Chemistry JAMB Syllabus 2027/2028 Download PDF

The JAMB Chemistry syllabus 2027/2028 shows the main chemistry topics, concepts and scientific skills you should study for the examination.

The syllabus covers important areas such as separation of mixtures, chemical combination, gas laws, atomic structure, chemical bonding, air, water, solubility, environmental pollution, acids and bases, oxidation and reduction, electrolysis, energy changes, reaction rates, chemical equilibrium, metals, non-metals, organic chemistry and chemical industries.

In this guide, you will see the major topics in the syllabus and what you should be able to identify, explain, calculate, interpret, compare or apply. You will also find the JAMB Chemistry syllabus PDF download section, recommended texts, and simple guidance on how to use the syllabus during revision.

Chemistry requires both understanding and application, so pay attention to chemical equations, calculations, experimental principles, graphs, reactions, properties of substances and how chemistry connects with industry and everyday life.

Download JAMB Chemistry Syllabus 2027/2028 PDF

You can keep the JAMB Chemistry syllabus PDF on your phone or computer and use it as a checklist while studying.

The PDF covers major areas such as separation of mixtures, stoichiometry, gas laws, atomic structure, chemical bonding, acids and bases, electrolysis, energy changes, reaction rates, chemical equilibrium, metals, non-metals, organic compounds and chemical industries.

Download the JAMB Chemistry Syllabus 2027/2028 PDF here:

You can download, tap or click it to open the syllabus PDF and save a copy for your revision.

Use the PDF regularly to check the topics you have completed, the calculations and reactions you still need to practise, and the objectives you should be able to explain, interpret, calculate or apply.

JAMB Chemistry Syllabus Topics and Objectives

1. Separation of Mixtures and Purification of Chemical Substances

This section covers pure and impure substances, elements, compounds, mixtures, physical and chemical changes, and the different methods used to separate mixtures.

You should understand the properties of substances and know how the appropriate separation method can be chosen for a particular mixture.

Pure and Impure Substances

A pure substance contains only one substance with definite properties.

An impure substance contains other substances mixed with it.

You should be able to distinguish between pure and impure substances.

Boiling and Melting Points

Boiling and melting points can be used as criteria for checking the purity of chemical substances.

You should understand how these physical properties can help distinguish a pure substance from an impure one.

Elements, Compounds and Mixtures

You should understand the differences among:

• elements;
• compounds;
• mixtures.

An element consists of one type of atom.

A compound contains elements chemically combined in fixed proportions.

A mixture contains substances that are physically combined and can often be separated by physical methods.

You should be able to distinguish among these three forms of matter.

Physical and Chemical Changes

You should understand the difference between:

• physical changes;
• chemical changes.

A physical change affects the form or state of a substance without producing a new substance.

A chemical change produces one or more new substances.

You should be able to identify examples of both types of change.

Properties of Components of a Mixture

The components of a mixture may have different physical properties.

These differences make it possible to separate the components using suitable methods.

You should be able to identify the properties that make a particular separation method appropriate.

Evaporation

Evaporation can be used to separate a dissolved solid from a solution by removing the solvent.

You should understand the principle involved and recognize situations where evaporation can be applied.

Simple Distillation

Simple distillation is used when a liquid needs to be separated from a solution or from another liquid with a sufficiently different boiling point.

You should understand the role of boiling and condensation in this method.

Fractional Distillation

Fractional distillation is used to separate liquids with different boiling points.

You should understand how it differs from simple distillation.

Sublimation

Sublimation can be used when one component of a mixture changes directly from solid to gas on heating.

You should understand the principle behind this separation method.

Filtration

Filtration is used to separate an insoluble solid from a liquid.

You should be able to identify situations where filtration is suitable.

Crystallization

Crystallization is used to obtain a dissolved solid in the form of crystals.

You should understand the basic principle involved in forming crystals from a solution.

Simple and Fractional Crystallization

You should study:

• simple crystallization;
• fractional crystallization.

You should understand how differences in solubility can be used to separate substances.

Paper Chromatography

Paper chromatography can be used to separate components of a mixture based on how they move through paper with a suitable solvent.

You should understand the principle behind this method.

Column Chromatography

You should also study column chromatography as a separation method.

You should understand that different components of a mixture can move through the column at different rates.

Magnetization

Magnetization can be used when one component of a mixture is attracted to a magnet.

You should understand how magnetic properties can be used for separation.

Decantation

Decantation involves carefully pouring off a liquid from a settled solid or from another liquid layer.

You should understand when this method is appropriate.

Applying Separation Methods

You should be able to:

• identify the properties of the components of a mixture;
• choose a suitable separation method;
• explain the principle behind the method;
• apply separation principles to everyday situations.

The main separation methods you should know are evaporation, simple and fractional distillation, sublimation, filtration, crystallization, chromatography, magnetization and decantation.

2. Chemical Combination

This section covers stoichiometry, chemical laws, symbols, formulae, equations, relative atomic mass, the mole concept and Avogadro’s number.

You should understand how substances combine in chemical reactions and be able to use chemical equations and numerical relationships to solve simple problems.

Stoichiometry

Stoichiometry deals with the quantitative relationships between substances involved in chemical reactions.

You should be able to use chemical formulae and equations to determine the amounts of substances taking part in a reaction.

Law of Definite Proportions

The law of definite proportions states that a particular chemical compound contains its elements in a fixed proportion.

You should understand this law and be able to recognize it from given statements, expressions or data.

Law of Multiple Proportions

The law of multiple proportions applies when two elements combine to form more than one compound.

You should understand the relationship between the quantities of the elements involved and be able to identify the law from given data.

Law of Conservation of Matter

The law of conservation of matter states that matter is neither created nor destroyed during a chemical reaction.

You should understand how this law relates to balanced chemical equations.

Gay-Lussac’s Law of Combining Volumes

You should study Gay-Lussac’s law of combining volumes.

You should understand how the volumes of reacting gases are related when measured under the same conditions.

You should also be able to interpret statements, data or graphical representations connected with this law.

Avogadro’s Law

Avogadro’s law relates the volume of a gas to the number of particles present under the same conditions.

