TABLE OF CONTENTS of Chemistry
A. Physical Chemistry
1. Fundamental Concepts
2. States of Matter
3. Atomic Structure
4. Chemical Bonding
5. Chemical Energetics
6. Solutions
7. Electrochemistry
8. Chemical Equilibrium
9. Reaction Kinetics
B. Inorganic Chemistry
1. Periods
2. Groups
3. Transition elements
4. Elements of Biological Importance
C. Organic Chemistry
1. Fundamental Principles
2. Hydrocarbon
3. Alkyl Halides
4. Alcohols and Phenols
5. Aldehydes and Ketones
6. Carboxylic Acid
7. Amino Acids
8. Macromolecules
9. Environmental Chemistry
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Topic
MCQs
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A. Physical Chemistry
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1. Fundamental concepts
02
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2. States of matter 02
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3. Atomic structure 02
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4. Chemical bonding 02
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5. Chemical energetics 02
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6. Solutions 02
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7. Electrochemistry 02
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8. Chemical Equilibrium 02
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9. Reaction kinetics 02
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B. Inorganic Chemistry
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1. Periods 02
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2. Groups 02
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3. Transition elements 02
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4. Elements of biological importance 04
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C. Organic Chemistry
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1. Fundamental principles 02
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2. Hydrocarbon 02
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3. Alkyl halides 02
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4. Alcohols and Phenols 04
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5. Aldehydes and Ketones 03
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6. Carboxylic acid 03
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7. Amino acids 06
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8. Macromolecules 06
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9. Environmental chemistry 02
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Total 58
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A. PHYSICAL CHEMISTRY
1. FUNDAMENTAL CONCEPTS:
In this topic, candidate should be able to:
a) Define
relative atomic, isotopic,
molecular and formula
masses, based on the
scale.
b) Explain mole in terms of the Avogadro’s constant.
c) Apply mass
spectrometric technique in
determining the relative
atomic mass of an
element using the mass spectral data provided.
d) Calculate empirical and molecular formulae, using
combustion data.
e) Understand stoichiometric calculations using mole concept
involving.
i) Reacting masses
ii) Volume of gases
2. STATES OF MATTER:
In this topic, candidate should be able to:
a) Understate gaseous state with reference to:
i) Postulates of kinetic molecular theory
ii) Deviation of real gases from ideal behavior
iii) Gas laws: Boyle’s
law, Charles law,
Avogadro’s law and
gas equation (PV=nRT)
and calculations involving gas laws.
iv) Deviation of real gases from ideal behaviour at low
temperature and high pressure
v) Causes of deviation from ideal behaviour
vi) Conditions necessary for gasses to approach ideal
behaviour
b) Discuss liquid state with reference to:
Evaporation, vapour
pressure, boiling and hydrogen bonding in water
c) Explain the lattice structure of a crystalline solid with
special emphasis on:
i) Giant ionic structure, as in sodium chloride.
ii) Simple molecular, as in iodine
iii) Giant molecular, as in graphite; diamond; silicon(IV)
oxide
iv) Hydrogen-bonded, as in ice
v) Metallic as in Cu and Fe.
d) Outline the importance of hydrogen bonding to the
physical properties of substances,
including NH3, H2O, C2H5OH and ice.
e) Suggest from quoted
physical data the
type of structure
and bonding present
in a
substance
3. ATOMIC STRUCTURE:
In this topic, candidate should be able to:
a) Identify and describe
the proton, neutron
and electron in
terms of their
relative
charges and relative masses
b) Discuss the behaviour of beams of protons, neutrons and
electrons in electric fields
c) Calculate the distribution of mass and charges within an
atom from the given data
d) Deduce the number
of protons, neutrons
and electrons present
in both atoms and
ions for a given proton and nucleon numbers/charge.
e)
i) Describe the contribution
of protons and
neutrons to atomic
nuclei in terms
of
proton number and nucleon number
ii) Distinguish
between isotopes on
the basis of
different numbers of
neutrons
present
f) Describe the number and relative energies of the s, p and
d orbitals for the principal
quantum numbers 1, 2 and 3 and also the 4s and 4p orbitals
g) Describe the shapes of s and p orbitals
h) State the electronic configuration of atoms and ions
given the proton number/charge
i) Explain:
i) Ionization energy
ii) The factors influencing the ionization energies of
elements
iii) The trends in ionization energies across a Period and
down a Group of the Periodic
Table
4. CHEMICAL BONDING:
In this topic, candidate should be able to:
a) Characterise electrovalent (ionic) bond as in sodium
chloride and Calcium oxide.
