JAMB Area of Concentration for Chemistry Subject 2027/2028

The JAMB Area of Concentration for Chemistry Subject 2027/2028 covers the major concepts, calculations and practical areas you need to study for the examination.

Chemistry deals with the composition, properties and changes of substances. You should understand important principles, interpret chemical data, solve simple calculations and apply chemical knowledge to everyday life and industry.

The major areas include separation techniques, stoichiometry, gas laws, atomic structure, bonding, acids and bases, electrolysis, reaction rates, equilibrium, metals, non-metals and organic chemistry.

As you revise the JAMB Chemistry topics, focus on understanding chemical relationships rather than memorizing facts alone. Pay attention to equations, calculations, laboratory tests, graphs and the practical uses of important substances.

Read also: Chemistry JAMB Syllabus 2026/2027 Download PDF

Separation of Mixtures and Purification of Chemical Substances

This area deals with how substances are identified, separated and purified.

Pure and Impure Substances

A pure substance contains only one type of substance, while an impure substance contains other materials mixed with it.

Melting point and boiling point can be used to test purity. A pure substance usually has a definite melting or boiling point.

Elements, Compounds and Mixtures

You should understand the differences between:

• elements;
• compounds;
• mixtures.

An element contains one type of atom. A compound contains elements chemically combined in fixed proportions, while a mixture contains substances that are physically combined.

Physical and Chemical Changes

A physical change does not produce a new substance.

A chemical change produces one or more new substances with different properties.

You should be able to distinguish between the two.

Separation Methods

Different mixtures require different separation techniques.

Important methods include:

• evaporation;
• simple distillation;
• fractional distillation;
• sublimation;
• filtration;
• crystallization;
• fractional crystallization;
• paper chromatography;
• column chromatography;
• magnetization;
• decantation.

Choosing the Correct Separation Method

The correct method depends on the properties of the substances in the mixture.

For example, separation may depend on differences in:

• boiling point;
• solubility;
• particle size;
• magnetic properties;
• ability to sublime.

You should understand the principle behind each method rather than memorizing the names alone.

Everyday Applications

Separation processes are also used outside the laboratory.

You should be able to connect the basic principles of separation with practical situations involving purification and recovery of useful substances.

Chemical Combination and Stoichiometry

Chemical combination explains how substances react in fixed relationships, while stoichiometry deals with the quantitative calculations involved in chemical reactions.

Laws of Chemical Combination

You should understand the main laws that describe how substances combine.

These include:

• law of definite proportions;
• law of multiple proportions;
• law of conservation of matter;
• Gay-Lussac’s law of combining volumes;
• Avogadro’s law.

You should be able to recognize these laws from statements, equations, data and simple graphs.

Chemical Symbols, Formulae and Equations

Chemical symbols represent elements, while chemical formulae show the composition of substances.

Chemical equations represent reactions.

You should be able to:

• write and interpret simple formulae;
• balance chemical equations;
• use equations to determine reacting quantities.

Relative Atomic Mass

Relative atomic mass is based on the carbon-12 standard.

You should understand how atomic and molecular masses are used in chemical calculations.

Mole Concept

The mole is an important unit for measuring the amount of substance.

You should understand:

• the mole concept;
• Avogadro’s number;
• molar relationships;
• chemical composition.

Stoichiometric Calculations

You should practise simple calculations involving:

• chemical formulae;
• balanced equations;
• relative masses;
• moles;
• reacting quantities.

Always begin with a correctly balanced equation before calculating the amount of a reactant or product.

Interpreting Chemical Relationships

Stoichiometry is not only about calculation.

You should also be able to use given data, equations and graphs to determine the relationship between substances taking part in a chemical reaction.

Kinetic Theory of Matter and Gas Laws

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

States of Matter

You should understand the differences between:

• solids;
• liquids;
• gases.

These differences are explained by the arrangement and motion of particles.

Changes of State

Important changes of state include:

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

You should be able to explain these changes in terms of molecular motion and energy.

Brownian Movement

Brownian movement provides evidence that particles are in constant random motion.

You should understand how this supports the kinetic theory of matter.

Gas Laws

Important gas laws include:

• Boyle’s law;
• Charles’ law;
• Graham’s law;
• Dalton’s law of partial pressure;
• the combined gas law.

