Recommended O Level Chemistry Text Book for Final Cambridge Exam
O Level Chemistry Syllabus
Cambridge O Level Chemistry (5070)
Use this syllabus for exams in 2022. Exams are available in the June and November series.
Syllabus content
1. Experimental chemistry
Content
1.1 Experimental design
1.2 Methods of purification and analysis
1.3 Identification of ions and gases
It is expected that any course in chemistry will be based on experimental work. Teachers are encouraged to develop appropriate practical work for candidates to facilitate a greater understanding of the subject. Candidates should be aware of the hazards and appropriate safety precautions to follow when handling the reagents mentioned in this section.
Learning outcomes
Candidates should be able to:
1.1 Experimental design
(a) name appropriate apparatus for the measurement of time, temperature, mass and volume, including burettes, pipettes, measuring cylinders and gas syringes
(b) suggest suitable apparatus, given relevant information, for a variety of simple experiments, including collection of gases and measurement of rates of reaction
1.2 Methods of purification and analysis
(a) describe methods of purification by the use of a suitable solvent, filtration and crystallisation, distillation and fractional distillation, with particular references to the fractional distillation of crude oil, liquid air and mixtures of liquids
(b) suggest suitable methods of purification, given information about the substances involved
(c) describe paper chromatography and interpret chromatograms including comparison with ‘known’ samples and the use of Rf values
(d) explain the need to use locating agents in the chromatography of colourless compounds
(e) deduce from given melting point and boiling point information, the identities of substances and their purity
(f) explain that the measurement of purity in substances used in everyday life, e.g. foodstuffs and drugs, is important
1.3 Identification of ions and gases
(a) describe the use of aqueous sodium hydroxide and aqueous ammonia to identify the following aqueous cations: aluminium, ammonium, calcium, chromium(III), copper(II), iron(II), iron(III) and zinc (formulae of complex ions are not required)
(b) describe tests to identify the following anions: carbonate (by the addition of dilute acid and subsequent use of limewater); chloride (by reaction of an aqueous solution with nitric acid and aqueous silver nitrate); iodide (by reaction of an aqueous solution with nitric acid and aqueous silver nitrate); nitrate (by reduction with aluminium and aqueous sodium hydroxide to ammonia and subsequent use of litmus paper), sulfate (by reaction of an aqueous solution with nitric acid and aqueous barium nitrate), and sulfite (by warming with dilute acid)
(c) describe tests to identify the following gases: ammonia (using damp red litmus paper); carbon dioxide (using limewater); chlorine (using damp litmus paper); hydrogen (using a burning splint); oxygen (using a glowing splint) and sulfur dioxide (using acidified potassium manganate(VII))
d) describe a chemical test for water
2 The particulate nature of matter
Content
2.1 Kinetic particle theory
2.2 Atomic structure
2.3 Structure and properties of materials
2.4 Ionic bonding
2.5 Covalent bonding
2.6 Metallic bonding
Learning outcomes Candidates should be able to:
2.1 Kinetic particle theory
(a) describe the solid, liquid and gaseous states of matter and explain their interconversion in terms of the kinetic particle theory and of the energy changes involved
(b) describe and explain evidence for the movement of particles in liquids and gases (the treatment of Brownian motion is not required)
(c) explain everyday effects of diffusion in terms of particles, e.g. the spread of perfumes and cooking aromas; tea and coffee grains in water
(d) state qualitatively the effect of molecular mass on the rate of diffusion and explain the dependence of rate of diffusion on temperature
(e) state qualitatively and explain the effects of temperature and pressure on the volumes of gases
2.2 Atomic structure
(a) state the relative charges and approximate relative masses of a proton, a neutron and an electron
(b) describe, with the aid of diagrams, the structure of an atom as containing protons and neutrons (nucleons) in the nucleus and electrons arranged in shells (energy levels) (no knowledge of s, p, d and f classification will be expected; a copy of the Periodic Table will be available in Papers 1 and 2)
(c) define proton number and nucleon number
(d) interpret and use symbols such as 6C12
(e) define the term isotopes
(f) deduce the numbers of protons, neutrons and electrons in atoms and ions from proton and nucleon numbers
Content
1.1 Experimental design
1.2 Methods of purification and analysis
1.3 Identification of ions and gases
It is expected that any course in chemistry will be based on experimental work. Teachers are encouraged to develop appropriate practical work for candidates to facilitate a greater understanding of the subject. Candidates should be aware of the hazards and appropriate safety precautions to follow when handling the reagents mentioned in this section.
