Introduction
Chapter-1. States of matter
1.1 understand the three states of matter in terms of the arrangement, movement and
energy of the particles
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.
1.3 understand how the results of experiments involving the 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.
1.5C know what is meant by the term solubility in the units g per 100 g of solvent
1.6C understand how to plot and interpret solubility curves
1.7C practical: investigate the solubility of a solid in water at a specific temperature
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Chapter-2. Elements, compounds and mixtures.
2.1.1 understand how to classify a substance as an element, compound or mixture
2.1.2understand that a pure substance has a fixed melting and boiling point, but that a
mixture may melt or boil over a range of temperatures
2.1.3 describe these experimental techniques for the separation of mixtures:
• simple distillation
• fractional distillation
• filtration
• crystallisation
• paper chromatography.
2.1.4 understand how a chromatogram provides information about the composition of a
mixture
2.1.5 understand how to use the calculation of Rf values to identify the components of a
mixture
2.1.6 practical: investigate paper chromatography using inks/food colourings
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Chapter-3. Atomic structure
3.1.1 know what is meant by the terms atom and molecule
3.1.2 know the structure of an atom in terms of the positions, relative masses and relative
charges of sub-atomic particles
3.1.3 know what is meant by the terms atomic number, mass number, isotopes and relative
atomic mass (Ar)
3.1.4 be able to calculate the relative atomic mass of an element (Ar) from isotopic
abundances
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Chapter-4. The Periodic Table.
4.1.1 understand how elements are arranged in the Periodic Table:
• in order of atomic number
• in groups and periods.
4.1.2 understand how to deduce the electronic configurations of the first 20 elements from
their positions in the Periodic Table
4.1.3 understand how to use electrical conductivity and the acid-base character of oxides to
classify elements as metals or non-metals
4.1.4 identify an element as a metal or a non-metal according to its position in the Periodic
Table
4.1.5 understand how the electronic configuration of a main group element is related to its
position in the Periodic Table4.1.6 understand why elements in the same group of the Periodic Table have similar
chemical properties
4.1.7 understand why the noble gases (Group 0) do not readily react
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Chapter-5. Chemical formulae, equations and calculations.
5.1.1 write word equations and balanced chemical equations (including state symbols):
• for reactions studied in this specification
• for unfamiliar reactions where suitable information is provided.
5.1.2 calculate relative formula masses (including relative molecular masses) (Mr) from
relative atomic masses (Ar)
5.1.3 know that the mole (mol) is the unit for the amount of a substance
5.1.4 understand how to carry out calculations involving amount of substance, relative
atomic mass (Ar) and relative formula mass (Mr)
5.1.5 calculate reacting masses using experimental data and chemical equations
5.1.6 calculate percentage yield
5.1.7 understand how the formulae of simple compounds can be obtained experimentally,
including metal oxides, water and salts containing water of crystallisation
5.1.8 know what is meant by the terms empirical formula and molecular formula
5.1.9 calculate empirical and molecular formulae from experimental data
5.1.10 understand how to carry out calculations involving amount of substance,
volume and concentration (in mol/dm3) of solution
5.1.11 understand how to carry out calculations involving gas volumes and the
molar volume of a gas (24 dm3 and 24 000 cm3 at room temperature and
pressure (rtp))
5.1.12 practical: know how to determine the formula of a metal oxide by combustion
(e.g. magnesium oxide) or by reduction (e.g. copper(II) oxide)
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Chapter-6. Group 1 (alkali metals) – lithium, sodium and potassium
6.1.1 understand how the similarities in the reactions of these elements with water provide
evidence for their recognition as a family of elements
6.1.2 understand how the differences between the reactions of these elements with air and
water provide evidence for the trend in reactivity in Group 1
6.1.3 use knowledge of trends in Group 1 to predict the properties of other alkali metals
6.1.4 explain the trend in reactivity in Group 1 in terms of electronic
configurations
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Chapter-7. Group 7 (halogens) – chlorine, bromine and iodine.
