Area Of Concentration (Syllabus) For WAEC Chemistry 2021/2022
Are you in search of an area of concentration for your waec chemistry examination? Well, I am glad to inform you that you have come to the right place.
Perhaps you might be wondering what does an area of concentration means. An area of concentration means those topics that do come out every year for chemistry examination, and you must ensure you read it over and over again so you can be well prepared for the upcoming examination.
Note: it does not mean you won’t read other topics not on the area of concentration for waec chemistry examination, actually you need to. So that you can be better than the best.
Things you should know about the area of concentration for waec chemistry
- You should note that area of concentration for your chemistry examination will set you on the right path and it will ensure you cover those pressing topics you need to cover without leaving anyone behind.
- It helps you to prepare better because you already know what is in vogue.
- It helps you to be better than your peers because you have a secret weapon they don’t have.
Having known all this, are you still dulling. Well if you have been dulling all this time, now you should not because you already know-how area of concentration for your chemistry examination will help you to score higher and become one of the best. Sincerely, there is no secret about it. One man once said a man who knows the way is the one that knows the book. How hilarious…
Now, having had a glimpse of the idea of how important area of concentration is, let’s move on to the things you will see in an area of concentration for your upcoming waec chemistry examination.
Things you will see on your area of concentration for your upcoming waec chemistry examination
- It is the simplest, easiest things or materials you will see forgetting vital information for your upcoming exam.
- When we talk about the area of concentration, we are also talking about waec syllabus for chemistry examination. Hence, it contains vital information on the topics to be read, contents of the topics e.t.c
- It is free of charge and very accessible once you have data on your phone, you can browse it online, just like you are doing here. hence it is free of charge and very accessible.
- It contains information on all what you need to cover before writing the exam, that will set you ahead of others.
- Why you need waec chemistry area of concentration/syllabus as a student
- Get important information concerning each topics aims and objectives.
- Have a general knowledge concerning where waec normally sets their questions from.
- Know the contents that are within each topic.
The objectives of waec chemistry area of concentration
- To have the necessary logical reasoning in solving any problems
- It will guide you to know about the short notes and recommended textbooks needed for the exams.
- To have a vital computational skill in solving any problems
- To prepare candidates so that they can know where to get the area of concentration, they can rely on.
- To ensure that the objectives of each topic are well understood and well taught to the students
- To apply these principles and theories taught to everyday life.
Waec chemistry examination pattern
- We should note that all chemistry waec examination is in objective forms.
- Candidates are expected to answer 180 questions within 2hours.
- Answering waec examination is easy, all candidates need to do is to recognise and to be able to have a good knowledge of the subject matter.
- Waec questions are indifferent, some could be true or false, while some could be multiple choice and the rest.
- Waec questions tend to cover more materials than waec essays, I hope you know that, if not. Ensure you know that now.
- Waec questions have only one correct answer.
- Waec requires strict preparation and well-versed knowledge of the subject matter.
Tips on how to cover waec syllabus within two weeks.
Go through the syllabus thoroughly.
- Collect necessary studying materials needed from different sources
- Visit different websites and textbooks to gain more knowledge and to make your necessary contribution if needed.
- Make your personal notes on every topic you read. This will help a lot.
- Make important points and make use of initials too so you can be able to remember what you ought to remember.
- Form a valid abbreviation for yourself and use them to study.
- Having too many textbooks will confuse you and give you a burden.
- You must find solutions to all problems met when reading or solving.
- Ensure you jot down the salient point and have your personal notebook while reading, this will keep you on managing your time.
- Practise at least 5 previous years past questions so you can see the format waec set its questions. Also, ensure you get the right answers to the questions.
- Read efficient textbooks and also ensure to read the textbooks that explain better, that enables you to grasp the subject matter very well.
- First, choose the easy topic that you know you can understand properly within a twinkle of an eye. You should complete the easy topic first, you can complete this in no time.
- After that, first, try to read the book and take short notes on that book.
- If you are preparing for waec exam, they sit down and analyze past questions of waec to see the format in which waec sets its question.
- Focus more on those topics that are repeated frequently in the past questions.
