Chemistry
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The aim of the Unified Tertiary Matriculation Examination (UTME) syllabus in Chemistry is to
prepare the candidates for the Board’s examination. It is designed to test their achievement of the
course objectives, which are to:
(i) apply the basic principles governing scientific methods in new situations;
(ii) interpret scientific data;
(iii) deduce the relationships between chemistry and other sciences;
(iv) apply the knowledge of chemistry to industry and everyday life.
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1. Separation of mixtures and Candidates should be able to:
purification of chemical
substances
(a) Pure and impure substances i) distinguish between pure and impure
substances;
(b) Boiling and melting points. ii) use boiling and melting points as criteria for
purity of chemical substances;
(c) Elements, compounds and mixtures (iii) distinguish between elements, compounds and
mixture;
(d) Chemical and physical changes. (iv) differentiate between chemical and physical
changes;
(e) Separation processes: (v) identify the properties of the components of a
evaporation, simple and fractional distillation, mixture;
sublimation, filtration, crystallization, paper (vi) specify the principle involved in each separation
and column chromatography, simple and method.
fractional crystallization.
2. Chemical combination Candidates should be able to:
Stoichiometry, laws of definite and multiple (i) perform simple calculations involving formulae,
proportions, law of conservation of matter, equations/chemical composition and the mole
Gay Lussac’s law of combining volumes, concept;
Avogadro’s law; chemical symbols, formulae, (ii) deduce the chemical laws from given
equations and their uses, relative atomic mass expressions/statements;
based on 12C=12, the mole concept and (iii) interpret data based on these laws;
Avogadro’s number.
(iv) interpret graphical representations related
to these laws.
ϯ͘Kinetic theory of matter and Gas Laws Candidates should be able to:
(a) An outline of the kinetic theory of matter, (i) apply the theory to distinguish between solids,
melting, vapourization and reverse processes; liquids and gases;
melting and boiling explained in terms of (ii) deduce reasons for change of state;
molecular motion and Brownian movement. (iii) draw inferences based on molecular motion;
ϰϯ
, Chemistry
612+%5%106'065016'5 1$,'%6+8'5
(b) The laws of Boyle, Charles, Graham and (iv) deduce chemical laws form given expressions/
Dalton (law of partial pressure); combined statements;
gas law, molar volume and atomicity of gases. (v) interpret graphical representations related to
these laws;
(vi) perform simple calculations based on these laws
and the relationship between the vapour density
of gases and the relative molecular mass.
4. Atomic structure and bonding
Candidates should be able to:
(a) (i)The concept of atoms, molecules and ions,
the works of Dalton, Millikan, Rutherford, (i) distinguish between atom, molecules and ions;
Mosely, Thompson and Bohr. Simple (ii) assess the contributions of these scientists to
hydrogen spectrum, Ionization of gases the development of the atomic structure;
illustrating the electron as fundamental (iii) deduce the number of protons, neutrons and
particle of matter. electrons from atomic and mass numbers of
an atom;
(ii) Atomic structure, electron configuration,
atomic number, mass number and isotopes; (iv) apply the rules guiding the arrangement of
specific examples should be drawn from electrons in an atom;
elements of atomic number 1 to 20. Shapes (v) relate isotopy to mass number;
of s and p orbitals. (vi) perform simple calculations on relative
atomic mass
(vii) determine the number of electrons in s and
(b) The periodic table and periodicity of p atomic orbitals.
elements, presentation of the periodic table (viii) relate atomic number to the position of an
with a view to recognizing families of element on the periodic table;
elements e.g. alkali metals, halogens, the (ix) relate properties of groups of elements on the
noble gases and transition metals. The periodic table;
variation of the following properties should (x) identify reasons for variation in properties
be noticed: ionization energy, ionic radii, across the period.
electron affinity and electronegativity.
(c) Chemical bonding.
Electrovalency and covalency, the electron (xi) differentiate between the different types
configuration of elements and their tendency of bonding.
to attain the noble gas structure. Hydrogen (xii) deduce bond types based on electron
bonding and metallic bonding as special configurations;
types of electrovalency and covalency (xiii) relate the nature of bonding to properties
respectively; coordinate bond as a type of compounds;
of covalent bond as illustrated by complexes (xiv) apply it in everyday chemistry;
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, 02, (xv) differentiate between the various shapes
C12,HCI and CO2), non-linear (H2O) and of molecules
tetrahedral; (CH4)
ϰϰ
%*'/+564;
)'0'4#.1$,'%6+8'5
The aim of the Unified Tertiary Matriculation Examination (UTME) syllabus in Chemistry is to
prepare the candidates for the Board’s examination. It is designed to test their achievement of the
course objectives, which are to:
(i) apply the basic principles governing scientific methods in new situations;
(ii) interpret scientific data;
(iii) deduce the relationships between chemistry and other sciences;
(iv) apply the knowledge of chemistry to industry and everyday life.
