R/ISU/11/02
NANYANG TECHNOLOGICAL UNIVERSITY
ENTRANCE EXAMINATION FOR FOREIGN APPLICANTS
SYLLABUS FOR CHEMISTRY
STRUCTURE OF EXAMINATION PAPER
1.
The examination consists of ONE (1) theory paper which contains THREE (3) sections:
a. Section A: Fifteen (15) multiple-choice questions which are relatively simple and do
not require the knowledge of more than one concept to answer. Each question carries
1 mark.
b. Section B: Fifteen (15) multiple-choice questions which may require the knowledge of
more than one concept to answer. Each question carries 3 marks.
c. Section C: Four (4) structured questions carrying 10 marks each.
2.
Candidates are required to answer ALL the questions.
3.
All the questions are derived from topics as described in the syllabus.
SYLLABUS
Section I - Physical Chemistry
1.
Atoms, Molecules and Stiochiometry
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2.
Atomic Structure
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3.
Relative masses of atoms and molecules
The mole, the Avogadro constant
The determination of relative atomic masses, Ar, and relative molecular masses, Mr,
from mass spectra
The calculation of empirical and molecular formulae.
Reacting masses and volumes (of solutions and gases)
The nucleus of the atom: neutrons and protons, isotopes, proton and nucleon numbers
Electrons: electronic energy levels, ionisation energies, atomic orbitals, extranuclear
structure
Chemical Bonding
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Ionic (electrovalent) bonding
Covalent bonding and co-ordinate (dative covalent) bonding
(a) The shapes of simple molecules
(b) Bond energies, bond lengths and bond polarities
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Intermolecular forces, including hydrogen bonding
Metallic bonding
Bonding and physical properties
1
4.
5.
States of Matter
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The gaseous state:
(a) Ideal gas behaviour and deviations from it
(b) pV = nRT and its use in determining a value for Mr
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The liquid state. The kinetic concept of the liquid state and simple kinetic-molecular
descriptions of changes of state
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The solid state. Lattice structures and spacing
Chemical Energetics
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6.
7.
8.
Enthalpy changes: H, of formation; combustion; hydration; solution;
neutralisation; atomisation; bond energy; lattice energy; electron affinity
Hess’ Law, including Born-Haber cycles
Electrochemistry
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Redox processes: electron transfer and changes in oxidation number (oxidation state)
Electrode potentials
(a) Standard electrode (redox) potentials, E; the redox series
(b) Standard cell potentials, E cell
(c) Batteries and fuel cells
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Electrolysis
(a) Factors affecting the amount of substance liberated during electrolysis
(b) The Faraday constant: the Avogadro constant: their relationship
(c) Industrial uses of electrolysis
Equilibria Content
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Chemical equilibria: reversible reactions; dynamic equilibrium
(a) Factors affecting chemical equilibria
(b) Equilibrium constants
(c) The Haber process
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Ionic equilibria
(a) Bronsted-Lowry theory of acids and bases
(b) Acid dissociation constants, Ka and the use of pKa
(c) The ionic product of water, Kw
(d) pH: choice of pH indicators
(e) Buffer solutions
(f)
Solubility product; the common ion effect
Reaction Kinetics
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Simple rate equations; orders of reaction; rate constants
Effect of temperature on rate constants; the concept of activation energy
Homogeneous and heterogeneous catalysis
2
Section II - Inorganic Chemistry
9.
10.
The Periodic Table: Chemical Periodicity
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Periodicity of physical properties of the elements: variation with proton number across
the third period (sodium to argon) of:
(a) atomic radius and ionic radius
(b) melting point
(c) electrical conductivity
(d) ionisation energy
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Periodicity of chemical properties of the elements in the third period
(a) Reaction of the elements with oxygen, chlorine and water
(b) Variation in oxidation number of the oxides (sodium to sulphur only) and of the
chlorides (sodium to phosphorus only)
(c) Reactions of these oxides and chlorides with water
(d) Acid/base behaviour of these oxides and the corresponding hydroxides
GROUP II
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11.
Similarities and trends in the properties of the Group II metals magnesium to barium
and their compounds
Some uses of Group II compounds
GROUP VII
The similarities and trends in the physical and chemical properties of chlorine, bromine and
iodine
 Characteristic physical properties
 The relative reactivity of the elements as oxidising agents
 Some reactions of the halide ions
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The manufacture of chlorine
 The reactions of chlorine with aqueous sodium hydroxide
 The important uses of the halogens and of halogen compounds (see also Section 10.4)
12.
An Introduction To The Chemistry Of Transition Elements
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General physical and characteristic chemical properties of the first set of transition
elements, titanium to copper
Colour of complexes
Section III - Organic Chemistry
13.
Introductory Topics
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Molecular, structural and empirical formulae
Functional groups and the naming of organic compounds
Characteristic organic reactions
Shapes of organic molecules; and bonds
Isomerism: structural; cis-trans; optical
3
14.
Structural Identification Of Organic Compounds By NMR Spectroscopy
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15.
16.
17.
18.
NMR spectroscopy
Hydrocarbons
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Alkanes (exemplified by ethane)
(a) Free-radical reactions
(b) Crude oil and ‘cracking’
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Alkenes (exemplified by ethene)
(a) Addition and oxidation reactions
(b) Industrial importance
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Arenes (exemplified by benzene and methylbenzene)
(a) Influence of delocalised electrons on structure and properties
(b) Substitution reactions with electrophiles
(c) Oxidation of side-chain
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Hydrocarbons as fuels
Halogen Derivatives
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Halogenoalkanes and halogenoarenes
(a) Nucleophilic substitution
(b) Hydrolysis
(c) Formation of nitriles, primary amines
(c) Elimination
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Relative strength of the C-Hal bond
Hydroxy Compounds
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Alcohols (exemplified by ethanol)
(a) Formation of halogenoalkanes
(b) Reaction with sodium; oxidation; dehydration; esterification; acylation
(c) The tri-iodomethane test
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Phenol
(a) Its acidity; reaction with sodium
(b) Nitration of, and bromination of, the aromatic ring
Carbonyl Compounds
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Aldehydes (exemplified by ethanal)
(a) Oxidation to carboxylic acid
(b) Reaction with hydrogen cyanide
(c) Characteristic tests for aldehydes
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Ketones (exemplified by propanone and phenylethanone)
(a) Reaction with hydrogen cyanide
(b) Characteristic tests for ketones
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19.
20.
21.
Carboxylic Acids And Derivatives
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Carboxylic acids (exemplified by ethanoic acid and benzoic acid)
(a) Formation from primary alcohols and nitriles
(b) Salt, ester and acyl chloride formation
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Acyl chlorides (exemplified by ethanoyl chloride)
(a) Ease of hydrolysis compared with alkyl and aryl chlorides
(b) Reaction with alcohols, phenols and primary amines
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Esters (exemplified by ethyl ethanoate and phenyl benzoate)
(a) Formation from carboxylic acids and from acyl chlorides
(b) Hydrolysis (under acidic and under basic conditions)
(c)
Uses of esters
Nitrogen Compounds
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Primary amines (exemplified by ethylamine and phenylamine)
(a) Their formation
(b) Salt formation
(c) Other reactions of phenylamine
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Amides (exemplified by ethanamide)
(a) Their formation from acyl chlorides
(b) Their hydrolysis
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Amino acids (exemplified by aminoethanoic acid)
(a) Their acid and base properties
(b) Zwitterion formation
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Proteins
(a) Their structure, based on the peptide linkage
(b) The hydrolysis of proteins
Polymerisation
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Addition polymerisation
Condensation polymerization
7 Oct 2002
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