empirical and molecular formulae from experimental dataUnit 3
• 1.36practical: know how to determine the formula of a metal oxide by combustion (e.g. magnesium oxide) or by reduction (e.g. copper(II) oxide)Unit 3

1. Reactivity series

• 2.1

  understand how metals can be arranged in a reactivity series based on their reactions with:

  • water
  • dilute hydrochloric or sulfuric acid
  Unit 3
• 2.2

  understand how metals can be arranged in a reactivity series based on their displacement reactions between:

  • metals and metal oxides
  • metals and aqueous solutions of metal salts
  Unit 3
• 2.3know the order of reactivity of these metals: potassium, sodium, lithium, calcium, magnesium, aluminium, zinc, iron, copper, silver, goldUnit 3
• 2.4know the conditions under which iron rustsUnit 3
• 2.5

  understand how the rusting of iron may be prevented by:

  • barrier methods
  • galvanising
  • sacrificial protection
  Unit 3
• 2.6

  understand the terms:

  • oxidation
  • reduction
  • redox
  • oxidising agent
  • reducing agent in terms of gain or loss of oxygen and loss or gain of electrons
  Unit 3
• 2.7practical: investigate reactions between dilute hydrochloric and sulfuric acids, and metals (e.g. magnesium, zinc and iron)Unit 3

2. Acids, alkalis and titrations

• 2.14describe the use of litmus, phenolphthalein and methyl orange to distinguish between acidic and alkaline solutionsUnit 3
• 2.15understand 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)Unit 3
• 2.16describe the use of universal indicator to measure the approximate pH value of an aqueous solutionUnit 3
• 2.17know that acids in aqueous solution are a source of hydrogen ions and alkalis in a aqueous solution are a source of hydroxide ionsUnit 3
• 2.18know that alkalis can neutralise acidsUnit 3

3. Acids, bases and salt preparations

• 2.20

  know the general rules for predicting the solubility of ionic compounds in water:

  • common sodium, potassium and ammonium compounds are soluble
  • all nitrates are soluble
  • common chlorides are soluble, except those of silver and lead(II)
  • common sulfates are soluble, except for those of barium, calcium and lead(II)
  • common carbonates are insoluble, except for those of sodium, potassium and ammonium
  • common hydroxides are insoluble except for those of sodium, potassium and calcium (calcium hydroxide is slightly soluble)
  Unit 3
• 2.21understand acids and bases in terms of proton transferUnit 3
• 2.22understand that an acid is a proton donor and a base is a proton acceptorUnit 3
• 2.23describe 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 saltsUnit 3
• 2.24know that metal oxides, metal hydroxides and ammonia can act as bases, and that alkalis are bases that are soluble in waterUnit 3
• 2.25describe an experiment to prepare a pure, dry sample of a soluble salt, starting from an insoluble reactantUnit 3
• 2.28practical: prepare a sample of pure, dry hydrated copper(II) sulfate crystals starting from copper(II) oxideUnit 3

1. Energetics

• 3.1know 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 endothermicUnit 3
• 3.2describe simple calorimetry experiments for reactions such as combustion, displacement, dissolving and neutralisationUnit 3
• 3.3calculate the heat energy change from a measured temperature change using the expression Q=mcΔTUnit 3
• 3.4calculate the molar enthalpy change (ΔH) from the heat energy changeQUnit 3
• 3.8

  practical: investigate temperature changes accompanying some of the following types of change:

  • salts dissolving in water
  • neutralisation reactions
  • displacement reactions
  • combustion reactions
  Unit 3

1. Introduction

• 4.1know that a hydrocarbon is a compound of hydrogen and carbon onlyUnit 3
• 4.2understand how to represent organic molecules using empirical formulae, molecular formulae, general formulae, structural formulae and displayed formulaeUnit 3
• 4.3know what is meant by the terms: homologous series, functional group and isomerismUnit 3
• 4.4understand how to name compounds relevant to this specification using the rules of International Union of Pure and Applied Chemistry (IUPAC) nomenclature learners will be expected to name compounds containing up to six carbon atomsUnit 3
• 4.5understand how to write the possible structural and displayed formulae of an organic molecule given its molecular formulaUnit 3
• 4.6understand how to classify reactions of organic compounds as substitution, addition and combustion knowledge of reaction mechanisms is not requiredUnit 3

2. Crude oil

• 4.7know that crude oil is a mixture of hydrocarbonsUnit 3
• 4.8describe how the industrial process of fractional distillation separates crude oil into fractionsUnit 3
• 4.9know the names and uses of the main fractions obtained from crude oil: refinery gases, gasoline, kerosene, diesel, fuel oil and bitumenUnit 3
• 4.10know the trend in colour, boiling point and viscosity of the main fractionsUnit 3
• 4.11know that a fuel is a substance that, when burned, releases heat energyUnit 3
• 4.12know the possible products of complete and incomplete combustion of hydrocarbons with oxygen in the airUnit 3
• 4.13understand why carbon monoxide is poisonous, in terms of its effect on the capacity of blood to transport oxygen references to haemoglobin are not requiredUnit 3
• 4.14know that, in car engines, the temperature reached is high enough to allow nitrogen and oxygen from air to react, forming oxides of nitrogenUnit 3
• 4.15explain how the combustion of some impurities in hydrocarbon fuels results in the formation of sulfur dioxideUnit 3
• 4.16understand how sulfur dioxide and oxides of nitrogen contribute to acid rainUnit 3
• 4.17describe how long-chain alkanes are converted to alkenes and shorter-chain alkanes by catalytic cracking (using silica or alumina as the catalyst and a temperature in the range of 600–700ºC)Unit 3
• 4.18explain why cracking is necessary, in terms of the balance between supply and demand for different fractionsUnit 3

3. Alkanes

• 4.19know the general formula for alkanesUnit 3
• 4.20explain why alkanes are classified as saturated hydrocarbonsUnit 3
• 4.21understand 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 isomersUnit 3
• 4.22describe the reactions of alkanes with halogens in the presence of ultraviolet radiation, limited to mono-substitution knowledge of reaction mechanisms is not requiredUnit 3

4. Alkenes

• 4.23know that alkenes contain the functional group >C=C<Unit 3
• 4.24know the general formula for alkenesUnit 3
• 4.25explain why alkenes are classified as unsaturated hydrocarbonsUnit 3
• 4.26understand how to draw the structural and displayed formulae for alkenes with up to four carbon atoms in the molecule, and name the unbranched-chain isomers knowledge of cis/trans or E/Z notation is not requiredUnit 3
• 4.27describe the reactions of alkenes with bromine to produce dibromoalkanesUnit 3
• 4.28describe how bromine water can be used to distinguish between an alkane and an alkeneUnit 3