2023–2024 JAMB Physics, chemistry,maths, Syllabus
Table of Contents for the UTME Physics Syllabus for 2023 and 2024.
General Objective of the Jamb Physics Syllabus for 2023–2024
Jamb Physics Syllabus for 2023–2024
Unit & Measurement
Vectors and Scalars
The gravitational field
Work Power and Energy
Friction, Simple Machines, and
Temperature and Its Measurement
Liquids at Rest
Heat Quantity; 16. State Change
. Kinetic Theory and Structure of Matter
Sound Wave Propagation, Chapter
Components of Sound Waves, Number
Light Refraction at Curved and Planar Surfaces
Light Refraction Through
Electricity in use now
Electrical power and energy
Magnetic fields and magnets
Pressure on a Conductor Carrying Current
Simple AC Circuits, Chapter
Electricity Conduction Through
Basic Modern Physics
Recommended Textbook for the Jamb Physics Syllabus
2023–2024 JAMB Physics Syllabus for the UTME.
This article is all about the most recent physics syllabus for the Jamb. First, what exactly is a syllabus? A syllabus is a written summary of all the material that will be covered in a class or during an exam. To prepare for the Unified Tertiary Matriculation Examination, students must read the Jamb Syllabus, which is a collection of specified topics.
Jamb Physics Syllabus: If you are preparing for the Joint Admission Matriculation Board’s Unified Tertiary Matriculation Examination, then you have nothing to lose. With the exception of expos, Newsedung.com will offer all the guides required to enable the student pass with flying colors.
This page is for you if you’re taking the upcoming UTME (Unified Tertiary Matriculation Examination) and require the Jamb Physics outlines topic to read in order to prepare for the Jamb Examination;
How to prepare for the 2023/2024 Jamb Exam;
selecting a course
conduct research on the subject.
Look up the course’s O-level requirements.
Finally, check the Jamb subject combination for the course you want to enroll in; if Physics is one of the options, you can start studying.
2023–2024 Jamb Physics Syllabus broader purpose
The Unified Tertiary Matriculation Examination (UTME) Physics syllabus’s purpose is to get candidates ready for the Board exam. It is intended to gauge how well they accomplished the course’s goals, which are to: (1) maintain their interest in physics;
(2) adopt a physics-related attitude that values precision, objectivity, and accuracy; (3) evaluate physical phenomena, laws, definitions, and other theories; and (4) show the capacity to appropriately solve physics problems utilizing pertinent theories and concepts.
Jamb Physics Syllabus for 2023–2024
- Measuring and Units (a) Length, area, and volume: Venier calipers and the metre rule Micrometer Screw-guage
(a) Mass: I the mass unit; (ii) the use of a basic beam balance
(c) Time: I the time unit (ii) the time-measuring tools
(d) Foundational physical constants
physical quantities derived from them and their units (e)
I The combination of basic quantities and the establishment of their units
Dimensions (f) Dimensions definition I
basic examples in (ii).
(g) Experimental measurement restrictions
(1) The precision of measuring devices (2) Easy estimation of mistakes
Significant figures, part (iii).
standard form (iv).
- Definition of scalar and vector quantities, examples of scalar and vector quantities, relative velocity, resolution of vectors into two perpendicular directions, and graphical techniques of solution.
- Motion (a) Different types of motion, include random, oscillatory, rotational, and translational
I speed, velocity, and acceleration (b) linear motion
Equations of uniformly accelerated motion (ii), motion under gravity (iii), and velocity (iv) are all included. Instantaneous velocity and acceleration on a time graph (v).
c) Projectiles: I applications of projectile motion; (ii) computation of range, maximum height, and time of fight
I Inertia, mass, and force are three of Newton’s laws of motion.
mass-acceleration relationship (ii) and the link between momentum and impulse (iii)
(iv) linear momentum conservation (Coefficient of restitution not necessary)
(e) Circular motion: I angular acceleration and angular velocity
centrifugal and centripetal forces are (ii).
Simple Harmonic Motion (S.H.M.) is discussed in Section f. Examples of systems that use S.H.M. are provided in Sections I and II.
