Republic of Zambia
CHEMISTRY
HIGH SCHOOL SYLLABUS
GRADES 10 – 12
Prepared by:
Curriculum Development Centre
P.O. Box 50092
LUSAKA
© Curriculum Development Centre
All rights are reserved. No part of this publication may be reproduced, stored in a retrieval system or transmitted in any form or by any means,
mechanical, photocopying, recording or otherwise, without the prior consent of the copyright holder.
i
CONTENTS .........................................................................................................................................................................................
Preface ..................................................................................................................................................................................................
Acknowledgements ..............................................................................................................................................................................
Introduction ..........................................................................................................................................................................................
General Aims ........................................................................................................................................................................................
Mathematical Requirements .................................................................................................................................................................
Assessment Objectives .........................................................................................................................................................................
Structure of the Examination ................................................................................................................................................................
Time Allocation ....................................................................................................................................................................................
UNIT
TOPIC
PAGE
1.0
Introduction to Chemistry
1
2.0
The Particulate nature of matter
2
2.1 Matter
2
2.2 Kinetic theory
2
3.0
Experimental techniques
3.1 Apparatus
3.2 Criteria of purity
3.3 Methods of purification
3
3
3
3
4.0
The Language of Chemistry
4.1 Atomic structure
4.2 Elements compound and mixtures
4.3 Chemical bonding
4.4 Chemical symbols, formulae and equations
4
4
4
5
5
5.0
The Periodic table
5.1 Groups and periods
5.2 Group properties
5.3 Transitional metals
6
6
6
6
ii
11
v
vi
vii
viii
ix
x
xi
xii
UNIT
TOPIC
PAGE
6.0
Acids bases and salts
6.1 Acids, bases and alkalis
6.2 Salts
6.3 Effects of acids in the environment
6.4 Uses of acids, alkalis and salts
7
7
8
8
8
7.0
The Mole concept
7.1 Relative masses
7.2 The mole
7.3 Empirical and molecular formulae
9
9
9
10
8.0
Chemical reactions and energy changes
8.1 Rate of chemical reactions and chemical equilibrium
8.2 Redox reactions
8.3 Energetics of reactions
11
11
12
12
9.0
Metals
9.1 Reactivity series
9.2 Alloys
9.3 Thermal stability of the compounds
13
13
14
14
10.0
Electricity and chemistry
10.1 Ectrolysis
15
15
10
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UNIT
TOPIC
PAGE
11.0
Organic chemistry
11.1 Saturated and unsaturated hydro carbons
11.2 Alcohols and acids
11.3 (Carboxylic acids) Macromotecules
11.4 Synthetic macromolecules
11.5 Natural macromolecules
16
16
16
17
17
18
12.0
Non Metals
12.1 Hydrogen
12.2 Oxygen
12.3 Nitrogen
12.4 Chlorine
12.5 Sulphur
12.6 Carbon and carbonates
12.7 Silicon
19
19
19
20
21
22
23
24
13.0
Chemistry, Society and the Environment
13.1 Chemistry and society
13.2 Pollution
25
25
25
19
iv
PREFACE
The review of this Syllabus was necessitated by the need to improve the quality of education at High School Level as stipulated in the national
policy document “Educating Our Future - 1996”.
Quality education raises the standard of living for all. This leads to sustainable national development. The syllabus also addresses issues of
national concern such as Environmental Education, Gender and Equity, Health Education and HIV/AIDS, Family Life Education, Human
Rights, Democracy, Reproductive Health, Population Education, Entrepreneurship and Vocation Skills, Life and Values Education.
Another reason for revising this syllabus was to fully localize the High School Examinations which were formerly set by University of
Cambridge Local Examinations Syndicate, UK.
It is hoped that this syllabus will provide the users with a sound premise on the basis of which meaningful and effective learning experiences will
be developed in order to provide a good foundation for further study of this subject area.
James Mulungushi (Dr.)
PERMANENT SECRETARY
MINISTRY OF EDUCATION
LUSAKA-ZAMBIA
v
ACKNOWLEDGEMENTS
The production of this syllabus has been undertaken under the aegis of the Curriculum Development Centre and with expert advice and
contributions from the following:
The Examinations Council of Zambia, the Ministry of Environment and Natural Resources through Environmental Education Programme for
Awareness, the University of Zambia, Zambia Science Education Association, Chemistry Curriculum Committee, Inspectors of Schools,
Examiners individual chemistry teachers too many to mention.
vi
INTRODUCTION
This syllabus is designed for Grades 10 – 12. It is intended for learners taking Chemistry at High School Level of education. It places less
emphasis on factual material and greater emphasis on understanding and application of scientific concepts and principles. This has been done so
that learners develop skills that will be of the value for a long time in an increasingly world and it is expected that these will be of relevance for a
very long time.
GENERAL AIMS
These provide the educational purposes of following a Chemistry Course at this level of education and are listed in a suggested order of priority:
The General aims are to:
1.
provide, through well designed studies of experimental and practical Chemistry, a worthwhile educational experience for all learners,
whether or not they go on to study Chemistry beyond this level and, in particular, to enable them to acquire sufficient understanding and
knowledge to:
1.1 become confident citizens in a technological world, able to take or develop an informed interest in matters of scientific import;
1.2 recognise the usefulness, and limitations, of scientific method and to appreciate its applicability in other disciplines and in everyday
life;
1.3 be suitably prepared for studies beyond High School level in Chemistry, in applied Sciences or in Science dependent vocational
courses.
2.
stimulate learners and create and sustain their interest in and enjoyment of Chemistry.
3.
develop abilities and skills that:
3.1 are relevant to the study and practice of chemistry;
3.2 are useful in everyday life;
3.3 encourage efficient and safe practice;
3.4 encourage effective communication.
4.
develop attitudes relevant to Chemistry such as:
4.1 concern for accuracy and precision;
4.2 objectivity;
4.3 integrity.
vii
5. assist the development of:
5.1
the skills of:
(i) enquiry;
(ii) initiative;
(iii) inventiveness.
6. stimulate interest in and care for the local and global environment.
