HomeJUPEB Syllabus 2026JUPEB Chemistry Syllabus 2026/2027 & Textbooks

JUPEB Chemistry Syllabus 2026/2027 & Textbooks

By February 3, 2026 JUPEB Syllabus 2026 0 Comments

The JUPEB Chemistry Syllabus 2026/2027 is structured into four main courses (CHM 001–004), covering foundational, physical, inorganic, and organic chemistry, along with practical applications. Key areas include atomic structure, stoichiometry, gas laws, thermodynamics, kinetics, equilibrium, s- & d-block elements, organic reaction mechanisms, and functional group chemistry. The syllabus emphasizes conceptual understanding and practical skills required for university admission.

The 2026 JUPEB Chemistry syllabus is critical for science students, as it serves as the official guide for Direct Entry admission into 200-level university courses, including Medicine, Engineering, and Pharmacy. Mastering this curriculum, which covers physical, organic, and Inorganic Chemistry, ensures high scores and foundational knowledge for advanced university studies.

JUPEB Chemistry Syllabus 2026/2027

JUPEB First Semester Courses Chemistry

COURSE CODECOURSE TITLE CREDIT LOAD
CHM001General Chemistry 3 Units
CHM002Physical Chemistry 3 Units

JUPEB FIRST SEMESTER Chemistry SYLLABUS

 JUPEB CHEMISTRY SYLLABUS
SNTOPICSOBJECTIVES
 FIRST SEMESTER
 CHM001: GENERAL CHEMISTRY
1MEASUREMENTSi. Units of measurement
a) Basic S.I. Units,
b) Derived units,
c) Conversion of units,
d) Significant figures,
e) Precision and accuracy,
f) Errors(systematic and random errors), g) Exact numbers
2NATURE OF MATTERi. States of matter
a) Solid, liquid and gaseous states,
b) Properties and inter-conversion.
3ATOMIC MASSESi. Definitions and calculations of molar masses of atoms and molecules based on “C scale,

ii. Use of mass spectrometry in the determination of Relative Atomic Mass and

iii. Relative Molecular mass
4ATOMIC STRUCTUREi. Dalton’s atomic theory.

ii. Discovery of sub-atomic particles
a) Various experiments that led to the discovery of neutrons, protons,
b) Electrons and nucleus (cathode ray,
c) Millikan’s oil drop,
d) Rutherford’s and Thompson’s experiments),
e) Calculations of relative abundances and isotopic mass;

iii. Planck’s Theory
a) Black body radiation,
b) Photoelectric effect,
c) Quantisation of energy;

iv. Bohr’s Theory
a) Bohr’s assumption,
b) Atomic spectra of hydrogen(no derivation is required) and
c) Determination of spectra lines, determination of ionisation energy from line spectra(when n=0);

v. Wave Theory of Atoms
a) Particle wave duality,
b) Atomic orbitals,
c) Quantum numbers(n,l,m,s),
d) Electronic ener levels,
e) Degeneracy of atomic orbitals,
f) Shapes of atomie orbitals(s,p and id orbitals)

vi. Electronic configuration of Atoms and ions
a) Aufbau principle,
b) Pauli’s exclusion principle,
c) Hund’s rule, (n+1) rule
5PERIODICITYi. Development of the modem periodic table,

ii. Building up periods,

iii. Atomic properties
a) Identifying blocks and groups of elements,
b) Periodic law.
c) Trends of atomic size,
d) Ionisation potential,
e) Electron affinity,
f) Electronegativity a and ionic radii,
g) Isoelectric species.
6MOLE CONCEPTi. Mole and Avogadro’s constant
a) Various ways of defining the molt,
b) Avogadro’s constant, molar mass.

ii. Empirical and molecular formula
a) Definition and calculations of Empirical and Molecular formulae from percentage composition by mass and combustion data.

iii. Solution Stoichiometry
a) Balancing chemical equations, calculations based on stoichiometric coefficients,
b) Reaction that involve limiting reactants,
c) Calculation of actual and percentage yields.
d) Calculation of molarity and gram concentration,
e) Preparation of standard solutions, serial dilution.
7TYPES OF CHEMICAL REACTIONSi. Neutralization
a) Definition identification of neutralization reactions.
b) Predicting solubilities.

ii. Precipitation, Oxidation and Reduction
a) Various definitions of oxidation and reduction reaction with emphasis on definition of terms of electron transfer,
b) Calculation of oxidation numbers, balancing of redox reactions by oxidation state and half-reaction method (both in acidic and basic media). OM
8CHEMICAL BONDINGi. Electrovalent/Ionic Bonding
a) Describe ionic bending using some ionic compounds e.g. NaCl,
b) Energy considerations of ionic bonding, definition of lattice energy (no derivation), properties of ionic compounds.