Learning outcomes
Candidates should be able to:
1.1 Experimental design
(a) name appropriate apparatus for the measurement of time, temperature, mass and volume, including burettes, pipettes, measuring cylinders and gas syringes
(b) suggest suitable apparatus, given relevant information, for a variety of simple experiments, including collection of gases and measurement of rates of reaction
1.2 Methods of purification and analysis
(a) describe methods of purification by the use of a suitable solvent, filtration and crystallisation, distillation and fractional distillation, with particular references to the fractional distillation of crude oil, liquid air and mixtures of liquids
(b) suggest suitable methods of purification, given information about the substances involved
(c) describe paper chromatography and interpret chromatograms including comparison with ‘known’ samples and the use of Rf values
(d) explain the need to use locating agents in the chromatography of colourless compounds
(e) deduce from given melting point and boiling point information, the identities of substances and their purity
(f) explain that the measurement of purity in substances used in everyday life, e.g. foodstuffs and drugs, is important
1.3 Identification of ions and gases
(a) describe the use of aqueous sodium hydroxide and aqueous ammonia to identify the following aqueous cations: aluminium, ammonium, calcium, chromium(III), copper(II), iron(II), iron(III) and zinc (formulae of complex ions are not required)
(b) describe tests to identify the following anions: carbonate (by the addition of dilute acid and subsequent use of limewater); chloride (by reaction of an aqueous solution with nitric acid and aqueous silver nitrate); iodide (by reaction of an aqueous solution with nitric acid and aqueous silver nitrate); nitrate (by reduction with aluminium and aqueous sodium hydroxide to ammonia and subsequent use of litmus paper), sulfate (by reaction of an aqueous solution with nitric acid and aqueous barium nitrate), and sulfite (by warming with dilute acid)
(c) describe tests to identify the following gases: ammonia (using damp red litmus paper); carbon dioxide (using limewater); chlorine (using damp litmus paper); hydrogen (using a burning splint); oxygen (using a glowing splint) and sulfur dioxide (using acidified potassium manganate(VII))
d) describe a chemical test for water
2 The particulate nature of matter
Content
2.1 Kinetic particle theory
2.2 Atomic structure
2.3 Structure and properties of materials
2.4 Ionic bonding
2.5 Covalent bonding
2.6 Metallic bonding
Learning outcomes Candidates should be able to:
2.1 Kinetic particle theory
(a) describe the solid, liquid and gaseous states of matter and explain their interconversion in terms of the kinetic particle theory and of the energy changes involved
(b) describe and explain evidence for the movement of particles in liquids and gases (the treatment of Brownian motion is not required)
(c) explain everyday effects of diffusion in terms of particles, e.g. the spread of perfumes and cooking aromas; tea and coffee grains in water
(d) state qualitatively the effect of molecular mass on the rate of diffusion and explain the dependence of rate of diffusion on temperature
(e) state qualitatively and explain the effects of temperature and pressure on the volumes of gases
2.2 Atomic structure
(a) state the relative charges and approximate relative masses of a proton, a neutron and an electron
(b) describe, with the aid of diagrams, the structure of an atom as containing protons and neutrons (nucleons) in the nucleus and electrons arranged in shells (energy levels) (no knowledge of s, p, d and f classification will be expected; a copy of the Periodic Table will be available in Papers 1 and 2)
(c) define proton number and nucleon number
(d) interpret and use symbols such as 6C12
(e) define the term isotopes
(f) deduce the numbers of protons, neutrons and electrons in atoms and ions from proton and nucleon numbers