You should be able to recognize these laws from statements, equations and graphs.

Molar Volume and Atomicity

You should understand:

• molar volume of gases;
• atomicity of gases;
• relationships between gas volume and amount of substance.

Ideal Gas Equation

The ideal gas equation is:

PV = nRT

You should understand the meaning of each symbol and be able to solve simple problems involving pressure, volume, temperature and number of moles.

Vapour Density

You should also understand the relationship between vapour density and relative molecular mass.

Gas-Law Calculations

Practise calculations involving:

• pressure;
• volume;
• temperature;
• number of moles;
• molar volume;
• vapour density.

You should also be able to interpret graphs connected with the gas laws and draw conclusions from them.

Atomic Structure, Periodicity and Bonding

Atomic structure explains how atoms are arranged, while periodicity and bonding show how elements behave and combine.

Atoms, Molecules and Ions

You should distinguish between:

• atoms;
• molecules;
• ions.

An atom is the basic unit of an element, while molecules contain atoms joined together. Ions are charged particles formed when electrons are gained or lost.

Development of Atomic Structure

Important scientists include:

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

You should understand their main contributions to the development of atomic theory.

Atomic Number and Mass Number

The atomic number gives the number of protons in an atom.

The mass number represents the total number of protons and neutrons.

You should be able to calculate:

• number of protons;
• number of neutrons;
• number of electrons.

Pay special attention to elements with atomic numbers 1 to 20.

Electron Configuration

You should understand how electrons are arranged in atoms.

Electron configuration helps explain:

• chemical behaviour;
• position on the periodic table;
• bonding.

Isotopes

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

You should be able to identify isotopes and solve simple calculations involving isotopic masses.

Atomic Orbitals

You should understand the shapes of:

• s orbitals;
• p orbitals.

Also know the number of electrons that can occupy these orbitals.

The Periodic Table

The periodic table arranges elements according to their atomic numbers and recurring properties.

Important families include:

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

You should be able to relate the position of an element to its atomic number and electron configuration.

Periodic Properties

Important periodic properties include:

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

You should understand how these properties change across periods and down groups.

Chemical Bonding

Atoms combine through different forms of bonding.

Important types include:

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

You should be able to identify bond types from electron configurations and relate bonding to the properties of compounds.

Coordinate Bonding

A coordinate bond is a type of covalent bond.

Examples include complexes such as:

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

You should recognize these as examples of coordinate bonding.

Shapes of Simple Molecules

Important molecular shapes include:

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

You should be able to distinguish these shapes and connect them with the bonding arrangement in each molecule.

Nuclear Chemistry

Nuclear Chemistry deals with changes that occur in the nucleus of an atom.

These changes are different from ordinary chemical reactions because they involve the atomic nucleus rather than only the electrons around it.

Radioactivity

Radioactivity is the spontaneous emission of radiation from unstable nuclei.

You should understand the main types of nuclear radiation and compare their properties.

Important areas include:

• types of radiation;
• penetrating ability;
• ionizing ability;
• behaviour in electric or magnetic fields.

Natural and Artificial Radioactivity

Radioactivity may be:

• natural, when it occurs spontaneously in unstable elements;
• artificial, when radioactive substances are produced through nuclear processes.

You should be able to distinguish between the two.

Nuclear Reactions

Nuclear reactions involve changes in atomic nuclei.

You should understand how to write and balance simple nuclear equations by conserving:

• mass number;
• atomic number.

Half-Life

Half-life is the time required for half of the radioactive nuclei in a sample to decay.

You should be able to solve simple half-life calculations and determine the amount of radioactive material remaining after a given period.

Uses of Radioactivity

Radioactivity has useful applications in different areas.

You should understand examples of its use in:

• medicine;
• industry;
• scientific research;
• other practical applications.

When revising, focus on the differences between ordinary chemical reactions and nuclear reactions, the properties of nuclear radiation, simple nuclear equations and half-life calculations.

Air and Water

Air and water are important substances in Chemistry because of their composition, properties and practical uses.

Air

Air is a mixture of gases.

Its main constituents include:

• nitrogen;
• oxygen;
• water vapour;
• carbon dioxide;
• noble gases such as argon and neon.

You should understand why air is classified as a mixture and know the basic principle involved in separating its components.