(iii) the S.H.M.’s period frequency and amplitude (iv) its velocity and acceleration
(v) a shift in S.H.M.’s energy
- The gravitational field is composed of the following components: I Newton’s law of universal gravitation (ii) gravitational potential (iii) conservative and non-conservative fields (iv) acceleration due to gravity (g=GM/R) (v) the distinction between mass and weight (vi) escape velocity (vii) parking orbit and weightlessness
- Force Equilibrium
(A) particle equilibrium:
Coplanar force equilibrium is the first.
triangles and the forces polygon
Lami’s Theorem (iii)
(b) Moments’ guiding principles
I the force’s moment
(ii) a straightforward procedure and a couple’s (torgue) moment (iii) applications
(c) requirements for rigid body equilibrium when parallel and non-parallel forces are at work:
Resolution of forces in two perpendicular directions, composition of such forces, and resultant and equilibrant
I stable, unstable, and neutral equilibrium (d) center of gravity and stability
- Work Energy and Power: Definition, Types of Energy, Conservation of Energy, Qualitative Treatment of Various Types of Energy, and Interpretation of Area Under Force Distance Curve
I Friction, both static and dynamic
(ii) the calculation of the limiting friction coefficient.
The benefits and drawbacks of friction
(iv) a decrease in friction
(v) a qualitative analysis of terminal viscosity and viscosity.
Stoke’s law is number seven.
- Simple Machines I Machine Types (ii) Definition of a Machine
(iii) machine efficiency, machine velocity ratio, and mechanical advantage
- The spring balance as a tool for measuring force. The work done in springs and elastic strings. The elastic limit, yield point, breaking point, Hooke’s law, and Young’s modulus.
A definition of atmospheric pressure can be found at I
(ii) Pressure (S.I.) unit measurements
(iii) measuring pressure (iv) using a manometer, an aneroid barometer, and a simple mercury barometer.
(V) Pressure changes with altitude (VI) Using a barometer as an altimeter
I The relationship between pressure, depth, and density (P = gh) in liquids
(ii) Pascal’s Principle: Pressure Transmission in Liquids
- Liquids at Rest Definition of relative density and measurement of solid and liquid densities
(iii) upthrust on a body submerged in a liquid (iv) the law of flotation and principle of Archimedes, as well as applications, such as ships and hydrometers.
- Measurement of temperature
Thermometric qualities and the idea of temperature
(iii) thermometer calibration (iv) the Celsius and Kelvin temperature scales
(v) Thermometer kinds
(vi) changing the scale used to measure temperature.
- Thermal Expansion Solids: I linear, volumetric, and area expansivities definition and determination
Effects and applications, such as the expansion of railroad tracks and building strips
Relationship between several expansivities (iii)
(iv) unusual water expansion
Boyle’s law (PV = constant) is one of the gas laws.
Charle’s law (V/P = constant) (ii)
(iii) The law of pressure (P/T = 1).
(iv) Temperature at absolute zero (v) Ideal gas equation (Pv = nRT) and universal gas equation (PV/T = constant)
- Quantity of Heat I meaning of the term “heat capacity” (ii) and “specific heat capacity of solids and liquids”
(iii) calculating the heat capacity and specific heat capacity of substances using straightforward techniques, such as the mixtures approach and the electrical method.
Change of State 16.
Latent heat, specific latent heats of fusion and vaporization, melting, evaporation, and boiling, and the effects of pressure and dissolved compounds on boiling and melting temperatures are all covered in this section.
Application to appliances (v)
- Relationship between boiling and saturated vapour pressure (S.V.P.) and unsaturated and saturated vapours
(iii) using a barometer tube to determine S.V.P
(iv) how dew, mist, fog, and rain form (v) how humidity and relative humidity are studied (vi) how hygrometry, or measuring the humidity of the air using wet and dry bulb hygrometers, works.
- Kinetic Theory and the Structure of Matter (a) Atomic and molecular structure
(ii) The molecular theory, which explains concepts like Brownian motion, surface tension, capillarity, adhesion, and angles of contact; (iii) examples and applications.
b) The kinetic theory, which includes the following concepts: Boyle’s law, Charles’ law, and the assumptions underlying the theory
melting, boiling, vapourization, evaporation due to a change in temperature, etc.
Heat Transfer 19.
I Heat transport modes: conduction, convention, and radiation
(ii) Heat flux, thermal conductivity, and temperature gradient
(iii) The impact of the surface’s makeup on the energy it emits and absorbs.
The conductivities of typical materials are item (iv).
Thermos flask (v)
(vii) the sea and land breeze
- Production and Propagation of Waves (a) Wave Motion,
(ii) the use of vibrating systems as wave sources
Waves as a method of transferring energy
(V=f) Relationship between frequency, wavelength, and wave velocity. (iv) Distinction between particle motion and wave motion.
phase difference in (vi) (vii) Equation for a progressive wave, such as y = A sin 2/(vt + x)
(b) Classification: I Mechanical and electromagnetic waves are examples of wave types
Transverse and longitudinal waves make up (ii)
(iii) Examples of waves made by springs, ropes, stretched strings, and the ripple tank (iii); and (iv) stationary and progressing waves.
