TABLE OF CONTENT
About Us...................................................................................Page 3
Chapter One
Aims & Objectives.....................................................................Page 5
Chapter Two
Syllabus...................................................................................Page 6
Chapter Three
Recommended Textbooks.......................................................Page 19
Chapter Four
JUPEB Grading System............................................................Page 21
ABOUT US
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ABOUT Joint Universities Preliminary
Examinations Board (JUPEB)
JUPEB means Joint Universities Preliminary Examinations Board. It was introduced
by the University of Lagos State (UNILAG) in December 2013. JUPEB is accepted in
over 95% of universities in Nigeria.
History of JUPEB
The Joint Universities Preliminary Examinations Board (JUPEB) is a national examinations body approved by the Federal Government of Nigeria first established in December 2013 but formally introduced in April 2014 by a consortium of ten (10) partnering universities led by the University of Lagos.
The board is responsible for conducting common and standard examinations for
candidates, who have been exposed to a minimum of one year of approved courses
in the different Universities’ Foundation and/or Diploma Programmes and are seeking Direct Entry admissions into University courses at the 200 Level in Nigerian and
partnering foreign universities.
The first JUPEB examination was conducted in August 2014 and successful candidates were admitted into the 200 Level by JAMB based on recommendations from
the universities from 2015, JUPEB Examinations are often held in June annually.
The main JUPEB syllabus is the property of The Joint University Preliminary Examinations.
This ebook is only for education purposes.
No copyright issues intended.
Chapter One
Aims & Objectives
ABOUT
Chemistry is an important subject for every science student who wants to
go into the medical field or related science courses. In some schools, even
Computer Science and some Engineering departments require you to write
and pass Chemistry before being admitted into 200 level.
Syllabus.ng has put out a well-detailed syllabus for the JUPEB
Chemistry. This material is for candidates who want to score high in their
JUPEB Chemistry exam.
Study and understand the syllabus, read up on past questions, and
follow the additional tips provided, we can assure you that you stand a
higher chance of scoring high in your exams if you do this. With this
syllabus, you don't have to be scared of Chemistry or the exam.
Download, read, and practice past questions and you are well on your way
to scoring higher than your coursemates in the JUPEB program.
What Course Of Study Can One Choose with JUPEB Chemistry?
With a pass in your JUPEB Chemistry exam, you can study Medicine, Nursing, Anatomy, or any Natural and/or Biological science course.
First Semester Courses + Unit For JUPEB Chemistry
COURSE CODE
COURSE TITLE
CREDIT LOAD
CHM001
GENERAL CHEMISTRY
3 Units
CHM002
PHYSICAL CHEMISTRY
3 Units
CHM001 Practicals
1. Sensitivity of weighing equipment, Graduation of measuring
equipment, and determination of significant figures in reading
2. Preparation of standard solutions: Serial dilution;
3. Volumetric analysis: Practice in volumetric analysis, acid-base redox, and
precipitation titrations. Acid-base titrimetry involving NaOH, oxalic acid, HCl,
and Na, CO, Determination of percentage composition of iron using KMnO,
(redox Titrimetry), Titrimetric analysis of mixtures, NaOH/NaHCO, and Na,
CO/NaHCO; and
4. Introduction to the statistical analysis of data: Use of supplied dan to illustrate elements of simple statistics.
CHM 002 Practicals
1. Experiments to calculate enthalpy changes.
2. Determination of molecular mass using freezing point depression.
Second Semester Courses + Unit For JUPEB Chemistry
COURSE CODE
COURSE TITLE
CREDIT
LOAD
CHM003
INORGANIC
CHEMISTRY
3 units
CHM004
ORGANIC CHEMISTRY
3 units
CHM003 PRACTICALS
● Qualitative Inorganic Practical
1. Flame tests and systematic analysis of mixtures containing two salts.
2. Identification of anions: preliminary tests for anions, preparation of Na,
CO, extracts, and confirmatory tests.
3. Identification of cations group I VI: Group separation and analysis of ions
within a group (group analysis).
