MCAT SYLLABUS OF CHEMISTRY FOR 2015

 

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

 
MCAT SYLLABUS OF CHEMISTRY FOR 2015


Topic                                                                                         MCQs
A. Physical Chemistry                                                                                        
1. Fundamental concepts                                                   02
2. States of matter                                                              02
3. Atomic structure                                                             02
4. Chemical bonding                                                             02
5. Chemical energetics                                                          02
6. Solutions                                                                            02
7. Electrochemistry                                                               02
8. Chemical Equilibrium                                                       02
9. Reaction kinetics                                                               02
B. Inorganic Chemistry
1. Periods                                                                               02
2. Groups                                                                               02
3. Transition elements                                                           02
4. Elements of biological importance                                   04
C. Organic Chemistry
1. Fundamental principles                                                     02
2. Hydrocarbon                                                                     02
3. Alkyl halides                                                                     02
4. Alcohols and Phenols                                                       04
5. Aldehydes and Ketones                                                   03
6. Carboxylic acid                                                               03
7. Amino acids                                                                     06
8. Macromolecules                                                             06
9. Environmental chemistry                                              02
Total                                                                                           58

  
             

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)
11

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
18

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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