1.1: explain how evidence supports the particulate theory of matter;

1.2: distinguish among the three states of matter;

1.3: explain the changes between the three states of matter in terms of energy and arrangement of particles.

2.1: distinguish between pure substances and mixtures;

2.2: distinguish among solutions, suspensions and colloids;

2.3: identify different types of solutions;

2.4: investigate the effect of temperature on solubility of solids in water;

2.5: apply suitable separation techniques based on differences in properties of the components of mixtures;

2.6: describe the extraction of sucrose from sugar cane.

3.1: describe with illustrations, the structure of atoms of atomic number 1 to 20;

3.2: state properties of electrons, protons and neutrons;

3.3: define atomic number and mass number;

3.4: define relative atomic mass;

3.5: interpret notations of the form a/b X c/d;

3.6: define isotopy;

3.7: list uses of radioactive isotopes.

4.1: explain the basis for the arrangement of elements in the periodic table;

4.2: explain trends in Group II;

4.3: explain trends in Group VII;

4.4: identify trends in period 3;

4.5: predict properties of unknown elements based on the position in periodic table.

5.1: explain the formation of ionic and covalent bonds;

5.2: predict the likelihood of an atom forming an ionic or a covalent bond based on atomic structure;

5.3: write formulae to represent ions, molecules and formula units;

5.4: explain metallic bonding;

5.5: describe ionic crystals, simple molecular crystals and giant molecular crystals;

5.6: distinguish between ionic and molecular solids;

5.7: relate structure of sodium chloride, diamond and graphite to their properties and uses;

5.8: explain the term allotropy.

6.1: define mole and molar mass;

6.2: perform calculations involving the mole;

6.3: state Avogadro's Law;

6.4: state the Law of Conservation of Matter;

6.5: write balanced equations;

6.6: apply the mole concept to equations, both ionic and molecular;

6.7: define the term standard solution.

7.1: define acid, acid anhydride, base, alkali, salt, acidic, basic, amphoteric and neutral oxides;

7.2: relate acidity and alkalinity to the pH scale;

7.3: discuss the strength of acids and alkalis on the basis of their completeness of ionisation;

7.4: investigate the reactions of non-oxidising acids;

7.5: list examples of acids in living systems;

7.6: investigate the reaction of bases with ammonium salts;

7.7: identify an appropriate method of salt preparation based on the solubility of the salt;

7.8: list the uses and dangers of salts;

7.9: distinguish between acid salts and normal salts;

7.10: investigate neutralisation reactions using indicators and temperature changes;

7.11: perform calculations using volumetric analysis data.

8.1: investigate the action of common oxidising and reducing substances in everyday activities;

8.2: define oxidation and reduction;

8.3: deduce oxidation number from formulae;

8.4: identify oxidation and reduction reactions including reactions at electrodes;

8.5: distinguish between oxidising and reducing agents;

8.6: perform tests for oxidising and reducing agents.

9.1: conduct investigations leading to the classification of substances as conductors or non-conductors;

9.2: distinguish between metallic and electrolytic conduction;

9.3: classify electrolytes as strong or weak based on their conductivity;

9.4: define electrolysis, cathode, anode, cation, anion;

9.5: identify ions present in electrolytes;

9.6: predict the electrode to which an ion will drift;

9.7: predict chemical reactions making use of electrochemical series;

9.8: discuss the electrolysis of certain substances;

9.9: define the Faraday constant;

9.10: calculate the masses and volumes of substances liberated during electrolysis;

9.11: describe industrial applications of electrolysis.

10.1: define rate of reaction;

10.2: identify the factors which affect the rate of reaction;

10.3: predict the effect of factors on rates of reaction from given data;

10.4: interpret graphical representation of data obtained in studying rates of reaction.

11.1: distinguish between exothermic and endothermic reactions;

11.2: draw energy profile diagrams to illustrate endothermic and exothermic change;

11.3: calculate energy changes from experiments or from experimental data.

1.1: identify natural gas and petroleum as natural sources of hydrocarbons;

1.2: list the main uses of at least three fractions obtained from the fractional distillation of petroleum;

1.3: describe cracking of petroleum fractions.

2.1: illustrate that carbon atoms can form single and double bonds, branched and unbranched chains and ring compounds;

2.2: write formulae to represent simple organic compounds;

2.3: list the general characteristics of a homologous series;

2.4: write general and molecular formulae for members of a given homologous series;

2.5: deduce the homologous series given the fully displayed and condensed formulae of compounds;

2.6: write fully displayed structures and names of branched and unbranched alkanes and unbranched alkenes, alcohols, and alkanoic acid;

2.7: define structural isomerism;

2.8: write the fully displayed structures of isomers given their molecular formulae.

3.1: describe the reactions of alkanes and alkenes;

3.2: relate the characteristic reactions of alkanes and alkenes to their structures;

3.3: distinguish between alkanes and alkenes;

3.4: relate the properties of hydrocarbons to their uses;

3.5: identify alcohols, acids and esters by their functional groups;

3.6: relate the properties of alcohols, acids and esters to their functional groups;

3.7: describe the reactions of ethanol;

3.8: describe the fermentation process by which ethanol is produced from carbohydrates;

3.9: describe the reactions of ethanoic acid;

3.10: explain hydrolysis of esters including saponification;

3.11: compare soapy and soapless detergents.

4.1: define polymers;

4.2: distinguish between addition and condensation as reactions in the formation of polymers;

4.3: state at least one use of each of the following types of polymers.

1.1: describe the physical and chemical properties of metals;

1.2: describe the reactions of metallic oxides, hydroxides, nitrates and carbonates.

2.1: discuss the reactivity of metals;

2.2: deduce the order of reactivity of metals based on experimental results or data supplied;

2.3: describe the extraction of aluminum and iron.

3.1: explain why metal alloys are often used in place of the metals;

3.2: relate the properties of the metals (aluminum, lead, iron) and their alloys to their uses.

4.1: investigate the conditions necessary for the corrosion of metals;

4.2: explain the importance of metals and their compounds on living systems and environment;

4.3: discuss the harmful effect of metals and their compounds to living systems and the environment.

5.1: describe the physical and chemical properties of non-metals;

5.2: describe the laboratory preparation of gases;

5.3: explain the use of gases based on their properties;

5.4: list uses of the non-metals: carbon, sulfur, phosphorus, chlorine, nitrogen, silicon and their compounds;

5.5: discuss the harmful effects of non-metal on living systems and the environment;

5.6: relate the unique properties of water to its functions in living systems;

5.7: discuss the consequences of the solvent properties of water;

5.8: describe the methods used in the treatment of water for domestic purposes;

5.9: define Green Chemistry;

5.10: outline the principles of Green Chemistry.

6.1: identify cations - Pb²⁺, Al³⁺, Ca²⁺, Zn²⁺, Fe³⁺, Fe²⁺, NH₄⁺, Cu²⁺;

6.2: identify anions - CO₃²⁻, SO₄²⁻, SO₃²⁻, NO₃⁻, Br⁻, I⁻, Cl⁻;

6.3: identify gases - H₂, O₂, CO₂, NH₃, SO₂, Cl₂, NO₂, H₂O.