CHM004 PRACTICALS
1. Reactions of simple functional groups: Simple organic tests, solubility,
sodium fusion test, functional group identification(with sand carboxylic
acids). emphasis on ketones aldehydes and carboxylic acids
2. Recrystallization and determination of the melting point of organic compounds
SN
Chapter Two
Syllabus
TOPICS
1 MEASUREMENTS
2 NATURE OF MATTER
3 ATOMIC MASSES
JUPEB CHEMISTRY SYLLABUS
OBJECTIVES
FIRST SEMESTER
CHM001: GENERAL CHEMISTRY
i. Units of measurement
a) Basic S.I. Units,
b) Derived units,
c) Conversion of units,
d) Significant figures,
e) Precision and accuracy,
f) Errors(systematic and random errors), g) Exact
numbers
i. States of matter
a) Solid, liquid and gaseous states,
b) Properties and inter-conversion.
i. Definitions and calculations of molar masses of
atoms and molecules based on "C scale,
ii. Use of mass spectrometry in the
determination of Relative Atomic Mass and
iii. Relative Molecular mass
4 ATOMIC STRUCTURE
i. Dalton's atomic theory.
ii. Discovery of sub-atomic particles
a) Various experiments that led to the discovery
of neutrons, protons,
b) Electrons and nucleus (cathode ray,
c) Millikan's oil drop,
d) Rutherford's and Thompson's experiments),
e) Calculations of relative abundances and
isotopic mass;
iii. Planck's Theory
a) Black body radiation,
b) Photoelectric effect,
c) Quantisation of energy;
iv. Bohr's Theory
a) Bohr's assumption,
b) Atomic spectra of hydrogen(no derivation is
required) and
c) Determination of spectra lines, determination
of ionisation energy from line spectra(when n=0);
v. Wave Theory of Atoms
a) Particle wave duality,
b) Atomic orbitals,
c) Quantum numbers(n,l,m,s),
d) Electronic ener levels,
e) Degeneracy of atomic orbitals,
f) Shapes of atomie orbitals(s,p and id orbitals)
vi. Electronic configuration of Atoms and ions
a) Aufbau principle,
b) Pauli's exclusion principle,
c) Hund's rule, (n+1) rule
5 PERIODICITY
i. Development of the modem periodic table,
ii. Building up periods,
6 MOLE CONCEPT
iii. Atomic properties
a) Identifying blocks and groups of elements,
b) Periodic law.
c) Trends of atomic size,
d) Ionisation potential,
e) Electron affinity,
f) Electronegativity a and ionic radii,
g) Isoelectric species.
i. Mole and Avogadro's constant
a) Various ways of defining the molt,
b) Avogadro's constant, molar mass.
ii. Empirical and molecular formula
a) Definition and calculations of Empirical and
Molecular formulae from percentage composition
by mass and combustion data.
7 TYPES OF CHEMICAL
REACTIONS
iii. Solution Stoichiometry
a) Balancing chemical equations, calculations
based on stoichiometric coefficients,
b) Reaction that involve limiting reactants,
c) Calculation of actual and percentage yields.
d) Calculation of molarity and gram
concentration,
e) Preparation of standard solutions, serial
dilution.
i. Neutralization
a) Definition identification of neutralization
reactions.
b) Predicting solubilities.
ii. Precipitation, Oxidation and Reduction
a) Various definitions of oxidation and reduction
reaction with emphasis on definition of terms of
electron transfer,
b) Calculation of oxidation numbers, balancing of
redox reactions by oxidation state and halfreaction method (both in acidic and basic
media). OM
8 CHEMICAL BONDING
i. Electrovalent/Ionic Bonding
a) Describe ionic bending using some ionic
compounds e.g. NaCl,
b) Energy considerations of ionic bonding,
definition of lattice energy (no derivation),
properties of ionic compounds.
ii. Covalent Bonding
a) Describe covalent bonding using simple
covalent compounds e,g, CO₂,
b) Coordinate/dative covalent bonding e.g. in
ammonium ion (NH4), Al,Cl,
c) Molecule, bond energy, bond length and bond
polarity(Fajan's rule),
d) Properties of covalent compounds,
hybridisation concept (sp, sp sp²),
e) Shapes of simple molecules using the valence
shell electron-pair repulsion theory eg. H₂O, NH,
CH, etc.
iii. Intermolecular Bonding
a) Van der waals forces,
b) Permanent and induced dipoles,
c) Hydrogen bonding.
iv. Metallic Bonding
a) Describe metallic bonding in terms of a lattice
of positive ions surrounded by delocalised
electrons.
v. Bonding and physical properties
a) The effect of different types of bonding on the
physical properties of substances (e.g. unusual
high boiling point of water, miscibile of water
and ethanol, nylon, polyester).