ii. Covalent Bonding
a) Describe covalent bonding using simple covalent compounds e,g, CO₂,
b) Coordinate/dative covalent bonding e.g. in ammonium ion (NH4), Al,Cl,
c) Molecule, bond energy, bond length and bond polarity(Fajan’s rule),
d) Properties of covalent compounds, hybridisation concept (sp, sp sp²),
e) Shapes of simple molecules using the valence shell electron-pair repulsion theory eg. H₂O, NH, CH, etc.

iii. Intermolecular Bonding
a) Van der waals forces,
b) Permanent and induced dipoles,
c) Hydrogen bonding.

iv. Metallic Bonding
a) Describe metallic bonding in terms of a lattice of positive ions surrounded by delocalised electrons.

v. Bonding and physical properties
a) The effect of different types of bonding on the physical properties of substances (e.g. unusual high boiling point of water, miscibile of water and ethanol, nylon, polyester).
 CHM002: PHYSICAL CHEMISTRY
9KINETIC MOLECULAR THEORY OF GASESi. Gas Laws
a) Statement of and calculations involving Boyle’s, Charles’, Dalton’s, Graham’s laws and Avogadro’s hypothesis.

ii. Ideal and Real Gases
a) Ideal gas equations,
b) Kinetic theory of gases (assumptions only),
c) Real gases deviation from ideal gas behaviour,
d) Van der Waal’s equation.
e) Use of the general gus equation. PV=nRT in calculations, including relative molecular mass determination
10SOLUTIONi. Phase and phase diagram
a) Interpretation of phase diagram for one component system.

ii. Ideal and non-ideal solutions
a) Definition of ideal and non-ideal solutions, Raoult’s Law

iii. Colligative Properties
a) Lowering of vapour pressure,
b) Depression of freezing,
c) Elevation of boiling point and osmotic pressure.
d) Determination of molar mass using osmotic pressure. (The derivation not required).
11THERMOCHEMISTRYi. Enthalpy change
a) Exothermic and endothermic changes,
b) Definition of enthalpy changes for processes (combustion, neutralization, hydration, formation, solution, atomization) under standard condition.

ii. Hess’ Law
a) State Hess’ law and construct energy cycles based on Hess’ law and carry out calculations based on Hess’ law
b) Use of bond energy to calculate energy changes.

iii. Introduction to Chemical Thermodynamics
a) Definition of entropy and Gibbs’s free energy.
b) Calculation of entropy change
c) Calculation of Gibb’s free energy change for reactions using AG AH-TAS.
d) Predicting the spontaneity of reactions
12ELECTROCHEMISTRYi. Electrolysis
a) Faraday’s first and second laws of electrolysis and calculations based on them.

ii. Electrochemical Cells
a) Identify the substances liberated during electrolysis based on the state of electrolyte,
b) Position in electrochemical series
c) Concentration of electrolyte and
d) Nature of electrodes

iii. Fuel Cells and Batteries
a) Definitions of electrode potential standard electrode potential,
b) Cell potential Calculations of e.m.f of a cell
c) Application of Nernst equation
d) Use of cell potential to predict the feasibility of reaction Industrial uses of electrolysis.

iv. H/O₂ fuel cell,

v. Rechargeable batteries
13CHEMICAL KINETICSi. Rate Equation
a) Definition of rate of reaction and reaction mechanism.
b) Factors affecting rate of reaction.
c) Orders of reaction, rate constants and molecularity.
d) Calculations of order of reaction from experimental date

ii. Activation Energy Catalysis
a) Simple collision theory.
b) Definition of activation energy.
c) Arrhenius equation.
d) Homogeneous and Heterogeneous catalysis
14EQUILIBRIUM STATEi. Mass Action
a) Equilibrium changes, reaction quotient (Q), equilibrium expressions (homogenous and heterogeneous equilibra).
b) Calculations of equilibrium constants in terms of concentration (K) and partial
pressure (K).
c) Relationship between Ke and K

ii. Le-Chatelier’s Principle
a) Statement and Application of Le- Chatelier’s principle to deduce the effects of changes in temperature, pressure and concentration on a system at equilibrium.
b) Definitions of acid and base in terms of; Arrhenius, Bronsted- Lowry and Lewis concept. Auto-ionisation of water.

iii. Acid-Base Equilibra
a) Acid strengths, pH solution.
b) Indicator theory
c) Solubility product, common ion effect.
d) Selective precipitation of ions.

iv. Ionic Equilibra in Aqueous System Radioactivity
15NUCLEAR CHEMISTRYI. Radioactivity
a) History of Radioactivity.
b) Types of radiations.
c) Radioactive disintegration.
d) Nuclear equations, half-life, radioactive carbon
e) Detectors and applications of radioactivity.

