Jamb 2019 chemistry syllabus

Syllabus for 2018 UTME. Please postpone your reading! Pick your textbook now and start reading. AllSchool is promising you that you will not regret it. 

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Official JAMB Syllabus for Chemistry

1. Separation of mixtures and purification of chemical substances

Under this topic, candidates should focus on;

• Pure and impure substances
• Boiling and melting
• Elements, compounds and mixtures
• Chemical and physical
• Separation processes: evaporation, simple and fractional distillation, sublimation, filtration, crystallization, paper and column chromatography, simple and fractional crystallization.

At the end of reading the above sub-topics candidates should be able to;

• distinguish between      pure      and     impure substances;
• use boiling and melting points as criteria for purity of chemical substances;
• distinguish between elements, compounds and mixture;
• differentiate between chemical and physical changes;
• identify the properties of the components of a mixture;
• specify the principle involved in each separation method

2. Chemical combination

Subtopics in the above topic are;

• Stoichiometry,
• laws of definite and multiple 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 on¹²C=12, the mole concept and Avogadro’s number.

At the end of reading the subtopics above, candidates should be able to;

• perform simple calculations involving formulae, equations/chemical composition and the mole concept;
• deduce the    chemical    laws     from    given expressions/statements;
• interpret data based on these laws;
• interpret graphical representations related to these laws

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3. Kinetic theory of matter and Gas Laws

Subtopics under the topic above are;

1. An outline of the kinetic theory of matter, melting, vapourization and reverse processes; melting and boiling explained in terms of molecular motion and Brownian movement
2. The laws of Boyle, Charles, Graham and Dalton (law of partial  pressure);  combined gas law, molar volume and atomicity of gases.

After reading the topic above candidates should be able to;

• apply the theory to distinguish between solids, liquids and gases;
• deduce reasons for change of state;
• draw inferences based on molecular motion
• deduce chemical laws form given expressions/ statements;
• interpret graphical representations related to these laws;

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4. Atomic structure and bonding

Candidate focus on the topic above should be;

1. here you should know;
   1. The concept of atoms, molecules  and  ions, the works of Dalton, Millikan, Rutherford, Mosely, Thompson and Bohr. Simple hydrogen spectrum, Ionization of gases illustrating the electron as fundamental particle of matter.
   2. Atomic structure,  electron  configuration, atomic number, mass number and isotopes; specific examples should be drawn from elements of  atomic number 1 to 20. Shapes  of s and p orbitals.
2. 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  should be noticed: ionization energy, ionic radii, electron affinity and electronegativity.
3. 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.
4. Shapes of simple molecules: linear ((H₂, 0₂, C1₂,HCI and CO₂), non-linear (H₂O) and tetrahedral; (CH₄)
5. Nuclear Chemistry:
   1.  Radioactivity (elementary treatment only)
   2. Nuclear reactions. Simple equations, uses and applications of natural and artificial radioactivity.

At the end of reading the topic, candidates should be able to;

1. distinguish between atom, molecules and ions;
2. assess the contributions of these scientists to the development of the atomic structure;
3. deduce the number of protons, neutrons and electrons from atomic and mass numbers of an atom;
4. apply the rules guiding the arrangement of electrons in an atom;
5. relate isotopy to mass number;
6. perform simple calculations on relative atomic mass
7. determine the number of electrons in s and p atomic
8. relate atomic number to the position of an element on the periodic table;
9. relate properties of groups of elements on the periodic table;
10. identify reasons for variation in properties across the period.
11. differentiate between the different types of
12. deduce bond types based on electron configurations;
13. relate the nature of bonding to properties of compounds;
14. apply it in everyday chemistry;
15. differentiate between the various shapes of molecules
16. distinguish between ordinary chemical reaction and nuclear reaction;
17. differentiate between natural and artificial radioactivity;
18. compare the properties of the different types of nuclear radiations;
19. compute simple calculations on the half-life of a radioactive material;
20. balance simple nuclear equation;
21. identify the various applications of radioactivity.

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5. Air

Candidates should focus on;

1. the usual gaseous constituents – nitrogen, oxygen, water vapour, carbon (IV) oxide and the noble gases (argon and neon),
2. proportion of oxygen in the air e.g. by burning phosphorus or by using alkaline pyrogallol,
3. air as a mixture and some uses of the noble gas.

At the end of reading the topic, candidates should be able to;

1. deduce reason (s) for the existence of air as a mixture;
2. identify the principle involved in the separation of air components;
3. deduce reasons for the variation in the composition of air in the environment;
4. specify the uses of some of the constituents of air

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6. Water

Under this topic, candidates should focus their attention on;

• Composition by volume:
• Water as a solvent, atmospheric gases dissolved in water and their biological significance.
• Water as a product of the combustion of hydrogen.
• Hard and soft water:
• Temporary and permanent hardness and methods of softening hard water.
• Purification of town water supplies.
• Water of crystallization, efflorescence, deliquescence and hygroscopy.
• Examples of the substances exhibiting these properties and their uses

At the end of reading the topic candidate should be able to;

1. identify the various uses of water;
2. distinguish between the properties of hard and soft water;
3. determine the causes of hardness;
4. identify methods of removal of hardness;
5. describe the processes involved in the purification of water for town supply;
6. distinguish between these phenomena;
7. identify the various compounds that exhibit these phenomena;

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7. Solubility

Under this topic, Candidates should focus on;

• Unsaturated, saturated and supersaturated solutions. Solubility curves and simple deductions from them, (solubility defined in terms of mole per dm³) and simple calculations
• Solvents for fats, oil and paints and the use of such solvents
• Suspensions and colloids: Harmattan haze and paints as examples of suspensions and fog, milk, aerosol spray and rubber solution as examples of colloids

At the end of reading this topic, each candidates should be able to;

• distinguish between the different types of solutions;
• interpret solubility curves;
• calculate the amount of solute that can dissolve in a given amount of solvent at a given temperature;
• deduce that solubility is temperature-dependent
• classify solvents based on their uses
• differentiate between a true solution, suspension and colloids;
• compare the properties of a true solution and a ‘false’ solution.

