Chemistry Specification

Topic 1: Principles of Chemistry

(a) States of Matter

• 1.1 Understand three states of matter in terms of:
  • Arrangement of particles
  • Movement of particles
  • Energy of particles
• 1.2 Understand interconversions between states:
  • Names of interconversions
  • How they are achieved
  • Changes in arrangement, movement and energy of particles
• 1.3 Understand how experiments involving dilution of coloured solutions and diffusion of gases can be explained
• 1.4 Know what is meant by the terms:
  • Solvent
  • Solute
  • Solution
  • Saturated solution

(b) Elements, Compounds and Mixtures

• 1.8 Understand how to classify a substance as:
  • Element
  • Compound
  • Mixture
• 1.9 Understand pure substance has fixed melting and boiling point, but mixture may melt/boil over range
• 1.10 Describe experimental techniques for separation:
  • Simple distillation
  • Fractional distillation
  • Filtration
  • Crystallisation
  • Paper chromatography
• 1.11 Understand how chromatogram provides information about composition of mixture
• 1.12 Understand how to use Rf values to identify components of mixture
• PRACTICAL: Investigate paper chromatography using inks/food colourings

(c) Atomic Structure

• 1.14 Know what is meant by:
  • Atom
  • Molecule
• 1.15 Know structure of atom in terms of:
  • Positions of sub-atomic particles
  • Relative masses of sub-atomic particles
  • Relative charges of sub-atomic particles
• 1.16 Know what is meant by:
  • Atomic number
  • Mass number
  • Isotopes
  • Relative atomic mass (Ar)
• 1.17 Calculate relative atomic mass from isotopic abundances

(d) The Periodic Table

• 1.18 Understand how elements are arranged in Periodic Table:
  • In order of atomic number
  • In groups and periods
• 1.19 Understand how to deduce electronic configurations of first 20 elements
• 1.20 Understand how to use electrical conductivity and acid-base character of oxides to classify elements
• 1.21 Identify element as metal or non-metal from position in Periodic Table
• 1.22 Understand how electronic configuration of main group element relates to position
• 1.23 Understand why elements in same group have similar chemical properties
• 1.24 Understand why noble gases (Group 0) do not readily react

(e) Chemical Formulae, Equations and Calculations

• 1.25 Write word equations and balanced chemical equations (including state symbols)
• 1.26 Calculate relative formula masses (Mr) from relative atomic masses (Ar)
• 1.27 Know mole (mol) is unit for amount of substance
• 1.28 Understand how to carry out calculations involving:
  • Amount of substance
  • Relative atomic mass (Ar)
  • Relative formula mass (Mr)
• 1.29 Calculate reacting masses using experimental data and chemical equations
• 1.30 Calculate percentage yield
• 1.31 Understand how formulae of simple compounds can be obtained experimentally
• 1.32 Know what is meant by:
  • Empirical formula
  • Molecular formula
• 1.33 Calculate empirical and molecular formulae from experimental data
• PRACTICAL: Determine formula of metal oxide by combustion or reduction

(f) Ionic Bonding

• 1.37 Understand how ions are formed by electron loss or gain
• 1.38 Know charges of these ions:
  • Metals in Groups 1, 2 and 3
  • Non-metals in Groups 5, 6 and 7
  • Common ions: Ag+, Cu2+, Fe2+, Fe3+, Pb2+, Zn2+
  • H+, OH–, NH4+, CO32–, NO3–, SO42–
• 1.39 Write formulae for compounds formed between listed ions
• 1.40 Draw dot-and-cross diagrams for ionic compounds (outer electrons only)
• 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
• 1.43 Know ionic compounds:
  • Do not conduct electricity when solid
  • Do conduct electricity when molten and in aqueous solution

(g) Covalent Bonding

• 1.44 Know covalent bond is formed by sharing pair of electrons
• 1.45 Understand covalent bonds in terms of electrostatic attractions
• 1.46 Understand how to use dot-and-cross diagrams for:
  • Diatomic molecules (H2, O2, N2, halogens, hydrogen halides)
  • Inorganic molecules (water, ammonia, carbon dioxide)
  • Organic molecules with up to 2 carbons
• 1.47 Explain why substances with simple molecular structures have low melting/boiling points
• 1.48 Explain why melting/boiling points of simple molecular substances increase with relative molecular mass
• 1.49 Explain why substances with giant covalent structures have high melting/boiling points
• 1.50 Explain how structures of diamond, graphite and C60 influence properties
• 1.51 Know covalent compounds do not usually conduct electricity

