WAEC TUTORIALS: Study Chemistry Online For Successful Exam - 2017/2018 Syllabus
(1) Short account of Dalton’s atomic theory andlimitations, J.J. Thompson’s experiment and Bohr’s model of the atom.
(2) Outline description of the Rutherford’salpha scattering experiment to establish the structure of the atom.
CONTENT
NOTES (ii) Relative atomic mass (Ar) and
relative molecular mass (Mr) based on Carbon-12 scale.(iii) Characteristics and
(ii) Orbitals
(iii) Rulesand principles
for filling in
electrons.
(1) Atomic mass as the weighted average mass of isotopes. Calculation of relative mass of chlorine should be used as an
example.(2) Carbon-12 scale as a unit
of measurement.
Physicalchange- melting of solids, magnetization of iron, dissolution of salt etc.
Chemical
change- burning of wood, rusting of iron, decay of leaves etc.
(1) Aufbau Principle, Hund’s Rule of Maximum
Multiplicity and Pauli Exclusion Principle.
4.0 PERIODIC CHEMISTRY
(c) Periodic law:
(ii) Periodic gradation of the elements in thethird period (Na – Ar).
(1) Progression from:
(f) Elements of the first transition series.
Formation and difference between pure covalent and
coordinate (dative) covalent bobonds.
(2) Differences and similarities in the properties between the second and the third period elements should be
stated.(i) Period three metals (Na, Mg,
Al).
(ii) Period four metals (K, Ca).
(iii) Chemical equations.
Recognition of
group variations noting any anomalies.
Treatment
should include the following:
(a) physical states, melting and boiling
points;
(b) variable oxidation states;
(c) redox properties of the elements;
(d) displacement reaction of one halogen by
another;
(e) reaction of the elements with water and
alkali (balanced equations required).
(1) Their electron configurations, physical
properties and chemical reactivity of the elements and their compounds.
(2) Physical properties should include: physical
states, metallic properties and magnetic properties.
(3) Reactivity of the metals with air, water,
acids and comparison with s-block elements (Li, Na, Be, Mg).
CONTENT
NOTES5.0 CHEMICAL BONDS
(a) Interatomic bonding
(b) (i) Formation of ionic bonds and compounds.
(ii)
Properties of ionic compounds.
(c) Naming of ionic compounds.
(d) Formation of covalent bonds and compounds.
(e) (i) Properties of covalent compounds.
(ii)
Coordinate (dative) covalent bonding.
(4) Other properties of transition metals should
include:(a) variable oxidation
states;
(b) formation of coloured compounds;
(c) complex formation;
(d) catalytic abilities;
(e) paramagnetism;
(f) hardness.
Meaning of
chemical bonding.
Lewis dot
structure for simple ionic and covalent compounds.
Formation of
stable compounds from ions. Factors influencing formation: ionzation energy;
electron affinity and electronegativity difference.
Solubility in
polar and non-polar solvents, electrical conductivity, hardness and melting
point.
IUPAC system
for simple ionic compounds.
Factors
influencing covalent bond formation. Electron affinity, ionization energy,
atomic size and electronegativity.
Solubility in
polar and non-polar solvents, melting point, boiling point and electrical
conductivity.
CONTENT NOTES
(f) Shapes of molecular
compounds.(g) (i) Metallic Bonding
(ii) Factors
influencing its formation.
(iii)
Properties of metals.
(h) (i) Inter molecular bonding
(ii)
Intermolecular forces in covalent compounds.
(iii) Hydrogen
bonding
(iii) van der Waals forces
(iv) Comparison of all bond types.
CONTENT
Linear,
planar, tetrahedral and shapes for some compounds e.g. BeCl2, BF3, CH4, NH3,
CO2.Factors should include: atomic radius, ionization energy and number of
valence electrons. Types of specific packing not required.
Typical
properties including heat and electrical conductivity, malleability, lustre,
ductility, sonority and hardness.
Relative
physical properties of polar and non-polar compounds.
Description of
formation and nature should be treated.
Dipole-dipole,
induced dipole-dipole, induced dipole-induced dipole forces should be treated
under van der Waal’s forces.
Variation of
the melting points and boiling points of noble gases, halogens and alkanes in
the homologous series explained in terms of van der Waal’s forces; and
variation in the boiling points of H2O, and H2S explained using Hydrogen
bonding.