- The G factor: Always ensure you pray to your maker before and after reading and also pray to him before and after your exams. Many students think they can pass on their own and therefore neglect the God factor. That will bring them failure of course because even the bible confirms it, lean not on your own understanding.
- Waec past questions and answers: when using waec questions, ensure you solve those questions on your own before checking the answer. Also ensure that the ones you don’t know or the one you are not sure of, make sure you give your teachers or people who are better than you in chemistry to put you through. Don’t always rely on the past question answer, some of them are not correct. Ensure you find the correct answers to all the questions.
- Waec chemistry textbook: when using any chemistry textbook, ensure you read the ones that you find it easy to remember. Don’t read the ones you find it hard to read as doing this could lead you to fail your exams woefully.
- Don’t be a jack of all trade by trying to remember everything. Instead, you should understand the concept, once you understand the concept, you can put it down in your own way.
- Ensure you take short and long breaks while studying.
- Engage in meaningful conversation with your friends to share knowledge and gain more knowledge since nobody is a mountain of knowledge.
- Ensure you don’t stress your brain too much by loading it with knowledge even when you ought to be sleeping. Ensure you sleep when you ought to.
- Get a mentor who will advise you on what and what you ought not to do. Ensure your mentor is someone who is successful and someone you can look up to.
- Ask for feedback from your mentor or your teachers on how far you are performing.
- Make reliable and realistic goals every day and achieve them.
- Form your own note as you study.
Tips you should note when writing your Chemistry exams to avoid had I known
- When you have less than 20 minutes to the end of the papers and you discovered you still have so many difficult questions that you have not answered, then you should ensure you use the prediction method.
- Never should you leave any questions unanswered. Even though you don’t know the answer, ensure you guess.
- It is advisable to start answering the simplest questions before moving on to the hard ones.
- Read and understand the questions properly before selecting an answer, ensure you note this.
- Do not waste much time on a particular question, if you don’t know one, then move on to the next one but in case you don’t have time, just guess.
- Evaluate each answer after reading the questions and understanding what it is telling you to do. Evaluate each answer as this will help you to discover the answer you should choose. There are some times whereby you will have two close answers, in this case, take a deep breath, relax and pray, then choose the option that inner mind tells you to choose, it normally ends up mostly to be the right answer.
- Remove each wrong answer from the option to get the right answer. For instance, you can be asked which gender is your mum, you should note that the answer is female, so any other answer that does not relate to the questions, you should eliminate it.
2021/2022 WAEC Chemistry Syllabus
INTRODUCTION TO CHEMISTRY
(a) (i) Measurement of physical quantities.
(ii) Scientific measurements and their importance in chemistry.
(b) Scientific Methods
2.0 STRUCTURE OF THE ATOM
(a) Gross features of the atom.
(b) (i) Atomic number/proton number, number of neutrons, isotopes, atomic mass, mass number.
(1) Measurement of mass, length, time, temperature and volume.
You can download your chemistry area of concentration here
(2) Appropriate SI units and significant figures.
(3) Precision and accuracy in measurement.
Outline the scientific method to include:
Observation, hypothesis, experimentation, formulation of laws and theories.
(1) Short account of Dalton’s atomic theory and limitations, J.J. Thompson’s experiment and Bohr’s model of the atom.
(2) Outline description of Rutherford’s alpha scattering experiment to establish the structure of the atom.
Meaning and representation in symbols of atoms and sub-atomic particles.
(ii) Relative atomic mass (Ar) and relative molecular mass (Mr) based on Carbon-12 scale. (iii) Characteristics and
nature of matter.
(c) Particulate nature of matter: physical and chemical changes.
(d) (i) Electron Configuration
(iii) Rules and principles
for filling in electrons.
(1) Atomic mass as the weighted average mass of isotopes. Calculation of the relative mass of chlorine should be used as an example. (2) Carbon-12 scale as a unit of measurement.
Definition of the atomic mass unit.
Atoms, molecules and ions.
Definition of particles and treatment of particles as building blocks of matter.
Explain physical and chemical changes with examples.
Physical change- melting of solids, the magnetization of iron, dissolution of salt etc.