&'6#+.'&5;..#$75
612+%5%106'065016'5 1$,'%6+8'5
1. Separation of mixtures and Candidates should be able to:
purification of chemical
substances
(a) Pure and impure substances i) distinguish between pure and impure
substances;
(b) Boiling and melting points. ii) use boiling and melting points as criteria for
purity of chemical substances;
(c) Elements, compounds and mixtures (iii) distinguish between elements, compounds and
mixture;
(d) Chemical and physical changes. (iv) differentiate between chemical and physical
changes;
(e) Separation processes: (v) identify the properties of the components of a
evaporation, simple and fractional distillation, mixture;
sublimation, filtration, crystallization, paper (vi) specify the principle involved in each separation
and column chromatography, simple and method.
fractional crystallization.
2. Chemical combination Candidates should be able to:
Stoichiometry, laws of definite and multiple (i) perform simple calculations involving formulae,
proportions, law of conservation of matter, equations/chemical composition and the mole
Gay Lussac’s law of combining volumes, concept;
Avogadro’s law; chemical symbols, formulae, (ii) deduce the chemical laws from given
equations and their uses, relative atomic mass expressions/statements;
based on 12C=12, the mole concept and (iii) interpret data based on these laws;
Avogadro’s number.
(iv) interpret graphical representations related
to these laws.
ϯ͘Kinetic theory of matter and Gas Laws Candidates should be able to:
(a) An outline of the kinetic theory of matter, (i) apply the theory to distinguish between solids,
melting, vapourization and reverse processes; liquids and gases;
melting and boiling explained in terms of (ii) deduce reasons for change of state;
molecular motion and Brownian movement. (iii) draw inferences based on molecular motion;
ϰϯ
, Chemistry
612+%5%106'065016'5 1$,'%6+8'5
(b) The laws of Boyle, Charles, Graham and (iv) deduce chemical laws form given expressions/
Dalton (law of partial pressure); combined statements;
gas law, molar volume and atomicity of gases. (v) interpret graphical representations related to
these laws;
(vi) perform simple calculations based on these laws
and the relationship between the vapour density
of gases and the relative molecular mass.
4. Atomic structure and bonding
Candidates should be able to:
(a) (i)The concept of atoms, molecules and ions,
the works of Dalton, Millikan, Rutherford, (i) distinguish between atom, molecules and ions;
Mosely, Thompson and Bohr. Simple (ii) assess the contributions of these scientists to
hydrogen spectrum, Ionization of gases the development of the atomic structure;
illustrating the electron as fundamental (iii) deduce the number of protons, neutrons and
particle of matter. electrons from atomic and mass numbers of
an atom;
(ii) Atomic structure, electron configuration,
atomic number, mass number and isotopes; (iv) apply the rules guiding the arrangement of
specific examples should be drawn from electrons in an atom;
elements of atomic number 1 to 20. Shapes (v) relate isotopy to mass number;
of s and p orbitals. (vi) perform simple calculations on relative
atomic mass
(vii) determine the number of electrons in s and
(b) The periodic table and periodicity of p atomic orbitals.
elements, presentation of the periodic table (viii) relate atomic number to the position of an
with a view to recognizing families of element on the periodic table;
elements e.g. alkali metals, halogens, the (ix) relate properties of groups of elements on the
noble gases and transition metals. The periodic table;
variation of the following properties should (x) identify reasons for variation in properties
be noticed: ionization energy, ionic radii, across the period.
electron affinity and electronegativity.
(c) Chemical bonding.
Electrovalency and covalency, the electron (xi) differentiate between the different types
configuration of elements and their tendency of bonding.
to attain the noble gas structure. Hydrogen (xii) deduce bond types based on electron
bonding and metallic bonding as special configurations;
types of electrovalency and covalency (xiii) relate the nature of bonding to properties
respectively; coordinate bond as a type of compounds;
of covalent bond as illustrated by complexes (xiv) apply it in everyday chemistry;
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, 02, (xv) differentiate between the various shapes
C12,HCI and CO2), non-linear (H2O) and of molecules
tetrahedral; (CH4)
ϰϰ