b) Use the ‘dot-and-cross’ diagrams to explain
i) Covalent
bonding, as in
hydrogen(H2); oxygen(O2); chlorine(Cl2); hydrogen
chloride; carbon dioxide; methane and ethane.
ii) Co-ordinate
(dative covalent) bonding,
as in the
formation of the
ammonium ion and in H3N+BF3
c) Describe the shapes and bond angles in molecules by using
the qualitative model of
electron-pair repulsion theory up to 4 pairs of electron
including bonded electron pair
and lone pair around central atom.
d) Describe covalent bonding in terms of orbital overlap,
giving σ and Π bonds
e) Explain the shape
of, and bond
angles in ethane,
ethene and benzene
molecules in
terms of σ and Π bonds
10
f) Describe
hydrogen bonding, using
ammonia and water
as simple examples
of
molecules containing N-H and O-H groups
g) Explain the terms
bond energy, bond
length and bond
polarity and use
them to
compare the reactivities of covalent bonds
h) Describe
intermolecular forces (Van
der Waal’s forces), based
on permanent and
induced dipoles, asin CHCl3,Br2 and in liquid noble gases
i) Describe metallic bonding in terms of a lattice of
positive ions surrounded by mobile
electrons
j) Describe,
interpret and/or predict
the effect of
different types of
bonding (ionic
bonding;
covalent bonding; hydrogen
bonding; Van der
Waal’s forces and metallic
bonding) on the physical properties of substances
k) Deduce the type of bonding present in a substance from
the given information
5. CHEMICAL ENERGETICS:
In this topic, candidate should be able to:
a) Understand
concept of energy
changes during chemical
reactions with examples
of
exothermic and endothermic reactions.
b) Explain and use the terms:
i) Enthalpy change of reaction and standard conditions, with
particular reference to:
Formation; combustion; hydration; solution; neutralization
and atomisation
ii) Bond energy (ΔH positive, i.e. bond breaking)
iii) Lattice energy (ΔH negative, i.e. gaseous ions to solid
lattice)
c) Find heat of
reactions/neutralization
from experimental results
using mathematical
relationship.
∆H=mc∆T
d) Explain, in
qualitative terms, the
effect of ionic
charge and of
ionic radius on the
numerical magnitude of lattice energy
e) Apply Hess’s
Law to
construct simple energy
cycles, and carry
out calculations
involving such cycles and relevant energy terms, with
particula r reference to:
i) Determining enthalpy changes that cannot be found by
direct experiment, e.g. an
enthalpy change of formation from enthalpy changes of
combustion
ii) Average bond energies
iii) Born-Haber cycles (including ionisation energy and
electron affinity)
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6. SOLUTIONS:
In this topic, candidate should be able to:
a) Describe and explain following concentration units of
solutions
i) Percentage composition
ii) Molarity (M)
iii) Molality (m)
iv) Mole fraction (X)
v) Parts of million (ppm)
b) Understand concept and applications of colligative
propertiessuch as:
i) Elevation of boiling point
ii) Depression of freezing point
iii) Osmotic pressure
7. ELECTROCHEMISTRY:
In this topic, candidate should be able to:
a) Explain the industrial processes of the electrolysis of
brine, using a diaphragm c ell
b) Describe and explain redox processes in terms of electron
transfer and/or of changes
in oxidation number
c) Define the terms:
Standard electrode (redox) potential and Standard cell
potential
d) Describe the standard hydrogen electrode as reference
electrode
e) Describe
methods used to
measure the standard
electrode potentials of metals or
non-metals in contact with their ions in aqueous solution
f) Calculate a standard cell potential by combining two
standard electrode potentials
g) Use standard cell potentials to:
i) Explain/deduce the direction of electron flow in the
external circuit.