You should understand the law and be able to apply it in simple chemical calculations.

Chemical Symbols

Chemical symbols are used to represent elements.

You should be able to recognize and correctly use symbols when writing chemical formulae and equations.

Chemical Formulae

A chemical formula shows the types and proportions of atoms present in a substance.

You should be able to use chemical formulae in calculations involving chemical composition.

Chemical Equations

Chemical equations represent chemical reactions using symbols and formulae.

You should understand how equations are used to show:

• reactants;
• products;
• quantitative relationships between substances.

You should also be able to use balanced chemical equations in simple stoichiometric calculations.

Relative Atomic Mass

You should understand relative atomic mass based on the carbon-12 scale, where:

¹²C = 12

You should be able to use relative atomic masses when performing calculations involving chemical substances.

Mole Concept

The mole concept is an important part of quantitative Chemistry.

You should understand how the mole is used to relate the amount of a substance to the number of particles present.

You should be able to perform simple calculations involving:

• chemical formulae;
• chemical equations;
• chemical composition;
• moles.

Avogadro’s Number

You should understand the meaning of Avogadro’s number and its relationship with the mole concept.

Use it when required to relate the amount of a substance to the number of particles present.

Applying Chemical Combination

You should be able to:

• perform simple calculations involving formulae and equations;
• use the mole concept;
• interpret chemical composition;
• identify chemical laws from given data or statements;
• interpret graphs connected with the laws of chemical combination;
• determine the stoichiometry of chemical reactions.

3. Kinetic Theory of Matter and Gas Laws

This section covers the kinetic theory of matter, changes of state, molecular motion and the major gas laws.

Kinetic Theory of Matter

The kinetic theory explains the behaviour of matter in terms of the movement of particles.

Study the differences among:

• solids;
• liquids;
• gases.

Also understand how molecular motion explains changes of state such as:

• melting;
• vaporization;
• boiling;
• freezing;
• condensation.

Brownian Movement

Brownian movement refers to the random motion of particles.

It helps to show that particles of matter are constantly moving.

Relate Brownian movement and molecular motion to the behaviour of solids, liquids and gases.

Boyle’s Law

Boyle’s law describes the relationship between the pressure and volume of a gas when other conditions remain constant.

Focus on:

• the relationship between pressure and volume;
• graphical representation of the law;
• simple calculations.

Charles’ Law

Charles’ law describes the relationship between the volume and temperature of a gas under suitable constant conditions.

Study:

• the relationship between volume and temperature;
• graphs connected with the law;
• simple calculations.

Graham’s Law

Graham’s law deals with the movement of gases and their relative rates.

Understand the relationship involved and how it can be applied in simple problems.

Dalton’s Law of Partial Pressure

Dalton’s law of partial pressure explains the relationship between the individual pressures of gases in a mixture and the total pressure.

Know how to interpret and apply the law in simple situations.

Combined Gas Law

The combined gas law brings together relationships involving:

• pressure;
• volume;
• temperature.

Practise simple calculations using these quantities.

Molar Volume

Study the concept of molar volume of gases and its use in calculations involving gaseous substances.

Atomicity of Gases

Understand the meaning of atomicity and how it applies to gaseous elements.

Ideal Gas Equation

The ideal gas equation is:

PV = nRT

Know the meaning of each symbol and practise simple calculations based on the equation.

Vapour Density and Relative Molecular Mass

Study the relationship between:

• vapour density;
• relative molecular mass.

Use the relationship when solving simple numerical problems.

Gas-Law Graphs and Calculations

Pay attention to graphs, equations and numerical relationships connected with the gas laws.

Be comfortable with:

• identifying the correct gas law;
• interpreting graphs;
• substituting values into equations;
• calculating unknown quantities;
• relating gas behaviour to kinetic theory.

4. Atomic Structure and Bonding

This section covers atoms, molecules, ions, electron arrangement, isotopes, the periodic table, chemical bonding, molecular shapes and nuclear chemistry.

Atoms, Molecules and Ions

Study the differences among:

• atoms;
• molecules;
• ions.

Also know the contributions of scientists such as:

• Dalton;
• Millikan;
• Rutherford;
• Moseley;
• Thomson;
• Bohr.

Their work contributed to the development of ideas about atomic structure.

Atomic Structure

Important parts of atomic structure include:

• protons;
• neutrons;
• electrons;
• atomic number;
• mass number.

Know how to determine the numbers of protons, neutrons and electrons from atomic and mass numbers.

Electron Configuration

Study how electrons are arranged in atoms, especially for elements with atomic numbers 1 to 20.

Pay attention to the rules guiding electron arrangement and how electron configuration relates to chemical behaviour.

Isotopes

Isotopes are atoms of the same element that have the same atomic number but different mass numbers.

Study:

• common examples of isotopes;
• relationship between isotopy and mass number;
• simple calculations involving isotopes.

Atomic Orbitals

Study the shapes of:

• s orbitals;
• p orbitals.

Also understand the number of electrons that can occupy s and p orbitals.

Periodic Table

The periodic table arranges elements in a way that shows relationships among their properties.

Important families include:

• alkali metals;
• halogens;
• noble gases;
• transition metals.

Know how atomic number relates to the position of an element in the periodic table.

Periodic Properties

Study how the following properties vary across periods and down groups:

• ionization energy;
• ionic radius;
• electron affinity;
• electronegativity.

Focus on the reasons for these variations and how elements within the same group are related.

Chemical Bonding

Important types of chemical bonding include:

• electrovalent bonding;
• covalent bonding;
• hydrogen bonding;
• metallic bonding;
• coordinate bonding;
• van der Waals’ forces.

Electron configuration can help in predicting the type of bond an element is likely to form.

Also understand how the nature of bonding affects the properties of compounds.

Coordinate Bonding

Coordinate bonding is illustrated by complexes such as:

• [Fe(CN)₆]³⁻;
• [Fe(CN)₆]⁴⁻;
• [Cu(NH₃)₄]²⁺;
• [Ag(NH₃)₂]⁺.

Study how coordinate bonding differs from other forms of covalent bonding.

