Updated JAMB Syllabus for Chemistry and Hot Topics 2019/2020

The purpose of the 2020 JAMB Syllabus for chemistry and Hot Topics is to prepare the candidates for the forthcoming Jamb examination. JAMB Syllabus for chemistry is a guide where all JAMB subject topic and textbooks are listed out. JAMB will tell you what to read and what you should be able to do after reading the topic.

You may also want to check out Jamb Chemistry Repeated Questions and Jamb Chemistry Past Questions and Answers. If you are worried about the JAMB Subject Combination for all Courses in Nigeria, click that link.

Jamb Syllabus for Chemistry 2019/2020 will help you achieve the following:

• Understand the basic principles and concepts in chemistry;
• Interpret scientific data relating to chemistry;
• Deduce the relationships between chemistry and other sciences;
• Apply the knowledge of chemistry to industry and everyday life.

These Jamb Syllabus for chemistry will also help you in other exams like WAEC and POST UTME.

JAMB SYLLABUS FOR CHEMISTRY

1. Separation of mixtures and purification of chemical substances

Objectives:

Candidates should be able to:
(i) distinguish between pure and impure substances;
(ii) use boiling and melting points as criteria for purity of chemical substances;
(iii) distinguish between elements, compounds and mixture;
(iv) differentiate between chemical and physical changes;
(v) identify the properties of the components of a mixture;
(vi) specify the principle involved in each separation method.
(vii) apply the basic principle of separation processes in everyday life.

Topics:

(a) Pure and impure substances
(b) Boiling and melting points.
(c) Elements, compounds and mixtures
(d) Chemical and physical changes.
(e) Separation processes: evaporation, simple and fractional distillation, sublimation, filtration, crystallization, paper and column chromatography, simple and fractional crystallization, magnetization, decantation.

2. Chemical combination

Objectives:

Candidates should be able to:
(i) perform simple calculations involving formulae, equations/chemical composition and the mole concept;
(ii) deduce the chemical laws from given expressions/statements/data;
(iii) interpret graphical representations related to these laws;
(iv) deduce the stoichiometry of chemical reactions.

Topics:

Stoichiometry, laws of definite and multiple proportions, law of conservation of matter, Gay Lussac’s law of combining volumes, Avogadro’s law; chemical symbols, formulae, equations and their uses, relative atomic mass based on 12C=12, the mole concept and Avogadro’s number.

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3. Air

Objectives:

Candidates should be able to:
(i) deduce reason (s) for the existence of air as a mixture;
(ii) identify the principle involved in the separation of air components;
(iii) deduce reasons for the variation in the composition of air in the environment;
(iv) specify the uses of some of the constituents of air.

Topics: 

(a) The natural gaseous constituents and their proportion in the air.- nitrogen, oxygen, water vapour, carbon (IV) oxide and the noble gases (argon and neon).
(b) Air as a mixture and some uses of the noble gas.

4. Atomic structure and bonding

Objectives:

Candidates should be able to:
(i) distinguish between atoms, molecules and ions;
(ii) identify the contributions of these scientists to the development of the atomic structure;
(iii) deduce the number of protons, neutrons and electrons from atomic and mass numbers of an atom;
(iv) apply the rules guiding the arrangement of electrons in an atom;
(v) identity common elements exhibiting isotopy;
(vi) relate isotopy to mass number;
(vii) perform simple calculations relating to isotopy;
(viii) differentiate between the shapes of the orbitals;
(ix) determine the number of electrons in s and p atomic orbitals;
(x) relate atomic number to the position of an element on the periodic table;
(xi) relate properties of groups of elements on the periodic table;
(xii) identify reasons for variation in properties across the period and down the groups.
(xiii) differentiate between the different types of bonding.
(xiv) deduce bond types based on electron configurations;
(xv) relate the nature of bonding to properties of compounds;
(xvi) differentiate between the various shapes of molecules
(xvii) distinguish between ordinary chemical reaction and nuclear reaction;
(xviii) differentiate between natural and artificial radioactivity;
(xix) compare the properties of the different types of nuclear radiations;
(xx) compute simple calculations on the half-life of a radioactive material;
(xxi) balance simple nuclear equation.