7. promote an awareness that:
7.1 scientific theories and methods have developed, and continue to do so as a result of co-operative activities of groups and individuals;
7.2 the study and practice of Chemistry is subject to social economic, technological, ethnical and cultural influences and limitations;
7.3 the applications of Chemistry may be both beneficial and detrimental to the individual, the community and the environment;
7.4 Chemistry transcends national boundaries and that language of science correctly and rigorously applied, is universal.
viii
MATHEMATICAL REQUIREMENTS
This syllabus offers a context in which mathematical skills and techniques may be applied in a relevant and more meaningful way. The study of
Chemistry through this syllabus, therefore strengthens the applications of Mathematics.
Candidates will be required to be competent in the following mathematical techniques:
1.
2.
3.
4.
5.
6.
7.
8.
9.
10.
11.
12.
13.
add, subtract, multiply and divide.
use averages, fractions, percentages, ratios and reciprocals.
recognise and use standard notation.
use direct and inverse proportion.
use positive, negative and whole number indices.
draw charts and graphs from given data.
interpret charts and graphs.
select suitable scales and axes for graphs.
make approximate evaluations of numerical expressions.
recognise and use the relationship between length, surface area and volume and their units on metric scales.
solve equations of the form x = yz for only one variable when the other two are known.
make accurate numerical work and handle calculations up to three (3) significant figures.
comprehend and use symbols notation such as ≥ and ≤.
ix
ASSESSMENT OBJECTIVES
The following aspects of the aims will be assessed:
1.
Knowledge with understanding
The candidates should be able to demonstrate knowledge and understanding in relation to:(a) scientific phenomena, facts, concepts, theories and laws.
(b) scientific terminology, use of symbols, quantities and units.
(c) scientific apparatus and instruments and their safe operations.
(d) scientific quantities and their determination.
(e) scientific and technological applications with social, economic and environmental relevance.
Questions testing these objectives will in most cases begin with the terms such as:
“describe, discuss, state, explain, name, outline or define”.
2.
Handling information and solving problems.
The candidate should be able to:(a) locate, select, organise and present information from a variety of sources.
(b) translate information from one form to another.
(c) manipulate numerical data.
(d) identify patterns and draw inferences from information.
(e) give reasonable explanations for patterns and relationships.
(f) make predictions and hypotheses.
(g) solve problems
questions testing these objectives will often begin with the term such as “predict, calculate, suggest or determine”.
3.
Experimental Skills and Investigating.
The candidate should be able to:(i) follow instructions.
x
(ii)
(iii)
(iv)
(v)
(vi)
(vii)
use basic laboratory techniques, apparatus and materials.
observe, measure and record.
plan investigations.
interpret and evaluate observations and results.
predicts trends.
evaluate methods and suggest possible improvements.
Questions testing these objectives will often begin with the terms such as “determine, calculate, plot, draw, conclude, interpret, suggest “.
STRUCTURE OF THE EXAMINATIONS.
The following will be the structure of the Examination. There will be three (3) papers as follows:
Paper 1 will comprise multiple choice questions (40 marks).
Paper 2 will comprise two parts:Part I will consist of compulsory structure questions (75 marks) and
Part II will comprise a number of question (30 marks) from which candidates will be required to choose from.
Paper 3. This is a practical paper. It will comprise two compulsory questions.
N.B.: Special consideration will be made for “Special Education Needs (SEN)”.
TIME ALLOCATION
A minimum of five teaching periods of forty (40) minutes each per week. Preferably two (2) double periods to be taken in lobaratory.
xi
UNIT 1.0
CONTENT
INTRODUCTION TO CHEMISTRY
OBJECTIVES (PSBAT)
1.1 INTRODUCTION
NOTES
1.1.1 Define Chemistry.
Refer to branches of chemistry:
- physical,
- inorganic,
- organic,
- analytical chemistry.
1.1.2
Discuss the importance of chemistry.
Include domestic, agricultural, industrial,
social, economic, technological, environmental,
medical importance.
1.1.3
Demonstrate an appreciation of chemistry.
Refer to local and international industries such
as plastic, cement, sugar and coca-cola.
1
CONTENT
OBJECTIVES (PSBAT)
NOTES
2.1 MATTER
2.1.1 Define matter.
Matter defined as anything that has mass and
occupies space.
Refer to ions, molecules and atoms.
Refer to solids, liquids and gases.
2.1.2 State the basic units of matter.
2.1.3 Discuss the three states of matter.
2.2 KINETIC THEORY
2.2.1 Describe diffusion.
2.2.2 State the factors that influence rates of
diffusion.
2.2.3 Describe the evidence of movement of
particles in liquids and gases.
2
Refer to diffusion of toxic gases and effluents.
Refer to gas law such as Brownian motion.
Refer to dilution.
UNIT 3.0
CONTENT
EXPERIMENTAL TECHNIQUES
OBJECTIVES (PSBAT)
3.1 APPARATUS
NOTES
3.1.1 Describe various apparatus used in
chemistry.
3.2 CRITERIA OF PURITY 3.2.1 Describe how to determine the purity of a
substance.
3.3 METHODS OF
PURIFICATION
3.2.2 Predict the effects of impurities on
substances.
3.2.3 Explain the importance of purity of
substances.
3.3.1 Describe the methods of purification.
3.3.2 Discuss the industrial application of the
methods of purification.
Such as burettes pipettes, volumetric flask,
conical flask, funnel, beaker, measuring
cylinder, balance, spatula, stands and clamp,
test-tubes, burners, thermometers, glass rods,
evaporating dish, stopwatch/clock.
Refer to density, melting point, boiling point
and chromatography.
Determination of purity should be done
practically.
Refer to graphical presentation of heating solid,
liquids (heating curve).
Refer to the importance of purity of food,
drinks and medicines.
Refer to filtration, crystallisation, simple and
fractional distillation and chromatography.
Refer to applications in local and international
industries such as cement, sugar, petroleum.
3.3.3 Explain the process of paper chromatography. Not limited to paper chromatography only.
3.3.4 Interpret a simple chromatogram.
3.3.5 Separate mixture using physical methods.
Refer to filtration, distillation, chromatography
with examples.