Shapes of Simple Molecules

Important molecular shapes include:

• linear: H₂, O₂, Cl₂, HCl and CO₂;
• non-linear: H₂O;
• tetrahedral: CH₄;
• pyramidal: NH₃.

Know how to distinguish among these shapes.

Nuclear Chemistry

Nuclear chemistry includes:

• radioactivity;
• nuclear reactions;
• natural radioactivity;
• artificial radioactivity.

Study the types and properties of nuclear radiation and the differences between ordinary chemical reactions and nuclear reactions.

Radioactivity

Focus on:

• types of radiation;
• properties of radiation;
• natural and artificial radioactivity;
• applications of radioactivity.

Also practise simple half-life calculations.

Nuclear Equations

Study simple nuclear equations and how to balance them correctly.

You should also understand the uses and applications of radioactive substances in different areas.

5. Air

This section covers the natural composition of air, air as a mixture, separation of its components, and the uses of some gases found in the atmosphere.

Composition of Air

The major natural gaseous constituents of air include:

• nitrogen;
• oxygen;
• water vapour;
• carbon(IV) oxide;
• noble gases, including argon and neon.

Study their relative presence in the atmosphere and the roles they play.

Air as a Mixture

Air is a mixture of gases rather than a single substance.

This is because its components:

• retain their individual properties;
• are not chemically combined in fixed proportions;
• can be separated by physical methods.

The composition of air may also vary slightly depending on environmental conditions.

Separation of Air Components

Study the principle involved in separating the different components of air.

Pay attention to how differences in physical properties make separation possible.

Uses of the Constituents of Air

Different gases in air have different uses.

Focus particularly on the uses of:

• nitrogen;
• oxygen;
• noble gases such as argon and neon.

Also understand why some atmospheric gases are important in everyday life and industrial activities.

Variation in the Composition of Air

The composition of air can vary from one environment to another.

Factors such as water vapour, carbon(IV) oxide, dust and other substances can affect the exact composition of the atmosphere in a particular place.

Study the reasons for these variations and how they affect the air around us.

6. Water

This section covers the composition and uses of water, dissolved gases, hard and soft water, water treatment, and special properties such as efflorescence, deliquescence and hygroscopy.

Composition of Water

Water can be formed by the combustion of hydrogen.

Study its composition by volume and the relationship between hydrogen and oxygen in water.

Water as a Solvent

Water dissolves many substances and is widely used as a solvent.

Also study the atmospheric gases that can dissolve in water and their biological importance.

Hard and Soft Water

Know the difference between:

• hard water;
• soft water.

Hardness may be:

• temporary;
• permanent.

Focus on the causes of each type and the methods used to remove hardness.

Softening Hard Water

Study the methods used to soften hard water and how they differ according to the type of hardness present.

Treatment of Water for Town Supply

Water meant for public use must be treated before distribution.

Study the main stages involved in making water suitable for town supply.

Water of Crystallization

Water of crystallization refers to water present as part of the crystal structure of certain compounds.

Know examples of substances that contain it and the importance of this property.

Efflorescence

Efflorescence occurs when a hydrated substance loses some or all of its water of crystallization when exposed to air.

Study examples of substances that show this behaviour.

Deliquescence

Deliquescence occurs when a substance absorbs moisture from the air until it dissolves in the absorbed water.

Know examples and uses of substances that exhibit this property.

Hygroscopy

Hygroscopy is the ability of a substance to absorb moisture from the atmosphere without necessarily dissolving in it.

Study the difference among:

• efflorescence;
• deliquescence;
• hygroscopy.

Also know examples of substances that exhibit each property and how these properties can be useful.

7. Solubility

This section covers types of solutions, solubility curves, the effect of temperature on solubility, suitable solvents, suspensions and colloids.

Unsaturated, Saturated and Supersaturated Solutions

Study the differences among:

• unsaturated solution;
• saturated solution;
• supersaturated solution.

An unsaturated solution can still dissolve more solute at a given temperature.

A saturated solution contains the maximum amount of solute that can dissolve under the same conditions.

A supersaturated solution contains more dissolved solute than would normally remain dissolved at that temperature.

Solubility

Solubility can be expressed in terms of moles per dm³.

Focus on simple calculations involving:

• amount of solute;
• amount of solvent;
• temperature;
• solubility values.

Solubility Curves

A solubility curve shows how the solubility of a substance changes with temperature.

Practise:

• reading values from solubility curves;
• comparing the solubility of substances;
• determining how much solute can dissolve at a given temperature;
• making simple deductions from graphs.

Effect of Temperature on Solubility

Solubility can change with temperature.

Study how temperature affects the amount of a substance that can dissolve and relate this to information shown on solubility curves.

Solvents for Fats, Oils and Paints

Different substances dissolve better in certain solvents.

Study suitable solvents for:

• fats;
• oils;
• paints.

Also understand how appropriate solvents can be used to remove stains.

True Solutions

A true solution is a homogeneous mixture in which the dissolved particles remain evenly distributed.

Know how true solutions differ from suspensions and colloids.

Suspensions

A suspension is a mixture containing particles that can remain dispersed for a time but may eventually settle.

Examples include:

• harmattan haze;
• water paints.

Study their main properties and how they differ from true solutions.

Colloids

A colloid contains particles dispersed throughout another substance.

Examples include:

• fog;
• milk;
• aerosol sprays;
• emulsion paints;
• rubber solution.

Focus on the properties of colloids and how they differ from both true solutions and suspensions.

Comparing Solutions, Suspensions and Colloids

Be familiar with the differences among:

• true solutions;
• suspensions;
• colloids.

Pay attention to their properties, examples and behaviour.

8. Environmental Pollution

This section covers the sources, types, effects and control of environmental pollution.

Types of Pollution

The main areas to study are:

• air pollution;
• water pollution;
• soil pollution.

Also understand the difference between:

• biodegradable pollutants;
• non-biodegradable pollutants.

Air Pollution

Examples of air pollutants include:

• hydrogen sulphide, H₂S;
• carbon monoxide, CO;
• sulphur(IV) oxide, SO₂;
• oxides of nitrogen;
• chlorofluorocarbons;
• dust.

