HomeNABTEB Syllabus 2026NABTEB Syllabus For Chemistry 2026/2027 [NTC]

NABTEB Syllabus For Chemistry 2026/2027 [NTC]

By March 12, 2026 NABTEB Syllabus 2026, Syllabus, Uncategorized 0 Comments

NABTEB Syllabus for Chemistry 2026/2027 [NTC]: The NABTEB Chemistry Syllabus is now available in PDF. The National Business and Technical Examinations Board (NABTEB) has released the syllabus to help prospective candidates prepare for upcoming exams.

This carefully compiled guide, designed by subject experts, provides essential topics and structure to support students planning to sit for NABTEB examinations. Candidates will find it a valuable resource for effective preparation.

Aims and Objectives

The syllabus is derived from the NBTE Curriculum for examination purposes. It assumes that candidates have already studied Integrated General Science and Mathematics at the Junior Secondary School (JSS) level. Schools presenting candidates for the National Technical Certificate (NTC) are expected to have well-equipped laboratories.

Aims of the syllabus:

  • Provide chemistry knowledge relevant to students in technical and vocational trades, especially those ending their chemistry studies at the NTC level.
  • Serve as a foundation for further technical education.
  • Equip students with basic concepts, principles, and generalizations behind technological processes and products.
  • Develop students’ abilities in scientific observation, application, problem-solving, and model formulation through practical and project work.
  • Introduce the use of SI units and the IUPAC system of nomenclature.
  • Show the relationship between chemistry and various trades/work environments.
  • Instill a strong culture of safety precautions in laboratory and technical work.

EXAMINATION SCHEME

The examination shall consist of two papers.
05-1 Paper I (2 ½ hours) 150 marks (Theory)
05-2 Paper 2 (2 hours) 50 marks (Practical)

PAPER I: This is a theory paper. It consist of two parts – Part A and Part B.

Part A: This shall consist of fifty (50) multiple-choice objective questions, to be
answered by candidates in 50 minutes for 50 marks.
Part B: This shall consist of five (5) essay questions from which candidates are expected to
Attempt FOUR (4) questions only. Each of the essay question carries 25 marks for a
a total of 100 marks in a duration of 1 hour 40 minutes.

PAPER 2 (Practical):
This shall be a 2-hour practical test, either the actual practical or an alternative to the practical. It shall
consist of THREE (3) compulsory questions for a total of 50 marks. The actual practical shall
be taken by schools WHILE the alternative to practical shall be taken by private candidates.

ALTERNATIVE TO PRACTICAL
The alternative to practical will test the knowledge of the practical skills and processes that the
candidates are expected to have acquired in the practical activities that are prescribed in the
syllabus.

NABTEB Syllabus For Chemistry 2026/2027 [NTC]