(c) Qualities or Properties:
I plane, reflection, refraction, and diffraction Polarization
(ii) wave superposition, such as interference
- Sound Wave Propagation I The Need for a Material Medium (ii) The Sound Speed in Solids, Liquids, and Air;
Sound reflection, echoes, reverberation, and their uses (iii)
(iv) Reverberations and echos have drawbacks
- Qualities, pitch, intensity, and loudness of sound waves, as well as their use in musical instruments; I noise and musical notes; and (ii) quality, pitch, and loudness;
Simple overtone treatment for strings and their columns that are vibrating
(iv) Acoustic resonance instances (v) frequency of a note produced by air columns in closed and open pipes in relation to their lengths. Fo= 1/2L Square root T/M.
- Light Energy (a) Source of Light: I Sources of Light, both Natural and Artificial
Light-emitting and non-light-emitting things
(a) Light propagation: I light’s velocity, frequency, and wavelength (ii) shadow formation and eclipse (iii) the pin-hole camera.
- Light Refraction at Curved and Planar Surfaces
laws of reflection, in I
Utilizing light reflection in (ii)
(iii) image generation using ray diagrams, concave, convex, and plane mirrors
Utilizing the mirror formula, l/F = I/U + I/V, and linear magnification, respectively
- Refraction of Light Through (a) Plane and Curved Surface: I Refraction explained in terms of light’s velocity in the medium.
(ii) Refraction laws
Definition of a medium’s refractive index (iii) Snell’s law is used to calculate the refractive indices of liquid and glass (iv).
(v) (vi) Critical angle and total internal reflection, real and apparent depth, and lateral displacement
(b) Glass Prism: I application of the formula for the smallest deviation, u=sin A+D/2 / A/2.
(ii) Lenses’ kind
use of the lens formula (iii)
Magnification formula: l = l + l f u v (iv)
I The principles governing microscopes, telescopes, projectors, cameras, and the human eye (physiological details of the eye are not required)
(ii) A lens’s power
Near and far points, angular magnification, sight impairments and how to fix them, and iii) angular magnification
- (a) Light and color diffraction I White light diffraction through a triangular prism (ii) Production of pure spectrum
(iii) adding and subtracting colors to create different hues (iv) using color filters and the color of things
(a) The electromagnetic spectrum I provides a description of the sources and applications of distinct radiation types.
- Charges in matter can be positive or negative. Charges can be applied to a body through friction, contact, and induction.
Electroscope, Coulomb’s inverse square law, electric field, and potential are all included in this list.
(vi) electric discharge and lightning (v) electric field and potential
- Parallel plate capacitors I functions of capacitors (ii)
(iii) A capacitor’s capacitance (iii) (iv) the connection between capacitance, the distance between the plates’ surfaces, and the medium between the plates. C = 3A/d (v) capacitors connected in series and parallel (vi) capacitor energy
Electric Cells: I Daniel and Leclanche cells; (ii) the simple voltaic cell and its flaws (wet and dry)
Lead-acid accumulator, Nickel-Iron (Nife), Lithium, and Cadmium are included in group (iii) (iv) Battery and cell maintenance (detailed cell chemistry treatment is not necessary) (v) cell arrangement
- Current Electricity includes the following concepts: I electromagnetic force (emf), potential difference (p.d.), current, internal resistance of a cell, and lost Volt (ii) Ohm’s law.
(iii) resistance measurement
(iv) The potentiometer method of measuring emf, current, and internal resistance of a cell (v), resistance in series and in parallel and their combination (vi), and meter bridge are all examples of resistance.
Electrical power and energy
I. Electrical energy and power principles II. Commercial electric energy and power units
Transmission of electric power (iii) and the heating effects of electric current (iv).
- Natural and manmade magnets, as well as the magnetic characteristics of soft iron and steel
(iii) Magnetization and demagnetization processes
(iv) The magnetic field notion
(vi) the magnetic field surrounding a solenoid, a circular wire, and a straight conductor conveying current (v)
(vii) the magnetic field’s characteristics, including its north and south poles, magnetic meridian, angle of dip, and declination
Applications of the earth’s magnetic field in navigation and mineral exploration are discussed in (viii) flux and flux density, (ix) change in magnetic field strength throughout the earth’s surface, and (x).
The force on a current-carrying conductor in a magnetic field is 34.
I Quantitative analysis of the force between two parallel wires carrying current
the d. c. motor, the force on a charge moving in a magnetic field, the carbon microphone, the electromagnets, the moving coil, and the moving iron instruments.