Uses of Air Components

Different gases in air have different uses.

You should be able to relate important constituents such as oxygen, nitrogen and noble gases to their practical applications.

Water

Water can be formed from the combustion of hydrogen.

You should understand its composition by volume and its importance as a solvent.

Atmospheric gases may dissolve in water, and some of these dissolved gases are important to living organisms.

Hard and Soft Water

Water may be classified as hard or soft.

Hardness may be:

• temporary;
• permanent.

You should understand the causes of each type of hardness and the methods used to soften hard water.

Water Treatment

Water supplied to towns must be treated before use.

You should understand the main processes involved in making water suitable for public supply.

Water of Crystallization

Some substances contain a definite amount of water within their crystals.

This is known as water of crystallization.

You should also distinguish between:

• efflorescence;
• deliquescence;
• hygroscopy.

Know examples of substances that show these properties and understand their practical significance.

Solubility and Solutions

Solubility deals with how much of a substance can dissolve in a given amount of solvent under specific conditions.

Types of Solutions

You should distinguish between:

• unsaturated solution, which can still dissolve more solute;
• saturated solution, which contains the maximum amount of solute that can dissolve at a given temperature;
• supersaturated solution, which contains more dissolved solute than a saturated solution under the same conditions.

Solubility

Solubility may be expressed in moles per dm³.

You should understand how temperature affects solubility and be able to calculate the amount of solute that can dissolve in a given amount of solvent.

Solubility Curves

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

You should be able to:

• read values from a solubility curve;
• compare the solubilities of substances;
• determine how much solute will dissolve at a given temperature;
• draw simple conclusions from the graph.

Solvents and Their Uses

Different solvents are suitable for different substances.

You should understand the use of solvents for:

• fats;
• oils;
• paints;
• removal of stains.

The nature of the solvent should be related to the substance it can dissolve.

True Solutions, Suspensions and Colloids

You should be able to distinguish among:

• true solutions;
• suspensions;
• colloids.

Important examples include:

• harmattan haze and water paints as suspensions;
• fog, milk, aerosol sprays, emulsion paints and rubber solution as colloids.

Focus on the differences in their properties and how the particles behave in each system.

Environmental Pollution

Environmental pollution occurs when harmful substances enter the surroundings and affect living organisms or natural resources.

You should understand the types, sources, effects and control of pollution.

Air Pollution

Air pollutants include:

• hydrogen sulphide, H₂S;
• carbon monoxide, CO;
• sulphur dioxide, SO₂;
• oxides of nitrogen;
• chlorofluorocarbons, CFCs;
• dust.

You should be able to identify their sources and explain how they can affect human health and the environment.

Water Pollution

Important causes of water pollution include:

• sewage;
• oil pollution.

You should understand how these pollutants affect water quality and living organisms.

Soil Pollution

Soil may be polluted by substances such as:

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

You should distinguish between biodegradable and non-biodegradable pollutants.

Biodegradable pollutants can be broken down naturally, while non-biodegradable pollutants persist in the environment for longer periods.

Effects and Control of Pollution

Pollution can damage ecosystems, reduce environmental quality and affect human health.

You should be able to:

• identify different pollutants;
• state their sources;
• classify them correctly;
• explain their environmental effects;
• suggest suitable control measures.

When revising pollution, connect each pollutant with its source, type, effect and method of control.

Acids, Bases and Salts

Acids, bases and salts are important classes of chemical substances with different properties and reactions.

Acids and Bases

An acid may be described as a substance that produces H₃O⁺ ions in aqueous solution or acts as a proton donor.

You should understand the general properties of acids and bases and be able to distinguish between them using suitable indicators.

Important naturally occurring organic acids include:

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

Basicity and Strength

You should understand the basicity of acids and distinguish between strong and weak acids and bases.

The strength of an acid or base depends on its degree of dissociation in solution.

This also affects electrical conductance because solutions containing more ions conduct electricity more effectively.

Salts

You should distinguish between:

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

Alums are examples of double salts.

Important methods of preparing salts include:

• neutralization;
• precipitation;
• reaction of acids with metals;
• reactions involving oxides and trioxocarbonate (IV) salts.

Indicators

Acid-base indicators help determine whether a solution is acidic or alkaline.