3
UNIT 4.0
THE LANGUAGE OF CHEMISTRY
CONTENT
OBJECTIVES (PSBAT)
4.1.1 Define an element, a compound and a
4.1 ELEMENTS,
mixture.
COMPOUNDS AND
4.1.2 Compare and contrast elements, compounds
MIXTURES.
and mixtures.
4.2 ATOMIC STRUCTURE
4.2.1 Define an atom.
4.2.2 State the relative charges of protons,
neutrons and electrons.
4.2.3 State the relative mass of a proton, a neutron
and an electron.
4.2.4 Draw the model of the atom.
4.2.5 Describe with the aid of diagrams the
electronic configuration of an atom.
4.2.6
4.2.7
4.2.8
4.2.9
Define atomic number.
Find the mass number of an atom.
Use and interpret as 126C.
Describe isotopes.
4.2.10 State that some isotopes are radioactive.
4.2.11 State some uses of isotopes.
4.2.12 Define relative atomic mass.
4.2.13 Calculate relative atomic mass.
4
NOTES
Refer to physical and chemical changes.
Refer to neutrons, protons and electrons.
Show the position of neutrons, electrons and
protons.
Refer to elements of atomic number 1 to 10 of
the periodic table. Distribution in S,P,D not
required.
Refer to isotopes of chlorine, hydrogen and
carbon.
Refer to dangers of radioactive isotopes.
Refer to uses in medicine. Agriculture and
Industries.
Ar as weighted average of atomic masses.
Use of relative abundance of isotopes to be
emphasised.
Refer to use of mass spectrometer.
Details of how it works not needed.
CONTENT
4.3 CHEMICAL BONDING
OBJECTIVES (PSBAT)
4.3.1 Describe the formation of ions by loss or
gain of electrons.
NOTES
Refer to cations and anions.
Give examples of H2O and HCL.
4.3.2 Define an ion.
4.3.3 Describe the formation of ionic bonds
between metallic and non-metallic elements.
4.3.4 Define a molecule.
4.3.5 Describe the formation of covalent bands by
sharing pair(s) of electrons.
Refer to cations and anions.
Mention the formation of crystal lattice e.g.
sodium chloride.
4.3.6 Use chemical symbols of elements to write
formulae of compounds (given the valency
of elements).
4.3.7 Deduce from given information the valency
of an element.
4.3.8 Compare and contrast properties of ionic and
covalent compounds.
4.4 CHEMICAL
SYMBOLS,
FORMULAE AND
EQUATIONS
4.3.9 Describe metallic bonding.
4.4.1 State chemical symbols of common
elements.
4.4.2 Explain the concept of valency.
4.4.3 Construct chemical formulae.
4.4.4 Construct balanced chemical equations.
4.4.5 Write ionic equations.
5
Work out the valency from the formula or
electronic configuration. Refer to shapes of H2O,
CO2, CH4, NH3 and HCl.
Refer to solubility, conductivity, refractory
nature and volatility. Refer to dangers of toxic
volatile inflammable, combustable substances.
Refer to free electrons, and malleability.
Refer to the symbols of the first 20 elements and
the first 10 transitional metal elements.
Refer to valency of radicals. Use of s,p,d,
configuration not required.
Include appropriate state symbols (aqs, l, and g).
UNIT 5.0
THE PERIODIC TABLE
CONTENT
OBJECTIVES (PSBAT)
5.1.1 Discuss the historical background of the
5.1 GROUPS AND THE
periodic table.
PERIODS
5.1.2 Explain how elements are arranged in the
periodic table.
5.2 GROUP PROPERTIES
5.1.3 Describe the chemical reactivity of elements
in groups, I, VII and VIII.
5.1.4 Describe the change from metallic to a nonmetallic character across a period.
5.2.1 Describe the chemical properties of the metal
oxides, nitrates, carbonates and hydrogen
carbonates.
5.2.2 Describe the physical properties of elements
in Group VII and VIII.
5.2.3 Predict the reactions of halogens with other
halide ions and metal compounds.
5.2.4 Discuss the importance/use of halogens.
5.2.5 Describe harmful effects of halides.
5.3 TRANSITIONAL
METALS
5.3.1 Describe transition metals.
5.3.2 Describe general properties of transition
metals.
6
NOTES
Mention of Dmitri Mendele v attempting to
arrange the elements in terms of atomic
weights.
Refer to relationship between group number,
oxidation state metallic or non-metallic
characteristics and number of valency
electrons.
Refer to the first 20 elements.
Include solubility, effect of heat, melting point
and boiling.
Mention chlorine, bromine and iodine only in
terms of colour.
Refer to their displacement reactions with other
halide ions.
Refer to the uses of nobles gases e.g. argon
electrical lamps, helium in balloons, neon in
advertising.
Refer to production of drugs, pesticides, and
their effect.
Refer to ozone layer depletion.
Refer to their position on the periodic table.
Refer to high melting points, high densities,
variable valency forming coloured compounds,
the elements and their compounds often act as
catalysts.
UNIT 6.0
ACIDS, BASES AND SALTS
CONTENT
OBJECTIVES (PSBAT)
NOTES
6.1 ACIDS, BASES AND
ALKALIS
6.1.1 Describe acid, bases and alkalis in terms of
the ions they contain or produce in aqueous
solution.
6.1.2 Demonstrate the effects of acids in solution
on indicators, metals, carbonates and
hydrogen carbonates.
6.1.3 Describe the properties of bases and alkalis.
Refer also to hydrogen chloride dissolved in
methyl benzene.
6.1.4 Describe acidity and alkalinity in terms of
pH.
6.1.5 Classify oxides as acidic, basic, amphoteric
or neutral.
6.1.6 Compare the relative solubility of oxides and
hydroxides.
6.1.7 Prepare insoluble hydroxides by
precipitation.
7
Emphasise the need of moisture in acid
formation.
Refer to their reaction with indicators and
ammonium salts.
Refer to industrial use in agriculture (soil)
Refer to oxides of iron, zinc and aluminium.