Chemical change- burning of wood, rusting of iron, the decay of leaves etc.
Detailed electron configurations (s,p,d) for atoms of the first thirty elements.
Origin of s,p and d orbitals as sub-energy levels; shapes of s and p orbitals only.
(1) Aufbau Principle, Hund’s Rule of Maximum Multiplicity and Pauli Exclusion Principle.
(2) Abbreviated and detailed electron configuration in terms of s, p, and d.
CONTENT NOTES 3.0 STANDARD SEPARATION TECHNIQUES FOR MIXTURES
(a) Classification of mixtures.
(b) Separation techniques
(c) Criteria for purity.
4.0 PERIODIC CHEMISTRY
(a) Periodicity of the elements.
(b) Different categories of elements in the periodic table.
(c) Periodic law:
(i) Trends on the periodic table;
(ii) Periodic gradation of the elements in the third period (Na – Ar).
Solid-solid, solid-liquid, liquid-liquid, gas-gas with examples.
Crystallization, distillation, precipitation, magnetization, chromatography, sublimation etc.
The boiling point for liquids and melting point for solids.
Electron configurations leading to a group and periodic classifications.
Metals, semi-metals, non-metals in the periodic table and halogens. Alkali metals, alkaline earth metals and transition metals as metals.
Explanation of the periodic law.
Periodic properties; atomic size, ionic size, ionization energy, electron affinity and electronegativity.
Simple discrepancies should be accounted for in respect to beryllium, boron, oxygen and nitrogen.
(1) Progression from:
(i) metallic to the non-metallic character of the element;
(ii) ionic to covalent bonding in compounds.
(d) Reactions between acids and metals, their oxides and trioxocarbonates (IV).
(e) Periodic gradation of elements in group seven, the halogens: F, Cl, Br and I.
(f) Elements of the first transition series.
21Sc – 30Zn
(2) Differences and similarities in the properties between the second and the third-period elements should be stated. (1) Period of three metals (Na, Mg, Al).
(2) Period of four metals (K, Ca).
(3) Chemical equations.
(4) the pH of solutions of the metallic oxides and trioxocarbonates.
Recognition of group variations noting any anomalies.
Treatment should include the following:
(a) physical states, melting and boiling points;
(b) variable oxidation states;
(c) redox properties of the elements;
(d) displacement reaction of one halogen by another;
(e) the reaction of the elements with water and alkali (balanced equations required).
(1) Their electron configurations, physical properties and chemical reactivity of the elements and their compounds.
(2) Physical properties should include physical states, metallic properties and magnetic properties.
(3) Reactivity of the metals with air, water, acids and comparison with s-block elements (Li, Na, Be, Mg).
CONTENT NOTES5.0 CHEMICAL BONDS
(a) Interatomic bonding
(b) (i) Formation of ionic bonds and compounds.
(ii) Properties of ionic compounds.
(c) Naming of ionic compounds.
(d) Formation of covalent bonds and compounds.
(e) (i) Properties of covalent compounds.
(ii) Coordinate (dative) covalent bonding.
(4) Other properties of transition metals should include:(a) variable oxidation states;
(b) formation of coloured compounds;
(c) complex formation;
(d) catalytic abilities;
Meaning of chemical bonding.
Lewis dot structure for simple ionic and covalent compounds.
Formation of stable compounds from ions. Factors influencing formation: ionization energy; electron affinity and electronegativity difference.
Solubility in polar and non-polar solvents, electrical conductivity, hardness and melting point.
IUPAC system for simple ionic compounds.
Factors influencing covalent bond formation. Electron affinity, ionization energy, atomic size and electronegativity.
Solubility in polar and non-polar solvents, melting point, boiling point and electrical conductivity.
Formation and difference between pure covalent and coordinate (dative) covalent bonds.
(f) Shapes of molecular compounds.
(g) (i) Metallic Bonding
(ii) Factors influencing its formation.
(iii) Properties of metals.
(h) (i) Intermolecular bonding
(ii) Intermolecular forces in covalent compounds.
(iii) Hydrogen bonding
(iii) van der Waals forces
(iv) Comparison of all bond types.