ii) Predict the feasibility of a reaction
h) Construct redox equations using the relevant
half-equations
i) State the possible advantages of developing the H2/O
2
fuel cell
j) Predict and to
identify the substance liberated
during electrolysis from
the state of
electrolyte (molten or aqueous), position in the redox
series (electrode potential) and
concentration
8. CHEMICAL EQUILIBRIUM:
In this topic, candidate should be able to:
a) Explain, in
terms of
rates of the
forward and reverse
reactions, what is
meant by a
reversible reaction and dynamic equilibrium
b) State Le Chatelier’s
Principle and apply
it to deduce
qualitatively the effects
of
changes in temperature, concentration or pressure, on a
system at equilibrium
c) Deduce
whether changes in
concentration, pressure or
temperature or the
presence
of a catalyst affect the value of the equilibrium constant
for a reaction
d) Deduce
expressions for equilibrium
constants in terms of
concentrations, Kc, and
partial pressures, Kp
e) Calculate the values
of equilibrium constants
in terms of
concentrations or partial
pressures from appropriate data
f) Calculate the quantities present at equilibrium, given
appropriate data
g) Describe and explain the conditions used in the Haber
process.
h) Understand and use the Bronsted-Lowry theory of acids and
bases
i) Explain qualitatively the differences in behaviour
between strong and weak acids and
bases and the
pH values of
their aqueous solutions
in terms of
the extent of
dissociation
j) Explain the terms pH; Ka; pKa; Kw and use them in
calculations
k) Calculate [H+(aq)] and pH values for strong and weak
acids and strong bases
l) Explain how buffer solutions control pH
m) Calculate the pH of buffer solutions from the given
appropriate data
n) Show understanding of, and use, the concept of solubility
product, Ksp
o) Calculate Ksp from concentrations and vice versa
p) Show understanding of the common ion effect
9. REACTION KINETICS:
In this topic, candidate should be able to:
a) Explain and
use the
terms: rate of
reaction; activation energy;
catalysis; rate
equation; order of
reaction; rate constant;
half-life of a
reaction; rate-determining
step
b) Explain qualitatively, in terms of collisions, the effect
of concentration changes on the
rate of a reaction
c) Explain that, in the presence of a catalyst, a reaction
has a different mechanism, i.e.
one of lower activation energy
d) Describe enzymes as biological catalysts (proteins) which
may have specific activity
e) Construct and use rate equations of theform
Rate = k[A]m[B]n with special emphasis on:
i) Deducing the order of a reaction by the initial rates
method
ii) Justifying,
for zero- and first-order
reactions, the order
of reaction from
concentration-time graphs
iii) Verifying
that a suggested
reaction mechanism is
consistent with the
observed
kinetics
iv) Predicting the order that would result from a given
reaction mechanism (and vice
versa)
v) Calculating an initial rate using concentration data
f) Show understanding that the half-life of a first-order
reaction is independent of initial
concentration and use the half-life to calculate order of
reaction.
g) Calculate the rate constant from the given data
h) Name a suitable method for studying the rate of a
reaction, from given information
B. INORGANIC CHEMISTRY
1. PERIODS:
In this topic, candidate should be able to:
Discuss the variation in the physical properties of elements
belonging to period 2 and 3
and to describe
and explain the
periodicity in the
following physical properties
of
elements.
a) Atomic radius
b) Ionic radius
c) Melting point
d) Boiling point
e) Electrical conductivity
f) Ionization energy
2. GROUPS:
In this topic, candidate should be able to:
Describe and explain
the variation in
the properties of
group II, IV
and VII elements
from top to bottom with special emphasis on:
a) Reactions of group-II elements with oxygen and water
b) Characteristics of oxides of carbon and silicon
c) Properties of halogens
and uses of
chlorine in water
purification and as
bleaching
agent
d) Uses of Nobel gases (group VIII)
3. TRANSITION ELEMENTS:
In this topic, candidate should be able to:
Discuss the chemistry of transition elements of 3-d series
with special emphasis on:
a) Electronic configuration
b) Variable oxidation states
c) Use as a catalyst
d) Formation of complexes
e) Colour of transition metal complexes
4. ELEMENTS OF BIOLOGICAL IMPORTANCE:
In this topic, candidate should be able to:
a) Describe the inertness of Nitrogen
b) Manufacture of Ammonia by Haber process
c) Discuss the preparation of Nitric acid and nitrogenous