CONTENT
6.2 SALTS
OBJECTIVES (PSBAT)
6.2.1 Classify salts into acidic, basic and normal
salts.
6.2.2 Prepare pure salts by various methods.
6.2.3 Prepare a salt by titration.
6.2.4 Describe a method of obtaining crystals.
6.2.5 Determine water of crystallisation.
6.3 EFFECTS OF
ACIDS IN THE
ENVIRONMENT
6.4 USES OF ACIDS,
ALKALIS AND SALTS
6.3.1 Describe the formation of acid rain.
6.3.2 Describe the harmful effects of acids and
acid rain in the environment.
6.4.1 Describe the important uses of acids, alkalis
and salts.
8
NOTES
Refer to ionisation of salts and their solubility.
Include preparation by action of an acid on:
(i) a metal
(ii) insoluble metal oxide
(iii) insoluble hydroxide.
Include insoluble and soluble carbonates by
precipitation.
Refer to the preparation of insoluble salts by
precipitation.
Refer to the commercial preparation of
ammonium sulphate and any other salts.
Refer to neutralisation reactions.
Refer to size, shape and purity.
Refer to water of crystallisation with respect to:
(i) hygroscopic
(ii) deliquescent
(iii) efflorescent
Refer to effects on land, plants, animals and
water.
Refer to corrosion and release of toxic gases.
Mention examples of uses in:
(i) lead – acid accumulator
(ii) household
(iii) agriculture
(iv) industry.
UNIT 7.0
CONTENT
STOICHIOMETRY AND THE MORE CONCEPT
OBJECTIVES (PSBAT)
7.1 RELATIVE MASSES
NOTES
7.1.1 Define relative molecular mass.
Mr as sum of Ar of atoms in the molecule
(formula mass).
7.1.2 Calculate the relative atomic mass given the
percentage abundance of the isotopes.
7.1.3 Calculate the relative molecular mass of a
compound.
7.2 THE MOLE
7.2.1 Define the mole.
7.2.2 Discuss the mole in term of Avogadro’s.
7.2.3 State Avogadro’s constant.
7.2.4 Calculate the molar mass and molar volume
of a gas using the mole concept.
7.2.5 Relate Avogadro’s law to reacting moles and
volumes of gases.
7.2.6 Explain the concentration of a solution.
7.2.7 Calculate stoichiometric reacting moles and
volumes of gases and solutions.
9
Mole of atoms, ions, molecules and electrons to
be specified.
Refer to constant number 6.02 x 1023 of
particles in one mole (atoms, molecules, ions
and electrons).
Take volume of a gas as 22.4 dm3 at STP and
24.0 dm3 at room temperature.
Express the concentration of solution in gdm-3
and more mol. dm-3.
Refer to chemical reactions and equations
including limiting reactants.
CONTENT
OBJECTIVES (PSBAT)
NOTES
7.3 EMPIRICAL AND
MOLECULAR
FORMULAE
7.3.1 Calculate the percentage composition of a
compound.
7.3.2 Calculate the empirical and molecular
formulae.
7.3.3 Define percentage yield and purity.
7.3.4 Calculate the percentage yield in a reaction.
7.3.5 Calculate percentage purity of a substance.
10
Compute the formula of a compound given
appropriate data.
UNIT 8.0
CONTENT
CHEMICAL REACTIONS AND ENERGY CHANGES
OBJECTIVES (PSBAT)
8.1 RATE OF CHEMICAL
REACTIONS AND
CHEMICAL
EQUILIBRIUM
NOTES
8.1.1 Describe a chemical reaction.
Include reactants and products.
8.1.2 Determine the effects of the following on the
speed of chemical reactions:
(i)
temperature
(ii) pressure
(iii) concentration
(iv) surface area (particle size)
(v) catalyst.
Refer to graphical representations and their
interpretations.
8.1.3 Interpret data on the speed of chemical
reactions.
8.1.4 Describe methods of controlling the speed of
chemical reactions.
8.1.5 Describe chemical equilibrium.
11
Refer to dangers of naked flames in flour mills
and coal mines
Refer to Lechatelier’s principle.
Refer to reversible reactions.
CONTENT
8.2 REDOX REACTIONS
OBJECTIVES (PSBAT)
8.2.1 Define oxidation and reduction.
8.2.2 Describe redox reactions.
8.2.3 Identify oxidizing and reducing agents in a
reaction.
8.2.4 Deduce the oxidation number of an element in a
compound.
8.3 ENERGETICS OF
REACTIONS
8.2.5 Deduce a redox reaction using oxidation
numbers.
8.2.6 Carry out tests to identify an oxidizing and
reducing agent.
8.3.1 Describe terms related to energy changes in
chemical reactions.
8.3.2 Describe the production and absorption of heat,
light and electrical energy in chemical reactions.
8.3.3 Explain the advantages and limitations of energy
sources.
8.3.4 Discuss the effects of products of energy changes
on the environment.
8.3.5 Explain the use of silver halide in photography.
12
NOTES
Refer to loss/gain of electrons (oxygen or
hydrogen) and also to increase and
decrease of oxidation number.
To be limited to inorganic compounds and
ions.
Recall of equations involving Potassium
manganate (VII) KMnO4 Potassium
dichromate (VI), K2 Cr2 07 not expected.
Refer to the definition of Redox reaction
using oxidation numbers.
Refer to colour changes.
Mention exothermic and endothermic,
enthalpy (∆H), bond breaking, bond
formation, burning of fuels, nuclear
energy, H2 as fuel. Refer to bond energies.
Refer to safety, cost of available reserves,
renewable and non-renewable sources,
energy yield of fossil and nuclear fuels.
Include pollution.
To be limited to the idea of reduction of
silver ions to silver.
UNIT 9.0
METALS
CONTENT
OBJECTIVES (PSBAT)
9.1.1 Describe the properties of metals.
9.1 REACTIVITY AND
ELECTRO CHEMICAL 9.1.2 Describe the reactions of metals with:
(i) air,
SERIES
(ii) water and steam,
(iii) dilute non-oxidizing acids, and
(iv) aqueous solutions of other metal ions.