CHM001 Practicals

  1. Measurement and Accuracy
    Sensitivity of weighing equipment; graduation of measuring instruments; and determination of significant figures in measurements and readings.
  2. Preparation of Standard Solutions
    Preparation of standard solutions, including serial dilution techniques.
  3. Volumetric Analysis
    Practical work in volumetric analysis, including:
    • Acid–base titrations
    • Redox titrations
    • Precipitation titrations
    • Acid–base titrimetry involving NaOH, oxalic acid, HCl, Na₂CO₃
    • Determination of percentage composition of iron using KMnO₄ (redox titrimetry)
    • Titrimetric analysis of mixtures such as NaOH/NaHCO₃ and Na₂CO₃/NaHCO₃
  4. Statistical Analysis of Experimental Data
    Introduction to statistical analysis of data using supplied data to illustrate elements of simple statistics.

CHM 002 Practicals

  • Calorimetric Experiments
  • Experiments designed to calculate enthalpy changes of reactions, including enthalpy of neutralization, solution, and displacement using calorimetric methods.
  • Determination of Molecular Mass
  • Determination of the molecular mass of substances using freezing point depression (cryoscopic method).

JUPEB Second Semester Courses for Chemistry

COURSE CODECOURSE TITLECREDIT LOAD 
CHM003Inorganic Chemistry 3 Units
CHM004Organic Chemistry  3 Units

JUPEB SECOND SEMESTER Chemistry SYLLABUS

 SECOND SEMESTER
 CHM003: INORGANIC CHEMISTRY
16PERIODICITY OF ELEMENTSi. General trends in properties of elements
a) Nature of elements, trends, in physical and chemical properties of elements
17CHEMISTRY OF HYDROGENi. Occurrence, isotopes, preparation and reactions of hydrides
18S-BLOCK ELEMENTSi. Group 1
a) Physical and chemical properties, extraction of group 1 metals e.g Sodium, trends in properties of their compounds.
b) Uses of group 1 metals.

ii. Group 2
a)Physical and chemical properties, extraction of group 2 metals e.g Calcium, trends in properties of their compounds. b) Uses of group 2 metals
19P-BLOCK ELEMENTSI. Group 13
a) Boron and Aluminium.
b) Occurrence and extraction, trends in properties of their compounds with oxygen, chlorine and hydrogen.

ii. Group 14
a) Occurrence, allotropic forms, physical and chemical properties, trends in properties of oxides, hydrides, halides.
b) Greenhouse effect,
c) Uses of group 14 elements.

iii. Group 15
a) Occurrence, allotropic forms, physical and chemical properties, simple oxides and nitrides, environmental impacts of NOx.
b) Uses of group 15 elements.

iv. Group 16
a) Occurrence, allotropic forms, physical and chemical properties, trends in properties of oxides, hydrides and halides. Environmental impact of SOx. Uses of group 16 elements.

v. Group 17
a) Occurrence, physical and chemical properties, hydrogen halides, metal halides and inter-halogen compounds.
b) Uses of group 17 elements
20D-BLOCK ELEMENTSi. First Row Transition Elements
a) Definition of transition element, electronic configuration, atomie radii, ionization potential, variable oxidation states, formation of metal complex.

ii. Introduction to Coordination Chemistry
a) Definition of metal complex and ligands, types of ligands. Bonding in metal complexes (chain theory and its limitations, Werner’s theory).
b) Valence bond theory and hybridization concept.
c) Study of structure and magnetic properties of octahedral and tetrahedral complexes.
d) Nomenclature of coordination compounds.
 CHM004: ORGANIC CHEMISTRY
21STRUCTURE AND BONDING IN ORGANIC COMPOUNDSi. Hybridization
a) Tetravalency and -hybridization of carbon

ii. Classes of carbon compounds
a) Functional groups, homologous series,
b) Determination of molecular formula from empirical formula.

iii. Nomenclature
a) Naming of organic compounds: alkanes, alkenes, alkynes, aldehydes, ketones, alcohols, alkyl halides, arenes, carboxylic acids, amines
22PURIFICATIONi. Purification of organic compounds
a) Determination of melting point, crystallization and recrystallization, simple distillation, liquid extraction, sublimation

ii. Determination of elements
a) Various methods of determining C,H, N, S and halogens in organic compounds.
b) Sodium fusion test.
23ORGANIC REACTIONSi. Covalent bond cleavage
Homolytic and heterolytic fission, free radical reaction Nucleophiles and electrophiles

ii. Types of Reactions
a) Addition, Substitution, Elimination, Hydrolysis, Condensation. COM

iii. Electronic concepts in organic chemistry
a) Inductive, steric electrometric effects.
24ISOMERISM IN ORGANIC COMPOUNDSi. Constitutional, chain, position, and functional groupgroup isomerism.

