JAMB 2024/2025 Syllabus for Chemistry is Out | Download PDF

JAMB UTME 2024 Chemistry syllabus is out online. It is compiled in a PDF file which can be easily downloaded into a smartphone or laptop for quick access.

Examination Type	UTME / Direct Entry
Examination Year	2024/2025
Syllabus	Chemistry
File Format	PDF
File Size	283KB

Chemistry, the study of matter and its properties, plays a vital role in science and technology. For students aspiring to smash the Joint Admissions and Matriculation Board (JAMB) examination, downloading and reviewing the syllabus is very important.

Consistent revision and practice are key to mastering the JAMB Chemistry Syllabus. Regularly solving problems, practicing chemical calculations, and revisiting key concepts contribute to a deeper understanding of the subject.

Recommended: Check JAMB 2024 Syllabus For All Subjects

Note: Chemistry is not just about theoretical knowledge; candidates should engage in practical applications.

General Objectives

1. understand the basic principles and concepts in chemistry
2. Interpret scientific data relating to chemistry
3. deduce the relationships between chemistry and other sciences
4. apply the knowledge of chemistry to industry and everyday life

JAMB 2024 Syllabus for Chemistry

TOPICS/CONTENTS/NOTES	OBJECTIVES
1. Separation of Mixtures and Purification of Chemical Substances (a) Pure and impure substances (b) Boiling and melting points (c) Elements, compounds and mixtures (d) Chemical and physical changes (e) Separation processes: – Evaporation, simple and fractional distillation, – sublimation, filtration, crystallization, paper and column chromatography, simple and fractional crystallization, magnetization, decantation.	Candidates should be able to: (i) distinguish between pure and impure substances; (ii) use boiling and melting points as criteria for purity of chemical substances; (iii) distinguish between elements, compounds and mixture; (iv) differentiate between chemical and physical changes; (v) identify the properties of the components of a mixture; (vi) specify the principle involved in each separation method; and (vii) apply the basic principle of separation processes in everyday life.
2. Chemical Combination Laws of definite, multiple and reciprocal proportions, law of conservation of matter, Gay Lussac’s law of combining volumes, Avogadro’s law; chemical symbols, formulae, equations and their uses, relative atomic mass based on 12C=12, the mole concept and Avogadro’s number and stoichiometry of reactions.	Candidates should be able to: (i) perform simple calculations involving formulae, equations/chemical composition and the mole concept; (ii) deduce the chemical laws from given expressions/statements/data; (iii) interpret graphical representations related to these laws; and (iv) deduce the stoichiometry of chemical reactions.
3. Kinetic Theory of Matter and Gas Laws (a) Phenomena to support the kinetic theory of matter using: (i) melting, (ii) vapourization (iii) boiling (iv) freezing (v) condensation in terms of molecular motion and Brownian movement. (b) (i) The laws of Boyle, Charles, Graham and Dalton (law of partial pressure); combined gas law, molar volume and atomicity of gases. (ii) The ideal gas equation (PV = nRT). (iii) The relationship between vapour density of gases and the relative molecular mass.	Candidates should be able to: (i) apply the theory to distinguish between solids, liquids and gases; (ii) deduce reasons for change of state; (iii) draw inferences based on molecular motion; (iv) deduce gas laws from given expressions/statements; (v) interpret graphical representations related to these laws; and (vi) perform simple calculations based on these laws, equations and relationships.
4. Atomic Structure and Bonding (a) (i)The concept of atoms, molecules and ions, the works of Dalton, Millikan, Rutherford, Moseley, Thompson and Bohr. (ii) Atomic structure, electron configuration, atomic number, mass number and isotopes; specific examples should be drawn from elements of atomic number 1 to 20. (iii) Shapes of s and p orbitals. (b) The periodic table and periodicity of elements, presentation of the periodic table with a view to recognizing families of elements e.g. alkali metals, halogens, the noble gases and transition metals. The variation of the following properties: ionization energy, ionic radii, electron affinity and electronegativity. (c) Chemical bonding. Electrovalency and covalency, the electron configuration of elements and their tendency to attain the noble gas structure. Hydrogen bonding and metallic bonding as special types of electrovalency and covalency respectively; coordinate bond as a type of covalent bond as illustrated by complexes like [Fe(CN)6] 3- , [Fe(CN)6] 4- , [Cu(NH3)4] 2+and [Ag(NH3)2] + ; van der Waals’ forces should be mentioned as a special type of bonding forces. (d) Shapes of simple molecules: linear ((H2, O2, C12, HCl and CO2), non-linear (H2O), tetrahedral; (CH4) and pyramidal (NH3). (e) Nuclear Chemistry: (i) Radioactivity – Types and properties of radiations (ii) Nuclear reactions. Simple equations, uses and applications of natural and artificial radioactivity.	Candidates should be able to: (i) distinguish between atoms, molecules and ions; (ii) identify the contributions of these scientists to the development of the atomic structure; (iii) deduce the number of protons, neutrons and electrons from atomic and mass numbers of an atom; (iv) apply the rules guiding the arrangement of electrons in an atom; (v) identify common elements exhibiting isotopy; (vi) relate isotopy to mass number; (vii) perform simple calculations relating to isotopy; (viii) differentiate between the shapes of the orbitals; (ix) determine the number of electrons in s and p atomic orbitals; (x) relate atomic number to the position of an element on the periodic table; (xi) relate properties of groups of elements on the periodic table; (xii) identify reasons for variation in properties across the period and down the groups; (xiii) differentiate between the different types of bonding; (xiv) deduce bond types based on electron configurations; (xv) relate the nature of bonding to properties of compounds; (xvi) differentiate between the various shapes of molecules; xvii) distinguish between ordinary chemical reaction and nuclear reaction; (xviii) differentiate between natural and artificial radioactivity; (xix) compare the properties of the different types of nuclear radiations; (xx) compute simple calculations on the half-life of a radioactive material; (xxi) balance simple nuclear equation; and (xxii) identify the various applications of radioactivity.

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Aspiring students should embrace the Chemistry syllabus as a valuable tool for success in the forthcoming UTME, aligning their efforts with the examination requirements.

By understanding and mastering the content outlined in this syllabus, candidates can approach the JAMB examination with confidence and excel in their academic pursuits.