Study the sources of these pollutants and their effects on the environment.

Water Pollution

Important examples include:

• sewage pollution;
• oil pollution.

Focus on how these pollutants enter water sources and the problems they can cause.

Soil Pollution

Examples include:

• oil spillage;
• biodegradable pollutants;
• non-biodegradable pollutants.

Know how soil pollution can affect the environment.

Sources and Effects of Pollutants

Pollutants may come from different human or natural activities.

Focus on:

• identifying common sources;
• classifying pollutants;
• explaining their effects on air, water and soil.

Control of Environmental Pollution

Study the measures used to reduce or control environmental pollution.

The main idea is to understand how harmful substances can be prevented from entering the environment or reduced before they cause serious damage.

9. Acids, Bases and Salts

This section covers the properties of acids, bases and salts, indicators, salt preparation, pH and pOH, titration, conductance and hydrolysis of salts.

Acids and Bases

Study the general characteristics and properties of:

• acids;
• bases;
• salts.

An acid can be described as a substance whose aqueous solution produces H₃O⁺ ions or as a proton donor.

Examples of naturally occurring organic acids include:

• ethanoic acid;
• citric acid;
• tartaric acid.

Acid-Base Indicators

Indicators help to show whether a solution is acidic or alkaline.

Focus on:

• identifying suitable indicators;
• using indicators to distinguish acidity from alkalinity;
• interpreting colour changes where required.

Basicity of Acids

Study the basicity of acids and how acids can differ according to the number of ionizable hydrogen ions they can supply.

Types of Salts

Important types include:

• normal salts;
• acidic salts;
• basic salts;
• double salts.

Alums are examples of double salts.

Know how to classify salts correctly.

Preparation of Salts

Study the main methods of preparing salts, including:

• neutralization;
• precipitation;
• action of acids on metals.

Also understand reactions involving oxides and trioxocarbonate(IV) salts.

Strong and Weak Acids and Bases

Compare strong and weak acids and bases in terms of their degree of dissociation.

Also study the relationship between:

• degree of dissociation;
• number of ions present;
• electrical conductance.

pH and pOH

Study the pH and pOH scales and practise simple calculations involving both.

Know how pH values relate to acidic, neutral and basic solutions.

Acid-Base Titration

Acid-base titration involves using measured volumes of acid and base to determine quantities in a reaction.

Focus on:

• choosing a suitable indicator;
• interpreting titration curves;
• applying the mole concept;
• carrying out simple calculations.

Hydrolysis of Salts

Study the principle of salt hydrolysis using examples such as:

• NH₄Cl;
• AlCl₃;
• Na₂CO₃;
• CH₃COONa.

Know how hydrolysis can produce solutions that are:

• acidic;
• basic;
• neutral.

Also practise balancing simple equations connected with salt hydrolysis.

10. Oxidation and Reduction

This section covers the different meanings of oxidation and reduction, electron transfer, oxidation numbers, redox equations, and oxidizing and reducing agents.

Meaning of Oxidation

Oxidation can be described as:

• addition of oxygen;
• removal of hydrogen;
• loss of electrons;
• increase in oxidation number.

Study how these different definitions describe the same type of chemical change.

Meaning of Reduction

Reduction can be described as:

• removal of oxygen;
• addition of hydrogen;
• gain of electrons;
• decrease in oxidation number.

Oxidation and reduction usually occur together in a redox reaction.

Electron Transfer

In terms of electrons:

• oxidation involves loss of electrons;
• reduction involves gain of electrons.

Focus on identifying which substance loses electrons and which one gains them in a reaction.

Oxidation Numbers

An oxidation number shows the apparent charge assigned to an atom in a compound or ion.

Study how to:

• determine oxidation numbers;
• identify changes in oxidation number;
• recognize oxidation and reduction from those changes.

Balancing Redox Equations

Oxidation numbers can be used to balance simple redox equations.

Pay attention to changes in oxidation number and the number of electrons transferred during the reaction.

Oxidizing Agents

An oxidizing agent causes another substance to be oxidized.

Study how to identify oxidizing agents from chemical reactions and relate common reagents to their oxidizing ability.

Reducing Agents

A reducing agent causes another substance to be reduced.

Know how to distinguish reducing agents from oxidizing agents in redox reactions.

IUPAC Naming Using Oxidation Numbers

Oxidation numbers are also used in the IUPAC nomenclature of inorganic compounds.

Practise identifying the oxidation state of an element and using it correctly when naming simple inorganic compounds.

Tests for Oxidizing and Reducing Agents

Study the chemical tests used to identify:

• oxidizing agents;
• reducing agents.

Focus on how different reagents behave during oxidation-reduction reactions and how their reactions can be used for identification.

11. Electrolysis

This section covers electrolytes, Faraday’s laws, electrolysis of selected substances, electrode reactions, electrochemical cells and corrosion.

Electrolytes and Non-Electrolytes

Study the difference between:

• electrolytes;
• non-electrolytes.

Electrolytes conduct electricity through the movement of ions, while non-electrolytes do not conduct in this way.

Faraday’s Laws of Electrolysis

Faraday’s laws describe the quantitative relationship between electricity passed through an electrolyte and the substances produced at the electrodes.

Focus on simple calculations involving Faraday as a mole of electrons.

Electrolysis of Selected Substances

Study the electrolysis of:

• dilute H₂SO₄;
• aqueous CuSO₄;
• CuCl₂ solution;
• dilute NaCl solution;
• concentrated NaCl solution;
• fused NaCl.

For each case, know the ions present, suitable electrodes, reactions at the electrodes and products formed.

Discharge of Ions

Different ions may compete for discharge during electrolysis.

Study the factors that determine which ions are discharged at:

• the anode;
• the cathode.

Also relate these factors to the products obtained during electrolysis.

Uses of Electrolysis

Important applications include:

• purification of metals such as copper;
• production of aluminium;
• production of sodium;
• production of oxygen;
• production of chlorine;
• production of sodium hydroxide.

Understand how electrolytic processes are used in these areas.