Topics:

(a) (i)The concept of atoms, molecules and ions, the works of Dalton, Millikan, Rutherford, Moseley, Thompson and Bohr.
(ii) Atomic structure, electron configuration, atomic number, mass number and isotopes; specific examples should be drawn from elements of atomic number 1 to 20.
(iii) Shapes of s and p orbitals.
(b) The periodic table and periodicity of elements, presentation of the periodic table with a view to recognizing families of elements e.g. alkali metals, halogens, the noble gases and transition metals. The variation of the following properties: ionization energy, ionic radii, electron affinity and electronegativity.
(c) Chemical bonding. Electrovalency and covalency, the electron configuration of elements and their tendency to attain the noble gas structure. Hydrogen bonding and metallic bonding as special types of electrovalency and covalency respectively; coordinate bond as a type of covalent bond as illustrated by complexes like [Fe(CN)6]3-, [Fe(CN)6]4-, [Cu(NH3)4]2+ and [Ag(NH3)2]+; van der Waals’ forces should be mentioned as a special type of bonding forces.
(d) Shapes of simple molecules: linear ((H2, O2, Cl2,HCl and CO2), non-linear (H2O) and tetrahedral; (CH4) and pyramidal (NH3).
(e) Nuclear Chemistry:
(i) Radioactivity – Types and properties of radiations
(ii) Nuclear reactions. Simple equations, uses and applications of natural and artificial radioactivity.

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5. Kinetic theory of matter and Gas Laws

Objectives:

Candidates should be able to:
(i) apply the theory to distinguish between solids, liquids and gases;
(ii) deduce reasons for change of state;
(iii) draw inferences based on molecular motion;
(iv) deduce gas laws from given expressions/ statements;
(v) interpret graphical representations related to these laws;
(vi) perform simple calculations based on these laws, equations and relationships

Topics:

(a) An outline of the kinetic theory of matter;
(i) melting,
(ii) vapourization
(iii) boiling
(iv) freezing
(v) condensation in terms of molecular motion and Brownian movement.
(b)(i) The laws of Boyle, Charles, Graham and Dalton (law of partial pressure); combined gas law, molar volume and atomicity of gases.
(ii) The ideal gas equation (PV = nRT).
(iii) The relationship between vapour density of gases and the relative molecular mass.

JAMB SYLLABUS FOR CHEMISTRY

6. Water

Objectives:

(i) identify the various uses of water;
(ii) identity the effects of dissolved atmospheric gases in water;
(iii) distinguish between the properties of hard and soft water;
(iv) determine the causes of hardness;
(v) identify methods of removal of hardness;
(vi) describe the processes involved in the treatment of water for town supply;
(vii) distinguish between these phenomena;
(viii) identify the various compounds that exhibit these phenomena.

Topics: 

(a) Water as a product of the combustion of hydrogen and its composition by volume.
(b) Water as a solvent, atmospheric gases dissolved in water and their biological significance.
(c) Hard and soft water: Temporary and permanent hardness and methods of softeninghard water.
(d) Treatment of water for town supply.
(e) Water of crystallization, efflorescence, deliquescence and hygroscopy. Examples of the substances exhibiting these properties and their uses.

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7. Solubility

Objectives:

Candidates should be able to:
(i) distinguish between the different types of solutions;
(ii) interpret solubility curves;
(iii) calculate the amount of solute that can dissolve in a given amount of solvent at a given temperature;
(iv) deduce that solubility is temperature-dependent;
(v) relate nature of solvents to their uses;
(vi) differentiate among true solution, suspension and colloids;
(vii) compare the properties of a true solution and a ‘false’ solution.
(viii) provide typical examples of suspensions and colloids.

Topics:

(a) Unsaturated, saturated and supersaturated solutions. Solubility curves and simple deductions from them, (solubility defined in terms of mole per dm3) and simple calculations.
(b) Solvents for fats, oil and paints and the use of such solvents for the removal of stains.
(c) False solution (Suspensions and colloids): Properties and examples. Harmattan haze and water paints as examples of suspensions and fog, milk, aerosol spray, emulsion paints and rubber solution as examples of colloids.

8. Environmental Pollution

Objectives:

Candidates should be able to:
(i) identify the different types of pollution and pollutants;
(ii) specify different sources of pollutants
(iii) classify pollutants as biodegradable and non-biodegradable;
(iv) specify the effects of pollution on the environment;
(v) identify measures for control of environmental pollution.