Topic 2: Inorganic Chemistry

(a) Group 1 (Alkali Metals)

• 2.1 Understand how similarities in reactions with water provide evidence for family of elements
• 2.2 Understand how differences in reactions with air and water provide evidence for trend in reactivity
• 2.3 Use knowledge of trends to predict properties of other alkali metals

(b) Group 7 (Halogens)

• 2.5 Know colours, physical states and trends in physical properties
• 2.6 Use knowledge of trends to predict properties of other halogens
• 2.7 Understand how displacement reactions provide evidence for trend in reactivity

(c) Gases in the Atmosphere

• 2.9 Know approximate percentages by volume of four most abundant gases in dry air
• 2.10 Understand how to determine percentage by volume of oxygen in air
• 2.11 Describe combustion of elements in oxygen:
  • Magnesium
  • Hydrogen
  • Sulfur
• 2.12 Describe formation of carbon dioxide from thermal decomposition of metal carbonates
• 2.13 Know carbon dioxide is greenhouse gas contributing to climate change
• PRACTICAL: Determine approximate percentage by volume of oxygen in air

(d) Reactivity Series

• 2.15 Understand how metals can be arranged in reactivity series based on reactions with:
  • Water
  • Dilute hydrochloric or sulfuric acid
• 2.16 Understand arrangement based on displacement reactions between:
  • Metals and metal oxides
  • Metals and aqueous solutions of metal salts
• 2.17 Know order of reactivity: K, Na, Li, Ca, Mg, Al, Zn, Fe, Cu, Ag, Au
• 2.18 Know conditions under which iron rusts
• 2.19 Understand how rusting may be prevented by:
  • Barrier methods
  • Galvanising
  • Sacrificial protection
• 2.20 Understand the terms:
  • Oxidation
  • Reduction
  • Redox
  • Oxidising agent
  • Reducing agent (in terms of gain/loss of oxygen and electrons)
• PRACTICAL: Investigate reactions between dilute acids and metals

(e) Acids, Alkalis and Titrations

• 2.28 Describe use of indicators:
  • Litmus
  • Phenolphthalein
  • Methyl orange
• 2.29 Understand how to use pH scale (0-14):
  • Strongly acidic (0-3)
  • Weakly acidic (4-6)
  • Neutral (7)
  • Weakly alkaline (8-10)
  • Strongly alkaline (11-14)
• 2.30 Describe use of universal indicator to measure approximate pH
• 2.31 Know acids are source of H+ ions and alkalis are source of OH– ions
• 2.32 Know alkalis can neutralise acids

(f) Acids, Bases and Salt Preparations

• 2.34 Know general rules for predicting solubility of ionic compounds in water
• 2.35 Understand acids and bases in terms of proton transfer
• 2.36 Understand acid is proton donor and base is proton acceptor
• 2.37 Describe reactions of acids with metals, bases and carbonates to form salts
• 2.38 Know metal oxides, metal hydroxides and ammonia can act as bases
• 2.39 Describe experiment to prepare pure, dry sample of soluble salt from insoluble reactant
• PRACTICAL: Prepare sample of pure, dry hydrated copper(II) sulfate crystals

(g) Chemical Tests

• 2.44 Describe tests for gases:
  • Hydrogen
  • Oxygen
  • Carbon dioxide
  • Ammonia
  • Chlorine
• 2.45 Describe how to carry out flame test
• 2.46 Know colours formed in flame tests:
  • Li+ = red
  • Na+ = yellow
  • K+ = lilac
  • Ca2+ = orange-red
  • Cu2+ = blue-green
• 2.47 Describe tests for cations:
  • NH4+ using sodium hydroxide solution
  • Cu2+, Fe2+, Fe3+ using sodium hydroxide solution
• 2.48 Describe tests for anions:
  • Cl–, Br–, I– using acidified silver nitrate
  • SO42– using acidified barium chloride
  • CO32– using hydrochloric acid
• 2.49 Describe test for water using anhydrous copper(II) sulfate
• 2.50 Describe physical test to show whether water is pure