Electrochemical Cells

Study electrochemical cells using the redox series:

K, Ca, Na, Mg, Al, Zn, Fe, Sn, Pb, H, Cu, Hg, Ag, Au

Important areas include:

• half-cell reactions;
• electrode potentials;
• simple calculations involving electrode potentials.

Corrosion

Corrosion can be treated as an electrolytic process.

Study methods used to protect metals from corrosion, including:

• cathodic protection;
• painting;
• electroplating;
• coating with grease;
• coating with oil.

Know how these methods help to reduce or prevent corrosion of iron and other metals.

12. Energy Changes

This section covers enthalpy changes, endothermic and exothermic reactions, entropy, spontaneity and Gibbs free energy.

Enthalpy Change

Energy changes that accompany physical or chemical processes are represented by ΔH.

Examples include:

• dissolution of substances in water;
• reactions involving substances such as Na, NaOH, K and NH₄Cl.

Study how heat may be absorbed or released during these changes.

Endothermic Reactions

An endothermic reaction absorbs heat from the surroundings.

It is represented by:

+ΔH

Know how to identify endothermic reactions from descriptions and energy-change graphs.

Exothermic Reactions

An exothermic reaction releases heat to the surroundings.

It is represented by:

−ΔH

Be familiar with the difference between endothermic and exothermic reactions and how both appear on energy diagrams.

Energy Change Graphs

Study graphical representations of heat changes.

Focus on identifying:

• reactants;
• products;
• energy levels;
• whether the reaction is endothermic or exothermic.

Entropy

Entropy is treated as a measure of order and disorder.

Simple examples include:

• mixing gases;
• dissolving salts.

Relate the physical state of a substance to its degree of orderliness.

Spontaneity of Reactions

The spontaneity of a chemical reaction can be considered using Gibbs free energy, ΔG.

The relationship is:

ΔG° = ΔH° − TΔS°

Study the following conditions:

• ΔG° < 0: spontaneous reaction;
• ΔG° > 0: non-spontaneous reaction;
• ΔG° = 0: equilibrium.

Gibbs Free Energy Calculations

Practise simple problems involving:

• ΔG°;
• ΔH°;
• ΔS°;
• temperature.

Also understand how enthalpy, entropy and Gibbs free energy are related to the driving force of a chemical reaction.

13. Rates of Chemical Reaction

This section covers the factors that affect reaction rate, reaction-rate curves, activation energy, Arrhenius’ law and collision theory.

Factors Affecting Reaction Rate

The main factors to study are:

• temperature;
• concentration;
• pressure;
• surface area;
• catalysts.

Know how each factor can increase or decrease the rate of a chemical reaction.

Effect of Temperature

Increasing temperature can change how quickly particles react.

Examples include reactions between:

• HCl and Na₂S₂O₃;
• Mg and HCl.

Relate temperature changes to particle motion and collision frequency.

Effect of Concentration

The concentration of reactants can affect reaction rate.

Examples include:

• HCl and Na₂S₂O₃;
• HCl and marble;
• iodine clock reaction.

For gaseous systems, pressure may be treated as a concentration factor.

Effect of Pressure

Changes in pressure can affect the rate of reactions involving gases.

Understand how pressure changes the frequency of collisions between gas particles.

Effect of Surface Area

Surface area affects how much of a solid reactant is exposed for reaction.

A common example is the reaction between marble and HCl using:

• powdered marble;
• marble lumps of the same mass.

Compare how the different surface areas affect reaction rate.

Effect of Catalysts

A catalyst changes the rate of a reaction without being permanently used up.

Examples include the decomposition of:

• H₂O₂;
• KClO₃;

in the presence or absence of MnO₂.

Study the types of catalysts suitable for different reactions and their effects.

Reaction-Rate Curves

Reaction-rate curves show how the progress of a reaction changes with time.

Practise interpreting these curves and using them to compare reaction rates.

Activation Energy

Activation energy is the minimum energy required for a reaction to occur.

Understand its importance and how it relates to the rate of a chemical reaction.

Also know how activation energy can be obtained from reaction-rate diagrams where required.

Arrhenius’ Law

Study the basic idea of Arrhenius’ law and its relationship with temperature and reaction rate.

A qualitative understanding is enough.

Collision Theory

The collision theory explains reactions in terms of particles colliding with one another.

Relate reaction rate to:

• frequency of collisions;
• energy of collisions;
• activation energy.

Effect of Light

Some reactions are affected by light.

An example is the halogenation of alkanes.

Understand that light can provide energy needed for certain reactions to proceed.

Simple Reaction-Rate Calculations

Practise simple problems involving reaction rate and be able to connect numerical results with the factors that affect how fast reactions occur.

14. Chemical Equilibria

This section covers reversible reactions, dynamic equilibrium, factors that affect equilibrium position, Le Chatelier’s principle and equilibrium constant.

Reversible Reactions

A reversible reaction can proceed in both the forward and backward directions.

Study examples such as:

• action of steam on iron;
• N₂O₄ ⇌ 2NO₂.

Dynamic Equilibrium

Dynamic equilibrium occurs when the forward and backward reactions continue at the same rate.

At this point, there is no overall change in the amounts of reactants and products.

Factors Affecting Equilibrium Position

The position of equilibrium can be affected by changes in conditions.

Focus on factors such as:

• concentration;
• pressure;
• temperature.

Understand how changing each factor can shift the equilibrium position.

Le Chatelier’s Principle

Le Chatelier’s principle explains how a system at equilibrium responds when its conditions are changed.

Use it to predict the effect of changes in:

• concentration;
• pressure;
• temperature.

Equilibrium Constant

Study the meaning of the equilibrium constant and how it relates to the equilibrium position of a reversible reaction.

For this topic, focus on understanding the concept and the effect of changing conditions rather than numerical calculations.

Predicting Equilibrium Changes

Practise using the ideas in this section to predict whether a change will favour:

• the forward reaction;
• the backward reaction;
• little or no shift in equilibrium.

Also understand how the factors affecting equilibrium relate to the equilibrium constant.

15. Non-Metals and Their Compounds

This section covers hydrogen, halogens, oxygen, sulphur, nitrogen, carbon and their important compounds.