Topics: 

(a) Sources and effects of pollutants.
(b) Air pollution: Examples of air pollutants such as H2S, CO, SO2, oxides of nitrogen, chlorofluorocarbons and dust.
(c) Water pollution Sewage and oil pollution should be known.
(d) Soil pollution: Oil spillage, Biodegradable and non-biodegradable pollutants.

9. Acids, bases and salts

Objectives:

Candidates should be able to:
(i) distinguish between the properties of acids and bases;
(ii) identify the different types of acids and bases;
(iii) determine the basicity of acids;
(iv) differentiate between acidity and alkalinity using acid/base indicators;
(v) identify the various methods of preparation of salts;
(vi) classify different types of salts;
(vii) relate degree of dissociation to strength of acids and bases;
(viii) relate degree of dissociation to conductance;
(ix) perform simple calculations on pH and pOH;
(x) identify the appropriate acid-base indicator;
(xi) interpret graphical representation of titration curves;
(xii) perform simple calculations based on the mole concept;
(xiii) balance equations for the hydrolysis of salts;
(xiv) deduce the properties (acidic, basic, neutral) of the resultant solution.

Topics:

(a) General characteristics and properties of acids, bases and salts. Acids/base indicators, basicity of acids; normal, acidic, basic and double salts. An acid defined as a substance whose aqueous solution furnishes H3O+ions or as a proton donor. Ethanoic, citric and tartaric acids as examples of naturally occurring organic acids, alums as examples of double salts, preparation of salts by neutralization, precipitation and action of acids on metals. Oxides and trioxocarbonate (IV) salts
(b) Qualitative comparison of the conductances of molar solutions of strong and weak acids and bases, relationship between conductance and amount of ions present.
(c) pH and pOH scale; Simple calculations
(d) Acid/base titrations.
(e) Hydrolysis of salts: Principle Simple examples such as NH4Cl, AlCl3, Na2CO3 and CH3COONa

10. Oxidation and reduction

Objectives:

Candidates should be able to:
(i) identify the various forms of expressing oxidation and reduction;
(ii) classify chemical reactions in terms of oxidation or reduction;
(iii) balance redox reaction equations;
(iv) deduce the oxidation number of chemical species;
(v) compute the number of electron transfer in redox reactions;
(vi) identify the name of redox species in a reaction
(vii) distinguish between oxidizing and reducing agents in redox reactions.
(viii) apply oxidation number in naming inorganic compounds
(ix) relate reagents to their oxidizing and reducing abilities.

Topics: 

(a) Oxidation in terms of the addition of oxygen or removal of hydrogen.
(b) Reduction as removal of oxygen or addition of hydrogen.
(c) Oxidation and reduction in terms of electron transfer.
(d) Use of oxidation numbers. Oxidation and reduction treated as change in oxidation number and use of oxidation numbers in balancing simple equations.
(e) IUPAC nomenclature of inorganic compounds using oxidation number.
(f) Tests for oxidizing and reducing agents.

11. Electrolysis

Objectives:

Candidates should be able to:
(i) distinguish between electrolytes and non-electrolytes;
(ii) perform calculations based on faraday as a mole of electrons.
(iii) identify suitable electrodes for different electrolytes.
(iv) specify the chemical reactions at the electrodes;
(v) determine the products at the electrodes;
(vi) identify the factors that affect the products of electrolysis;
(vii) specify the different areas of application of electrolysis;
(viii) identify the various electrochemical cells;
(ix) calculate electrode potentials using half-cell reaction equations;
(x) determine the different areas of application of electrolytic processes;
(xi) identify methods used in protecting metals.

Topics:

(a) Electrolytes and non-electrolytes. Faraday’s laws of electrolysis.
(b) (i) Electrolysis of dilute H2SO4, aqueous CuSO4, CuC12 solution, dilute and concentrated NaC1 solutions and fused NaC1
(ii) Factors affecting discharge of ions at the electrodes.
(c) Uses of electrolysis: Purification of metals e.g. copper and production of elements and compounds (Al, Na, O2, Cl2 and NaOH).
(d) Electrochemical cells: Redox series (K, Ca, Na, Mg, Al, Zn, Fe, Sn, Pb, H, Cu, Hg, Ag, Au,) half-cell reactions and electrode potentials. (Simple calculations only).
(e) Corrosion as an electrolytic process, cathodic protection of metals, painting, electroplating and coating with grease or oil as ways of preventing iron from corrosion.

That’s all we have for Jamb syllabus for chemistry. Do well to follow up this to score high in your chemistry exam.

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