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8. Environmental Pollution

After reading the topic: “Environmental Pollution”, candidate should be able to;

• identify the different types of pollution and pollutants;
• classify pollutants as biodegradable and non-biodegradable;
• assess the effects of pollution on the environment;
• recommend measures for control of environment

Under the topic: Environmental Pollution, candidates should focus on;

1. Sources and effects of pollutants.
2. Air pollution: Examples of air pollutants such as H₂S, CO, SO₂, oxides of nitrogen, fluorocarbons and dust.
3. Water pollution: Sewage and oil pollution should be known
4. Soil pollution: Oil spillage, Biodegradable and non-biodegradable pollutants

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9. Acids, bases and salts

Under this topic, Candidates should focus;

1. 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   Oxides  and trioxocarbonate (IV) salts
2. Qualitative comparison of the conductances of molar solutions of strong and weak acids and bases, relationship between conductance, amount of ions present and their relative mobilities
3. pH and pOH scale
   1. pH defined as – log[H₃O⁺]
4. Acid/base titrations
5. Hydrolysis of salts: Simple examples such as NH₄C1, AICI₃, Na₂CO₃, CH₃COONa to be mentioned

After reading the topic, candidate should be able to;

• distinguish between the properties of acids and bases;
• identify the different types of acids and bases;
• differentiate between acidity and alkalinity using acid/base indicators;
• identify the various methods of preparation of salts;
• classify different types of salts;
• relate degree of dissociation to strength of acids and bases;
• relate degree of dissociation to conductance;
• perform simple calculations on pH;
• identify the appropriate acid-base indicator;
• interpret graphical representation of titration curves;
• perform simple calculations based on the mole concept;
• balance equations for the hydrolysis of salts;
• deduce the properties (acidic, basic, neutral) of the resultant

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10. Oxidation and reduction

Under this topic, candidates should focus on;

• Oxidation in terms of the addition of oxygen or removal of hydrogen.
• Reduction as removal of oxygen or addition of
• Oxidation and reduction in terms of electron
• Use of oxidation numbers. Oxidation and reduction treated as change in number and use of oxidation numbers in balancing simple equations.
• IUPAC nomenclature of inorganic compounds.
• Tests for oxidizing and reducing agents.

After reading the topic: “Oxidation and Reduction”, candidates should be able to

• identify the various forms of expressing oxidation and reduction;
• classify chemical reactions in terms of oxidation or reduction;
• balance redox reaction equations;
• deduce the oxidation number of chemical species;
• compute the number of electron transfer in redox reactions
• identify the name of redox species using IUPAC nomenclature.
• distinguish between oxidizing and reducing agents in redox reactions

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11. Electrolysis

candidates should focus on;

1. Electrolytes and non-electrolytes. Faraday’s laws of electrolysis
2. Electrolysis of dilute H₂SO₄, aqueous CuSO₄, CuC1₂ solution,  dilute and concentrated NaC1 solutions and fused NaC1 and factors affecting discharge of ions at the electrodes
3. Uses of electrolysis: Purification of metals e.g. copper and production of elements and compounds e.g. A1, Na, O₂, Cl₂and NaOH.
4. Electrochemical cells: Redox series (K, Na, Ca,  Mg, AI, Zn, Fe, PbII, H, Cu, Hg, Au,)
5. half-cell reactions and electrode potentials. Simple calculations only
6. Corrosion as an electrolytic process, cathodic protection of metals, painting, electroplating and coating with grease or oil as ways of preventing iron from corrosion

After reading the topic Electrolysis, candidates should be able to;

• identify between electrolytes and non- electrolytes;
• perform calculations based on faraday as a mole of
• identify suitable electrodes for different electrolytes.
• specify the chemical reactions at the electrodes;
• determine the products at the electrodes;
• identify the factors that affect the product of electrolysis;
• specify the different areas of application of electrolysis;
• identify the various electrochemical cells;
• calculate electrode potentials using half- cell reaction equation
• determine the different areas of applications of electrolytic processes;
• apply the methods to protect metals

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12. Energy changes

Under this topic candidates should focus on;

1. Energy changes(∆H) accompanying physical and chemical changes: dissolution of substances in or reaction with water e.g. Na, NaOH, K, NH₄, Cl. Endothermic (+∆H) and exothermic (-∆H) reactions
2. Entropy as an order-disorder phenomenon: simple illustrations like mixing of gases and dissolution of salts.
3. Spontaneity of reactions: ∆G⁰ = 0 as a criterion for equilibrium, ∆G greater or less than zero as a criterion for non-spontaneity or spontaneity

After reading the topic: “Energy Changes” candidates should be able to;

• determine the types of heat changes
• (∆H) in physical and chemical processes;
• interpret graphical representations of heat changes;
• relate the physical state of a substance to the degree of orderliness;
• determine the conditions for spontaneity of a reaction ;
• relate (∆H), ∆S⁰ and ∆G⁰ as the driving forces for chemical reactions;
• solve simple problems based on the relationships ∆G⁰= ∆H⁰ -T∆S⁰)