(vii) employing shunts and multipliers to convert galvanometers to ammeters and voltmeters
- (a) Faraday’s laws of electromagnetic induction I factors affecting induced emf (ii) electromagnetic induction
Lenz’s law as an example of the energy-conservation concept (iii); a.c. and d.c. generators; transformers; and (iv); the induction coil
I An explanation of inductance in (b)
(ii) Inductance unit
Energy held in inductors (iii) Applications and uses of inductors (iv)
(c) Eddy Current: I eddy current reduction (ii) eddy current applications
- Simple AC Circuits I Definitions of AC Current and Voltage (ii) Peak and RMS Values
(iii) An a.c. source coupled with a resistor; (iv) An a.c. source coupled with a capacitive reactance capacitor
a.c. source coupled with an inductor and an inductive reactance (v)
(vii) Vector diagram (viii) Alternative reactance and impedance values (ix) Effective voltage in an R-L-C circuit (x) Resonance frequency and resonance
- Electricity Conduction By way of (a) liquids:
I Non-electrolytes and Electrolytes
(ii) Electrolysis idea
(iii) The electrolysis of Faraday’s law
(iv) using electrolysis for things like electroplating and ammeter calibration.
I release through gas (quantitative treatment only)
Application of electrical conduction through gases
- Elementary modern physics I atomic models and their limits (ii) atomic structure in its simplest form;
Energy levels and spectra, thermionic emissions, photoelectric effects, Einstein’s equation, stopping potential, and applications of thermionic emissions and photoelectric effects are all covered in this section.
(vii) a straightforward x-ray production technique
(viii) alpha, beta, and gamma ray characteristics and uses
Half-life and decay constant are in (xiii).
simple concepts for fusion and fission energy generation (xiv); binding energy, mass defect, and Einstein’s energy equation (xv); (xvi) Particle-wave paradox (duality of matter)
The uncertainty principle (xviii), electron diffraction (xvii), and
- Introductory Electronics: I distinguishing between metals, semiconductors, and insulators; (ii) intrinsic and extrinsic semi-conductors;
(iii) applications of semiconductors, diodes, and transistors in rectification and amplification (iv) n- and p-type semiconductors (v) rudimentary understanding of transistors and diodes (vi) applications of semiconductors, diodes, and transistors in rectification and amplification.
Recommended Textbook for the Jamb Physics Syllabus
Ogunkoya O. and Olumuyionwa A (1992). Physics Comprehensive Certificate, University Press Plc., Ibadan.
Ike, E. E (2006). Fundamental Physics Principles, Aba Enic Publishers
Ike, E. E (2005). Mathematics and Physics: Numerical Issues and Solutions, F = Ma Enic Publishers, Aba
M. Nelkon (1977). Fundamentals of Physics, Hart-Davis Educational, Great Britain.
M. Nelkon and J. Parker (1989). High Level Physics (Sixth Edition),
P. N. Heinemann and M. W. Anyakoha (2000). Lagos Senior Secondary Physics: Pacific Printers
note: if you can endevor to follow this series of studies be sure of success.
FOR CHEMISRTY 2023 JAMB
The Unified Tertiary Matriculation Examination (UTME) Chemistry syllabus’s goal is to get candidates ready for the Board exam. It is intended to gauge how well they have mastered the course’s goals, which are to:
Apply the fundamental tenets of scientific methodology to novel circumstances;
interpreting data from science;
Figure out how chemistry and other sciences are related;
Use your knowledge of chemistry in business and daily life.
Separation of Mixtures and Chemical Substance Purification
Pure and impure materials
c) The melting and boiling points.
(c) Compounds, mixes, and elements
(d) Physical and chemical modifications.
evaporation, simple and fractional distillation, sublimation, filtration, crystallization, paper and column chromatography, and simple and fractional crystallization are examples of separation processes.
Stoichiometry, laws of definite and multiple proportions, the law of conservation of matter, Gay Lussac’s law of combining volumes, Avogadro’s law, chemical symbols, formulae, equations, and their applications, relative atomic mass based on 12C=12, the concept of a mole, and Avogadro’s number are all covered in this course.
Gas law and the Kinetic Theory of Matter (a) An explanation of the kinetic theory of matter, including its discussion of melting, vaporization, and reverse processes. Melting and boiling are explained in terms of molecular motion and Brownian movement.
(b) The combined gas law, molar volume, and atomicity of gases; the laws of Boyle, Charles, Graham, and Dalton (law of partial pressure);
Atomic Bonding and Structure (a) The theories of Dalton, Millikan, Rutherford, Mosely, Thompson, and Bohr concerning atoms, molecules, and ions Simple hydrogen spectra and the ionization of gases serve to highlight the electron’s role as a basic building block of matter.
(ii) Specific examples should be taken from elements with an atomic number between 1 and 20, as well as atomic structure, electron configuration, mass number, and isotopes. Shapes
orbitals, both s and p.