7.1.1 know the colours, physical states (at room temperature) and trends in physical
properties of these elements
7.1.2 use knowledge of trends in Group 7 to predict the properties of other halogens
7.1.3 understand how displacement reactions involving halogens and halides provide
evidence for the trend in reactivity in Group 7
7.1.4 explain the trend in reactivity in Group 7 in terms of electronic
configurations
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Chapter-8. Gases in the atmosphere
8.1.1 know the approximate percentages by volume of the four most abundant gases in dry
air
8.1.2 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
8.1.3 describe the combustion of elements in oxygen, including magnesium, hydrogen and
sulfur
8.1.4 describe the formation of carbon dioxide from the thermal decomposition of metal
carbonates, including copper(II) carbonate
8.1.5 know that carbon dioxide is a greenhouse gas and that increasing amounts in the
atmosphere may contribute to climate change
8.1.6 practical: determine the approximate percentage by volume of oxygen in air using a
metal or a non-metal
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Chapter-9. Reactivity series.
9.1.1 understand how metals can be arranged in a reactivity series based on their reactions
with:
• water
• dilute hydrochloric or sulfuric acid.
9.1.2 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.
9.1.3 know the order of reactivity of these metals: potassium, sodium, lithium, calcium,
magnesium, aluminium, zinc, iron, copper, silver, gold
9.1.4 know the conditions under which iron rusts
9.1.5 understand how the rusting of iron may be prevented by:
• barrier methods
• galvanising
• sacrificial protection.
9.1.6 understand the terms:
• oxidation
• reduction
• redox
• oxidising agent
• reducing agent
in terms of gain or loss of oxygen and loss or gain of electrons.9.1.7 practical: investigate reactions between dilute hydrochloric and sulfuric acids and
metals (e.g. magnesium, zinc and iron)
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Chapter-10. Acids, alkalis and titrations.
10.1.1 describe the use of litmus, phenolphthalein and methyl orange to distinguish between
acidic and alkaline solutions
10.1.2 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)
10.1.3 describe the use of universal indicator to measure the approximate pH value of an
aqueous solution
10.1.4 know that acids in aqueous solution are a source of hydrogen ions and alkalis in a
aqueous solution are a source of hydroxide ions
10.1.5 know that alkalis can neutralise acids
10.1.6 describe how to carry out an acid-alkali titration
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Chapter-11. Acids, bases and salt preparations.
11.1.1 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).
11.1.2 understand acids and bases in terms of proton transfer
11.1.3 understand that an acid is a proton donor and a base is a proton acceptor
11.1.4 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
11.1.5 know that metal oxides, metal hydroxides and ammonia can act as bases, and that
alkalis are bases that are soluble in water
11.1.6 describe an experiment to prepare a pure, dry sample of a soluble salt, starting from
an insoluble reactant
11.1.7 describe an experiment to prepare a pure, dry sample of a soluble salt,
starting from an acid and alkali
11.1.8 describe an experiment to prepare a pure, dry sample of an insoluble salt,
starting from two soluble reactants
11.1.9 practical: prepare a sample of pure, dry hydrated copper(II) sulfate crystals starting
from copper(II) oxide
11.1.10 practical: prepare a sample of pure, dry lead(II) sulfate
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Chapter-12. Ionic Bonding
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Chapter-13. Covalent Bonding
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Chapter-14. Metallic Bonding
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Chapter-15. Electrolysis
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Chapter-16. Extraction and Uses of Metals
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Chapter-17. Chemical Tests
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Chapter-18. Energetics
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Chapter-19. Rates of Reactions
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Chapter-20. Reversible Reactions and Equilibria
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Chapter-21. Introduction of Organic Chemistry
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Chapter-22. Crude Oil
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Chapter-23. Alkanes
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Chapter-24. Alkenes
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Chapter-25. Alcohols
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Chapter-26. Carboxylic Acids
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Chapter-27. Esters
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Chapter-28. Synthetic Polymers
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Test Yourself