Focus on their preparation, properties, uses and common laboratory tests.

Hydrogen

Study:

• commercial production from water gas and cracking of petroleum fractions;
• laboratory preparation;
• properties;
• uses;
• test for hydrogen.

Also know the reagents used for its preparation and how its properties relate to its uses.

Halogens

Use chlorine as the main example of the halogens.

Study:

• laboratory preparation;
• industrial preparation by electrolysis;
• properties;
• uses.

Important uses of chlorine include:

• water sterilization;
• bleaching;
• manufacture of hydrochloric acid;
• manufacture of plastics;
• manufacture of insecticides.

Hydrogen Chloride and Hydrochloric Acid

Study:

• preparation of hydrogen chloride;
• properties of HCl gas;
• properties of hydrochloric acid;
• chlorides;
• test for chloride ions.

Pay attention to the differences between HCl(g) and HCl(aq).

Oxygen

Study the:

• laboratory preparation of oxygen;
• commercial production from liquid air;
• properties;
• uses.

Also cover the different classes of oxides:

• acidic oxides;
• basic oxides;
• amphoteric oxides;
• neutral oxides.

Ozone

Ozone is an allotrope of oxygen.

Study its importance in the atmosphere and how it differs from ordinary oxygen.

Sulphur

Study the:

• allotropes of sulphur;
• uses of sulphur.

Preparation of the allotropes is not required.

Sulphur(IV) Oxide

Study:

• preparation;
• properties;
• uses;
• reaction with alkalis.

Also cover trioxosulphate(IV) acid and its salts and the effect of acids on trioxosulphate(IV) salts.

Tetraoxosulphate(VI) Acid

Study the commercial preparation of H₂SO₄ by the Contact Process.

Also cover its properties as:

• a dilute acid;
• an oxidizing agent;
• a dehydrating agent.

Know its uses and the test for SO₄²⁻ ions.

Hydrogen Sulphide

Study the preparation and properties of H₂S as:

• a weak acid;
• a reducing agent;
• a precipitating agent.

Also know the test for S²⁻ ions.

Nitrogen

Study:

• laboratory preparation of nitrogen;
• production from liquid air.

Also understand the nitrogen cycle and its importance to the environment.

Ammonia

Study:

• laboratory preparation;
• industrial preparation using the Haber Process;
• properties;
• uses;
• ammonium salts and their uses.

Also cover the oxidation of ammonia to nitrogen(IV) oxide and trioxonitrate(V) acid.

Know the test for NH₄⁺ ions.

Trioxonitrate(V) Acid

Study:

• laboratory preparation from ammonia;
• properties;
• uses;
• trioxonitrate(V) salts;
• effect of heat on the salts.

Also know the test for NO₃⁻ ions.

Oxides of Nitrogen

Study the properties of:

• N₂O;
• NO;
• NO₂.

Carbon

Study the allotropes of carbon, their properties and uses.

Carbon(IV) Oxide

Study:

• laboratory preparation;
• properties;
• uses;
• action of heat on trioxocarbonate(IV) salts.

Also know the test for CO₃²⁻ ions.

Carbon(II) Oxide

Study:

• laboratory preparation;
• properties;
• effects on blood;
• common sources.

Sources include:

• charcoal fires;
• exhaust fumes.

Pay particular attention to the harmful effects of carbon monoxide on humans.

Coal

Study the different types of coal and the products obtained from the destructive distillation of wood and coal.

Know the uses of these products.

Coke and Synthetic Gas

Study:

• gasification of coke;
• uses of coke;
• manufacture of synthetic gas;
• uses of synthetic gas.

Also be familiar with common qualitative tests for ions such as Cl⁻, SO₄²⁻, SO₃²⁻, S²⁻, NH₄⁺, NO₃⁻, CO₃²⁻ and HCO₃⁻.

16. Metals and Their Compounds

This section covers the general properties of metals, methods of extraction, important metallic compounds, transition metals, iron, copper and alloys.

General Properties of Metals

Study the common properties of metals and how these properties relate to their uses.

Also focus on:

• chemical reactivity;
• suitable methods of extraction;
• tests for metallic ions.

Extraction of Metals

Different metals require different extraction methods.

Understand how the extraction method depends on the properties and reactivity of the metal.

Also compare the reactivities of different metals.

Alkali Metals

Use sodium as an important example.

Study:

• sodium hydroxide;
• sodium trioxocarbonate(IV);
• sodium hydrogen trioxocarbonate(IV);
• sodium chloride.

Sodium Hydroxide

Study its production by electrolysis of brine.

Also cover:

• reactions with aluminium, zinc and lead ions;
• uses, including precipitation of metallic hydroxides.

Sodium Trioxocarbonate(IV)

Study its production by the Solvay process, together with its properties and uses.

One important use is in the manufacture of glass.

Sodium Hydrogen Trioxocarbonate(IV)

Study its preparation, properties and uses alongside sodium trioxocarbonate(IV).

Sodium Chloride

Study:

• occurrence in seawater;
• uses;
• economic importance of seawater;
• recovery of sodium chloride.

Alkaline-Earth Metals

Use calcium as the main example.

Important compounds include:

• calcium oxide;
• calcium hydroxide;
• calcium trioxocarbonate(IV).

Study their properties and uses.

Also cover:

• preparation of calcium oxide from seashells;
• chemical composition of cement;
• setting of mortar;
• test for Ca²⁺ ions.

Aluminium

Study:

• purification of bauxite;
• electrolytic extraction of aluminium;
• properties;
• uses;
• compounds of aluminium;
• test for Al³⁺ ions.

Tin

Study:

• ores of tin;
• extraction;
• properties;
• uses.

Relate the extraction method to the properties of the metal.

First Transition Series

Important characteristic properties include:

• electron configuration;
• variable oxidation states;
• complex-ion formation;
• formation of coloured ions;
• catalytic behaviour.

Also practise simple IUPAC naming of transition-metal complexes.

Iron

Study:

• extraction from sulphide and oxide ores;
• properties;
• uses;
• different forms of iron;
• properties of the different forms;
• advantages of steel over iron.