(b) The periodic table and periodicity of elements. The periodic table is presented with an eye toward identifying families of elements, such as alkali metals, halogens, the noble gases, and transition metals. It is important to pay attention to how the following characteristics vary: electron affinity, electronegativity, ionization energy, and ionic radii.
(c) Chemical bonding: The electron configuration of elements, their propensity to adopt the noble gas structure, and their electrovalency and covalency. As special forms of electrovalency and covalency, respectively, hydrogen bonding and metallic bonding should be mentioned. Complexes like [Fe(CN)6]3-, [Fe(CN)6]4-, [Cu(NH3)4]2+, and [Ag(NH3)2]+ serve as examples of coordinate bonds. Van der Waals forces should also be mentioned as a special form of bonding forces.
(d) Simple molecular shapes, including tetrahedral, linear (H2, 02, C12, HCI, and CO2), and non-linear (H2O); (CH4)
e) Radioactivity I Nuclear Chemistry (elementary treatment only)
Nuclear reactions are (ii). simple formulas, applications, and uses for both natural and man-made radioactivity. Air
The common gaseous components, such as nitrogen, oxygen, water vapor, carbon (IV) oxide, and the noble gases (argon and neon), as well as various applications for the noble gases, affect the amount of oxygen in the air. Examples of these include burning phosphorus or employing alkaline pyrogallol.
Water as a solvent, atmospheric gases dissolved in water, and their biological relevance are all included in the water composition by volume. The byproduct of hydrogen combustion is water. contrasting types of water Hardness, both temporary and permanent, and techniques for softening hard water water supplies in the town are purified. the water of hygroscopy, efflorescence, deliquescence, and crystallization. Examples of the substances with these characteristics and their applications.
Unsaturated, saturated, and supersaturated solutions are soluble (a). Simple calculations and conclusions from solubility curves (solubility is defined in terms of mole per dm3).
(b) Oil, paint, and fat solvents, as well as how to use them to get rid of stains.
(c) Suspensions and colloids: Harmattan haze, paints, milk, aerosol spray, and rubber solution are a few examples of suspensions and colloids, respectively.
Acids, Bases, and Salts (a) Overview of general traits and features of acids, bases, and salts. acidity of acids, normal, acidic, basic, and double salts are some examples of acid/base indicators. An object that is an acid
who acts as a proton donor or one whose aqueous solution provides H3O+ions. Examples of naturally occurring organic acids include ethanol, citric, and tartaric acids; alums are double salts; and salts are made through neutralization, precipitation, and the action of acids on metals. Salts of trioxocarbonate (IV) and oxides
(b) Comparing qualitatively the conductances of molar solutions of strong and weak acids and bases, as well as the correlations between conductance, ion concentrations, and relative ion mobilities.
the scales for pH and pOH. pH is expressed as -log[H3O+].
Acid/base titrations are (d).
(e) Salt hydrolysis: A few straightforward examples include NH4C1, AICI3, Na2CO3, and CH3COONa.
The terms “oxidation” and “reduction” refer to the addition or removal of oxygen or hydrogen, respectively.
(b) Reduction, which involves either hydrogen addition or oxygen removal.
c) The transfer of electrons during oxidation and reduction.
Utilizing oxidation numbers is (d). The terms “oxidation” and “reduction” are used interchangeably.
Utilizing oxidation numbers to balance basic equations. Inorganic compound nomenclature according to IUPAC.
Examinations for oxidizing and reducing agents (e).
Electrolytes and non-electrolytes in electrolysis (a). The electrolysis of Faraday’s laws.
(b) Factors impacting the discharge of ions at the electrodes, electrolysis of diluted H2SO4, aqueous CuSO4, CuC12 solution, diluted and concentrated NaC1 solutions, and fused NaC1.
(c) The purification of metals, such as copper, and the creation of elements and compounds, such as A1, Na, O2, and Cl2.
(d) Electrochemical cells: half-cell reactions, electrode potentials, and the redox series (K, Na, Ca, Mg, AI, Zn, Fe, PbII, H, Cu, Hg, Au). only simple computations.
(e) Methods for avoiding corrosion of iron include painting, electroplating, coating with grease or oil, cathodic protection of metals, and corrosion as an electrolytic process.
Energy Charge (a) Energy changes (H) associated with physical and chemical changes: chemicals such as Na, NaOH, K, NH4, and Cl dissolve in or react with water. reactions that are endothermic (+H) and exothermic (-H).
(b) Entropy as an order-disorder phenomenon: basic examples include gas mixing and salt dissolving.