Linear, planar, tetrahedral and shapes for some compounds e.g. BeCl2, BF3, CH4, NH3, CO2. Factors should include atomic radius, ionization energy and the number of valence electrons. Types of specific packing not required.
Typical properties including heat and electrical conductivity, malleability, lustre, ductility, sonority and hardness.
Relative physical properties of polar and non-polar compounds.
Description of formation and nature should be treated.
Dipole-dipole, induced dipole-dipole, induced dipole-induced dipole forces should be treated under van der Waal’s forces.
Variation of the melting points and boiling points of noble gases, halogens and alkanes in the homologous series explained in terms of van der Waal’s forces; and variation in the boiling points of H2O, and H2S explained using Hydrogen bonding.
6.0 STOICHIOMETRY AND CHEMICAL REACTIONS
(i) Symbols, formulae and equations.
(ii) chemical symbols
(iii) Empirical and molecular formulae.
(iv) Chemical equations and IUPAC names of chemical compounds.
(v) Laws of chemical combination.
(b) Amount of substance.
Symbols of the first thirty elements and other common elements that are not among the first thirty elements.
Calculations involving formulae and equations will be required. Mass and volume relationships in chemical reactions and the stoichiometry of such reactions such as calculation of percentage composition of the element.
(1) Combustion reactions (including combustion of simple hydrocarbons)
(3) Displacement or replacement
(5) Ionic reactions
(1) Laws of conservation of mass.
(2) Law of constant composition.
(3) Law of multiple proportions. Explanation of the laws to balance given equations.
(4) Experimental illustration of the law of conservation of mass.
(1) Mass and volume measurements.
(2) The mole as a unit of measurement; Avogadro’s constant, L= 6.02 x 1023 entities mol-1.
(3) Molar quantities and their uses.
(4) Moles of electrons, atoms, molecules, formula units etc.
(c) Mole ratios(d) (i) Solutions
(ii) Concentration terms
(iii) Standard solutions.
(e) Preparation of solutions from liquid solutes by the method of dilution.
Use of mole ratios in determining the stoichiometry of chemical reactions. Simple calculations to determine the number of entities, amount of substance, mass, concentration, volume and percentage yield of the product. (1) Concept of a solution as made up of solvent and solute.
(2) Distinguishing between the dilute solution and the concentrated solution.
(3) Basic, acidic and neutral solutions.
Mass (g) or moles (mol) per unit volume. Emphasis on current IUPAC chemical terminology, symbols and conventions. Concentration is expressed as a mass concentration, g dm-3, molar concentration, mol dm-3.
(1) Preparation of some primary standards e.g anhydrous Na2CO3, (COOH)2, 2H2O/H2C2O4.2H2O.
(2) Meaning of the terms primary standard, secondary standard and standard solution.
7.0 STATES OF MATTER
(i) Kinetic theory of matter.
(ii) Changes in the state of matter.
(1) Postulates of the kinetic theory of matter.
(2) Use of the kinetic theory to explain the following processes: melting of solids, boiling of liquids, evaporation of liquids, dissolution of solutes, Brownian motion and diffusion.
(1) Changes of state of matter should be explained in terms of movement of particles. It should be emphasized that randomness decreases (and orderliness increases) from a gaseous state to a liquid state and to solid-state and vice versa.
(2) Illustrations of changes of state using the different forms of water, iodine, sulphur, naphthalene etc.
(3) Brownian motion to be illustrated using any of the following experiments:
(a) pollen grains/powdered sulphur in water (viewed under a microscope);
(b) smoke in a glass container illuminated by a strong light from the side;
(c) a dusty room being swept and viewed from outside under sunlight.
(1) Experimental demonstration of diffusion of two gases.
(2) Relationship between the speed at which different gas particles move and the masses of particles.
(3) Experimental demonstration of diffusion of solute particles in liquids.
(i) Characteristics and nature of gases;
(ii) The gas laws;
(iii) Laboratory preparation and properties of some gases.
(ii) Vapour and gases.
Arrangement of particles, density, shape and compressibility.
