JAMB CBT Practice Chemistry: Questions, Tips & Free Practice (2027)

Student studying chemistry equations and periodic table

Introduction: Why Chemistry Is the Bridge Subject That Determines Your JAMB Score

Chemistry sits at the crossroads of science. It is required for Medicine, Engineering, Pharmacy, Biochemistry, Industrial Chemistry, Agriculture, and virtually every science-related university programme. For many candidates, Chemistry is the subject that makes or breaks their JAMB score.

The challenge with JAMB Chemistry is that it combines three distinct skill sets: conceptual understanding (like Biology), mathematical calculation (like Physics), and rote memorisation (chemical equations, periodic table trends, IUPAC nomenclature). Students who prepare for only one or two of these dimensions get caught off guard by questions that test the third.

The candidates who score 30+ in JAMB Chemistry are the ones who practise all three dimensions consistently under timed CBT conditions. They know the equations, understand the concepts, can perform the calculations, and do it all within 45 seconds per question.

This guide covers the full JAMB Chemistry syllabus, gives you 20 practice questions with worked solutions, provides the essential equations and constants you must memorise, and lays out a study plan to push your score past 70/100.

Start Practising Now: SchoolHub's Free JAMB CBT Practice App covers Chemistry with AI-generated questions, a 20-minute timer, and detailed explanations, all completely free.

JAMB Chemistry at a Glance

Aspect	Detail
Number of questions	40
Time allocated	~30 minutes (within the 2-hour total)
Maximum score	100 (each question = 2.5 marks)
Question format	Multiple choice (A, B, C, D)
Calculator allowed	No
Key requirements	Periodic table knowledge, balanced equations, mole calculations

Key fact: JAMB does not provide a periodic table during the exam. You are expected to know the atomic numbers, symbols, and relative atomic masses of common elements from memory.

Complete JAMB Chemistry Syllabus Breakdown

1. Physical Chemistry (Approximately 35% of questions)

This is the calculation-heavy section and the largest portion of the paper.

Topics covered:

Atomic structure (atomic number, mass number, isotopes, electronic configuration)
Chemical bonding (ionic, covalent, metallic, van der Waals forces, hydrogen bonding)
Stoichiometry and the mole concept (molar mass, mole calculations, empirical and molecular formulas)
Gas laws (Boyle's, Charles', general gas equation, Avogadro's law, molar volume at STP)
Energy changes (exothermic, endothermic reactions, enthalpy, Hess's law)
Rates of reaction (factors affecting rate, collision theory, activation energy)
Chemical equilibrium (Le Chatelier's principle, equilibrium constant)
Acids, bases, and salts (pH, indicators, neutralisation, solubility)
Redox reactions (oxidation numbers, electrochemical cells, electrolysis)
Solubility and solubility curves

Why it matters: Physical Chemistry generates roughly 14 of your 40 questions. The mole concept alone can produce 3-5 questions. Students who master stoichiometry have a significant advantage.

2. Organic Chemistry (Approximately 30% of questions)

Topics covered:

IUPAC nomenclature (naming alkanes, alkenes, alkynes, alcohols, carboxylic acids, etc.)
Hydrocarbons: Alkanes (properties, reactions, substitution)
Hydrocarbons: Alkenes (properties, reactions, addition, polymerisation)
Hydrocarbons: Alkynes (properties, reactions)
Alcohols (types, properties, reactions, fermentation)
Carboxylic acids (properties, reactions, esterification)
Esters (formation, hydrolysis, uses)
Fats and oils (saponification, properties)
Polymers (addition and condensation polymerisation)
Petroleum and petrochemicals (fractional distillation, cracking)
Functional groups and homologous series
Isomerism (structural isomerism)

Why it matters: Organic Chemistry is highly predictable. IUPAC naming, functional group identification, and reaction types repeat every year. Students who learn the naming rules and key reactions score consistently.

3. Inorganic Chemistry (Approximately 20% of questions)

Topics covered:

Periodic table (groups, periods, trends in properties)
Properties of elements in Groups I, II, IV, VII, and transition metals
Extraction of metals (iron, aluminium, copper)
Water (treatment, hardness, softening)
Air (composition, pollution, greenhouse effect)
Hydrogen, oxygen, nitrogen, chlorine, and their compounds
Acids, bases, and salts (preparation, properties)
Qualitative analysis (tests for gases, cations, anions)

Frequently tested: Periodic table trends (atomic radius, ionisation energy, electronegativity across periods and down groups), tests for gases (CO₂, H₂, O₂, NH₃, Cl₂, SO₂, HCl), properties of Group I and VII elements.