9.1.3 Determine the reactivity series of calcium,
copper, iron, lead, zinc, magnesium,
potassium and sodium.
9.1.4 Describe the reduction of the oxides of metals
with:
(i) carbon,
(ii) carbon monoxide,
(iii) hydrogen.
9.1.5 Relate electro chemical series to the tendency
of a metal to form its positive ion.
9.1.6 Describe extraction of copper, iron and zinc
from their ores.
9.1.7 Discuss the uses of metals.
13
NOTES
Refer to physical and chemical properties.
Practical determinations of reactions with Al, Cu,
Fe, Mg, Pb and Zn.
Refer to unreactivity of aluminium due to the
oxide layers.
Refer to free electrons.
Refer to iron from haematite and Zinc blende in
terms of choice of reduction method.
Refer to copper zinc and iron processing in
Zambia.
Refer to important uses of zinc, iron and copper.
Refer to the toxic gases and effluents from
factories.
Refer to disposal of scrap metal as contributing to
land pollution.
Refer to land degradation due to mining and
dumpings.
Refer to metals as non renewable resources.
CONTENT
9.2 ALLOYS
OBJECTIVES (PSBAT)
9.2.1 Describe an alloy.
NOTES
Mention steel, brass, bronze, invar.
9.2.2 Explain the advantages of using alloys over pure
metals in some industrial processes.
Refer to semi conductors and other
properties of alloys.
9.2.3 Describe common uses of alloys.
9.3 THERMAL
STABILITY OF THE
COMPOUNDS
9.3.1 Explain the effects of heat on hydroxides,
carbonates, nitrates of metals and ammonium
compounds.
Relate to difficulty in decomposition of
compounds of al, Ca, Cu, Fe,Pb, Zn, Mg,
K, Na and NH4+.
9.3.2 Describe the action of sodium hydroxide on
aqueous solutions containing metal ions and
ammonium radical.
Refer to identification tests of Al3+, Ca2+,
Cu2+, Fe2+, Pb2+, Zn2+, NH4+.
9.3.3 Describe the action of aqueous ammonia on
solutions containing metal ions.
14
UNIT 10.0
ELECTRICITY AND CHEMISTRY
CONTENT
OBJECTIVES (PSBAT)
10.1.1 Describe electrolysis.
10.1 ELECTROLYSIS
10.1.2
Describe the products at the electrodes during
the electrolysis of:
(i) molten lead (II) bromide
(ii) acidified water
(iii) concentrated aqueous sodium chloride
(brine)
(iv) aqueous copper (II) sulphate using
carbon and copper electrodes.
10.1.3
Discuss the industrial applications of
electrolysis.
10.1.4
Describe the extraction of aluminium from its
oxide.
Calculate the quantity of electrolytic products.
10.1.5
15
NOTES
Refer to conductivity of metals and
electrolytes.
Mention electrodes, electrolyte and ions.
Refer to ions as cations and anions.
With electrolysis of (II) sulphate use inert
and copper electrodes (inert e.g. platinum).
Refer to purifications of copper at a
refinery, uses of aluminium and
electroplating with silver and gold, and
manufacture of NaOH, Cl2 and H2.
Refer to Faraday’s laws.
UNIT 11.0
ORGANIC CHEMISTRY
CONTENT
OBJECTIVES (PSBAT)
11.1.1 Describe an organic compound.
11.1 SATURATED AND
11.1.2 Name and draw the structures of the alkanes up
UNSATURATED
to five carbon atoms.
HYDROCARBONS
11.1.3 Name and draw structures of isomers of butane
and pentane.
11.1.4 Explain the factional distillation of petroleum
(Crude oil).
11.1.5 Describe uses of the products of fractional
distillation of crude oil.
11.1.6 Describe the properties of alkanes.
11.1.7 Explain that alkanes are unsaturated
hydrocarbons.
11.1.8 Name and draw the structures of alkanes up to 5
carbon atoms.
11.1.9 Describe the properties of alkanes.
11.2 ALCOHOLS AND
ACIDS (CARBOXYLIC
ACIDS)
11.1.10 Distinguish between saturated and unsaturated
hydrocarbons.
11.2.1 Define an alcohol.
11.2.2 Name and draw structures of primary alcohols
up to four carbon atoms.
16
NOTES
Introduce the term homologous series and
mention that alkanes are saturated
hydrocarbons.
Refer to important uses of the various
fractions (as fuels).
Refer to oil spills as an environmental
hazard.
Refer to methane as an alkanes example.
Refer to burning and substitution reactions.
Refer to CFC and their action on ozone
layer depletion.
Refer to double (C=C) bond and the
homologous series.
Refer to ethane as an alkane example.
Refer to burning, addition of hydrogen,
bromine, chlorine, steam and formation of
polyethene and PVC)
Refer to tests for alkanes using aqueous
bromine and acidified K Mn O4.
Refer to functional group – OH.
CONTENT
OBJECTIVES (PSBAT)
11.2.3 Describe the formation of alcohols.
NOTES
Refer to the formation of alcohol from
alkanes and by fermentation.
Refer to methanol and ethanol.
11.2.4 Describe the properties of alcohols.
Refer to Physical and Chemical properties
of alcohols, such as boiling and melting
point and reactions.
11.2.5 Describe the formation of carboxylic acids from
the oxidation of alcohols.
Refer to oxidation of ethanol to ethansic
acid.
11.2.6 Describe properties of carboxylic acids.
Refer to boiling points, melting points and
reactions as acids including esterification
reactions with alcohols.
Emphasise macromolecules as having
different units/linkages. (As large
molecules built from small units).
Other common addition polymers e.g.
P.V.C.
Refer to polymerisation.
11.3 MACROMOLECULES 11.3.1 Describe macromolecules.
11.4.1 Describe the formation of polythene by
11.4 SYNTHETIC
addition.
MACROMOLECULES
11.4.2 Describe the formation of nylon and terylene by
condensation polymerisation.