CHM002: PHYSICAL CHEMISTRY
9 KINETIC MOLECULAR
i. Gas Laws
THEORY OF GASES
a) Statement of and calculations involving
Boyle's, Charles', Dalton's, Graham's laws and
Avogadro's hypothesis.
10 SOLUTION
ii. Ideal and Real Gases
a) Ideal gas equations,
b) Kinetic theory of gases (assumptions only),
c) Real gases deviation from ideal gas behaviour,
d) Van der Waal's equation.
e) Use of the general gus equation. PV=nRT in
calculations, including relative molecular mass
determination
i. Phase and phase diagram
a) Interpretation of phase diagram for one
component system.
ii. Ideal and non-ideal solutions
a) Definition of ideal and non-ideal solutions,
Raoult's Law
iii. Colligative Properties
a) Lowering of vapour pressure,
b) Depression of freezing,
c) Elevation of boiling point and osmotic
pressure.
d) Determination of molar mass using osmotic
pressure. (The derivation not required).
11 THERMOCHEMISTRY
i. Enthalpy change
a) Exothermic and endothermic changes,
b) Definition of enthalpy changes for processes
(combustion, neutralization, hydration,
formation, solution, atomization) under standard
condition.
ii. Hess' Law
a) State Hess' law and construct energy cycles
based on Hess' law and carry out calculations
based on Hess' law
b) Use of bond energy to calculate energy
changes.
12 ELECTROCHEMISTRY
iii. Introduction to Chemical Thermodynamics
a) Definition of entropy and Gibbs's free energy.
b) Calculation of entropy change
c) Calculation of Gibb's free energy change for
reactions using AG AH-TAS.
d) Predicting the spontaneity of reactions
i. Electrolysis
a) Faraday's first and second laws of electrolysis
and calculations based on them.
ii. Electrochemical Cells
a) Identify the substances liberated during
electrolysis based on the state of electrolyte,
b) Position in electrochemical series
c) Concentration of electrolyte and
d) Nature of electrodes
iii. Fuel Cells and Batteries
a) Definitions of electrode potential standard
electrode potential,
b) Cell potential Calculations of e.m.f of a cell
c) Application of Nernst equation
d) Use of cell potential to predict the feasibility
of reaction Industrial uses of electrolysis.
iv. H/O₂ fuel cell,
v. Rechargeable batteries
13 CHEMICAL KINETICS
14 EQUILIBRIUM STATE
i. Rate Equation
a) Definition of rate of reaction and reaction
mechanism.
b) Factors affecting rate of reaction.
c) Orders of reaction, rate constants and
molecularity.
d) Calculations of order of reaction from
experimental date
ii. Activation Energy Catalysis
a) Simple collision theory.
b) Definition of activation energy.
c) Arrhenius equation.
d) Homogeneous and Heterogeneous catalysis
i. Mass Action
a) Equilibrium changes, reaction quotient (Q),
equilibrium expressions (homogenous and
heterogeneous equilibra).
b) Calculations of equilibrium constants in terms
of concentration (K) and partial
pressure (K).
c) Relationship between Ke and K
ii. Le-Chatelier's Principle
a) Statement and Application of Le- Chatelier's
principle to deduce the effects of changes in
temperature, pressure and concentration on a
system at equilibrium.
b) Definitions of acid and base in terms of;
Arrhenius, Bronsted- Lowry and Lewis concept.