4. Environmental and Industrial Chemistry (Approximately 15% of questions)

Topics covered:

Industrial processes (Haber process, Contact process, Solvay process)
Alloys and their uses
Soaps and detergents
Plastics and synthetic fibres
Environmental pollution (acid rain, ozone depletion, global warming)
Water treatment and purification
Biotechnology applications in chemistry

Essential Chemistry Data You Must Memorise

Relative Atomic Masses (Most Common in JAMB)

Element	Symbol	Atomic Number	Relative Atomic Mass
Hydrogen	H	1	1
Carbon	C	6	12
Nitrogen	N	7	14
Oxygen	O	8	16
Sodium	Na	11	23
Magnesium	Mg	12	24
Aluminium	Al	13	27
Silicon	Si	14	28
Phosphorus	P	15	31
Sulphur	S	16	32
Chlorine	Cl	17	35.5
Potassium	K	19	39
Calcium	Ca	20	40
Iron	Fe	26	56
Copper	Cu	29	64
Zinc	Zn	30	65
Silver	Ag	47	108
Barium	Ba	56	137
Lead	Pb	82	207

Standard Constants

Constant	Value
Avogadro's number	6.02 × 10²³ mol⁻¹
Molar volume at STP	22.4 dm³
Faraday's constant	96,500 C/mol
Standard temperature (STP)	273K (0°C)
Standard pressure (STP)	1 atm (760 mmHg)
Molar gas constant (R)	8.314 J/mol·K

Key Formulas

Formula	Use
Number of moles = mass / molar mass	Mole calculations
Number of moles = volume (dm³) / 22.4	Gases at STP
Number of moles = concentration × volume (dm³)	Solutions
PV = nRT	Ideal gas equation
P₁V₁/T₁ = P₂V₂/T₂	General gas law
% composition = (mass of element / molar mass) × 100	Percentage composition
Q = It	Quantity of electricity
Mass deposited = (QM) / (nF)	Electrolysis (Faraday's law)

20 JAMB Chemistry Practice Questions With Solutions

Work through these under timed conditions. Give yourself 15 minutes for all 20, then check the solutions.

Physical Chemistry

Question 1: How many moles are in 11g of CO₂? (C = 12, O = 16)

(A) 0.20 (B) 0.25 (C) 0.50 (D) 1.00

Solution: Molar mass of CO₂ = 12 + 2(16) = 44 g/mol. Moles = 11/44 = 0.25 mol. Answer: (B)

Question 2: What volume does 2 moles of an ideal gas occupy at STP?

(A) 11.2 dm³ (B) 22.4 dm³ (C) 44.8 dm³ (D) 67.2 dm³

Solution: At STP, 1 mole of gas = 22.4 dm³. So 2 moles = 2 × 22.4 = 44.8 dm³. Answer: (C)

Question 3: The electronic configuration of an element is 1s² 2s² 2p⁶ 3s² 3p³. The element belongs to

(A) Group III, Period 3 (B) Group V, Period 3 (C) Group III, Period 5 (D) Group V, Period 2

Solution: The highest energy level is 3 (Period 3). The number of electrons in the outermost shell: 3s² 3p³ = 5 electrons (Group V). Answer: (B)

Question 4: An increase in temperature increases the rate of a chemical reaction because it

(A) decreases the activation energy
(B) increases the number of particles with energy greater than or equal to the activation energy
(C) decreases the concentration of reactants
(D) increases the volume of the container

Explanation: Higher temperature means more particles have kinetic energy equal to or greater than the activation energy. More effective collisions occur per unit time, increasing the reaction rate. The activation energy itself does not change (only a catalyst changes that). Answer: (B)

Question 5: What is the oxidation number of manganese in KMnO₄?