17
The structure of nylon (a polyamide) is
represented as:
CONTENT
11.5 NATURAL
MACROMOLECULE
OBJECTIVES (PSBAT)
11.4.3 Differentiate between the structure of polymide
and polyester.
NOTES
11.4.4 State typical uses of plastics and synthetic
fibres.
11.5.1 Describe proteins, fats and carbohydrates:
as examples of natural polymers.
Units linked by oxygen i.e.
-o- -o- -o- O
Refer to structures showing linkages in
carbohydrates in terms of large number of
sugar molecules.
11.5.2 Identify linkages of:
(i) proteins,
(ii) fats,
(iii) carbohydrates.
Refer to acid hydrolysis of:
(i)
proteins to amino acids
(ii) fats and oils to fatty acids and
glycerol
(iii) carbohydrates to simple sugars
(Monossacharides).
11.5.3 Outline the usefulness of chromatography in
separating and identifying the products of
carbohydrates and proteins.
Refer to paper chromatography.
18
UNIT 12.0
NON METALS
CONTENT
OBJECTIVES (PSBAT)
12.1.1 Describe the properties of non-metals.
12.1 HYDROGEN
12.2 OXYGEN
NOTES
Refer physical and chemical properties of
hydrogen.
12.1.2 Describe the production of hydrogen as a
product of the action of reactive metals on water,
steam and dilute acids.
12.1.3 Prepare, collect and test a sample of hydrogen.
Refer to the method of collection in terms
of properties of the gas.
12.1.4 Describe industrial manufacture of hydrogen.
Refer to steam reforming on natural gas or
coal.
12.1.5 Describe the reducing properties of hydrogen.
Refer to the reaction of hydrogen with
oxygen chlorine and copper (II) oxide.
Include hydrogenation of oils.
12.1.6 Describe the uses of hydrogen.
Refer to uses of hydrogen in the
manufacture of ammonia, as a fuel for
rockets, hydrogen action of oils, and the
explosive nature of hydrogen.
12.1.7 Discuss water as an important oxide of
Refer to some of the use, of water in
hydrogen.
homes and industry.
12.1.8 Describe a chemical test for water.
Include purification of water supply, by
chlorination and pollution.
12.2.1 Prepare and collect oxygen in the laboratory
Potassium chlorine may be used but there
from hydrogen peroxide and potassium
is danger of an explosion.
manganate (VII).
12.2.2 Test for oxygen.
Recall volume composition of oxygen in
air (20%).
12.2.3 Describe the properties of oxygen.
Refer to oxygen cycle and photosynthesis.
12.2.4 Describe the industrial preparation of oxygen.
Refer to fractional distillation of air in an
industry.
19
CONTENT
OBJECTIVES (PSBAT)
12.2.5 Discuss the uses of oxygen in industry and in
natural processes.
NOTES
Refer to the process in which oxygen is
involved burning respiration rusting and
methods of rust prevention.
12.2.6 Discuss the effects of pollutants arising from
reactions involving oxygen.
Refer to the common pollutants
(e.g. CO, CO2, SO2, PbO2, N2).
12.2.7 Discuss the importance of ozone.
Refer to dangers of ozone layer depletion,
skin cancers, respiratory diseases.
20
CONTENT
12.3 NITROGEN
OBJECTIVES (PSBAT)
12.3.1 Discuss the importance and characteristics of
Nitrogen as a gas.
12.3.2 Prepare and collect ammonia in the laboratory.
12.3.3 Carry out tests for ammonia.
12.3.4 Describe the manufacture of ammonia using the
Haber process.
12.3.5 Describe the reactions of ammonia as:
(i) a reducing agent
(ii) a base
(iii) a complexing reagent
(iv) an alkali.
12.3.6 Describe the properties of ammonia.
12.3.7 Identify nitrate ions by reduction with
aluminium.
12.3.8 Describe the thermal dissociation of ammonium
salts.
12.3.9 Describe the manufacture of nitric acid from
ammonia.
12.3.10 Describe the reactions of nitric acid as an
oxidizing agent.
21
NOTES
Emphasise the use of calcium oxide as a
drying agent.
Emphasise the essential reactions and
conditions for the manufacture of
ammonia.
Refer to the reaction of ammonia with:
(i) oxygen and copper (II) oxid,
(ii) dilute hydrochloric acid,
(iii) a solution containing.
Al2+, Ca2+, Cu2+, Fe2+, Pb2+, Zn2+.
Refer to the density, solubility, and
alkalinity of ammonia.
Mention physical and chemical properties.
Refer to ammonium chloride, ammonium
carbonate and ammonium nitrate.
Mention reactions with:
(i) a base and metal carbonates,
(ii) copper, carbon and iron.
CONTENT
OBJECTIVES (PSBAT)
12.3.11 Describe the uses of ammonia.
NOTES
Such as manufacture of fertilizers of nitric
acid, and of metal nitrates. Refer to
domestic uses, too.
12.3.12 Explain the importance of nitrogen in
fertilizers.
12.4 CHLORINE
12.3.13 Discuss the effects of nitrogenous fertilizers on Refer to the effluent washed into the river
the environment.
from industries and farms dealing with
such products.
12.4.1 Describe the laboratory preparation and
Oxidation of hydrochloric acid and with
collection of chlorine gas.
Manganese (IV) oxide or potassium
12.4.2 Describe the test for chlorine.
permanganate (VII). Use a fume cupboard
and ensure that there is good ventilation
when preparing Cl2.
12.4.3 Describe the properties of chlorine.
State physical and chemical; properties of
12.4.4 Describe the reactions of chlorine with:
chlorine.
(i) iron
(ii) non-metals
(iii) sulphur dioxide
(iv) iron (II) salts
(v) halide ions.
12.4.5 Describe the uses of chlorine.
Mention use in bleaching, water treatment,
pesticides and in industry. Refer to the
correct proportions of Cl2 added to water
supply.
12.4.6 Describe the industrial preparation of chlorine. Refer to use in the electrolysis of brine.
Mention colour changes of Ag, Br, Ag I.
