SPECIFIC OBJECTIVE

CONTENT

Learners should be able to:

·        Define the term affinity.

·        Describe the reaction between a given metal and metal oxide.

·        Explain the reaction between a given metal and metal oxide.

·        State the order of elements in the reactivity series.

·        Definition of affinity for oxygen.

·        Displacement reactions.

·        Competition reactions of the metals for oxygen 

·        Experiments to demonstrate the reactions of metals with metal oxides e.g. CO₂/Mg, PbO/Mg

·        The reactivity series ( K, Na, Ca, Mg, Al, C, Zn)

SPECIFIC OBJECTIVE

CONTENT

Learners should be able to:

·        State the composition of water.

·        Test for the products of burning organic matter.

·        Explain the experiment showing that water contains hydrogen.

·        State the products of reaction of water and steam with different metals.

·        List the reactivity series obtained from metal/water reaction.

·        Composition of water.

·        The water cycle.

·        Burning of organic matter (energy source).

·        Water as an oxide of hydrogen.(Burning hydrogen and a candle in air)

·        Reactions of metals with water/steam.( Na, Ca, Mg with water and Mg, Zn, Fe with steam)

SPECIFIC OBJECTIVE

CONTENT

Learners should be able to:

·        Prepare and test for hydrogen in the laboratory.

·        State the physical and chemical properties of hydrogen.

·        Outline the uses of hydrogen.

·        Explain oxidation as gain of oxygen and reduction as loss of oxygen with reference to metal oxide-hydrogen reactions.

·        Laboratory preparation of hydrogen.

·        Test for hydrogen

·        Reactions of hydrogen gas.

·        Uses of hydrogen gas: -

-         manufacture of margarine

-         weather balloons.

-         manufacture of ammonia.

·        Oxidation and reduction in terms of gaining oxygen and losing hydrogen.(use copper (II) oxide, hydrogen reduction)

SPECIFIC OBJECTIVE

CONTENT

Learners should be able to:

·        Define an atom.

·        Name the particles of the atom.

·        Draw the simple atomic structure.

·        State the charges on each of the particles of the atom.

·        Define atomic number, relative atomic mass and isotope.

·        Write electronic configuration of various elements (1^st 20 elements in the Periodic Table).

·        Definition of atom

·        Particles of an atom

·         Draw the structure of an atom.

·        Definition of atomic number and mass number.

·        Definition of isotopes, relative atomic mass, and examples and their significance.

·        Electronic configuration of the 1^st 20 elements in periodic table.

·        Positive and negative charges (should be introduced through simple electrostatics, experiments with charges, rods and spheres.)

SPECIFIC OBJECTIVE

CONTENT

Learners should be able to:

·        Define the Periodic Table.

·        Describe the history of the periodic time.

·        Arrange the first 20 elements in the Periodic Table.

·        Identify metals, non-metals and noble gases in relation to outermost electrons.

·        Describe the Period and group.

·        Definition of the Periodic Table and its history.

·        Groups in the Periodic Table (i.e. I, II, VII, O) and periods.

·        Arrangement of the 1^st 20 elements in the Periodic Table.

SPECIFIC OBJECTIVE

CONTENT

Learners should be able to:

·        Define an ion.

·        Describe an octet and duplet.

·        Outline common ions.

·        Determine valencies of different elements.

·        Write simple chemical formulae.

·        Define multivalency.

·        Define a radical.

·        Identify elements that are multivalent.

·        Describe how simple ionic compounds are formed (e.g. sodium chloride).

·        Definition of an ion.

·        The characteristics feature of the outermost energy level (i.e. octet and duplet).

·        Formation of ions and determination of valencies.

·        The reaction between sodium and chlorine.

·        The reaction between magnesium and oxygen.

·        Common ions (e.g. Li⁺, Na⁺, Mg^2+, Ca^2+, Al^3+, etc. F^-, Cl^-, NO₃^-, CO₃^2-, etc.