NOTES
6.0 STOICHIOMETRY AND CHEMICAL REACTIONS(a) (i) Symbols, formulae and equations.
(ii) chemical
symbols
(iii)
Empirical and molecular formulae.
(iv) Chemical
equations and IUPAC names of chemical compounds.
(v) Laws of
chemical combination.
(b) Amount of substance.
CONTENT
Symbols of the
first thirty elements and other common elements that are not among the first
thirty elements.
Calculations
involving formulae and equations will be required. Mass and volume
relationships in chemical reactions and the stoichiometry of such reactions
such as: calculation of percentage composition of element.
(1) Combustion reactions (including combustion
of simple hydrocarbons)
(2) Synthesis
(3) Displacement or replacement
(4) Decomposition
(5) Ionic reactions
(1) Laws of conservation of mass.
(2) Law of constant composition.
(3) Law of multiple proportions. Explanation of
the laws to balance given equations.
(4) Experimental illustration of the law of
conservation of mass.
(1) Mass and volume measurements.
(2) The mole as a unit of measurement;
Avogadro’s constant, L= 6.02 x 1023 entities mol-1.
(3) Molar quantities and their uses.
(4) Moles of electrons, atoms, molecules,
formula units etc.
NOTES
(c) Mole ratios(d) (i) Solutions
(ii)
Concentration terms
(iii) Standard
solutions.
(e) Preparation of solutions from liquid
solutes by the method of dilution.
CONTENT
Use of mole
ratios in determining stoichiometry of chemical reactions. Simple calculations
to determine the number of entities, amount of substance, mass, concentration,
volume and percentage yield of product.(1)
Concept of a solution as made up of solvent and solute.
(2) Distinguishing between dilute solution and
concentrated solution.
(3) Basic, acidic and neutral solutions.
Mass (g) or
moles (mol) per unit volume. Emphasis on current IUPAC chemical terminology,
symbols and conventions. Concentration be expressed as mass concentration, g
dm-3, molar concentration, mol dm-3.
(1) Preparation of some primary standards e.g
anhydrous Na2CO3, (COOH)2, 2H2O/H2C2O4.2H2O.
(2) Meanning of the terms primary standard,
secondary standard and standard solution.
Dilution
factor
.
NOTES
7.0 STATES OF MATTER(a) (i) Kinetic theory of matter.
(ii) Changesof state of matter.
(iii)
Diffusion
CONTENT
(2) Use of the kinetic theory to explain the
following processes: melting of solids, boiling of liquids, evaporation of
liquids, dissolution of solutes, Brownian motion and diffusion.
(1) Changes of state of matter should be
explained in terms of movement of particles. It should be emphasized that
randomness decreases (and orderliness increases) from gaseous state to liquid
state and to solid state and vice versa.
(2)
Illustrations of changes of state using the different forms of water, iodine,
sulphur, naphthalene etc.
(3) Brownian
motion to be illustrated using any of the following experiments:
(a) pollen grains/powdered sulphur in water
(viewed under a microscope);
(b) smoke in a glass container illuminated by a
strong light from the side;
(c) a dusty room being swept and viewed from
outside under sunlight.
(1) Experimental demonstration of diffusion of
two gases.
(2) Relationship between speed at which
different gas particles move and the masses of particles.
(3) Experimental demonstration of diffusion of
solute particles in liquids.
\
NOTES
(b) Gases:(i)
Characteristics and nature of gases;
(ii) The gas
laws;
(iii)
Laboratory preparation and properties of some gases.
(c) (i) Liquids
(ii) Vapour
and gases.
CONTENT
Arrangement of
particles, density, shape and compressibility.
The Gas laws:
Charles’; Boyle’s; Dalton’s law of partial pressure; Graham’s law of diffusion,
Avogadro’s law. The ideal gas equation of state. Qualitative explanation of
each of the gas laws using the kinetic model.
The use of
Kinetic molecular theory to explain changes in gas volumes, pressure,
temperature.
Mathematical
relations of the gas law
PV= nRT
Ideal and Real
gases
Factors
responsible for the deviation of real gases from ideal situation.
(1) Preparation of the following gases: H2, NH3
and CO2. Principles of purification and collection of gases.
(2) Physical and chemical properties of the
gases.
Characteristics
and nature of liquids based on the arrangement of particles, shape, volume,
compressibility, density and viscosity.
(1) Concept of vapour, vapour pressure,
saturated vapour pressure, boiling and evaporation.