22
CONTENT
12.5 SULPHUR
OBJECTIVES (PSBAT)
12.4.7 Identify chloride ions by acidified silver nitrate.
NOTES
12.4.8
Describe the laboratory preparation and
collection of hydrogen chloride.
12.4.9 Carry out tests for hydrogen chloride.
12.4.10 Describe the physical properties of hydrogen
chloride.
12.4.11 Describe a method of preparation of
hydrochloric acid.
12.4.12 Describe the reaction of hydrogen chloride
with:
(i) alkalis,
(ii) metals,
(iii) ammonia and
(iv) silver nitrate.
Refer to displacement from chlorides.
12.5.1
12.5.2
Mention sulphur dioxide as a pollutant.
As an acid, refer to action on litmus, water
and sodium hydroxide.
12.5.3
12.5.4
Describe the burning of sulphur.
Explain the behaviour of sulphur dioxide in
reactions as acidic oxide and as a reducing
agent.
Describe the industrial preparation of sulphuric
acid by the contact process.
Describe the reactions of sulphuric acid.
23
Refer to solubility, (fountain experiment)
density acidity.
As a reducing agent, refer to its reaction
with chlorine, water potassium
permanganate (VII) and potassium
dichromate (VI). Recall of equations not
required.
As a dehydrating agent, its oxidising
properties, and as non-volatile acid.
CONTENT
12.6 CARBON AND
CARBONATES
OBJECTIVES (PSBAT)
12.5.5 Discuss the uses of sulphuric acid.
12.5.6
12.6.1
NOTES
Refer to the manufacture of fertilizers and
explosives and other manufacturing
industries.
Test for sulphur ions.
Using acidified Barium nitrate or chloride.
Compare and contrast the physical properties of Mention the macromolecular structure of
the allotropes of carbon.
diamond and graphite.
12.6.2
Describe the formation and properties of carbon Refer to incomplete combustion of carbon,
monoxide.
toxicity and risks associated with its
formation.
12.6.3
Prepare and collect pure, dry carbon dioxide.
12.6.4
12.6.5
Test for the presence of carbon dioxide.
Describe the physical properties and reactions
of carbon dioxide.
Describe the uses of carbon dioxide.
Describe the manufacture of lime from
limestone.
Explain the uses of:
(i) lime and
(ii) slaked lime.
Describe the uses of limestone in the
manufacture of:
(i) cement
(ii) glass and
(iii) iron.
12.6.6
12.6.7
12.6.8
12.6.9
24
Use action of heat and reaction of dilute
acids on carbonates.
Refer to density, colour, smell, solubility
and reaction with alkali.
Refer to processes at a lime industry.
Refer to dangers of over application of
lime in agriculture.
CONTENT
12.7 SILICON
OBJECTIVES (PSBAT)
12.6.10 Identify carbonate ions.
12.6.11 Discuss the greenhouse effect.
12.7.1
Describe the properties of silicon.
12.7.2
12.7.3
12.4.4
Discuss the use of silicon in semi conductors*.
State that silicones are able to exist as oils,
waxes or plastics.
Explain the fire resistance of a silicon plastic
with reference to the nature of combustion
product and compare this to a carbon based
polymer.
12.7.5
State the use of sand in making glass.
25
NOTES
Refer to climate changes. Refer to various
sources of CO and CO2.
A common element in rocks.
Silicon dioxide in quart and complex
silicates in mica. Refer to silicosis as a
health hazard.
Refer to structure of silicons.
Include safe glass disposal.
Refer to sand as an impure form of silicon
(IV) oxide.
UNIT 13.0
CHEMISTRY, SOCIETY AND THE ENVIRONMENT
CONTENT
OBJECTIVES (PSBAT)
13.1.1 Discuss the importance of chemistry in society.
13.1 CHEMISTRY AND
SOCIETY
13.2 POLLUTION
NOTES
Refer to the processes, products and their
usefulness. Consider harmful effects as
well.
13.2.1
13.2.2
Describe pollution.
Explain the effects of air pollution.
13.3.3
Explain the effects of water pollution.
Refer to industrial waste, fertilisers
pesticides and domestic waste.
13.3.4
Explain the effects of land pollution.
13.3.5
Discuss the effects of combustion products of
fossil fuels in the environment.
13.3.6
Outline methods of controlling pollution of air
and water.
Refer to bio diversity, land degradation.
Refer to industrial waste and human
activities.
Refer to extraction and use of coal,
petroleum products.
Refer to the effect of combustion products
of fussil fuels.
Include recycling and bio degradable
materials.
Refer to agencies involved in monitoring
environmental pollution.
26
Refer to the industrial waste.
Refer to effects on animal life, plant life
and buildings.
Chemistry Practical Syllabus
The following points should be considered during practicals in chemistry:
(i)
The student should have the knowledge of volumetric analysis in relation to one set of titrations.
The student is expected to comprehend acid/alkali titrations in relations to ordinary methyl orange or screened methyl orange. Other
titrations using different reagents may be set as well.
(ii)
Other experiments involving the determinations of quantity, temperature change and rate of reactions are necessary. Experiments of this
nature will rely on the use of ordinary apparatus in the laboratory.
(iii) Experiments involving identification of an unknown substance or mixture could be set up. A student is expected to observe and
investigate the expected outcome. This may mainly comprise elementary chromatography and simple tests for oxidising and reducing
agents as well as filtration. Detailed analysis is not necessary but a student is expected to have the knowledge of the reactions of the
cations such as aqueous sodium hydroxide and aqueous ammonia which should include elementary substances like calcium, copper, iron
(II), iron (III), zinc, ammonium and aluminium.
A student should also carry out the tests for the anions such as sulphate, carbonate, iodide, chloride and nitrate. Simple tests for gases
such as hydrogen, carbon dioxide, ammonia, chlorine, sulphur dioxide, oxygen.
Organic substances and ions not mentioned above may be included in the practical lesions. A student is expected to have sufficient
knowledge in this area.
N.B. No exercises books, course books, information booklets and text books will be allowed in the practical examination.
A student shall be expected to perform simple calculations as outlined by the chemistry syllabus.