Topic 3: Physical Chemistry

(a) Energetics

• 3.1 Know chemical reactions can be:
  • Exothermic (heat energy given out)
  • Endothermic (heat energy taken in)
• 3.2 Describe simple calorimetry experiments for:
  • Combustion
  • Displacement
  • Dissolving
  • Neutralisation
• 3.3 Calculate heat energy change using Q = mcΔT
• 3.4 Calculate molar enthalpy change (ΔH) from heat energy change Q
• PRACTICAL: Investigate temperature changes for:
  • Salts dissolving in water
  • Neutralisation reactions
  • Displacement reactions
  • Combustion reactions

(b) Rates of Reaction

• 3.9 Describe experiments to investigate effects on rate of:
  • Surface area of solid
  • Concentration of solution
  • Temperature
  • Use of catalyst
• 3.10 Describe effects of changes in these factors on rate
• 3.11 Explain effects using particle collision theory
• 3.12 Know catalyst increases rate but is chemically unchanged
• 3.13 Know catalyst works by providing alternative pathway with lower activation energy
• PRACTICAL: Investigate effect of:
  • Surface area of marble chips
  • Concentration of hydrochloric acid on rate of reaction
• PRACTICAL: Investigate effect of different solids on catalytic decomposition of hydrogen peroxide

(c) Reversible Reactions and Equilibria

• 3.17 Know some reactions are reversible (indicated by ⇌)
• 3.18 Describe reversible reactions:
  • Dehydration of hydrated copper(II) sulfate
  • Effect of heat on ammonium chloride

Topic 4: Organic Chemistry

(a) Introduction

• 4.1 Know hydrocarbon is compound of hydrogen and carbon only
• 4.2 Understand how to represent organic molecules using:
  • Empirical formulae
  • Molecular formulae
  • General formulae
  • Structural formulae
  • Displayed formulae
• 4.3 Know what is meant by:
  • Homologous series
  • Functional group
  • Isomerism
• 4.4 Understand how to name compounds using IUPAC nomenclature (up to 6 carbons)
• 4.5 Understand how to write possible structural and displayed formulae from molecular formula
• 4.6 Understand how to classify reactions as:
  • Substitution
  • Addition
  • Combustion

(b) Crude Oil

• 4.7 Know crude oil is mixture of hydrocarbons
• 4.8 Describe industrial process of fractional distillation
• 4.9 Know names and uses of main fractions:
  • Refinery gases
  • Gasoline
  • Kerosene
  • Diesel
  • Fuel oil
  • Bitumen
• 4.10 Know trend in colour, boiling point and viscosity of fractions
• 4.11 Know fuel releases heat energy when burned
• 4.12 Know possible products of complete and incomplete combustion
• 4.13 Understand why carbon monoxide is poisonous (effect on blood oxygen transport)
• 4.14 Know nitrogen and oxygen from air react at high temperatures forming oxides of nitrogen
• 4.15 Explain how combustion of impurities results in sulfur dioxide formation
• 4.16 Understand how sulfur dioxide and nitrogen oxides contribute to acid rain
• 4.17 Describe how long-chain alkanes are converted to alkenes and shorter-chain alkanes by cracking
• 4.18 Explain why cracking is necessary (balance between supply and demand)

(c) Alkanes

• 4.19 Know general formula for alkanes
• 4.20 Explain why alkanes are classified as saturated hydrocarbons
• 4.21 Understand how to draw structural and displayed formulae for alkanes (up to 5 carbons)
• 4.22 Describe reactions of alkanes with halogens in UV radiation (mono-substitution)

(d) Alkenes

• 4.23 Know alkenes contain >C=C< functional group
• 4.24 Know general formula for alkenes
• 4.25 Explain why alkenes are classified as unsaturated hydrocarbons
• 4.26 Understand how to draw formulae for alkenes (up to 4 carbons)
• 4.27 Describe reactions of alkenes with bromine to produce dibromoalkanes
• 4.28 Describe how bromine water distinguishes between alkane and alkene

(e) Synthetic Polymers

• 4.44 Know addition polymer is formed by joining monomers
• 4.45 Understand how to draw repeat unit of addition polymers
• 4.46 Understand how to deduce monomer from repeat unit and vice versa
• 4.47 Explain problems in disposal of addition polymers:
  • Inertness and inability to biodegrade
  • Production of toxic gases when burned