fertilizers
d) Describe the presence of Suphur dioxide in the atmosphere
which causes acid rain
e) Describe the manufacture of Sulphuric acid by contact
method
C. ORGANIC CHEMISTRY
1. FUNDAMENTAL PRINCIPLES:
In this topic, candidate should be able to:
a) Classify the organic compounds
b) Explain the types of bond fission, homolytic and
heterolytic
c) Discuss the types of organic reactions; Polar and free
radical
d) Discuss the types of reagents; nucleophile, electrophile
and free radicals
e) Explain isomerism; structural and cis-trans
f) Describe and explain condensed structural formula,
displayed and skeletal formula
g) Discuss
nomenclature of organic
compounds with reference
to IUPAC names
of
Alkanes, Alkenes, Alcohols and Acids
2. HYDROCARBON:
In this topic, candidate should be able to:
Describe the chemistry of Alkanes with emphasis on
a) Combustion
b) Free radical substitution including mechanism
Discuss the chemistry of Alkeneswith emphasis on
a) Preparation of alkenes by elimination reactions
i) Dehydration of alcohols
ii) Dehydrohalogenation of Alkyl halide
b) Reaction of Alkenes suchas
i) Catalytic hydrogenation
ii) Halogenation (Br2
addition to be used as a test of an alkene)
iii) Hydration of alkenes
iv) Reaction with HBr with special reference to
Markownikoff’s rule
v) Oxidation of alkenes
using Bayer’s reagent
(cold alkaline KMnO4
) and using
hot
concentrated acidic KMnO4
for cleavage of double bond
vi) Polymerization of ethene
Discuss chemistry of Benzenewith examples
a) Structure of benzene
showing the delocalized Π-orbital
which causes stability
of
benzene
b) Electrolphillic substitution reactions of benzene
i) Nitration including mechanism
ii) Halogenation
iii) Friedel Craft’s reaction
3. ALKYL HALIDES:
In this topic, candidate should be able to:
a) Discuss importance
of halogenoalkanes in
everyday life with
special use of
CFCs,
halothanes, CCl4
, CHCl3and Teflon
b) Reaction of alkyl halides such as:
SN-reactions,
(Reactions of alcohols
with aqueous KOH, KCN in
alcohol and with
aqueous NH3)
Elimination reaction with alcoholic KOH to give alkenes.
4. ALCOHOLS AND PHENOLS:
In this topic, candidate should be able to:
Discus Alcohols with reference to
a) Classification of alcohols into primary, secondary and
tertiary
b) Preparation of ethanol byfermentation process
c) Reaction of alcohol with
i) K2
Cr2O7 + H2SO4
ii) PCl
iii) Na-metal
iv) Alkaline aqueous Iodine
v) Esterification
vi) Dehydration
Phenols
a) Discuss reactions of phenol with:
i) Bromine ii) HNO
b) Explain the relative acidity of water, ethanol and phenol
5. ALDEHYDES AND KETONES:
In this topic, candidate should be able to:
a) Describe the structure of aldehyde and ketones
b) Discuss preparation of aldehydes and ketones by oxidation
of alcohols
c) Discuss following reactions of aldehydes and ketones
i) Common to both
2,4-DNPH
HCN
ii) Reactions in which Aldehydes differs from ketones
Oxidation with K2
Cr2O7 + H2SO4, Tollen’s reagent and Fehling solution
Reduction with sodium
boron hydride
iii) Reaction which show presence of CH3
CO group in aldehydes and ketones
Triiodomethane test
(Iodo form test) using alkaline aqueous iodine.
6. CARBOXYLIC ACID:
In this topic, candidate should be able to:
a) Show preparation of ethanoic acid by oxidation of ethanol
or by the hydrolysis of
CH3CN
b) Discuss the reactions of ethanoic acid with emphasis on:
i) Salt formation
ii) Esterification
iii) Acid chloride formation
iv) Amide formation
c) Hydrolysis of amide in basic and acidic medium
d) Describe the strength of organic acids relative to chloro
substituted acids
7. AMINO ACIDS:
In this topic, candidate should be able to:
a) Describe the general structure of α-amino acids found in
proteins
b) Classify the amino acids on the basis of nature of
R-group
c) Describe what is meant by essential amino acids
d) Understand peptide bond formation and hydrolysis of
polypeptides/protein
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8. MACROMOLECULES:
In this topic, candidate should be able to describe and
explain
a) Addition polymers such as polyethene, polypropene,
polystyrene and PVC.
b) Condensation polymers such as polyesters, nylon
c) Structure of proteins
d) Chemistry of carbohydrates
e) Chemistry of lipids
f) Enzymes
g) Structureand function of nucleic acid (DNA & RNA)
9.
ENVIRONMENTAL CHEMISTRY:
In this topic, candidate should be able to
a) Understand causes of water pollution
b) Discuss disposal of solid wastes
c) Understand chemistry and causes of
i) Smog
ii) Acid rain
iii) Ozone layer
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