(2) Distinction between vapour and gas.
(3) Effect of vapour pressure on boiling points
of liquids.
(4) Boiling at reduced pressure.
NOTES
(d) Solids:(i) Characteristics and nature;
(ii) Types and
structures;
(iii)
Properties of solids.
(e) Structures, properties and uses of diamond
and graphite.
(f) Determination of melting points of covalent
solids.
8.0 ENERGY AND ENERGY CHANGES
(a) Energy and enthalpy
(b) Description, definition and illustrations of
energy changes and their effects.
CONTENT
(1) Ionic, metallic, covalent network and
molecular solids. Examples in each case.
(2) Arrangements of particles ions, molecules
and atoms in the solid state.
Relate the
properties of solids to the type of interatomic and intermolecular bonding in
the solids. Identification of the types of chemical bonds in graphite and
differences in the physical properties.
The uses of
diamond and graphite related to the structure.
The use of
iodine in everyday life.
Melting points
as indicator of purity of solids e.g. Phenyl methanedioic acid (benzoic acid),
ethanedioic acid (oxalic) and ethanamide.
Explanation of
the terms energy and enthalpy. Energy changes associated with chemical
processes.
(1) Exothermic and endothermic processes.
(2) Total energy of a system as the sum of
various forms of energy e.g. kinetic, potential, electrical, heat, sound etc.
(3) Enthalpy changes involved in the following
processes: combustion, dissolution and neutralization.
NOTES
9.0 ACIDS,
BASES AND SALTS(a) Definitions of acids and bases.
(b) Physical
and chemical properties of acids and bases.
(c) Acids, bases and salts as electrolytes.
(d) Classification of acids and bases.
(e) Concept of pH
(1) Arrhenius concepts of acids and bases in
terms of H3O+ and OH– ions in water.
(2) Effects of acids and bases on indicators,
metal Zn, Fe and trioxocarbonate (IV) salts and hydrogentrioxocarbonate (IV)
salts.
Characteristic
properties of acids and bases in aqueous solution to include:
(a)
conductivities, taste, litmus/indicators, feel etc.;
(b) balanced
chemical equations of all reactions.
Electrolytes
and non-electrolytes; strong and weak electrolytes. Evidence from conductivity
and enthalpy of neutralization.
(1) Strength of acids and bases.
(2) Classify acids and bases into strong and
weak.
(3) Extent of dissociation reaction with water
and conductivity.
(4) Behaviour of weak acids and weak bases in
water as example of equilibrium systems.
(1) Definition of pH and knowledge of pH scale.
(2) Measurement of pH of solutions using pH
meter, calometric methods or universal indicator.
(3) Significance of pH values in everyday life
e.g. acid rain, pH of soil, blood, urine.
CONTENT NOTES
(f) Salts:(i) Laboratory and
industrial preparation of salts;
(ii) Uses;
(iii) Hydrolysis of salt.
(g) Deliquescent, efflorescent and hygroscopic
compound.
(h) Acid-Base indicators
(i) Acid-Base titration
CONTENT
Meaning of
salts.Types of salts: normal, acidic, basic, double and complex salts.
(1) Description of laboratory and industrial
production of salts.
(2) Mining of impure sodium chloride and
conversion into granulated salt.
(3) Preparation of NaOH, Cl2 and H2.
(1) Explanation of how salts forms acidic,
alkaline and neutral aqueous solutions.
(2) Behaviour of some salts (e.g NH4Cl, AlCl3,
Na2CO3, CH3COONa) in water as examples of equilibrium systems.
(3) Effects of charge density of some cations
and anions on the hydrolysis of their aqueous solution. Examples to be taken
from group 1, group 2, group 3 and the d-block element.
Use of
hygroscopic compounds as drying agent should be emphasized.
(1) Qualitative description of how acid-base
indicator works.
(2) Indicators as weak organic acids or bases
(organic dyes).
(3) Colour of indicator at any pH dependent on
relative amounts of acid and forms.
(4) Working pH ranges of methyl orange and
phenolphthalein.
(1) Knowledge and correct use of relevant
apparatus.
(2) Knowledge of how acid-bases indicators work
in titrations.
NOTES
10.0
SOLUBILITY OF SUBTANCES
(a) General
principles
(b) Practical
application of solubility.