Auto-ionisation of water.
iii. Acid-Base Equilibra
a) Acid strengths, pH solution.
b) Indicator theory
c) Solubility product, common ion effect.
d) Selective precipitation of ions.
iv. Ionic Equilibra in Aqueous System
Radioactivity
15 NUCLEAR CHEMISTRY
I. Radioactivity
a) History of Radioactivity.
b) Types of radiations.
c) Radioactive disintegration.
d) Nuclear equations, half-life, radioactive
carbon
e) Detectors and applications of radioactivity.
SECOND SEMESTER
CHM003: INORGANIC CHEMISTRY
i. General trends in properties of elements
16 PERIODICITY OF
a) Nature of elements, trends, in physical and
ELEMENTS
chemical properties of elements
17 CHEMISTRY OF HYDROGEN i. Occurrence, isotopes, preparation and
reactions of hydrides
i. Group 1
18 S-BLOCK ELEMENTS
a) Physical and chemical properties, extraction of
group 1 metals e.g Sodium, trends in properties
of their compounds.
b) Uses of group 1 metals.
ii. Group 2
a)Physical and chemical properties, extraction of
group 2 metals e.g Calcium, trends in properties
of their compounds. b) Uses of group 2 metals
19 P-BLOCK ELEMENTS
I. Group 13
a) Boron and Aluminium.
b) Occurrence and extraction, trends in
properties of their compounds with oxygen,
chlorine and hydrogen.
ii. Group 14
a) Occurrence, allotropic forms, physical and
chemical properties, trends in properties of
oxides, hydrides, halides.
b) Greenhouse effect,
c) Uses of group 14 elements.
iii. Group 15
a) Occurrence, allotropic forms, physical and
chemical properties, simple oxides and nitrides,
environmental impacts of NOx.
b) Uses of group 15 elements.
iv. Group 16
a) Occurrence, allotropic forms, physical and
chemical properties, trends in properties of
oxides, hydrides and halides. Environmental
impact of SOx. Uses of group 16 elements.
20 D-BLOCK ELEMENTS
v. Group 17
a) Occurrence, physical and chemical properties,
hydrogen halides, metal halides and interhalogen compounds.
b) Uses of group 17 elements
i. First Row Transition Elements
a) Definition of transition element, electronic
configuration, atomie radii, ionization potential,
variable oxidation states, formation of metal
complex.
ii. Introduction to Coordination Chemistry
a) Definition of metal complex and ligands, types
of ligands. Bonding in metal complexes (chain
theory and its limitations, Werner's theory).
b) Valence bond theory and hybridization
concept.
c) Study of structure and magnetic properties of
octahedral and tetrahedral complexes.
d) Nomenclature of coordination compounds.
CHM004: ORGANIC CHEMISTRY
21 STRUCTURE AND BONDING i. Hybridization
IN ORGANIC COMPOUNDS a) Tetravalency and -hybridization of carbon
ii. Classes of carbon compounds
a) Functional groups, homologous series,
b) Determination of molecular formula from
empirical formula.
22 PURIFICATION
23 ORGANIC REACTIONS
iii. Nomenclature
a) Naming of organic compounds: alkanes,
alkenes, alkynes, aldehydes, ketones, alcohols,
alkyl halides, arenes, carboxylic acids, amines
i. Purification of organic compounds
a) Determination of melting point, crystallization
and recrystallization, simple distillation, liquid
extraction, sublimation
ii. Determination of elements
a) Various methods of determining C,H, N, S and
halogens in organic compounds.
b) Sodium fusion test.
i. Covalent bond cleavage
Homolytic and heterolytic fission, free radical
reaction Nucleophiles and electrophiles
ii. Types of Reactions
a) Addition, Substitution, Elimination, Hydrolysis,
Condensation. COM
24 ISOMERISM IN ORGANIC
COMPOUNDS
iii. Electronic concepts in organic chemistry
a) Inductive, steric electrometric effects.
i. Constitutional, chain, position, and functional
groupgroup isomerism.
ii. Tautomerism, Stereoisomerism.
iii. Geometrical and optical
25 ORGANIC COMPOUNDS
i. Alkanes, alkanes, and alkanes
Nomenclature, structure, synthesis, properties
and reactions
ii. Alcohols
Nomenclature, structure, synthesis, properties
and reactions(combustion, substitution to give
halogenoalkanes, reaction with Na, oxidation to
carbonyl compounds and carboxylic acids,
dehydration to alkenes, formation of esters by
esterification with carboxylic acids and acyl
chlorides). Classes of alcohols.