Know the tests for:

• Fe²⁺;
• Fe³⁺.

Copper

Study:

• extraction from sulphide and oxide ores;
• properties;
• uses;
• preparation of copper(II) tetraoxosulphate(VI);
• uses of copper(II) tetraoxosulphate(VI);
• test for Cu²⁺ ions.

Alloys

Study the constituents and uses of:

• steel;
• stainless steel;
• brass;
• bronze;
• type metal;
• duralumin;
• soft solder;
• permalloy;
• alnico.

Also understand how the properties and uses of alloys can differ from those of pure metals.

17. Organic Compounds

This section covers the basic principles of organic chemistry, hydrocarbons, petroleum, alkanols, carbonyl compounds, alkanoic acids, alkanoates, amines, carbohydrates, proteins and polymers.

Introduction to Organic Chemistry

Start with the tetravalency of carbon and its ability to form chains of compounds, known as catenation.

Also study:

• general formulae;
• IUPAC nomenclature;
• empirical formulae;
• molecular formulae;
• functional groups;
• isomerism.

Know how the structure and functional group of an organic compound relate to its properties.

Alkanes

Study alkanes as a homologous series, including:

• physical properties;
• substitution reactions;
• uses of halogenated products;
• structural isomerism.

Examples of isomerism should not go beyond compounds containing six carbon atoms.

Petroleum

Crude petroleum is a complex mixture of hydrocarbons.

Study:

• composition of petroleum;
• fractional distillation;
• major fractions and their uses;
• cracking;
• reforming;
• petrochemicals;
• octane number.

Understand how cracking and reforming improve or change petroleum fractions.

Alkenes

Study:

• structural isomerism;
• geometric isomerism;
• addition reactions;
• polymerization.

Important products of polymerization include:

• polythene;
• synthetic rubber.

Also study the role of synthetic rubber in vulcanization.

Alkynes

Use ethyne as the main example.

Study:

• preparation from the reaction of water with carbides;
• properties;
• simple reactions;
• chemical test for terminal alkynes.

Aromatic Hydrocarbons

Use benzene as the main example.

Focus on:

• structure;
• properties;
• uses.

Also understand the difference between aromatic and aliphatic hydrocarbons.

Alkanols

Study:

• primary alkanols;
• secondary alkanols;
• tertiary alkanols.

For ethanol, cover production by:

• fermentation;
• petroleum by-products.

Local examples of fermentation and distillation may include alcohol produced from palm wine and other local sources.

Also study glycerol as a polyhydric alkanol.

Reactions of Alkanols

Focus on reactions involving the OH group.

Oxidation can be used to distinguish among primary, secondary and tertiary alkanols.

Also study the Lucas test.

Alkanals and Alkanones

Study the properties of:

• alkanals;
• alkanones.

Know the chemical tests used to distinguish between them.

Alkanoic Acids

Study:

• chemical reactions;
• neutralization;
• esterification.

Examples include:

• ethanedioic acid as a dicarboxylic acid;
• benzene carboxylic acid as an aromatic acid.

Alkanoates

Alkanoates can be formed from alkanoic acids and alkanols.

Study:

• fats and oils as alkanoates;
• natural sources of alkanoates;
• saponification;
• production of soap;
• production of margarine;
• differences between soaps and detergents.

Amines

Study the three main classes of alkanamines:

• primary;
• secondary;
• tertiary.

Know how the classes differ.

Carbohydrates

Study the classification of carbohydrates into:

• monosaccharides;
• disaccharides;
• polysaccharides.

Also cover:

• composition;
• chemical tests for simple sugars;
• hydrolysis of complex sugars;
• cellulose from cotton;
• starch from cassava.

Carbohydrates are used in areas such as:

• alcoholic beverage production;
• pharmaceuticals;
• textiles.

Proteins

Study:

• primary structure;
• hydrolysis;
• tests for proteins;
• enzymes and their functions.

Important protein tests include:

• Ninhydrin test;
• Biuret test;
• Millon’s test;
• Xanthoproteic test.

Polymers

Study both:

• natural polymers;
• synthetic polymers.

Important areas include:

• natural rubber;
• synthetic rubber;
• addition polymerization;
• condensation polymerization;
• methods of preparation;
• examples;
• uses.

Also distinguish between:

• thermoplastics;
• thermosetting plastics.

18. Chemistry and Industry

This section covers chemical industries, their raw materials, the products they produce, their importance and the relationship between industrial chemistry and biotechnology.

Chemical Industries

Chemical industries can be classified according to the products they manufacture.

Study the different types of chemical industries and the materials they use in production.

Raw Materials

Every chemical industry depends on suitable raw materials.

Focus on identifying the raw materials used by different industries and relating them to the products obtained.

Fine Chemicals

Fine chemicals are chemical products produced for specific uses.

Know how they differ from heavy chemicals and be able to identify industries associated with them.

Heavy Chemicals

Heavy chemicals are produced on a larger industrial scale.

Study the difference between:

• fine chemicals;
• heavy chemicals.

Also relate each type to its industrial applications.

Importance of Chemical Industries

Chemical industries contribute to different areas of economic and everyday activity.

Focus on the relevance of these industries and the products they provide.

Industrial Processes

Study how raw materials are converted into useful chemical products through industrial processes.

Relate these processes to the Chemistry principles covered in other parts of the syllabus.

Biotechnology

Biotechnology involves the use of biological systems or organisms in useful production processes.

Study how biotechnology is connected with industrial processes and chemical production.

How to Use the JAMB Chemistry Syllabus for Revision

The JAMB Chemistry syllabus can help you organize your revision by showing the topics to cover and the skills expected under each one.

Read also: JAMB Area of Concentration for Chemistry Subject 2027/2028

Chemistry combines theory, calculations, equations, graphs and experimental ideas, so your revision should cover all of these areas.

Start with the basic topics such as:

• separation of mixtures;
• chemical combination;
• kinetic theory;
• gas laws;
• atomic structure;
• chemical bonding.

Make sure you understand the main concepts before moving to more advanced areas.