(3) Acid-base titration experiments involving
HCl, HNO3, H2SO4 and NaOH, KOH, Ca(OH)2, CO32-, HCO3–.(4) Titration involving weak acids versus strong
bases, strong acids versus weak bases and strong acids versus strong bases
using the appropriate indicators and their applications in quantitative
determination; e.g. concentrations, mole ratio, purity, water of
crystallization and composition.
(1) Meaning of Solubility.
(2) Saturated and unsaturated solutions.
(3) Saturated solution as an equilibrium system.
(4) Solubility expressed in terms of: mol dm-3
and g dm-3 of solution/solvent.
(5) Solubility curves and their uses.
(6) Effect of temperature on solubility of a
substance.
(7) Relationship between solubility and crystallization.
(8) Crystallization/recrystallization as a
method of purification.
(9) Knowledge of soluble and insoluble salts of
stated cations and anions.
(10)
Calculations on solubility.
Generalization
about solubility of salts and their applications to qualitative analysis. e.g.
Pb2+, Ca2+, Al3+, Cu2+, Fe2+, Fe3+, Cl–, Br–, I–, SO42-, S2-, and CO32-, Zn2+,
NH4+, SO32-
Explanation of
solubility rules.
CONTENT NOTES
11.0 CHEMICAL KINETICS AND EQUILIBRIUM SYSTEM(a) Rate of reactions:
(i) Factors
affecting rates;
(ii) Theories
of reaction rates;
(iii) Analysis
and interpretation of graphs.
(b)
Equilibrium:
(i) General
Principle;
CONTENT
(1)
Definition of reaction rate.
(2) Observable physical and changes: colour,
mass, temperature, pH, formation of precipitate etc.
(1) Physical states, concentration/ pressure of
reactants, temperature, catalysts, light, particle size and nature of
reactants.
(2) Appropriate experimental demonstration for
each factor is required.
(1) Collision and transition state theories to be
treated qualitatively only.
(2) Factors influencing collisions: temperature
and concentration.
(3) Effective collision.
(4) Activation energy.
(5) Energy profile showing activation energy and
enthalpy change.
Drawing of
graphs and charts.
Explanation of
reversible and irreversible reactions. Reversible reaction i.e. dynamic
equilibrium. Equilibrium constant K must be treated qualitatively. It must be
stressed that K for a system is constant at constant temperature.
Simple
experiment to demonstrate reversible reactions.
NOTES
(ii) Le
Chatelier’s principle.12.0 REDOX REACTIONS
(a) Oxidation
and reduction process.
(b) Oxidizing
and reducing agents.
(c) Redox
equations
(d)
Electrochemical cells:
(i) Standard
electrode potential;
(ii) Drawing
of cell diagram and writing cell notation.
CONTENT
Prediction of the effects of external
influence of concentration, temperature pressure and volume changes on
equilibrium systems.
(1) Oxidation and reduction in terms of:
(a) addition
and removal of oxygen and hydrogen;
(b) loss and
gain of electrons;
(c) change in
oxidation numbers/states.
(2) Determination of oxidation numbers/states.
(1) Description of oxidizing and reducing agents
in terms of:
(a) addition
and removal of oxygen and hydrogen;
(b) loss and
gain of electrons;
(c) change in
oxidation numbers/state.
Balancing
redox equations by:
(a) ion, electron or change in oxidation
number/states;
(b) half reactions and overall reaction.
Definition/Explanation
(1) Standard hydrogen electrode: meaning of
standard electrode potential (Eo) and its measurement.
(2) Only metal/metal ion systems should be used.
NOTES
(iii) e.m.f of
cells;(iv) Application of Electrochemical cells.
(e)
Electrolysis:
(i)
Electrolytic cells;
(ii)
Principles of electrolysis;
(iii) Factors
influencing discharge of species;
(iv) Faraday’s
laws;
(v) Practical
application;
CONTENT
(1) Electrochemical cells as a combination of
two half-cells.(2) The meaning of
magnitude and sign of the e.m.f.
(1) Distinction between primary and secondary
cells
(2) Daniell cell, lead acid battery cell, dry
cells, fuel cells and their use as generators of electrical energy from
chemical reactions.
Definition.
Comparison of
electrolytic and electrochemical cells; weak and strong electrolyte.
Mechanism of
electrolysis.
Limit
electrolytes to molten PbBr2
and NaCl,
dilute NaCl solution, concentrated NaCl solution, CuSO4(aq), dilute H2SO4,
NaOH(aq) and CaCl2(aq) (using platinum or graphite and copper electrodes).