(c) The spontaneity of reactions: The criterion for equilibrium is G0 = 0, while the criterion for spontaneity or non-spontaneity is G higher or less than 0.
Rates of Chemical Reaction (a) A brief discussion of the following variables that can affect a chemical reaction’s rate:
I Temperature, such as when HCI reacts with Na2S2O3 or Mg
(ii) Concentration – For gaseous systems, pressure may be employed as the concentration term. Examples include the reactions between HCl and Na2S2O3, HCl and marble, and the iodine clock reaction.
(iii) Surface area, as in the reaction of marble in I powdered form (ii) lumps of the same mass with HCI.
(iv) Catalyst, such as the breakdown of H2O2 or KCIO3 with or without the presence of MnO2.
(b) Curves of concentration and time.
Activation energy, (c) Arrhenius’ law, the collision theory, and the impact of light on various reactions are treated qualitatively. for instance, halogenating alkanes
A state of equilibrium
Reversible processes and variables controlling the equilibrium state. dynamic stability. The equilibrium constant and the Le Chatelier principle. Simple illustrations are the effect of steam on iron and N2O4 2NO2. There won’t be a computation necessary.
Non-metals and their compounds (a) Hydrogen: It is produced commercially from water gas and petroleum fractions by cracking, and its properties, usage, and detection are tested for in a laboratory.
Chlorine serves as a representative example of a halogen in (b). For example, water purification, bleaching, producing HCl, making plastics, and pesticides are only a few examples of the electrolysis-based industrial preparation, laboratory preparation, and uses of the substance. Preparation and characteristics of hydrogen chloride and hydrochloric acid. Test for chlorides and chlorides.
I Oxygen: Laboratory preparation, characteristics, and usage. (c) Oxygen and Sulfur. manufacture of liquid air for commerce. Oxides: Trioxygen (ozone) as an allotrope, acidic, basic, amphoteric, and neutral, as well as its significance in the atmosphere.
Sulfur’s applications and allotropes are not anticipated to be prepared. Sulphur (IV) oxide is created when SO2 reacts with alkalis. It has certain features and uses. Tetraoxosulphate (VI) acid: commercial synthesis (contact method only), qualities as a dilute acid, an oxidizing and a dehydrating agent, and uses. Trioxosulphate (IV) acid and its salts. The impact of acids on salts of trioxosulphate (IV). Examine for SO42-. Preparation of hydrogen sulfide and its characteristics as a weak acid, a reducing agent, and a precipitating agent. Check for S2
preparation in a lab; production using liquid air; and
(iii) Ammonia: Laboratory and industrial preparations (only for the Haber Process), characteristics, and applications; ammonium salts; oxidation of ammonia to nitrogen (IV) oxide and trioxonitrate (V) acid; and ammonium salts and applications. Examine for NH4+ (iv) Trioxonitrate (V) acid: a lab-made product from ammonia; characteristics and applications. Heat action and applications of trioxonitrate (V) salt. Oxides of nitrogen: Test for NO3- (v): Properties. the cycle of nitrogen.
Carbon: I Allotropes: Applications and Characteristics
(ii) Laboratory preparation, characteristics, and applications of carbon(IV) oxide. Heat-induced changes in trioxocarbonate(IV) salts and a CO32- test
(iii) Carbon(II) oxide: preparation for use in laboratories, characteristics such as how it affects blood, and sources such as charcoal, fire, and exhaust emissions.
(iv) Coal: Various varieties, by-products of the destructive distillation of coal and wood.
Coke: Gasification and applications. Synthesis gas production and applications.
Metallurgy and its compounds
(a) Metals’ general characteristics
Alkali metals, such as sodium
I Production of sodium hydroxide through brine electrolysis and its impact on lead, zinc, and aluminum ions metallic hydroxides to precipitate, among other uses.
(ii) Sodium trioxocarbonate (IV) and sodium hydrogen trioxocarbonate (IV): Solvay method production, characteristics, and applications, such as Na2CO3 in glassmaking.
(iii) Sodium chloride: its presence in seawater, applications, the value of seawater economically, and sodium chloride recovery.
(c) Alkaline-earth metals, including calcium and its oxides, hydroxides, and trioxocarbonates (IV);
features and applications. preparation of calcium oxide from seashells, cement’s chemical makeup, and mortar’s settling. Make a Ca2+ test.