The Gas laws: Charles’; Boyle’s; Dalton’s law of partial pressure; Graham’s law of diffusion, Avogadro’s law. The ideal gas equation of state. A qualitative explanation of each of the gas laws using the kinetic model.
The use of Kinetic molecular theory to explain changes in gas volumes, pressure, temperature.
Mathematical relations of the gas law
Ideal and Real Gases
Factors responsible for the deviation of real gases from an ideal situation.
(1) Preparation of the following gases: H2, NH3 and CO2. Principles of purification and collection of gases.
(2) Physical and chemical properties of the gases.
Characteristics and nature of liquids based on the arrangement of particles, shape, volume, compressibility, density and viscosity.
(1) Concept of vapour, vapour pressure, saturated vapour pressure, boiling and evaporation.
(2) Distinction between vapour and gas.
(3) Effect of vapour pressure on boiling points of liquids.
(4) Boiling at reduced pressure.
(d) Solids:(i) Characteristics and nature;
(ii) Types and structures;
(iii) Properties of solids.
(e) Structures, properties and uses of diamond and graphite.
(f) Determination of melting points of covalent solids.
8.0 ENERGY AND ENERGY CHANGES
(a) Energy and enthalpy
(b) Description, definition and illustrations of energy changes and their effects.
(1) Ionic, metallic, covalent network and molecular solids. Examples in each case.
(2) Arrangements of particles ions, molecules and atoms in the solid-state.
Relate the properties of solids to the type of interatomic and intermolecular bonding in the solids. Identification of the types of chemical bonds in graphite and differences in the physical properties.
The uses of diamond and graphite related to the structure.
The use of iodine in everyday life.
Melting points as an indicator of the purity of solids e.g. Phenyl methanoic acid (benzoic acid), ethanedioic acid (oxalic) and ethanamide.
Explanation of the terms energy and enthalpy. Energy changes associated with chemical processes.
(1) Exothermic and endothermic processes.
(2) Total energy of a system as the sum of various forms of energy e.g. kinetic, potential, electrical, heat, sound etc.
(3) Enthalpy changes involved in the following processes: combustion, dissolution and neutralization.
9.0 ACIDS, BASES AND SALTS(a) Definitions of acids and bases.
(b) Physical and chemical properties of acids and bases.
(c) Acids, bases and salts as electrolytes.
(d) Classification of acids and bases.
(e) Concept of pH
(1) Arrhenius concepts of acids and bases in terms of H3O+ and OH– ions in water.
(2) Effects of acids and bases on indicators, metal Zn, Fe and trioxocarbonate (IV) salts and hydrogentrioxocarbonate (IV) salts.
Characteristic properties of acids and bases in aqueous solution to include:
(a) conductivities, taste, litmus/indicators, feel etc.;
(b) balanced chemical equations of all reactions.
Electrolytes and non-electrolytes; strong and weak electrolytes. Evidence from conductivity and enthalpy of neutralization.
(1) Strength of acids and bases.
(2) Classify acids and bases into strong and weak.
(3) Extent of dissociation reaction with water and conductivity.
(4) Behaviour of weak acids and weak bases in water as an example of equilibrium systems.
(1) Definition of pH and knowledge of pH scale.
(2) Measurement of pH of solutions using pH meter, calorimetric methods or universal indicator.
(3) Significance of pH values in everyday life e.g. acid rain, pH of the soil, blood, urine.
(i) Laboratory and industrial preparation of salts;
(iii) Hydrolysis of salt.
(g) Deliquescent, efflorescent and hygroscopic compound.
(h) Acid-Base indicators
(i) Acid-Base titration
Meaning of salts.Types of salts: normal, acidic, basic, double and complex salts.
(1) Description of laboratory and industrial production of salts.
(2) Mining of impure sodium chloride and conversion into granulated salt.
(3) Preparation of NaOH, Cl2 and H2.
(1) Explanation of how salts from acidic, alkaline and neutral aqueous solutions.
(2) Behaviour of some salts (e.g NH4Cl, AlCl3, Na2CO3, CH3COONa) in water as examples of equilibrium systems.