Simple
calculations based on the relation 1F= 96,500 C and mole ratios to determine
mass, volume of gases, number of entities, charges etc. using half and overall
reactions.
Electroplating,
extraction and purification of metals.
NOTES
(vi) Corrosion
of metals.13.0 CHEMISTRY OF CARBON COMPOUNDS
(a)
Classification
(b) Functional
group
(b) Separation
and purification of organic compounds.
(c)
Petroleum/crude oil
CONTENT
(1) Corrosion treated as a redox process.
(2) Rusting of iron and its economic costs.
(3) Prevention based on relative magnitude of
electrode potentials and preventive methods like galvanizing,
sacrificial/cathodic protection and non-redox methods (painting,
greasing/oiling etc.).
Broad
classification into straight chain, branched chain, aromatic and alicyclic
compounds.
Systematic
nomenclature of compounds with the following functional groups: alkanes,
alkenes, alkynes, hydroxyl compounds (aliphatic and aromatic), alkanoic acids,
alkyl alkanoates (esters and salts) and amines.
Methods to be
discussed should include: distillation; crystallization; drying and
chromatography.
(1) Composition and classification.
(2) Fractional distillation and major products.
(3) Cracking and reforming.
(4) Petro-chemicals: sources; uses e.g. as
starting materials of organic synthesis.
(5) Quality of petrol, meaning of octane number
and its importance to the petroleum industry.
NOTES
(d) Determination of empirical and molecular
formulae and molecular structures of organic compounds.(e) General properties of organic compounds:
(i) Homologous
series;
(ii)
Isomerism.
(f) Alkanes:
(i) Sources,
properties;
(ii) Uses.
(g) Alkenes:
(i) Sources
and properties;
CONTENT
(1) Gradation in physical properties.
(2) Effects on the physical properties by
introduction of active groups into the inert alkane.
(1) Examples should be limited to compounds
having maximum of five carbon atoms.
(2) Differences between structural and
geometric/stereo isomerism.
(1) Laboratory
and industrial preparations and other sources.
(2)
Nomenclature and structure.
(3)
Reactivity:
(a)
combustion;
(b) substitution reactions;
(c) cracking
of large alkane molecules.
As fuels, as
starting materials for synthesis. Uses of haloakanes and pollution effects.
(1) Laboratory preparation.
(2) Nomenclature and structure.
NOTES
(ii) Uses;
(iii)
Laboratory detection.
(h) Alkynes:
(i) Sources,
characteristic properties and uses;
(ii) Chemical
reactions.
(i) Benzene:
(i) Structure
and physical properties;
(ii) Chemical
properties.
CONTENT
(3) Addition reactions with halogens hydrogen,
bromine water, hydrogen halides and acidified water.(4) Oxidation: hydroxylation with aqueous KMnO4.
(5) Polymerization.
Use of
reaction with Br2/water, Br2/CCl4 and KMnO4(aq) as means of characterizing
alkenes.
(1) Nomenclature and structure.
(2) Industrial production of ethyne.
(3) Uses of ethyne.
(4) Distinguishing test between terminal and
non-terminal alkynes.
(5) Test to distinguish between alkane, alkene
and alkyne.
Chemical
reactions: halogenation, combustion, hydration and hydrogenation.
Resonance in
benzene. Stability leading to substitution reactions.
(1) Addition reactions: hydrogenation and
halogenation (mechanism not required).
(2) Compare reactions with those of alkenes.
NOTES
(J)
Alkanols:(i) Sources, nomenclature and structure;
(ii)
Classification;
(iii) Physical
properties;
(iv) Chemical
properties;
(v) Laboratory test;
(vi) Uses.
(k) Alkanoic
acids:
(i) Sources,
nomenclature and structure;
(ii) Physical
properties;
CONTENT
(1) Laboratory preparation including hydration
of alkenes.
(2) Industrial and local production of ethanol
including alcoholic beverages,
(3) Harmful impurities and methods of
purification should be mentioned.
(4) Recognition of the structure of mono-, di-
and triols.
Primary,
secondary and tertiary alkanols.
Boiling point,
solubility in water. Including hydrogen bonding effect.
(1) Reaction with:
(a) Na;
(b) alkanoic acids (esterification);
(c) conc. H2SO4.