Aluminum (d) Bauxite purification, electrolytic extraction, characteristics, and applications of aluminum and its compounds Examine for A13+
Extraction of tin from its ore (e). features and applications.
f) The first transition series of metals. distinctive qualities:
oxidation states and electron configuration
Complex ion formation (iii)
(iv) Colored ion production (v) catalysis
(g) Iron The process of extracting iron from sulphide and oxide ores, its characteristics and applications, its various forms and features, and the benefits of steel over iron. Fe2+ and Fe3+ tests
Copper (h) Copper’s extraction from sulphide and oxide ores, characteristics, and applications. Prepared copper (II) tetraoxosulphate and its applications (VI). Alloy steel, stainless steel, brass, bronze, type-metal, duralumin, soft solder, permallory, and alnico are among the materials tested for Cu2+ (constituents and uses only).
the determination of the empirical formula for each class of the organic compounds listed below, as well as an introduction to the tetravalency of carbon, the general formula, and IUPAC nomenclature.
I Alkanes Homologous series with respect to physical attributes, substitution reaction, and a few illustrations and usage of halogenated products. a) Aliphatic hydrocarbons. Isomerism: only structural (examples on isomerism should not go beyond six carbon atoms). Petroleum: constitution, principal products, fractional distillation, cracking, and reforming Petrochemicals: the raw materials for organic synthesis, the characteristics of gasoline, and the significance of the octane number (ii) Alkenes Isomerism: Polythene, added and polymerization processes, structural and geometric isomerism
and synthetic rubber as examples of polymerization-produced goods and their application in vulcanization.
(iii) Alkynes Ethyne – production from water’s reaction with carbides, easy reactions, and ethyne’s characteristics.
b) The structure, characteristics, and usage of aromatic hydrocarbons, such as benzene.
Alkanols (c) Ethanol is produced in three stages: primary, secondary, and tertiary using fermentation and petroleum waste. Examples of local fermentation and distillation processes include gin made from palm wine and other regional ingredients, as well as glycerol, a polyhydric alkanol. OH group oxidation reactions as a criterion for differentiating between primary, secondary, and tertiary alkanols (Lucas test)
Alkanals and alkanones are (d). To differentiate between alkanals and alkanones, use a chemical test.
Alkanoic acids are (e). Chemical processes like esterification and neutralization, with benzene carboxylic acid as an example of an aromatic acid and ethanedioic (oxalic) acid as an example of a dicarboxylic acid.
Alkanoates (f) Fats and oils are formed as alkanoates from alkanoic acids and alkanols. Saponification: The process of turning alkanoates into soap and margarine and separating them from detergents.
(g) Primary, Secondary, and Tertiary Amines (Alkanamines)
(h) Mono-, di-, and polysaccharide classification of carbohydrates; composition; chemical tests for simple sugars; and response to concentrated tetraoxosulphate (VI) acid Complex sugars like cellulose from cotton and cassava starch are hydrolyzed, and sugar and starch are used to make alcoholic beverages, medicines, and textiles, among other things.
I Proteins: Basic Building Blocks, Hydrolysis, and Tests (Ninhydrin, Biuret, Millon’s, and Xanthoproteic), as well as Enzymes and Their Uses.
(j) Polymers: addition and condensation polymerization; natural and synthetic rubber. Examples, preparatory techniques, and applications. Plastics that are thermoplastic and thermosetting.
Industry and Chemistry
Chemical industries: varieties, inputs, and applicability; biotechnology.
Recommended Textbook for the Jamb Chemistry Exam
O.O. Sylvester (2004). Senior Secondary Schools: A Comprehensive Practical Chemistry, Ibadan: Evans Uche, I.O., Adenuga, I.J., and Iwuagwu, S.L. (2003). The WASSCE/SSCE, NECO, JME Chemistry, and
Evans Wisdomline Pass JAMB Once in Ibadan.
O.Y. Ababio (2005). For Senior Secondary Schools: New Chemistry (Third Edition),
Africana FIRST Publishers Limited, Onitsha
Onwu, G., Bajah, S.T., Teibo, B.O., and Obikwere, A. (1999). Secondary Chemistry, senior
Longman Bajah, S.T., Teibo, B.O., Onwu, and Obikwere are the authors of Book 1 in Lagos (2000). Lagos: Longman, Senior Secondary Chemistry, Books 2 and 3.
Ohia, G.N.C., Akpan, B.B., and Adewoyin, F.A. (1997). Chemistry Exam Focus for WASSCE & JME: University Press Plc STAN, Ibadan (1987). Heinemann’s Chemistry for Senior Secondary Schools, Ibadan
FOR MATHEMATICS 2023
JAMB’s 2023–2024 Mathematics Syllabus for the UTME The latest mathematics syllabus for the Jamb is the focus of this article. First, what exactly is a syllabus? A syllabus is a written summary of all the material that will be covered in a class or during an exam. However, the Jamb Syllabus is a set of topics that are outlined and that students must read to gain
Number and numeration in Part A
(a) Operations in various number bases ranging from 2 to 10;
(b) Conversion between bases, taking fractional parts into account.
a) Fractions and decimals; b) Approximation; and c) Percentage.