Distinguishing tests for alcohols (Lucas and
Jones reagents)
iv. Alkylhalides
Nomenclature, structure, synthesis, properties
and reactions
v. Carbonyl compounds (Aliphatic and Aromatic)
Nomenclature, structure, synthesis, properties
and reactions ( reduction, reaction with HCN,
NACN, reaction with acqueous I2.
Tests for aldehydes and ketones using 2,4dinitrophenylhydrazin4-dinitrophenylhydrazin.
vi. Carboxylic compounds and their derivatives
a) Nomenclature, properties, preparation from
alcohols, aldehydes, and nitrites
b) Reactions of carboxylic acids with reactive
metals, reduction to alcohol using LiAlH6
vii. Primary Amines
a) Hydrolysis of esters by acid and base.
b) Hydrolysis of acylchlorides
c) Preparation of alkylamines.
d) Basicity of amines in terms of their structure.
e) Reactions of amines (formation of diazonium
salt) Aromaticity, Kekule structures
viiI. Introduction to aromatic compounds
26 MACROMOLECULES
i. Carbohydrates
a) Classes of carbohydrates.
b) Simple tests
ii. Proteins
a) Amino acids, formation of peptide bonds in
peptides.
b) Simple description of electrophoresis.
27 BIOTECHNOLOGY
28 PETROLEUM INDUSTRY
iii. Polymers
a) Types of polymerization reactions and their
differences.
b) Simple structures of polymers.
c) Uses of polymers
i. Biotechnology and it's application in food and
drugs
i. Constituents of crude oil, refining, cracking.
ii. Chemicals derived from crude oil.
Chapter Three
Recommended Textbooks
Recommended Text For JUPEB Chemistry
1. E. N. Ramsden: A-Level Chemistry, 4th Edition (2000). Stanley Thornes
(Pub) Ltd. ISBN 0748752994.
2. Phillips Mathews: Advanced Level Chemistry.
3. Basic Organic Chemistry by B. A. Osuntogun, O. B. Familoni, and B.1.Alo;
3rd Edition (2012) University to Lagos Press.
4. Chemistry by Ted Lister and Janet Renshaw (2009)Nelson Thornes Ltd.
(Pub).
5. Understanding Advanced Physical Inorganic Chemistry: The Learner's Approach. by Jeanne Tan, Kim Seng Chan (2009) World Scientific (Pub).
6. Chemistry: The Central Science by Theodore E. Brown, Theodor Lawrence
Brown, H. Eugene H. LeMay, Bruce E. Burster Catherine
Murphy, Patrick Woodward 12th Edition (2012) Pearson Education (Pub.).
7. Martins S. Silverberg (2010). Principles of General Chemia Second
edition. McGraw Hill Publishers. New York.
8. University General Chemistry, Inorganic and Physical. YO Wong, C.T. Wong,
S.O. Onyiruka and L.E.S Akpanisi. Africana FEP Publishers Ltd (2002).
Chapter Four
JUPEB Grading System
Students’ academic efforts are interpreted into grades and points at the end
of the program. The table below contains information on the calculation of
these grades, points, and examples.
POINTS
70-100
5
Excellent
60-69
4
Very Good
50-59
3
Good
45-49
2
Merit
40-44
1
Pass
43 and below
0
Fail
______________________________________________________________ JUPEB Grading System
So if A = 5, B = 4, C = 3, D = 2, E = 1, F = 0 (and 1 point is added to a candidate who
doesn’t have an F in their result)
For example, a student who gets a C grade in all three subjects entered has a
point calculated like this:
CCC=3+3+3+1 = 10pts
Maximum point AAA in your three subject courses = 15+ 1 = 16 points.
Note: JUPEB results are released a maximum of 60 days after the final examination.