ii. Tautomerism, Stereoisomerism.

iii. Geometrical and optical
25ORGANIC COMPOUNDSi. Alkanes, alkanes, and alkanes
Nomenclature, structure, synthesis, properties and reactionsii. Alcohols
Nomenclature, structure, synthesis, properties and reactions(combustion, substitution to give halogenoalkanes, reaction with Na, oxidation to carbonyl compounds and carboxylic acids, dehydration to alkenes, formation of esters by esterification with carboxylic acids and acyl chlorides). Classes of alcohols.
Distinguishing tests for alcohols (Lucas and Jones reagents)iv. Alkylhalides
Nomenclature, structure, synthesis, properties and reactionsv. Carbonyl compounds (Aliphatic and Aromatic)
Nomenclature, structure, synthesis, properties and reactions ( reduction, reaction with HCN, NACN, reaction with acqueous I2.
Tests for aldehydes and ketones using 2,4-dinitrophenylhydrazin4-dinitrophenylhydrazin.vi. Carboxylic compounds and their derivatives
a) Nomenclature, properties, preparation from alcohols, aldehydes, and nitrites
b) Reactions of carboxylic acids with reactive metals, reduction to alcohol using LiAlH6vii. Primary Amines
a) Hydrolysis of esters by acid and base.
b) Hydrolysis of acylchlorides
c) Preparation of alkylamines.
d) Basicity of amines in terms of their structure.
e) Reactions of amines (formation of diazonium salt) Aromaticity, Kekule structuresviiI. Introduction to aromatic compounds
26MACROMOLECULESi. Carbohydrates
a) Classes of carbohydrates.
b) Simple tests

ii. Proteins
a) Amino acids, formation of peptide bonds in peptides.
b) Simple description of electrophoresis.

iii. Polymers
a) Types of polymerization reactions and their differences.
b) Simple structures of polymers.
c) Uses of polymers
27BIOTECHNOLOGYi. Biotechnology and it’s application in food and drugs
28PETROLEUM INDUSTRYi. Constituents of crude oil, refining, cracking.

ii. Chemicals derived from crude oil.

CHM 003 PRACTICALS

  1. Flame Tests and Analysis of Mixtures
    Flame tests and systematic qualitative analysis of mixtures containing two inorganic salts.
  2. Identification of Anions
    Preliminary tests for anions; preparation of sodium carbonate (Na₂CO₃) extracts; and confirmatory tests for common anions.
  3. Identification of Cations (Groups I–VI)
    Group separation and qualitative analysis of cations using systematic group analysis, including identification of ions within each group.

CHM 004 PRACTICALS

  1. Reactions of Simple Functional Groups
    Simple organic qualitative tests, including solubility tests, sodium fusion (Lassaigne’s) test, and functional group identification, with emphasis on aldehydes, ketones, and carboxylic acids (excluding carboxylic acid derivatives).
  2. Purification and Characterisation of Organic Compounds
    Recrystallization of organic compounds and determination of melting points.

JUPEB Chemistry Textbooks 2026/2027

1. E. N. Ramsden: A-Level Chemistry, 4th Edition (2000). Stanley Thornes (Pub) Ltd. ISBN 0748752994.

2. Phillips Mathews: Advanced Level Chemistry.

3. Basic Organic Chemistry by B. A. Osuntogun, O. B. Familoni, and B.1.Alo; 3rd Edition (2012) University to Lagos Press.

4. Chemistry by Ted Lister and Janet Renshaw (2009)Nelson Thornes Ltd. (Pub).

5. Understanding Advanced Physical Inorganic Chemistry: The Learner’s Approach. by Jeanne Tan, Kim Seng Chan (2009) World Scientific (Pub).

6. Chemistry: The Central Science by Theodore E. Brown, Theodor Lawrence Brown, H. Eugene H. LeMay, Bruce E. Burster Catherine Murphy, Patrick Woodward 12th Edition (2012) Pearson Education (Pub.).

7. Martins S. Silverberg (2010). Principles of General Chemia Second edition. McGraw Hill Publishers. New York.

8. University General Chemistry, Inorganic and Physical. YO Wong, C.T. Wong, S.O. Onyiruka and L.E.S Akpanisi. Africana FEP Publishers Ltd (2002).

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