·        Formulae of ionic compounds.

SPECIFIC OBJECTIVE

CONTENT

Learners should be able to:

·        State the specified reactions of the alkali, alkaline-earth metals and halogens.

·        Describe the difference in reactivity within these chemical families

·        State the properties of noble gas family and its un-reactivity.

·        Predict the reactions and reactivity of elements within each family on qualitative basis.

·        Reaction of alkali metals (Li, Na, K) with air, water and chlorine.

·        Reaction of alkaline- earth metals (Ca, Mg,) with air, water, chlorine and dilute acids.

·         Reaction of halogens (Cl₂, Br₂, I₂) with sodium, water (bleaching action), zinc powder, sodium hydroxide solution.

·        Noble gases.

-         recognize their low reactivity based on their electronic configuration

·        Note: Word equation should be used though formulae of simple compounds and elements may be given.

SPECIFIC OBJECTIVE

CONTENT

Learners should be able to:

·        Define bonding.

·        Describe the formation of:

-         electrovalent bond.

-         covalent bond.

-         metallic bond

·        Identify different elements which form the above bonds.

·        Definition of bonding.

·        Description of electrovalent, covalent, dative and metallic bonding.

·        Differences between electrovalent, covalent, metallic and dative bonding.

SPECIFIC OBJECTIVE

CONTENT

Learners should be able to:

·        Define word equation.

·        Write word equations.

·        Define formulae equation.

·        Write formulae equations.

·        Balance formulae equations.

·        Definition of word equation and formulae equation.

·        Word equations.

·        Formulae (chemical) equations.

·        Balancing formulae (chemical equation.

SPECIFIC OBJECTIVE

CONTENT

learners should be able to:

·        Define an acid, base and indicator.

·        Prepare and use plant extracts as acid – base indicators.

·        Use universal indicator to determine the ph of solution.

·        State characteristics of acids and bases.

·        Give examples of acids and bases.

·        Outline some applications of acid – base neutralization.

·        Definition of acid, base and indicator.

·        Indicators
- preparing and using indicators. (flower, extracts as simple indicators.)
- universal indicator (ph scale.)

·        Acidic, neutral and basic/alkaline solution.

·        Strength of acids and bases.

·        Simple properties of mineral acids. test solutions: nh₄cl,

      (nh₄)₂ so₄, nh₃, naoh, h₂so₄,     etc.)

·        Neutralization reactions of acids and bases.

·        application of acid – base neutralization reactions

SPECIFIC OBJECTIVE

CONTENT

Learners should be able to:

·        Define salt.

·        Identify soluble and insoluble salts.

·        Select an appropriate method for preparation of a particular salt.

·        Explain the terms solution, saturated solution, crystallization, neutralization and precipitation.

·        Describe and explain from experimental observations, the action of heat on various salts.

·        Definition of salt.

·        Normal salts and acid salts.

·        Soluble and insoluble salts.

·        Solution.

·        Crystals.

·        Crystallization by evaporation.

·        Preparation of soluble salts.

·        Preparation of insoluble salts-double decomposition.

·        Preparation of salts by direct synthesis.

·        Hydrated salts.

·        The effect of heat on salts.

SPECIFIC OBJECTIVE

CONTENT

Learners should be able to:

·        Define conductor/non-conductor and electrolyte/ non-electrolyte.

·        State the relationship between electrolytes, non-electrolytes and the particles they contain (ions, molecules).

·        Name the products of electrolysis of simple binary electrolytes.

·        Explain that, electrolysis is a means of obtaining elements from chemical compounds.

·        Definition of conductor, non-conductor, electrolyte and non – electrolyte.

·        Definition of cathode and anode.

·        Which substances conduct

·        Tests for conduction by solids (metals, non-metals, plastic, wood).

·        Solution: sugar, urea, sodium chloride and copper (II) chloride, dilute mineral acids and molten substances.

·        Electrolysis of ionic compounds (CuCl₂, HCl, PbBr₂.)