You should be able to select a suitable indicator for a given acid-base reaction.

pH and pOH

The pH scale measures acidity, while pOH is related to alkalinity.

You should be able to perform simple calculations involving:

• pH;
• pOH.

You should also interpret the values correctly to determine whether a solution is acidic, neutral or alkaline.

Acid-Base Titration

Titration is used to determine the reacting quantities of acids and bases.

You should understand:

• suitable indicators;
• titration curves;
• mole relationships;
• simple calculations based on the mole concept.

Always use the balanced chemical equation when determining reacting amounts.

Hydrolysis of Salts

Some salts react with water and produce acidic, basic or neutral solutions.

Important examples include:

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

You should understand the basic principle of salt hydrolysis and be able to determine the nature of the resulting solution.

What to Focus On

When revising acids, bases and salts, make sure you can:

• distinguish acids from bases;
• classify salts;
• identify preparation methods;
• use indicators correctly;
• relate dissociation to conductance;
• calculate pH and pOH;
• solve simple titration problems;
• determine whether hydrolysed salt solutions are acidic, basic or neutral.

Oxidation and Reduction

Oxidation and reduction are chemical changes that involve oxygen, hydrogen, electrons or changes in oxidation number.

Meaning of Oxidation

Oxidation may involve:

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

Meaning of Reduction

Reduction may involve:

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

Oxidation and reduction usually occur together in a redox reaction.

Oxidation Numbers

You should understand how to determine the oxidation number of an element in a compound or ion.

Oxidation numbers can be used to:

• identify oxidation and reduction;
• determine electron transfer;
• balance simple redox equations;
• name inorganic compounds correctly.

Oxidizing and Reducing Agents

An oxidizing agent causes another substance to be oxidized, while a reducing agent causes another substance to be reduced.

You should be able to identify both agents in a chemical reaction.

Balancing Redox Equations

Practise balancing simple redox equations using changes in oxidation number.

Pay attention to:

• which species is oxidized;
• which species is reduced;
• number of electrons transferred;
• correct balanced equation.

Tests and IUPAC Naming

You should also understand common tests used to identify oxidizing and reducing agents.

Oxidation numbers may also be used when giving the IUPAC names of inorganic compounds.

Electrolysis and Electrochemical Cells

Electrolysis uses electricity to cause chemical changes in an electrolyte.

Electrolytes and Non-Electrolytes

An electrolyte conducts electricity when molten or dissolved in water because it contains mobile ions.

A non-electrolyte does not conduct electricity through ion movement.

You should be able to distinguish between the two and identify suitable electrodes for different electrolytes.

Faraday’s Laws of Electrolysis

Faraday’s laws relate the amount of substance produced during electrolysis to the quantity of electricity passed.

You should practise simple calculations involving Faraday as a mole of electrons.

Electrolysis of Common Substances

Important examples include the electrolysis of:

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

You should be able to determine:

• the ions present;
• the products formed at each electrode;
• the reactions occurring at the electrodes;
• factors affecting the discharge of ions.

Uses of Electrolysis

Electrolysis is used for:

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

Electrochemical Cells

You should understand the redox series:

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

Also study half-cell reactions and electrode potentials.

Practise simple calculations involving electrode potentials.

Corrosion and Its Prevention

Corrosion can occur through an electrolytic process.

Methods of protecting iron include:

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

You should understand how these methods reduce or prevent corrosion.

Energy Changes

Chemical and physical changes may involve the absorption or release of energy.

Enthalpy Change

The heat change that accompanies a process is represented by ΔH.

Examples include:

• dissolution of substances in water;
• reaction of sodium with water;
• reaction of potassium with water;
• dissolution of NaOH;
• dissolution of NH₄Cl.

An exothermic reaction releases heat and has a negative ΔH value.

An endothermic reaction absorbs heat and has a positive ΔH value.

You should also be able to interpret simple graphs showing energy changes.

Entropy

Entropy describes the degree of order or disorder in a system.

Simple examples include:

• mixing gases;
• dissolving salts.

Greater disorder generally means higher entropy.

Spontaneity of Reactions

The spontaneity of a reaction can be related to Gibbs free energy, ΔG.

Remember:

• ΔG = 0 at equilibrium;
• ΔG > 0 for a non-spontaneous process;
• ΔG < 0 for a spontaneous process.