S/NTopic/ObjectivesContentsActivities/Remarks
1Elements, Compounds and Mixtures1.1 Explain concepts of elements, compounds, mixtures.
1.2 Identify properties (melting point, boiling point, solubility) of common substances for separation methods.		– Concepts of Elements, Compounds and Mixtures.
– Physical and chemical changes.
– Definitions.
– Separation methods.
– Use burning candle to demonstrate physical and chemical changes.
– Experimental illustration of separation methods.
2Structure of the Atom1.1 Concepts of atoms, molecules, ions.
1.2 Features of the atom.
1.3 Draw & label electronic shells; explain atomic number, isotopes, Ar, Mr.
1.4 Electron arrangement in main & sub-energy levels.
1.5 Explain orbitals and electron filling rules.
1.6 Distinguish chemical and nuclear reactions.
1.7 Explain types of radiation.
1.8 Define radioactivity, natural & artificial.
1.9 Define half-life.
1.10 Write/balance nuclear equations.
1.11 Effects and uses of radioactive radiation.		– Dalton’s atomic theory.
– J.J. Thomson’s & Bohr-Rutherford’s experiments.
– Atomic number, mass number, isotopes.
– Electron shells (K, L, M), orbitals (s, p, d, f).
– Aufbau Principle, Hund’s rule, Pauli’s exclusion.
– Nuclear chemistry concepts.
– Use chlorine isotope calculation as example.
– Geiger-Muller counter description.
– Highlight nuclear reactions creating new elements.
– Symbols for radiation types.
3Periodicity of the Element1.1 State periodic law and application.
1.2 Outline periodic properties & trends.
1.3 Periodic graduation of halogen properties.
1.4 Explain transition metals and their properties.		– Electronic configuration relating to groups/periods.
– Uniqueness of hydrogen.
– Periodic properties: atomic size, ionization energy, electron affinity, electronegativity.
– Trends in metallic to nonmetallic character.
– Halogen properties: physical states, melting points, redox & displacement reactions.
– Transition metals: variable oxidation states, magnetic properties, catalysis.
– Highlight variable oxidation states in non-metals and constant states in metals like zinc.
4Chemical Bonding4.1 Explain chemical bonding and types.
4.2 Illustrate ionic bonding with examples; list influencing factors & properties.
4.3 Illustrate covalent & coordinate bonding; factors & properties.
4.4 Draw shapes of simple molecules.
4.5 Explain metallic bonding, influencing factors, and properties.
4.6 Explain Van der Waals forces with examples.
4.7 Explain hydrogen bonding and its effect on boiling points of HF, H2O, NH3.		– Chemical bonding as achieving noble gas structure.
– Lewis dot structures for ionic & covalent compounds.
– Ionic bonding factors: ionization energy, electron affinity, electronegativity difference.
– Covalent bonding factors & molecular shapes (linear, non-linear, tetrahedral).
– Metallic bonding: atomic radius, valence electrons, conductivity, malleability.
– Intermolecular forces: Van der Waals, dipole-dipole, hydrogen bonding.
– Use metal samples like Mg, Zn, Sn, Fe for demonstrations.
– Models and molecular shapes for illustration.
5Stoichiometry and Chemical Reactions5.1 Explain symbols, formulae, equations.
5.2 State laws of chemical combination.
5.3 Explain moles, Avogadro number, mole ratios.
5.4 Explain concept of solutions and concentration.		– Chemical symbols, empirical & molecular formulae.
– Balancing chemical equations.
– Law of conservation of mass, constant composition, multiple proportions.
– Mole concepts: mass, volume, Avogadro constant, mole ratio.
– Calculations involving molar concentration.
– Preparation of standard solutions (e.g., Na2CO3).
– Experimental illustrations of laws.
– Concept of solutions: solute, solvent, concentration terms.
– Dilution factor calculations.
6States of Matter1.1 Define law, theory, hypothesis.
1.2 Postulates of kinetic theory.
1.3 Gas laws with mathematical & graphical representation.
1.4 Relationship of vapor pressure with boiling points.
1.5 Classify solids; compare properties & describe structure of diamond and graphite.		– Kinetic theory: solids, liquids, gases.
– Changes of state: melting, boiling, diffusion.
– Gas laws: Boyle’s, Charles’s, Dalton’s, Graham’s, Avogadro’s laws.
– General gas law derivation & calculations.
– Vapor pressure and boiling point determination.
– Solid types: ionic, metallic, covalent, molecular.
– Brownian motion demonstrations.
– Experimental boiling point determination.
– Structure and uses of diamond & graphite.
– Differentiate Dalton’s law from Dalton’s atomic theory.
7Energy and Energy Changes7.1 Define energy and its forms.
7.2 Explain exothermic/endothermic reactions, heats of reaction, formation, combustion, neutralization, solution.
7.3 Concepts of free energy and entropy.		– Energy changes during physical & chemical processes.
– Enthalpy and energy diagrams.
– Measurement and calculation of heat changes.
– Conservation of energy law.
– Applications of energy concept

Practical for NABTEB Chemistry

General Skills and Principles

You are expected to be familiar with the following practical skills and principles:

  • Measurement of length, mass, and volume.
  • Preparation and dilution of standard solutions.
  • Filtration, recrystallization, and determination of melting points.
  • Measurement of heats of neutralization and solution.
  • Determination of pH values of various solutions using colorimetry.
  • Determination of reaction rates from concentration versus time curves.

20.2 Quantitative Analysis

You should be skilled in acid-base titrations, including:

Preparation of standard solutions, including primary and secondary standards.

Using standard acid and alkali solutions with indicators such as methyl orange and phenolphthalein to determine:

  1. The concentration of acid and alkali solutions.
  2. The molar masses of acids, bases, and water of crystallization.
  3. The solubility of acids, bases, and salts.
  4. The percentage purity of acids and bases.

Be able to perform calculations for both direct and back titrations, with answers rounded to 3 significant figures.

20.3 Qualitative Analysis

No formal scheme of analysis is required, but you should be able to:

(a) Tests for Cations

  • Perform characteristic tests for the following cations using dilute NaOH and NH₃(aq): NH₄⁺, Ca²⁺, Pb²⁺, Cu²⁺, Fe²⁺, Fe³⁺, Al³⁺, and Zn²⁺
  • Carry out confirmatory tests for these cations.

(b) Tests for Anions

Understand the characteristic reactions of dilute HCl on solid samples or aqueous solutions and concentrated H₂SO₄ on solid samples for the following anions:

  • Cl⁻, SO₃²⁻, CO₃²⁻, NO₃⁻, SO₄²⁻

Perform confirmatory tests for these anions.

(c) Comparative Study of Halogens

  • Observe displacement reactions among halogens.

(d) Tests for Gases

  • Identify the following gases through characteristic tests: O₂, H₂, NH₃, CO₂, HCl, SO₂, H₂S
  • Note: The use of litmus paper is only acceptable for identifying ammonia gas and not as a confirmatory test for others.

(e) Test Tube Reactions for Functional Groups in Organic Compounds

Perform characteristic reactions for the following compounds:

Proteins (using Ninhydrin test, Xanthoproteic test, Biuret test, and Millon’s test only)

Alkenes

Alkanols

Alkanoic acids

Sugars (using Fehling’s and Benedict’s solutions only)

Starch (iodine test only)

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