(A) +2 (B) +4 (C) +5 (D) +7

Solution: K = +1, O = -2 (×4 = -8). Let Mn = x. +1 + x + (-8) = 0. x = +7. Answer: (D)

Question 6: A solution has a pH of 3. This means the solution is

(A) strongly acidic (B) weakly acidic (C) neutral (D) weakly alkaline

Explanation: pH scale: 0-6 = acidic, 7 = neutral, 8-14 = alkaline. pH 3 is strongly acidic (close to 0). pH 5-6 would be weakly acidic. Answer: (A)

Question 7: According to Le Chatelier's principle, an increase in pressure favours the side of an equilibrium with

(A) more moles of gas (B) fewer moles of gas (C) more heat (D) less heat

Explanation: Increasing pressure shifts equilibrium to the side with fewer moles of gas, as this reduces pressure. This is Le Chatelier's principle: the system adjusts to oppose the change. Answer: (B)

Organic Chemistry

Question 8: The IUPAC name of CH₃CH₂CH₂OH is

(A) methanol (B) ethanol (C) propan-1-ol (D) propan-2-ol

Explanation: Three carbon atoms = propan-. The OH group is on carbon 1 = -1-ol. Full name: propan-1-ol. Methanol has 1 carbon, ethanol has 2. Propan-2-ol would have the OH on the middle carbon. Answer: (C)

Question 9: Which of the following is the general formula for alkenes?

(A) CₙH₂ₙ₊₂ (B) CₙH₂ₙ (C) CₙH₂ₙ₋₂ (D) CₙHₙ

Explanation: Alkanes = CₙH₂ₙ₊₂ (saturated). Alkenes = CₙH₂ₙ (one double bond). Alkynes = CₙH₂ₙ₋₂ (one triple bond). Answer: (B)

Question 10: Ethanol can be converted to ethanoic acid by

(A) reduction (B) oxidation (C) hydrolysis (D) polymerisation

Explanation: Converting an alcohol to a carboxylic acid involves adding oxygen (oxidation). CH₃CH₂OH (ethanol) is oxidised to CH₃COOH (ethanoic acid). Acidified potassium dichromate (K₂Cr₂O₇) is a common oxidising agent for this reaction. Answer: (B)

Question 11: The process of breaking down large hydrocarbon molecules into smaller, more useful ones is called

(A) polymerisation (B) cracking (C) distillation (D) combustion

Explanation: Cracking breaks large, less useful hydrocarbon molecules (from petroleum) into smaller, more useful ones like petrol and ethene. Polymerisation is the opposite (joining small molecules). Distillation separates mixtures. Combustion is burning. Answer: (B)

Question 12: Which functional group is present in carboxylic acids?

(A) -OH (B) -CHO (C) -COOH (D) -CO-

Explanation: Carboxylic acids contain the -COOH (carboxyl) group. -OH is the hydroxyl group (alcohols). -CHO is the aldehyde group. -CO- is the ketone group. Answer: (C)

Question 13: The reaction between an alcohol and a carboxylic acid to form an ester is called

(A) saponification (B) esterification (C) fermentation (D) hydrogenation

Explanation: Esterification: alcohol + carboxylic acid → ester + water (in the presence of concentrated H₂SO₄ as catalyst). Saponification is the hydrolysis of esters/fats with alkali to produce soap. Fermentation converts sugars to ethanol. Hydrogenation adds hydrogen to unsaturated compounds. Answer: (B)

Inorganic Chemistry

Question 14: Which of the following gases turns lime water milky?

(A) Hydrogen (B) Oxygen (C) Carbon dioxide (D) Nitrogen

Explanation: CO₂ + Ca(OH)₂ → CaCO₃ + H₂O. Calcium carbonate (CaCO₃) is insoluble and forms a white precipitate, turning the lime water milky. This is the standard test for carbon dioxide. Answer: (C)

Question 15: Down a group in the periodic table, atomic radius

(A) increases (B) decreases (C) remains the same (D) first increases then decreases

Explanation: Down a group, new electron shells are added with each period. More shells = larger distance between the nucleus and outermost electrons = larger atomic radius. Across a period, atomic radius decreases (more protons pulling electrons closer). Answer: (A)

Question 16: The ore from which aluminium is extracted is

(A) haematite (B) bauxite (C) galena (D) chalcopyrite

Explanation: Bauxite (Al₂O₃·2H₂O) is the principal ore of aluminium. Haematite (Fe₂O₃) is iron ore. Galena (PbS) is lead ore. Chalcopyrite (CuFeS₂) is copper ore. Answer: (B)

Question 17: Temporary hardness of water is caused by

(A) calcium sulphate (B) magnesium sulphate (C) calcium hydrogencarbonate (D) sodium chloride

Explanation: Temporary hardness is caused by dissolved calcium hydrogencarbonate Ca(HCO₃)₂ or magnesium hydrogencarbonate. It can be removed by boiling (the hydrogencarbonates decompose). Permanent hardness is caused by sulphates (CaSO₄, MgSO₄), which cannot be removed by boiling. Answer: (C)