The relationship is:

ΔG = ΔH − TΔS

You should understand the relationship among ΔH, ΔS and ΔG and be able to solve simple calculations using this equation.

Rates of Chemical Reaction

The rate of a chemical reaction describes how quickly reactants are converted into products.

Factors Affecting Reaction Rate

Important factors include:

• Temperature: increasing temperature usually increases reaction rate because particles move faster and collide more frequently.
• Concentration: higher concentration increases the number of reacting particles available for collision.
• Pressure: in gaseous reactions, increased pressure can increase reaction rate.
• Surface area: powdered solids generally react faster than lumps of the same mass because more surface is exposed.
• Catalysts: a catalyst changes the rate of a reaction without being permanently used up.

Examples to understand include reactions involving HCl with Na₂S₂O₃, magnesium or marble, the iodine clock reaction, and decomposition of H₂O₂ or KClO₃ using MnO₂.

Reaction Rate Curves and Activation Energy

You should be able to interpret reaction rate curves and solve simple rate problems.

Activation energy, Ea, is the minimum energy particles need for a successful reaction. You should understand its importance and identify it from suitable energy or rate curves.

Collision Theory

Collision theory explains reaction rates in terms of collisions between reacting particles. Successful reactions require suitable collisions with enough energy.

You should also understand the qualitative idea behind Arrhenius’ law and how light can affect some reactions, such as the halogenation of alkanes.

Chemical Equilibrium

Chemical equilibrium occurs in a reversible reaction when the forward and backward reactions continue at the same rate.

Reversible Reactions

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

At equilibrium, the reaction does not stop. Instead, it reaches dynamic equilibrium, where both reactions continue at equal rates.

Examples include:

• the reaction of steam with iron;
• N₂O₄ ⇌ 2NO₂.

Factors Affecting Equilibrium

The position of equilibrium can be affected by changes in:

• concentration;
• pressure;
• temperature.

You should understand how each change can shift the equilibrium position.

Le Chatelier’s Principle

Le Chatelier’s principle states that when a system at equilibrium is disturbed, it responds in a way that reduces the effect of the disturbance.

Use this principle to predict how changes in concentration, pressure or temperature affect a reversible reaction.

Equilibrium Constant

The equilibrium constant describes the relationship between reactants and products at equilibrium.

You should understand the factors that affect the equilibrium position and how these factors relate to the equilibrium constant.

Focus mainly on interpreting equilibrium changes and predicting their effects. Detailed calculations are not required for this area.

Non-metals and Their Compounds

You should understand the preparation, properties, uses and tests of important non-metals and their compounds.

Hydrogen

Study the laboratory preparation of hydrogen and its commercial production from water gas and cracking of petroleum fractions.

Know its properties, uses and test.

Halogens

Chlorine is the main representative of the halogens.

Focus on:

• laboratory and industrial preparation of chlorine;
• its properties and uses;
• water sterilization and bleaching;
• manufacture of HCl, plastics and insecticides.

Also study hydrogen chloride and hydrochloric acid, including their preparation and properties, as well as the test for chloride ions.

Oxygen and Sulphur

For oxygen, study:

• laboratory preparation;
• commercial production from liquid air;
• properties and uses;
• acidic, basic, amphoteric and neutral oxides;
• ozone and its importance in the atmosphere.

For sulphur, understand its allotropes and uses.

Important sulphur compounds include SO₂, H₂SO₃, H₂SO₄ and H₂S. Know their preparation, properties and uses where required, including the Contact Process for H₂SO₄.

Also know the tests for sulphate, sulphite and sulphide ions.

Nitrogen and Its Compounds

Study the laboratory preparation of nitrogen and its production from liquid air.

For ammonia, understand:

• laboratory preparation;
• industrial preparation by the Haber Process;
• properties and uses;
• ammonium salts;
• test for NH₄⁺.

Also study nitric acid, nitrates and the properties of nitrogen oxides such as N₂O, NO and NO₂.

Understand the nitrogen cycle and its environmental importance.

Carbon and Its Compounds

Know the allotropes of carbon and their uses.

Study CO₂ and CO, including their preparation, properties and uses. Pay attention to the harmful effect of carbon monoxide on blood and its sources such as charcoal fires and exhaust fumes.