(b) Important numbers;
Decimal places (c);
(d) Error percentages;
Simple interest (e);
(f) Gross and net profit margins;
(g) Rate, ratio, and percentage;
(h) Value-added tax and shares (VAT).
Logarithms, indices, and surds:
(a) Indexing laws;
Standard form (b);
(c) Logarithm laws;
(d) Any positive number’s logarithm to a specified base;
(e) Modification of bases in applications and logarithms;
(f) How indices and logarithms relate;
Sets: (a) Set types
(b) Sets algebra
Venn diagrams and their uses (c).
Algebra in Part B
Polynomials; (a) Modifying the formula’s topic
(b) Theorems of factors and remainders
(c) Factorization of polynomials with no more than three degrees.
(d) Polynomial division and multiplication
(e) Polynomial roots with a maximum degree of three
f) Equations occurring simultaneously, including one linear and one quadratic;
(g) Polynomial graphs with degrees no higher than three.
Change; (a) Direct
(e) Increases and decreases in percentage.
es; (a) Linear inequality solutions that are analytical and graphical;
(b) Only integral-rooted quadratic inequality.
(a) The progression’s nth term
(b) the binary operations’ sum for A. P. and G. P.;
(a) Closure, commutativity, associativity, and distributivity characteristics;
(b) Elements of identity and inverse (simple cases only).
Determinants and matrixes;
(a) Matrix algebra with no more than 3 x 3 dimensions;
(b) Matrix determinants not larger than 3 x 3;
(c) Inverses of 2 x 2 matrices, excluding quadratic equations and equations of higher degree.
Geometry and trigonometry in Part C
Euclidean Geometry; (a) Angle and Line Properties
(b) Triangles, quadrilaterals, and other types of polygons;
(c) Angle characteristics, cyclic quadrilaterals, and intersecting chords of circles;
Construction is (d).
Mensuration; (a) Areas and lengths of geometrical forms in the plane;
(b) The lengths of a circle’s arcs and chords;
(c) Circle perimeters, sector areas, and circle segments;
(e) Simple solids’ surface areas and volumes, as well as composite figures;
(f) The longitudes and latitudes of the earth as a sphere.
Locus; (a) a geometric locus in two dimensions
(b) Lines and curves-related principles.
Coordinate geometry; (a) a line segment’s midpoint and gradient;
(b) The separation of two points;
(c) Lines that are perpendicular and parallel;
Equations involving straight lines (d).
a) Angelic trigonometric ratios;
(b) Elevation and depression angles;
(d) Triangle areas and solutions;
e) Sine and cosine graphs;
formulas for sine and cosine.
Calculus Differentiation in Part D;
(a) A function’s limit
(b) Differentiation of the sine, cosine, and tangent trigonometrical functions, which are explicit algebraic functions.
the use of differentiation;
(a) Change in rate;
Maxima and minima (b).
integration; (a) integration of straightforward trigonometrical and explicit algebraic functions;
(b) the curve’s undercut area.
Statistical Representation of Data, Part E
a) Distribution of frequencies;
(b) A pie chart, a bar chart, and a histogram.
(a) Ungrouped and grouped data mean, mode, and median (simple cases only);
Cumulative frequency is (b).
A range, a mean deviation, a variance, and a standard deviation.
Combination and Permutation;
(a) Circular and linear configurations;
(b) Setups that use repeated objects.
Probability; (a) Experimental probability (coin tossing, dice-tossing, etc.);
(a) Probability addition and multiplication (mutual and independent cases).
Mathematics Syllabus for the Jamb Recommend Textbook
M. David-Osuagwu et al (2000) Africana – FIRST Publishers, “New School Mathematics for Senior Secondary Schools,” Onitsha.
Egbe, E., et al (2000) Additional Mathematics, Onitsha: FIRST Publishers
S. O. Ibude and others (2003) LINCEL Publishers: Agebra and Calculus for Schools and Colleges.
Further Mathematics Project Books 1 to 3 by Tuttuh-Adegun M. R. et al., Ibadan: NPS Educational Wisdomline Pass at Once JAMB, 1997.
Distinction in Mathematics: Comprehensive Revision Text, Adelodun A. A. (3rd Edition) Ekiti: Ado FNPL.
A. J. B. Anyebe (1998) Kenny Moore, Lagos, Basic Mathematics for Senior Secondary Schools and Remedial Students in Higher Institutions.
New General Mathematics for West Africa SSS 1 to 3, Lagos: Longman, Channon, J. B. and Smith, A. M. 2001.