Environmental and Industrial Chemistry

Question 18: In the Haber process, nitrogen and hydrogen react to form ammonia. The conditions used are

(A) high temperature, low pressure, iron catalyst
(B) moderate temperature (450°C), high pressure (200 atm), iron catalyst
(C) low temperature, low pressure, no catalyst
(D) high temperature, high pressure, vanadium pentoxide catalyst

Explanation: The Haber process: N₂ + 3H₂ ⇌ 2NH₃. Conditions: 450°C (moderate, compromise between rate and yield), 200 atm (high pressure favours fewer moles of gas, i.e., the product side), iron catalyst (increases rate without affecting equilibrium position). Vanadium pentoxide is the catalyst for the Contact process (making H₂SO₄). Answer: (B)

Question 19: Acid rain is primarily caused by

(A) CO₂ and H₂O (B) SO₂ and NO₂ (C) O₃ and CO (D) CH₄ and N₂O

Explanation: Sulphur dioxide (SO₂) and nitrogen dioxide (NO₂) dissolve in rainwater to form sulphuric acid (H₂SO₄) and nitric acid (HNO₃), producing acid rain. CO₂ dissolves to form weak carbonic acid, but this is normal rain, not acid rain. Answer: (B)

Question 20: During the electrolysis of brine (concentrated NaCl solution), the products at the cathode, anode, and in solution are respectively

(A) hydrogen, chlorine, sodium hydroxide
(B) sodium, chlorine, hydrogen
(C) chlorine, hydrogen, sodium hydroxide
(D) sodium hydroxide, hydrogen, chlorine

Explanation: At the cathode (negative electrode): H₂ gas is produced (hydrogen ions are preferentially discharged over sodium ions). At the anode (positive electrode): Cl₂ gas is produced (chloride ions are discharged). In solution: NaOH (sodium hydroxide) remains. Answer: (A)

How to Score 35+ Out of 40 in JAMB Chemistry

Strategy 1: Divide Your Study Into the Three Dimensions

Chemistry requires three types of knowledge, and your study plan must cover all three:

Dimension	What It Involves	Example Topics
Conceptual	Understanding why reactions happen	Le Chatelier's principle, collision theory, periodic trends
Calculation	Applying formulas to get numerical answers	Mole calculations, gas laws, electrolysis calculations
Memorisation	Knowing specific facts, names, and equations	IUPAC naming, atomic masses, colours of precipitates, industrial processes

A common mistake is preparing for only one or two dimensions. Balance your study time across all three.

Strategy 2: Master the Mole Concept

The mole concept is the single most important topic in JAMB Chemistry. It appears in multiple forms:

Direct mole calculations (mass to moles, moles to mass)
Gas volume calculations at STP
Solution concentration calculations
Stoichiometric calculations from balanced equations
Percentage composition and empirical formula
Electrolysis calculations using Faraday's law

Practice approach: Solve 5 mole-related problems daily until you can do them in your sleep. If you master stoichiometry, you can answer 5-8 questions confidently.

Strategy 3: Learn IUPAC Naming Rules Systematically

IUPAC naming questions appear in every JAMB Chemistry paper. Learn the system, not individual names:

Find the longest carbon chain (this gives the parent name: meth-, eth-, prop-, but-, pent-, hex-)
Identify the functional group (this gives the suffix: -ane, -ene, -yne, -ol, -al, -one, -oic acid)
Number from the end nearest the functional group
Name any branches (methyl, ethyl, etc.) with their position numbers

Carbon Count	Prefix
1	Meth-
2	Eth-
3	Prop-
4	But-
5	Pent-
6	Hex-
7	Hept-
8	Oct-
9	Non-
10	Dec-

Functional Group	Class	Suffix
C-C (single bonds only)	Alkane	-ane
C=C	Alkene	-ene
C≡C	Alkyne	-yne
-OH	Alcohol	-ol
-CHO	Aldehyde	-al
-CO-	Ketone	-one
-COOH	Carboxylic acid	-oic acid

Strategy 4: Know the Standard Gas Tests

JAMB frequently tests gas identification. Memorise these:

Gas	Test	Result
CO₂	Pass through lime water	Turns milky
O₂	Insert a glowing splint	Relights the splint
H₂	Insert a burning splint	Burns with a "pop" sound
NH₃	Hold damp red litmus paper	Turns blue
Cl₂	Hold damp litmus paper	Bleaches it (turns white)
SO₂	Pass through acidified K₂Cr₂O₇	Turns from orange to green
HCl	Hold near ammonia gas	White fumes of NH₄Cl

Strategy 5: Understand Periodic Table Trends

Several questions test your knowledge of how properties change across periods and down groups:

Property	Across a Period (left to right)	Down a Group (top to bottom)
Atomic radius	Decreases	Increases
Ionisation energy	Increases	Decreases
Electronegativity	Increases	Decreases
Metallic character	Decreases	Increases
Non-metallic character	Increases	Decreases
Electron affinity	Generally increases	Generally decreases

Strategy 6: Practise With a Timer Every Day

Chemistry requires quick recall of facts AND quick calculation. Use SchoolHub's JAMB CBT Practice App daily:

40 Chemistry questions per session
20-minute timer matching real exam pressure
AI-generated questions covering all syllabus areas
Detailed explanations for every answer

Topic-by-Topic Study Plan for JAMB Chemistry

Week 1-2: Atomic Structure, Bonding, and Stoichiometry

Day 1-2: Atomic structure (subatomic particles, isotopes, electronic configuration)
Day 3-4: Chemical bonding (ionic, covalent, metallic, intermolecular forces)
Day 5-6: Mole concept (molar mass, mole calculations, Avogadro's number)
Day 7-8: Chemical equations (balancing, stoichiometric calculations)
Day 9-10: Empirical and molecular formulas, percentage composition
Daily: 1 CBT session on SchoolHub + 5 mole calculation problems

Week 3-4: Gas Laws, Energetics, and Rates

Day 1-2: Gas laws (Boyle's, Charles', general gas equation, molar volume)
Day 3-4: Energy changes (exothermic/endothermic, enthalpy, Hess's law)
Day 5-6: Rates of reaction (factors, collision theory, activation energy)
Day 7-8: Chemical equilibrium (Le Chatelier's principle, equilibrium constant)
Day 9-10: Acids, bases, pH, indicators, neutralisation
Daily: 1 CBT session

Week 5-6: Organic Chemistry

Day 1-2: IUPAC nomenclature and functional groups
Day 3-4: Alkanes (properties, substitution reactions)
Day 5-6: Alkenes (properties, addition reactions, polymerisation)
Day 7-8: Alcohols, carboxylic acids, esters (reactions, preparation)
Day 9-10: Petroleum (fractional distillation, cracking), polymers
Daily: 1 CBT session + practice naming 10 compounds

Week 7-8: Inorganic Chemistry and Electrochemistry

Day 1-2: Periodic table (trends, group properties)
Day 3-4: Extraction of metals (iron, aluminium)
Day 5-6: Qualitative analysis (tests for gases, cations, anions)
Day 7-8: Redox reactions (oxidation numbers, balancing redox equations)
Day 9-10: Electrolysis (Faraday's laws, calculations, products at electrodes)
Daily: 1 CBT session

Week 9-10: Industrial/Environmental Chemistry + Revision

Day 1-2: Industrial processes (Haber, Contact, Solvay)
Day 3-4: Water treatment, hardness, air pollution
Day 5-6: Environmental chemistry (acid rain, ozone depletion, greenhouse effect)
Day 7-10: Full mock exams daily on SchoolHub, review all weak areas
Target: Consistent 32+/40

Common Chemistry Mistakes in JAMB (and How to Avoid Them)

1. Wrong Molar Mass Calculation

Students add atomic masses incorrectly or forget to multiply for subscripts (e.g., O₂ = 32, not 16). Fix: Write out the formula. List each element with its count. Multiply each by its atomic mass. Sum carefully.

2. Confusing Empirical and Molecular Formulas

The empirical formula is the simplest ratio. The molecular formula is the actual number of atoms. Fix: Empirical formula of glucose = CH₂O. Molecular formula = C₆H₁₂O₆. Molecular formula = n × empirical formula.

3. Forgetting to Convert Temperature to Kelvin

Gas law calculations require absolute temperature. Fix: Always add 273 to Celsius before substituting into PV = nRT or P₁V₁/T₁ = P₂V₂/T₂.

4. Mixing Up Oxidation and Reduction

Fix: OIL RIG: Oxidation Is Loss (of electrons), Reduction Is Gain (of electrons). The substance that is oxidised is the reducing agent. The substance that is reduced is the oxidising agent.

