CHEMISTRY 2019 JAMB SYLLABUS DETAILS

SUB TOPIC

ACIDS, BASES AND SALTS

OBJECTIVES

Candidates should be able to:

i. Distinguish between the properties of acids and bases.

ii. Identify the different types of acids and bases.

iii. Determine the basicity of acids.

iv. Differentiate between acidity and alkalinity using acid/base indicators.

v. Identify the various methods of preparation of salts.

vi. Classify different types of salts.

vii. Relate degree of dissociation to strength of acids and bases.

viii. Relate degree of dissociation to conductance.

ix. Perform simple calculations on pH and pOH.

x. Identify the appropriate acid-base indicator.

xi. Interpret graphical representation of titration curves.

xii. Perform simple calculations based on the mole concept.

xiii. Balance equations for the hydrolysis of salts.

xiv. Deduce the properties (acidic, basic, neutral) of the resultant solution.

CONTENT

(a) General characteristics and properties of acids, bases and salts; acids/base indicators, basicity of acids, normal, acidic, basic and double salts; An acid defined as a substance whose aqueous solution furnishes H3O+ions or as a proton donor; ethanoic, citric and tartaric acids as examples of naturally occurring organic acids; alums as examples of double salts; preparation of salts by neutralization, precipitation and action of acids on metals; oxides and trioxocarbonate (IV) salts.

(b) Qualitative comparison of the conductances of molar solutions of strong and weak acids and bases; relationship between conductance and amount of ions present and their relative mobilities.

(c) Ph and Poh scale; Simple calculations.

(d) Acid/base titrations.

(e) Hydrolysis of salts; Principle, simple examples such as NH4C1, AICI3, Na2CO3, CH3COONa.

SUB TOPIC

AIR

OBJECTIVES

Candidates should be able to:

i. deduce reason (s) for the existence of air as a mixture.

ii. identify the principle involved in the separation of air components.

iii. deduce reasons for the variation in the composition of air in the environment.

iv. specify the uses of some of the constituents of air.

CONTENT

(a) The natural gaseous constituents and their proportion in the air – nitrogen, oxygen, water vapour, carbon (IV) oxide and the noble gases (argon and neon).

(b) Air as a mixture and some uses of the noble gas.

SUB TOPIC

ATOMIC STRUCTURE AND BONDING

OBJECTIVES

Candidates should be able to:

i. distinguish between atom, molecules and ions.

ii. assess 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. identity common elements exhibiting isotopy;
vi. relate isotopy to mass number.

vii. perform simple calculations on relative atomic mass.

viii. determine the number of electrons in s and p atomic orbitals.

ix. relate atomic number to the position of an element on the periodic table.

x. relate properties of groups of elements on the periodic table.

xi. identify reasons for variation in properties across the period.

xii. differentiate between the different types of bonding.

xiii. deduce bond types based on electron configurations.

xiv. relate the nature of bonding to properties of compounds.

xv. apply it in everyday chemistry.

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.

xxii. identify the various applications of radioactivity.

CONTENT

(a)

1. The concept of atoms, molecules and ions, the works of Dalton, Millikan, Rutherford, Mosely, Thompson and Bohr.

2. Atomic structure, electron configuration, atomic number, mass number and isotopes; specific examples should be
drawn from elements of atomic number 1 to 20.

3. Shapes of s and p orbitals.

(b)

1. The periodic table and periodicity of elements.

2. Presentation of the periodic table with a view to recognizing families of elements e.g. alkali metals, halogens, the noble gases and transition metals.

3. The variation of the following properties should be noticed: ionization energy, ionic radii, electron affinity and electronegativity.

(c)

1. Chemical Bonding: Electrovalency and covalency, the electron configuration of elements and their tendency to attain the noble gas structure.

2. Hydrogen bonding and metallic bonding as special types of electrovalency and covalency respectively.

3. Coordinate bond as a typ 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)

1. Shapes of simple molecules: linear ((2, O2C12,HCI and CO2), non-linear (H2O) and tetrahedral. (CH)

(e) Nuclear Chemistry:

1. Radioactivity (elementary treatment only).

2. Nuclear reactions, simple equations, uses and applications of natural and artificial radioactivity.

SUB TOPIC

CHEMICAL COMBINATION

OBJECTIVES

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.

iv. deduce the stoichiometry of chemical reactions.

CONTENT

(a) Stoichiometry.

(b) Laws of definite and multiple proportions.

(c) Law of conservation of matter.

(d) Gay Lussac’s law of combining volumes.

(e) Avogadro’s law.

(f) Chemical symbols, formulae, equations and their uses.

(g) Relative atomic mass based on 12C=12.

(i) The mole concept and Avogadro’s number.

SUB TOPIC

CHEMICAL COMBINATION

OBJECTIVES

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.

iv. deduce the stoichiometry of chemical reactions.

CONTENT

(a) Stoichiometry.

(b) Laws of definite and multiple proportions.

(c) Law of conservation of matter.

(d) Gay Lussac’s law of combining volumes.

(e) Avogadro’s law.

(f) Chemical symbols, formulae, equations and their uses.

(g) Relative atomic mass based on 12C=12.

(i) The mole concept and Avogadro’s number.

SUB TOPIC

CHEMISTRY AND INDUSTRY

OBJECTIVES

Candidates should be able to:

i. classify chemical industri in terms products.

ii. identify raw materials for eacindustry.

iii. distinguish between fine and heav chemicals.

iv. enumerate the relevance of each of theindustries.

v. relate industrial processes to biotechnology.

SUB TOPIC

ELECTROLYSIS

OBJECTIVES

Candidates should be able to:

i. identify between electrolytes and non- electrolytes.

ii. perform calculations based on faraday as a mole of electrons.

iii. identify suitable electrodes for different electrolytes.

iv. specify the chemical reactions at the electrodes.

v. determine the products at the electrodes.

vi. identify the factors that affect the product of electrolysis.

vii. specify the different areas of application of electrolysis.

viii. identify the various electrochemical cells.

ix. calculate electrode potentials using half-cell reaction equations.

x. determine the different areas of applications of electrolytic processes.

xi. identify methods used in protecting metals.