(2) Oxidation by:
(a) KMnO4(aq);
(b) K2Cr2O7(aq);
(c) I2 in NaOH(aq).
Laboratory
test for ethanol.
Methanoic acid
–insect bite.
Ethanoic acid
– vinegar.
Recognition of
mono and dioic acid.
Boiling point,
solubility in water.
Including
hydrogen bonding effect.
NOTES
(iii) Chemical
properties;(iv) Laboratory test;
(iv) Uses.
(l) Alkanoates
as drivatives of alkanoic acids:
(i) Sources,
nomenclature, preparation and structure;
(ii) Physical
properties;
(iii) Chemical
properties;
(iv) Uses.
14.0
CHEMISTRY, INDUSTRY AND THE ENVIRONMENT
(a) Chemical
industry
CONTENT
Acid
properties only i.e. reactions with H2O, NaOH, NH3, NaHCO3, Zn and Mg.
Reaction with
NaHCO3, Na2CO3.
Uses of
ethanoic and phenyl methanoic (benzoic) acids as examples of aliphatic and
aromatic acids respectively.
Preparation of
alkyl alkanoates (esters) from alkanoic acids.
Solubility,
boiling and melting point.
Hydrolysis of
alkyl alkanoates (mechanism not required).
Uses of
alkanoates to include production of soap, flavouring agent, plasticizers, as
solvents and in perfumes.
(1) Natural resources in candidate’s won
country.
(2) Chemical
industries in candidates own country and their corresponding raw materials.
(3) Distinction between fine and heavy
chemicals.
NOTES
(b) Pollution:
air, water and soil pollution;
(c)
Biotechnology.
15.0 BASIC
BIOCHEMISTRY AND SYNTHETIC POLYMERS
(a) Proteins:
(i) Sources
and properties;
(ii) Uses of
protein.
(b) Amino acids
CONTACT
(4) Factors that determine location of chemical
industries.(5) Effect of industries on
the community.
(1) Sources, effects and control.
(2) Greenhouse effect and depletion of the ozone
layer.
(3) Biodegradable and non-biodegradable
pollutants.
Food
processing, fermentation including production of gari, bread and alcoholic
beverages e.g. Local gin.
Proteins as
polymers of amino acids molecules linked by peptide or amide linkage.
Physical properties
e.g. solubility
Chemical
properties to include:
(a) hydrolysis of proteins;
(b) laboratory test using Ninhydrin/Biuret
reagent/Millons reagent.
(1) Nomenclature and general structure of amino
acids.
(2) Difunctional nature of amino acids.
NOTES
(c)
Fats/oils:(i) Sources and properties;
(ii) General
structure of fats/oils;
(iii)
Preparation of soap;
(iv) Uses of
fats/oils.
(d) Carbohydrates:
(i) Sources
and nomenclature;
(ii)
Properties;
CONTENT
As alkyl
alkanoates (esters).
From animals
and plants.
Physical
properties such as solubility.
Chemical
properties:
(a) acidic and alkaline hydrolysis;
(b) hydrogenation;
(c) test for fats and oil.
As mono-, di-,
and tri- esters of propane-1,2,3-triol (glycerol).
(1) Preparation of soap (saponification) from
fats and oils.
(2) Comparison of soap less detergents and their
action on soft and hard water.
(1) Classes of carbohydrates as:
(a) monosaccharides;
(b) disaccharides;
(c) polysaccharides.
(2) Name and components of various classes of
carbohydrates.
(1) Physical properties such as solubility of
sugars.
(2) Chemical properties- Hydrolysis of
disaccharides into monosaccharides.
(3) Test for reducing sugars using sugar strips,
Fehling’s or Benedicts solution or Tollen’s reagent.
NOTES
(iii)
Carbohydrate as examples of polymer;(iv) Uses.
(e) Synthetic
polymers:
(i)
Properties;
(ii) Uses of
polymers.
(1) Starch as a polymer made up of glucose
units.
(2) Condensation of monosaccharides to form
disaccharides and polysaccharides.
(1) Definition of terms: monomers, polymers and
polymerization.
(2) Addition and condensation polymerization.
(3) Classification and preparation based on the
monomers and comonomers.
(1) Thermoplastics and thermosets.
(2) Modification of properties of polymers.
(3) Plastics and resins.
(4) Chemical test on plastics using:
(a) heat;
(b) acids;
(c) alkalis.
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