(3) Effects of charge density of some cations and anions on the hydrolysis of their aqueous solution. Examples to be taken from group 1, group 2, group 3 and the d-block element.
Use of hygroscopic compounds as drying agent should be emphasized.
(1) Qualitative description of how acid-base indicator works.
(2) Indicators as weak organic acids or bases (organic dyes).
(3) Colour of an indicator at any pH dependent on relative amounts of acid and forms.
(4) Working pH ranges of methyl orange and phenolphthalein.
(1) Knowledge and correct use of relevant apparatus.
(2) Knowledge of how acid-bases indicators work in titrations.
10.0 SOLUBILITY OF SUBSTANCES
(a) General principles
(b) Practical application of solubility.
(3) Acid-base titration experiments involving HCl, HNO3, H2SO4 and NaOH, KOH, Ca(OH)2, CO32-, HCO3–. (4) Titration involving weak acids versus strong bases, strong acids versus weak bases and strong acids versus strong bases using the appropriate indicators and their applications in quantitative determination; e.g. concentrations, mole ratio, purity, the water of crystallization and composition.
(1) Meaning of Solubility.
(2) Saturated and unsaturated solutions.
(3) Saturated solution as an equilibrium system.
(4) Solubility expressed in terms of mol dm-3 and g dm-3 of solution/solvent.
(5) Solubility curves and their uses.
(6) Effect of temperature on solubility of a substance.
(7) Relationship between solubility and crystallization.
(8) Crystallization/recrystallization as a method of purification.
(9) Knowledge of soluble and insoluble salts of stated cations and anions.
(10) Calculations on solubility.
Generalization about the solubility of salts and their applications to qualitative analysis. e.g. Pb2+, Ca2+, Al3+, Cu2+, Fe2+, Fe3+, Cl–, Br–, I–, SO42-, S2-, and CO32-, Zn2+, NH4+, SO32-
Explanation of solubility rules.
CONTENT NOTES 11.0 CHEMICAL KINETICS AND EQUILIBRIUM SYSTEM
(a) Rate of reactions:
(i) Factors affecting rates;
(ii) Theories of reaction rates;
(iii) Analysis and interpretation of graphs.
(i) General Principle;
(1) Definition of reaction rate.
(2) Observable physical and changes: colour, mass, temperature, pH, the formation of precipitate etc.
(1) Physical states, concentration/ pressure of reactants, temperature, catalysts, light, particle size and nature of reactants.
(2) Appropriate experimental demonstration for each factor is required.
(1) Collision and transition state theories to be treated qualitatively only.
(2) Factors influencing collisions: temperature and concentration.
(3) Effective collision.
(4) Activation energy.
(5) Energy profile showing activation energy and enthalpy change.
Drawing of graphs and charts.
Explanation of reversible and irreversible reactions. Reversible reaction i.e. dynamic equilibrium. Equilibrium constant K must be treated qualitatively. It must be stressed that K for a system is constant at a constant temperature.
A simple experiment to demonstrate reversible reactions.
(ii) Le Chatelier’s principle.
12.0 REDOX REACTIONS
(a) Oxidation and reduction process.
(b) Oxidizing and reducing agents.
(c) Redox equations
(d) Electrochemical cells:
(i) Standard electrode potential;
(ii) Drawing of cell diagram and writing cell notation.
Prediction of the effects of external influence of concentration, temperature pressure and volume changes on equilibrium systems.
(1) Oxidation and reduction in terms of:
(a) addition and removal of oxygen and hydrogen;
(b) loss and gain of electrons;
(c) change in oxidation numbers/states.
(2) Determination of oxidation numbers/states.
(1) Description of oxidizing and reducing agents in terms of:
(a) addition and removal of oxygen and hydrogen;
(b) loss and gain of electrons;
(c) change in oxidation numbers/state.
Balancing redox equations by:
(a) ion, electron or change in oxidation number/states;
(b) half-reactions and overall reaction.
(1) Standard hydrogen electrode: the meaning of standard electrode potential (Eo) and its measurement.
(2) Only metal/metal ion systems should be used.
(iii) e.m.f of cells;(iv) Application of Electrochemical cells.