Also understand:

• types of coal;
• destructive distillation of wood and coal;
• coke and its uses;
• gasification;
• manufacture and uses of synthetic gas.

Important ion tests include Cl⁻, SO₄²⁻, SO₃²⁻, S²⁻, NH₄⁺, NO₃⁻, CO₃²⁻ and HCO₃⁻.

Metals and Their Compounds

Metals have characteristic physical and chemical properties, and their methods of extraction depend largely on their reactivity.

You should understand the general properties of metals, compare their reactivities and relate their properties to their uses.

Sodium and Its Compounds

For sodium, study important compounds such as:

• sodium hydroxide, NaOH;
• sodium trioxocarbonate (IV), Na₂CO₃;
• sodium hydrogen trioxocarbonate (IV), NaHCO₃;
• sodium chloride, NaCl.

Understand the production of NaOH by electrolysis of brine and its reactions with aluminium, zinc and lead ions.

Know the Solvay process for producing sodium trioxocarbonate (IV), its properties and uses, including glass manufacture.

Also study the occurrence of NaCl in seawater, its recovery, uses and the economic importance of seawater.

Calcium and Its Compounds

Important calcium compounds include:

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

You should know their properties and uses.

Also understand:

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

Aluminium and Tin

For aluminium, study:

• purification of bauxite;
• electrolytic extraction;
• properties and uses;
• test for Al³⁺.

For tin, know its ores, extraction, properties and uses.

Transition Metals

The first transition metals show important characteristics such as:

• variable oxidation states;
• formation of complex ions;
• coloured ions;
• catalytic behaviour.

You should also understand their electron configurations and the IUPAC naming of simple transition-metal complexes.

Iron and Copper

For iron, study extraction from its ores, properties, uses and different forms of iron.

Understand the advantages of steel over iron and know the tests for Fe²⁺ and Fe³⁺.

For copper, study its extraction, properties and uses, as well as the preparation and uses of copper(II) tetraoxosulphate(VI), CuSO₄. Know the test for Cu²⁺.

Alloys

Important alloys include:

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

You should know their main constituents and uses and be able to compare alloys with pure metals.

Organic Chemistry

Organic Chemistry deals mainly with carbon compounds. You should understand carbon tetravalency, catenation, functional groups, general formulae, IUPAC naming, empirical formulae and isomerism.

Hydrocarbons

Hydrocarbons contain only carbon and hydrogen.

Alkanes form a homologous series and mainly undergo substitution reactions. Study their physical properties, structural isomerism up to six carbon atoms and uses of halogenated products.

Alkenes undergo addition and polymerization reactions. Understand structural and geometric isomerism and the production of materials such as polythene and synthetic rubber.

Alkynes include ethyne, which can be prepared by the action of water on suitable carbides. Know its properties, simple reactions and the test for terminal alkynes.

For benzene, study its structure, properties and uses as an aromatic hydrocarbon.

Petroleum

Crude petroleum is a complex mixture of hydrocarbons.

Understand:

• fractional distillation and its major products;
• cracking and reforming;
• petrochemicals;
• quality of petrol;
• meaning of octane number.

Alkanols

Alkanols may be primary, secondary or tertiary.

Study the production of ethanol through fermentation and from petroleum products. Also understand glycerol as a polyhydric alkanol.

Know how oxidation and the Lucas test can help distinguish different classes of alkanols.

Alkanals, Alkanones and Alkanoic Acids

You should know the chemical tests used to distinguish alkanals from alkanones.

For alkanoic acids, focus on:

• neutralization;
• esterification;
• ethanedioic acid as a dicarboxylic acid;
• benzenecarboxylic acid as an aromatic acid.

Alkanoates, Fats and Oils

Alkanoates are formed from alkanoic acids and alkanols.

Fats and oils are examples of alkanoates. Study saponification, soap production, margarine production and the differences between soaps and detergents.

Amines

Understand the classification of amines into:

• primary;
• secondary;
• tertiary.

Carbohydrates and Proteins

Carbohydrates are classified as monosaccharides, disaccharides and polysaccharides.

Know their sources, hydrolysis, uses and tests for simple sugars. Examples of complex carbohydrates include cellulose from cotton and starch from cassava.

For proteins, study:

• basic structure;
• hydrolysis;
• Ninhydrin test;
• Biuret test;
• Millon’s test;
• xanthoproteic test;
• enzymes and their functions.