For calculation-based topics, practise regularly. Important areas include:

• mole concept;
• stoichiometry;
• gas laws;
• isotopes;
• solubility;
• pH and pOH;
• titration;
• electrolysis;
• electrode potentials;
• energy changes;
• rates of reaction.

Do not only memorize formulas. Learn what each quantity means and when a particular equation should be used.

For topics involving chemical reactions, practise writing and balancing equations. Pay attention to:

• oxidation and reduction;
• electrolysis;
• acids, bases and salts;
• non-metals and their compounds;
• metals and their compounds;
• organic reactions.

Also learn the common laboratory tests for gases and ions where they appear in the syllabus.

For graphs and data interpretation, revise:

• gas-law graphs;
• solubility curves;
• titration curves;
• energy-change diagrams;
• reaction-rate curves.

Practise reading values from graphs and making deductions from the information presented.

When studying Organic Chemistry, group compounds according to their functional groups. Revise their:

• general formulae;
• nomenclature;
• properties;
• reactions;
• preparation;
• uses;
• distinguishing tests.

Give special attention to hydrocarbons, alkanols, alkanals, alkanones, alkanoic acids, alkanoates, carbohydrates, proteins and polymers.

For Inorganic Chemistry, connect each element or compound with its:

• preparation;
• properties;
• uses;
• reactions;
• laboratory tests.

Use the objectives under each syllabus topic as a checklist. After studying a topic, check whether you can explain the concept, perform the required calculation, interpret the graph, identify the reaction or apply the chemical principle.

Where possible, combine textbook reading with worked examples and past questions. This will help you identify areas where you understand the theory but still need more practice with calculations or applications.

You can also use the recommended Chemistry textbooks when you need clearer explanations, worked examples or additional practice.

Recommended Texts for JAMB Chemistry

The following textbooks can support your JAMB Chemistry revision:

1. Ababio, O. Y. (2009), New School Chemistry for Senior Secondary Schools, Fourth Edition. Onitsha: Africana FIRST Publishers Limited.
2. Bajah, S. T., Teibo, B. O., Onwu, G. and Obikwere, A., Senior Secondary Chemistry. Book 1 (1999), Books 2 and 3 (2000). Lagos: Longman.

Read also: Full List of JAMB Recommended Textbooks for Chemistry 2027/2028

These books can help with areas such as stoichiometry, gas laws, atomic structure, chemical bonding, acids and bases, electrolysis, energy changes, organic chemistry, metals, non-metals and chemical calculations.

Use them when you need clearer explanations, worked examples or additional practice on difficult Chemistry topics.

Key Points to Remember

• Chemistry covers both theory and calculations, so revise concepts, equations, graphs and numerical problems together.
• Important separation methods include filtration, evaporation, crystallization, sublimation, distillation, chromatography, magnetization and decantation.
• In chemical combination, focus on stoichiometry, the mole concept, Avogadro’s number, chemical equations and the major laws of chemical combination.
• For gas laws, understand Boyle’s law, Charles’ law, Graham’s law, Dalton’s law, the combined gas law and the ideal gas equation PV = nRT.
• Atomic structure includes protons, neutrons, electrons, isotopes, electron configuration, orbitals and periodicity.
• Important types of bonding include electrovalent, covalent, coordinate, hydrogen and metallic bonding.
• Nuclear chemistry includes radioactivity, nuclear reactions, half-life calculations and applications of radioactive substances.
• Revise the composition and properties of air and water, including hardness of water, water treatment, efflorescence, deliquescence and hygroscopy.
• In solubility, understand saturated, unsaturated and supersaturated solutions, solubility curves, suspensions and colloids.
• Environmental pollution covers air, water and soil pollution, their sources, effects and control.
• For acids, bases and salts, revise indicators, salt preparation, pH, pOH, titration, conductance and hydrolysis.
• In oxidation and reduction, know electron transfer, oxidation numbers, redox equations, oxidizing agents and reducing agents.
• Electrolysis includes electrolytes, Faraday’s laws, electrode reactions, ion discharge, electrochemical cells and corrosion prevention.
• Energy changes cover enthalpy, entropy, endothermic and exothermic reactions, Gibbs free energy and spontaneity.
• Reaction rate is affected by temperature, concentration, pressure, surface area and catalysts.
• For chemical equilibrium, understand reversible reactions, dynamic equilibrium and Le Chatelier’s principle.
• The non-metals section covers hydrogen, chlorine, oxygen, sulphur, nitrogen and carbon, together with their important compounds, preparations, properties, uses and tests.
• The metals section covers sodium, calcium, aluminium, tin, transition metals, iron, copper and alloys.
• Organic Chemistry includes alkanes, alkenes, alkynes, benzene, alkanols, alkanals, alkanones, alkanoic acids, alkanoates, amines, carbohydrates, proteins and polymers.
• For organic compounds, pay attention to functional groups, IUPAC nomenclature, isomerism, reactions, preparation and distinguishing tests.
• Chemistry and industry includes chemical industries, raw materials, fine and heavy chemicals, industrial processes and biotechnology.
• Practise the calculations required in topics such as stoichiometry, gas laws, solubility, pH and pOH, titration, electrolysis, electrode potentials, energy changes and reaction rates.
• Do not depend only on memorizing definitions. Be ready to interpret data, balance equations, identify reactions, read graphs and apply chemical principles to practical situations.

Frequently Asked Questions

Conclusion

The JAMB Chemistry syllabus 2027/2028 gives you a clear guide to the main topics, calculations and practical ideas you should study for the examination.

It covers areas such as separation of mixtures, stoichiometry, gas laws, atomic structure, chemical bonding, acids and bases, electrolysis, energy changes, reaction rates, chemical equilibrium, metals, non-metals, organic chemistry and chemical industries.

Use the syllabus to organize your revision and make sure you understand both the theory and the calculations. Give enough attention to chemical equations, graphs, laboratory principles, reactions, properties of substances and the relationships between different Chemistry concepts.

You can also return to the JAMB Chemistry syllabus PDF whenever you need to check the topics and objectives you have already covered.

If you have any questions about the JAMB Chemistry syllabus, leave a comment. You can also share this guide with other students who may find it useful.