5. Wrong Products in Electrolysis

Students confuse which ions are discharged at which electrode. Fix: Cations (positive ions) go to the cathode (negative electrode). Anions (negative ions) go to the anode (positive electrode). Remember: Cation = Cathode, Anion = Anode.

6. Confusing the Haber and Contact Processes

Students mix up the catalysts and conditions. Fix: Haber process = ammonia, iron catalyst, 450°C, 200 atm. Contact process = sulphuric acid, vanadium pentoxide (V₂O₅) catalyst, 450°C, 1-2 atm.

7. Not Balancing Equations Before Calculations

Stoichiometric calculations from unbalanced equations give wrong answers. Fix: Always balance the equation first. Count atoms on both sides. Only then use mole ratios.

Why SchoolHub Is the Best Platform for JAMB Chemistry Practice

AI-Generated Chemistry Questions

Every session presents fresh Chemistry questions across Physical, Organic, Inorganic, and Environmental Chemistry. You build real understanding rather than memorising past question answers.

Calculation Training

Chemistry requires both knowledge and calculation. SchoolHub's explanations walk you through each step: identify the formula, substitute values, compute the answer.

All Syllabus Areas Covered

From mole calculations to IUPAC naming, from gas laws to electrolysis, every corner of the JAMB Chemistry syllabus is represented.

Timed Practice for Speed

45 seconds per question means you need instant recall of facts and efficient calculation. SchoolHub's timer trains you for this.

Start Free JAMB Chemistry Practice on SchoolHub

Frequently Asked Questions

How many Chemistry questions are in JAMB?

There are 40 Chemistry questions in the JAMB UTME, to be answered within approximately 30 minutes as part of the 2-hour exam. Each question carries 2.5 marks, totalling 100 marks.

Is JAMB Chemistry hard?

JAMB Chemistry is considered one of the harder JAMB subjects because it requires conceptual understanding, mathematical calculations, and memorisation of specific facts. However, the syllabus is predictable. Students who cover all four sections and practise regularly score well.

What topics are most important for JAMB Chemistry?

Physical Chemistry (35%, especially the mole concept and gas laws) and Organic Chemistry (30%, especially IUPAC naming and reactions of hydrocarbons/alcohols/acids) together make up about two-thirds of the paper. See the full breakdown above.

Do I need to memorise the periodic table for JAMB?

You do not need to memorise the entire table, but you must know the symbols, atomic numbers, and relative atomic masses of the 20 most common elements (see the table in this article). You should also know periodic trends (atomic radius, ionisation energy, electronegativity).

How do I solve mole calculation questions?

Always start by finding the molar mass. Then use the appropriate formula: moles = mass/molar mass (for solids), moles = volume/22.4 (for gases at STP), or moles = concentration × volume (for solutions). Use the balanced equation to find mole ratios between reactants and products.

What is the best app to practise JAMB Chemistry?

SchoolHub JAMB CBT Practice offers AI-generated Chemistry questions covering all four syllabus sections, timed sessions matching the real exam format, and detailed step-by-step explanations.

How many hours should I study Chemistry for JAMB daily?

Study 1.5-2 hours daily: 30 minutes on theory (one topic), 30 minutes solving calculation problems, 20 minutes on a CBT session on SchoolHub, and 20 minutes reviewing explanations and memorising key facts.

Are JAMB past questions enough for Chemistry?

Past questions are valuable for understanding patterns, but JAMB introduces new question variations every year, especially in Organic Chemistry. Combining past questions with AI-generated practice on SchoolHub provides the most thorough preparation.

Start Practising JAMB Chemistry Today

Chemistry rewards students who prepare across all three dimensions: concepts, calculations, and memorisation. The candidates who score 35+/40 are not necessarily the smartest. They are the ones who practised the most questions and covered the full syllabus.

Your action plan:

Right now: Visit jamb.schoolhub.tech and take a free Chemistry session
Today: Memorise the relative atomic masses of the 20 common elements listed above
This week: Focus on the mole concept (solve 5 problems daily)
This month: Follow the 10-week study plan above
Exam day: Walk in knowing every formula, every naming rule, and every gas test

Chemistry connects everything in science. Master it, and your other science subjects become easier too.

Practice JAMB Chemistry Free on SchoolHub

Last Updated: September 2026 Written by the SchoolHub Team

JAMB CBT Practice Chemistry: Questions, Tips & Free Practice (2027)