Polymers

You should distinguish between natural and synthetic polymers and between:

• addition polymerization;
• condensation polymerization.

Also understand natural and synthetic rubber, their uses, and the difference between thermoplastics and thermosetting plastics.

For this broad topic, concentrate on identifying functional groups, naming compounds, distinguishing organic classes, recognizing important reactions and relating structures to properties.

Chemistry and Industry

Chemistry plays an important role in industries that convert raw materials into useful products.

You should understand how chemical industries are classified and how their activities relate to everyday life and economic development.

Types of Chemical Industries

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

You should be able to identify the major raw materials used by different industries and relate those materials to the products obtained.

Fine and Heavy Chemicals

You should distinguish between:

• fine chemicals, which are usually produced in smaller quantities for specialized uses;
• heavy chemicals, which are produced in large quantities for industrial purposes.

Know suitable examples and understand why each group is important.

Raw Materials and Industrial Processes

Chemical industries depend on suitable raw materials.

You should be able to:

• identify raw materials used in chemical production;
• connect raw materials with their industries;
• relate chemical processes to useful products;
• explain the relevance of chemical industries.

Biotechnology

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

You should understand how biotechnology can be connected with industrial chemical production and the manufacture of useful products.

How to Use JAMB Chemistry Topics for Revision

A good Chemistry revision plan should combine understanding, calculations and regular practice.

Start by arranging the JAMB Chemistry topics into smaller groups. Study one group at a time instead of trying to cover the entire subject at once.

Pay more attention to areas that require calculations, such as:

• mole and stoichiometric calculations;
• gas laws;
• pH and pOH;
• electrolysis;
• electrode potentials;
• energy changes;
• reaction rates.

For descriptive topics, focus on understanding preparation methods, properties, reactions, uses and chemical tests.

Practise writing and balancing chemical equations correctly. Also revise graphs, laboratory observations, periodic trends, functional groups and important chemical processes.

When studying organic chemistry, learn how to identify compounds from their structures and functional groups rather than memorizing names alone.

Use past questions after studying each major topic to check whether you can apply what you have learned. Review any area where you repeatedly make mistakes before moving to another topic.

A simple revision pattern is to study the concept, practise examples, answer questions and correct mistakes.

Recommended Texts for JAMB Chemistry

The following Chemistry textbooks can support your study and revision:

1. O. Y. Ababio, New School Chemistry for Senior Secondary Schools, 4th Edition, Africana FIRST Publishers Limited.
2. S. T. Bajah, B. O. Teibo, G. Onwu and A. Obikwere, Senior Secondary Chemistry, Books 1, 2 and 3, Longman.

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

Use these texts to strengthen your understanding of concepts, worked examples, chemical equations and calculations across the major Chemistry topics.

Key Points to Remember

When studying the JAMB Chemistry Area of Concentration, keep these important points in mind:

• Understand concepts instead of memorizing definitions only.
• Learn how to write and balance chemical equations correctly.
• Practise calculations involving moles, gas laws, pH, electrolysis, energy changes and reaction rates.
• Know important laboratory preparations, properties, uses and tests of common substances.
• Understand periodic trends, chemical bonding and molecular shapes.
• Be able to identify oxidation and reduction using electron transfer and oxidation numbers.
• Learn the factors that affect reaction rates and chemical equilibrium.
• Know the extraction, properties and uses of important metals and non-metals.
• In organic chemistry, focus on functional groups, nomenclature, reactions, isomerism and chemical tests.
• Practise interpreting graphs, experimental data and chemical relationships.
• Review weak topics repeatedly and use practice questions to test your understanding.

Frequently Asked Questions about JAMB Chemistry Area of Concentration

Conclusion

The JAMB Area of Concentration for Chemistry Subject 2027/2028 covers a wide range of topics, from basic chemical principles to calculations, laboratory concepts, inorganic chemistry and organic chemistry.

Your main goal should be to understand how the different topics connect. Pay attention to chemical equations, calculations, properties of substances, laboratory tests, industrial processes and practical applications.

Use the topics in this guide to organize your study, revise each section carefully and practise questions after completing every major area.

With steady revision and a clear understanding of the important Chemistry concepts, you will be better prepared to handle questions across the different areas of the subject.