(i) Electrolytic cells;
(ii) Principles of electrolysis;
(iii) Factors influencing discharge of species;
(iv) Faraday’s laws;
(v) Practical application;
(1) Electrochemical cells as a combination of two half-cells. (2) The meaning of magnitude and sign of the e.m.f.
(1) Distinction between primary and secondary cells
(2) Daniell cell, lead-acid battery cell, dry cells, fuel cells and their use as generators of electrical energy from chemical reactions.
Comparison of electrolytic and electrochemical cells; weak and strong electrolyte.
Mechanism of electrolysis.
Limit electrolytes to molten PbBr2
and NaCl, dilute NaCl solution, concentrated NaCl solution, CuSO4(aq), dilute H2SO4, NaOH(aq)and CaCl2(aq) (using platinum or graphite and copper electrodes).
Simple calculations based on the relation 1F= 96,500 C and mole ratios to determine the mass, the volume of gases, number of entities, charges etc. using half and overall reactions.
Electroplating, extraction and purification of metals.
(vi) Corrosion of metals.
13.0 CHEMISTRY OF CARBON COMPOUNDS
(b) Functional group
(b) Separation and purification of organic compounds.
(c) Petroleum/crude oil
(1) Corrosion treated as a redox process.
(2) Rusting of iron and its economic costs.
(3) Prevention based on the relative magnitude of electrode potentials and preventive methods like galvanizing, sacrificial/cathodic protection and non-redox methods (painting, greasing/oiling etc.).
Broad classification into a straight-chain, branched-chain, aromatic and alicyclic compounds.
Systematic nomenclature of compounds with the following functional groups: alkanes, alkenes, alkynes, hydroxyl compounds (aliphatic and aromatic), alkanoic acids, alkyl alkanoates (esters and salts) and amines.
Methods to be discussed should include distillation; crystallization; drying and chromatography.
(1) Composition and classification.
(2) Fractional distillation and major products.
(3) Cracking and reforming.
(4) Petro-chemicals: sources; uses e.g. as starting materials of organic synthesis.
(5) Quality of petrol, the meaning of octane number and its importance to the petroleum industry.
(d) Determination of empirical and molecular formulae and molecular structures of organic compounds. (e) General properties of organic compounds:
(i) Homologous series;
(i) Sources, properties;
(i) Sources and properties;
(1) Gradation in physical properties.
(2) Effects on the physical properties by the introduction of active groups into the inert alkane.
(1) Examples should be limited to compounds having a maximum of five carbon atoms.
(2) Differences between structural and geometric/stereoisomerism.
(1) Laboratory and industrial preparations and other sources.
(2) Nomenclature and structure.
(b) substitution reactions;
(c) cracking of large alkane molecules.
As fuels, as starting materials for synthesis. Uses of haloalkanes and pollution effects.
(1) Laboratory preparation.
(2) Nomenclature and structure.
(iii) Laboratory detection.
(i) Sources, characteristic properties and uses;
(ii) Chemical reactions.
(i) Structure and physical properties;
(ii) Chemical properties.
(3) Addition reactions with halogens hydrogen, bromine water, hydrogen halides and acidified water. (4) Oxidation: hydroxylation with aqueous KMnO4.
Use of reaction with Br2/water, Br2/CCl4 and KMnO4(aq) as means of characterizing alkenes.
(1) Nomenclature and structure.
(2) Industrial production of ethyne.
(3) Uses of ethyne.
(4) Distinguishing test between a terminal and non-terminal alkynes.
(5) Test to distinguish between alkane, alkene and alkyne.
Chemical reactions: halogenation, combustion, hydration and hydrogenation.
Resonance in benzene. Stability leading to substitution reactions.
(1) Addition reactions: hydrogenation and halogenation (mechanism not required).
(2) Compare reactions with those of alkenes.
(J) Alkanols:(i) Sources, nomenclature and structure;
(iii) Physical properties;
(iv) Chemical properties;
(v) Laboratory test;
(k) Alkanoic acids:
(i) Sources, nomenclature and structure;
(ii) Physical properties;
(1) Laboratory preparation including hydration of alkenes.