Practical techniques
Schools and students are reminded of the importance of accuracy in quantitative and qualitative exercises during the practical lessons.
(i)
A student is expected to read the burette accurately and to the nearest volume of 0.1cm 3. At least 3 titrations should be done by a student
to ensure a correct result.
(ii)
A student is expected to take note of the temperature readings to the nearest 0.5oC. Recommended thermometer range is -10oC to 110oC.
The time should be recorded in seconds and the stop clock will be the most convenient timing instrument.
In case of qualitative exercises a student should use around 1cm depth of a solution i.e. (0 to 2cm3) in a test tube. Reagents should be added drop
by drop and thoroughly mixing them, to ensure effective results for each test. The student should make sure that no further changes may occur if
more reagents are added.
27
A learner should take note of the stage at which the change occurs. A learner should take note of colour changes, precipitates and chemicals used
to detect gases, if any, during the experiments. Correct observations recorded are essential and equations are not required during practicals.
Apparatus
Schools offering chemistry as a coded subject are expected to stock the apparatus mentioned below for teaching purposes. In addition schools
should also have standard apparatus such as Bunsen burner and test tubes. Each student should be provided with the necessary apparatus to
conduct the experiments. The apparatus are:
Measuring cylinder calibrated 25cm3 or 50cm3.
Filter funnel.
Beaker with flat bottom and lip with a volume of 250cm3.
Conical flasks with volume of 150cm3 to 250cm3.
Burette with a volume of 50cm3.
Pipettes with volumes of 25cm3.
Pipette fillers.
Thermometers calibrated -10oC to 110oC at intervals of 1oC.
Polystyrene or plastic beaker 150cm3.
Stop clocks which record time in seconds (Personal watches may be used).
Wash bottles.
Pyrex test tubes are essential for heating purposes with capacities 125cm.
Boiling tubes i.e. of dimension 150mm x 25mm.
Stirring rods for stirring or mixing purposes.
Reagents
Schools offering chemistry as a coded subject are reminded of the necessity of stocking standard reagents. These are of paramount importance
during the practicals. The teacher of chemistry should ensure that standard reagents are available as indicated below:
Hydrochloric acid 1.0 moldm-3, nitric acid 1.0 moldm-3, sulphur acid 0.5 moldm-3, aqueous ammonia 1.0 moldm-3, and aqueous sodium
hydroxide 1.0moldm-3.
28
Besides the above mentioned chemicals the following should also be available:
Lime water (a solution of calcium hydroxide), aqueous silver nitrate 0.05 moldm3, aqueous potassium dichromate (VI) 0.1 moldm3, aqueous
potassium iodide 0.1 moldm3, aqueous lead (II) nitrate 0.2 moldm3, and acqueous potassium permanganate (VII) approximate 0.02 moldm3.
The teacher of chemistry should also ensure that chemical substances such as aluminium foil, red litmus paper, blue litmus paper and universal
indicators are in stock.
QUALITATIVE ANALYSIS TESTS
IDENTIFICATION OF ANIONS
Sometimes student will be asked to test for anions. The most common anions are:
1.
Sulphate (SO42-)
This is usually in the solution form. Add dilute nitric acid to sulphate solution to make it acidic. The aqueous barium nitrate should be
added.
Result:
A write precipitate of barium sulphate is formed.
2.
Carbonate (CO32-)
Add any dilute acid such as hydrochloric acid. Effervescence occurs and bubbles of carbon dioxide are liberated.
Result:
Carbon dioxide is liberated.
3.
Nitrate (NO3-)
It is solution form. Add few drops of acqueous sodium hydroxide. Then add aluminium foil or Devarda’s alloy and heat the mixture
gently. Test for ammonia gas.
Result: Moist red litmus paper turns blue.
Ammonia gas is produced.
29
4.
Chloride (Cl - )
The chloride is in the solution state. Add few drops of dilute nitric acid to chloride solution so that it is acidified. Then add few drops of
silver nitrate to the mixture.
Result:
A white precipitate of silver chloride is formed.
5.
Iodine (I - )
The Iodine is in the solution state. Add few drops of dilute nitric acid to make the solution acidified. Then add few drops of fresh aqueous
lead (II) nitrate.
Result:
A yellow precipitate of lead (II) Iodine nitrate is formed.
IDENTIFICATION OF GASES
There are seven gases which are often examinable. A student is expected to carry out tests and record the results in a systematic manner. The
common gases are listed below.
1.
Sulphur dioxide (SO2)
It has a pungent smell.
It turns blue litmus to red.
It turns aqueous potassium dichromated to green.
2.
Carbon dioxide (CO2)
Bubble carbon dioxide into calcium hydroxide (lime water). The lime water turns milky white.
3.
Oxygen (O2)
Introduce a glowing splint in the test tube containing oxygen. Oxygen relights a glowing splint.
30
4.
Hydrogen (H2)
Introduce a burning splint in the test tube containing hydrogen, the hydrogen gas burns with a ‘pop’ sound.
5.
Ammonia (NH3)
It has a pungent smell.
It turns damp red litmus paper to blue colour.
6.
Chlorine (Cl2)
Chlorine is yellowish green in colour. It turns blue litmus to red and it bleaches the damp blue litmus paper.
Practical chemistry may require a student to identify cations. The most common cations likely to be tested are:
1.
Copper (II) (Cu2+)
(a) Add few drops of aqueous sodium hydroxide to copper salt solution. A light blue precipitate is formed. This is insoluble when it is
in excess.
(b) Add few drops of aqueous ammonia to copper solution.
Result:
A light blue precipitate is formed. If excess aqueous ammonia is added to the light blue precipitate changes to a dark blue solution which
becomes soluble.
2.
Zinc (Zn2+)
(a) Add few drops of aqueous sodium hydroxide to Zinc solution. A white precipitate is formed. If more sodium hydroxide is added to
Zinc solution, the precipitate dissolves and gives rise to a colourless solution.
(b) Add few drops of aqueous ammonia to the Zinc salt solution. A white precipitate of Zinc hydroxide is formed. If excess aqueous
ammonia is added to the precipitate, the solution becomes colourless.
31