(2) Industrial and local production of ethanol including alcoholic beverages,
(3) Harmful impurities and methods of purification should be mentioned.
(4) Recognition of the structure of mono-, di- and triols.
Primary, secondary and tertiary alkanols.
Boiling point, solubility in water. Including the hydrogen bonding effect.
(1) Reaction with:
(b) alkanoic acids (esterification);
(c) conc. H2SO4.
(2) Oxidation by:
(c) I2 in NaOH(aq).
Laboratory test for ethanol.
Methanoic acid –insect bite.
Ethanoic acid – vinegar.
Recognition of mono and dioic acid.
Boiling point, solubility in water.
Including the hydrogen bonding effect.
(iii) Chemical properties;(iv) Laboratory test;
(l) Alkanoates as derivatives of alkanoic acids:
(i) Sources, nomenclature, preparation and structure;
(ii) Physical properties;
(iii) Chemical properties;
14.0 CHEMISTRY, INDUSTRY AND THE ENVIRONMENT
(a) Chemical industry
Acid properties only i.e. reactions with H2O, NaOH, NH3, NaHCO3, Zn and Mg.
Reaction with NaHCO3, Na2CO3.
Uses of ethanoic and phenyl methanoic (benzoic) acids as examples of aliphatic and aromatic acids respectively.
Preparation of alkyl alkanoates (esters) from alkanoic acids.
Solubility, boiling and melting point.
Hydrolysis of alkyl alkanoates (mechanism not required).
Uses of alkanoates to include the production of soap, flavouring agent, plasticizers, as solvents and in perfumes.
(1) Natural resources in a candidate’s own country.
(2) Chemical industries in candidates own country and their corresponding raw materials.
(3) Distinction between fine and heavy chemicals.
(b) Pollution: air, water and soil pollution;
15.0 BASIC BIOCHEMISTRY AND SYNTHETIC POLYMERS
(i) Sources and properties;
(ii) Uses of protein.
(b) Amino acids
(4) Factors that determine the location of chemical industries. (5) Effect of industries on the community.
(1) Sources, effects and control.
(2) Greenhouse effect and depletion of the ozone layer.
(3) Biodegradable and non-biodegradable pollutants.
Food processing, fermentation including the production of gari, bread and alcoholic beverages e.g. Local gin.
Proteins as polymers of amino acids molecules linked by peptide or amide linkage.
Physical properties e.g. solubility
Chemical properties to include:
(a) Hydrolysis of proteins;
(b) Alaboratory test using Ninhydrin/Biuret reagent/Millon’s reagent.
(1) Nomenclature and general structure of amino acids.
(2) Difunctional nature of amino acids.
(c) Fats/oils:(i) Sources and properties;
(ii) General structure of fats/oils;
(iii) Preparation of soap;
(iv) Uses of fats/oils.
(i) Sources and nomenclature;
As alkyl alkanoates (esters).
From animals and plants.
Physical properties such as solubility.
(a) acidic and alkaline hydrolysis;
(c) test for fats and oil.
As mono-, di-, and tri- esters of propane-1,2,3-triol (glycerol).
(1) Preparation of soap (saponification) from fats and oils.
(2) Comparison of soapless detergents and their action on soft and hard water.
(1) Classes of carbohydrates as:
(2) Name and components of various classes of carbohydrates.
(1) Physical properties such as solubility of sugars.
(2) Chemical properties- Hydrolysis of disaccharides into monosaccharides.
(3) Test for reducing sugars using sugar strips, Fehling’s or Benedict’s solution or Tollen’s reagent.
(iii) Carbohydrate as examples of polymer;(iv) Uses.
(e) Synthetic polymers:
(ii) Uses of polymers.
(1) Starch as a polymer made up of glucose units.
(2) Condensation of monosaccharides to form disaccharides and polysaccharides.
(1) Definition of terms: monomers, polymers and polymerization.
(2) Addition and condensation polymerization.
(3) Classification and preparation based on the monomers and polymers.
(1) Thermoplastics and thermosets.
(2) Modification of properties of polymers.
(3) Plastics and resins.
(4) Chemical test on plastics using: