Annual Planning
Academic Year 2023-2024
Subject: Chemistry
Teacher: Andreea Visanescu
Year: Grade 12
Course Book: Chemistry for Cambridge International AS&A
Level CourseBook-Lawrie Ryan & Roger Norris
Main Aims and Description of Course
The aims are to enable students to:
• acquire knowledge and understanding and develop practical skills, including efficient, accurate and safe
scientific practices
• learn to apply the scientific method, while developing an awareness of the limitations of scientific theories and
models
• develop skills in data analysis, evaluation and drawing conclusions, cultivating attitudes relevant to science
such as objectivity, integrity, enquiry, initiative and inventiveness
• develop effective scientific communication skills, using appropriate terminology and scientific conventions
• understand their responsibility to others/society and to care for the environment
• enjoy science and develop an informed interest in the subject that may lead to further study.
1st Module
Academic
Week/
Date
Unit
Main Theme or Topic
Key Learning Objectives
Resources
Assessment
Week 1
11.09.202315.09.2023
Revision
Week
Week 2
18.09.202322.09.2023
Revision week-As
level preparing for A
Level
Unit 1. Physical
Chemistry
1.1.Chemical
energetics
1.1.1 Lattice energy and
Born-Haber cycles
 Define and use the
terms:
(a) enthalpy change of
atomisation, ΔHat
(b) lattice energy, ΔHlatt
(the change from gas
phase ions to solid lattice)
 Define and use the
term first electron affinity,
EA
 Explain the factors
affecting the electron
affinities of elements
 Describe and explain
the trends in the electron
affinities of the Group 16
and Group 17 elements
 Explain, in
qualitative terms, the
effect of ionic charge and
of ionic radius on the
numerical magnitude of a
lattice energy
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Define and use the
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Past Papers
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Oral assessment
Past Papers
Coursebook
PowerPoint
WorkBook
Links provided
YouTube videos
Practical work
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Oral assessment
Quiz
Past Papers
1.1.2. Enthalpies of solution
and hydration
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term enthalpy change
with reference to hydration,
Δhhyd, and
solution, Δhsol.
Experimental work:
Measuring the enthalpies of
solution for a range of salts
sites.middlebury.edu/chem103lab/2017/
01/24/heats-of-reaction/
 Construct and use
an energy cycle involving
enthalpy change of
solution, lattice energy
and enthalpy change of
hydration.
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Reference videos:
www.youtube.com/watch?v=xRwVOK
JkXZI [explanation in terms of energy
cycles]
www.youtube.com/watch?v=Qyhe8hOf
hu8 [for calculation examples]
1.1.3. Entropy change, ΔS
 Define the term
entropy, S, as the number of
possible arrangements
 Example of a sandcastle to
explain entropy:
of the particles and their energy
www.youtube.com/watch?v=uQSoa
in a given system.
Oral assessment:For each example
of a state change, learners should
decide whether the entropy is
increasing or decreasing each time.
iubuA0
 Calculate the
entropy change for a
reaction, ΔS, given the
standard entropies, S⦵, of the
reactants andproducts, ΔS⦵ =
ΣS⦵(products) – ΣS⦵
(reactants)
Week 3
25.09.202329.09.2023
1.1.Chemical
energetics
1.1.4. Gibbs free energy
change, ΔG
State and use the Gibbs
equation ΔG⦵ = ΔH⦵ –
TΔS⦵
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Practical work
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General revision problems
on all of the Energetics
topics for AS and A Level:
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Oral assessment
Quiz
edu.rsc.org/resources/
Perform calculations using the
equation
ΔG⦵ = ΔH⦵ – TΔS⦵
1.2.Electrochemistry
1.2.1. Electrolysis
1.2.2. Standard electrode
potentials E⦵;
standard cell
potentials E⦵cell and
the Nernst equation
Predict the identities of
substances
liberated during
electrolysis from the state of
electrolyte (molten or aqueous),
position in the
redox series (electrode
potential) and concentration.
State and apply
the relationship F = Le
between the Faraday
constant, F, the Avogadro
constant, L, and the
charge on the electron, e.
Construct redox
equations using the
relevant half-equations.
Define the terms:
(a) standard electrode
(reduction) potential
Experimental work: Carry out the
electrolysis of dilute copper (II)
chloride solution or copper (II)
sulfate using inert carbon electrodes
(b) standard cell potential.
1.2.2. Standard electrode
potentials E⦵;
standard cell
potentials E⦵cell and
the Nernst equation
Calculate a
standard cell potential by
combining two standard
electrode potentials.
Use standard cell
potentials to:
(a) deduce the polarity of
each electrode and hence
explain/deduce the
direction of electron flow
in the external circuit of a
simple cell
(b) predict the feasibility of
a reaction.
Week 4
02.10.202306.10.2023
1.3. Equilibria
1.3.1. Acids and bases
Understand and
use the terms conjugate
acid and conjugate base.
Define conjugate
acid–base pairs,
identifying such pairs in
reactions.
Define
mathematically the terms
pH, Ka, pka and Kw and
use them in calculations.
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PowerPoint
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Practical work
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Quiz
Understand and
use the term solubility
product, Ksp.
1.3.2.Partition
coefficients
State what is
meant by the term
partition coefficient, Kpc.
Calculate and use
a partition coefficient for a
system in which the solute is in
the same
physical state in the two
solvents.
Understand the
factors affecting the
numerical value of a
partition coefficient in
terms of the polarities of
the solute and the
solvents used.
Week 5
09.10.202314.10.2023
1.4.Reaction kinetics
1.4.1. Simple rate
equations, orders of
reaction and rate
constants
Explain and use
the terms rate equation,
order of reaction, overall
order of reaction, rate
constant, half-life,
ratedetermining step and
intermediate.
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PowerPoint
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Practical work
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Oral assessment
Quiz
Understand and use
rate equations of the form
rate = k [a]m[b]n (for which
m and n are 0, 1 or 2).
Show understanding
that the half-life of a firstorder
reaction is
independent of
concentration.
Describe
qualitatively the effect of
temperature change on the rate
constant and
hence the rate of a
reaction.
1.4.2.Homogeneous and
heterogeneous catalysts
Explain that
catalysts can be
homogeneous or
heterogeneous.
Describe the mode
of action of a
heterogeneous catalyst to
include adsorption of
reactants, bond
weakening and
desorption of products,
for example:
(a) iron in the Haber
process
(b) palladium, platinum
and rhodium in the
catalytic removal of
oxides of nitrogen from
the exhaust gases of car
engines.
Week 6
16.10.202320.10.2023
Revision for 1st
Chapture-Quiz I
(q1)
Unit 2. Group 2
2.1.
Similarities and
trends in the
properties of the
Group 2
2.1.1. Similarities and
trends in the
properties of the
Group 2 metals,
magnesium to
barium, and their
compounds.
Describe and
explain qualitatively the
trend in the thermal
stability of the nitrates
and carbonates including
the effect of ionic radius
on the polarisation of the
large anion.
2.2. Chemistry of the
transition elements
2.2.1. General physical and
chemical properties
of the first row of
transition elements,
Describe and explain
qualitatively the
variation in solubility and
of enthalpy change of
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Quiz
titanium to copper
solution, ΔH⦵sol, of the
hydroxides and sulfates
in terms of relative
magnitudes of the
enthalpy change of
hydration and the lattice
energy.
Understand that
transition elements have
the following properties:
(a) they have variable
oxidation states
(b) they behave as
catalysts
(c) they form complex
ions
(d) they form coloured
compounds.
Define a transition
element as a d-block
element which forms one
or more stable ions with
incomplete d orbitals.
Explain why
transition elements form
complex ions in terms of
vacant d orbitals that are
energetically accessible.
2.2.2. Colour of complexes
2.2.3. Stereoisomerism in
transition element
complexes
Week 7
2.2. Chemistry of the
transition elements
2.2.4. Stability constants,
Kstab
Define and use the
terms degenerate and
non-degenerate d
orbitals.
Describe the types
of stereoisomerism shown
by complexes, including
those associated with
bidentate ligands:
(a) geometrical (cis-trans)
isomerism, e.g. square
planar such as
[Pt(NH3)2Cl2] and
octahedral such as
[Co(NH3)4(H2O)2]
2+ and
[Ni(H2NCH2CH2NH2)2(H2O)
2]
2+
(b) optical isomerism, e.g.
[Ni(H2NCH2CH2NH2)3]2+
and
[Ni(H2NCH2CH2NH2)2(H2O)
2]
2+
Define the stability
constant, Kstab, of a
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Oral assessment
Quiz
23.10.2023 27.10.2023
complex as the
equilibrium constant for
the formation of the
complex ion in a solvent
(from its constituent ions
or molecules)
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Practical work
Revision for 2nd
Chapture-Quiz I
(q2)
HOLIDAY
28.10.2023 – 05.11.2023
2nd Module
Week 8
06.11.2023–
10.11.2023
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Unit 3. Organic
Chemistry
3.1.An introduction
to organic chemistry
3.1.1. Formulae, functional
groups and the
naming of organic
compounds
Understand and
use systematic
nomenclature of simple
aliphatic organic
molecules (including
cyclic compounds
containing a single ring of
up to six carbon atoms)
with functional groups
detailed in the table on
page 42, up to six carbon
Oral assessment
Quiz
atoms (six plus six for
esters and amides,
straight chains only for
esters and nitriles)
Understand and
use the following
terminology associated
with types of organic
mechanisms:
(a) electrophilic
substitution
(b) addition-elimination.
3.1.2.Characteristic
organic reactions
Describe and
explain the shape of
benzene and other
aromatic molecules,
including sp2
hybridisation, in terms of
σ bonds and a
delocalised π system.
3.1.3. Shapes of aromatic
organic molecules; σ and π
bonds
Understand that
enantiomers have
identical physical and
chemical properties apart
from their ability to rotate
plane polarised light and
their potential biological
Week 9
13.11.2023–
17.11.2023
3.2.Hydrocarbons
3.1.4. Isomerism:
optical
3.2.1. Arenes
activity.
Describe the
chemistry of arenes as
exemplified by the
following reactions of
benzene and
methylbenzene:
(a) substitution reactions
with Cl2 and with Br2 in
the presence of a
catalyst, AlCl3 or AlBr3, to
form halogenoarenes
(aryl halides)
(b) nitration with a mixture
of concentrated HNO3
and concentrated H2SO4
at a temperature between
25°c and 60°c
(c) Friedel–Crafts
alkylation by CH3Cl and
AlCl3 and heat
(d) Friedel–Crafts
acylation by CH3COCl
and AlCl3 and heat
(e) complete oxidation of
the side-chain using hot
alkaline KMnO4 and then
dilute acid to give a
benzoic acid
(f) hydrogenation of the
benzene ring using H2
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Practical work
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Oral assessment
Quiz
3.3.Halogen
compounds
3.3.1. Halogen
compounds
and Pt/Ni catalyst and
heat to form a
cyclohexane ring.
Describe the
mechanism of
electrophilic substitution
in arenes:
(a) as exemplified by the
formation of nitrobenzene
and bromobenzene
(b) with regards to the
effect of delocalisation
(aromatic stabilisation) of
electrons in arenes to
explain the predomination
of substitution over
addition.
Recall the
reactions by which
halogenoarenes can be
produced:
(a) substitution of an
arene with Cl2 or Br2 in
the presence of a
catalyst, AlCl3 or AlBr3 to
form a halogenoarene,
exemplified by benzene
to form chlorobenzene
and methylbenzene to
form
2-chloromethylbenzene
and 4-
chloromethylbenzene.
Week 10
20.11.2023–
24.11.2023
3.4. Hydroxy
compounds
3.4.1. Phenols
Explain the
difference in reactivity
between a
halogenoalkane and a
halogenoarene as
exemplified by
chloroethane and
chlorobenzene.
Describe the
reaction with acyl
chlorides to form esters
using ethyl ethanoate.
Explain the acidity
of phenol.
Describe and
explain the relative
acidities of water, phenol
and ethanol.
Week 11
27.11.2023–
29.11.2023
(Free days
30.11.2023
&01.12.2023)
3.5. Carboxylic acids
and derivates
3.5.1. Carboxylic acids
Apply knowledge
of the reactions of phenol
to those of other phenolic
compounds, e.g.
naphthol.
Describe and
explain the relative
acidities of carboxylic
acids, phenols and
alcohols.
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PowerPoint
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Quiz
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Oral assessment
Quiz
Describe and
explain the relative
acidities of chlorine-substituted
carboxylic
acids.
3.6. Nitrogen
compounds
3.5.2. Esters
Recall the reaction
by which esters can be
produced:
(a) reaction of alcohols
with acyl chlorides using
the formation of ethyl
ethanoate and phenyl
benzoate as examples.
3.5.3. Acyl chlorides
Recall the
reactions (reagents and
conditions) by which acyl
chlorides can be
produced:
(a) reaction of carboxylic
acids with PCl3 and heat,
PCl5, or SOCl2.
3.6.1. Primary and
secondary amines
Describe the
condensation reaction of
ammonia or an amine
with an acyl chloride at
room temperature to give
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Practical work
an amide.
Week 12
04.12.202308.12.2023
Revision
Week
Week 13
11.12.202315.12.2023
Final Exams
Week
Week 14
18.12.202322.12.2023
Revision
Unit 1->Unit
3
(subunit3.6)
Quiz 3
Check the exam
papers and mark
them
Average
(Q1+Q2+Q3)
HOLIDAY
23.12.2023 – 07.01.2024
3rd Module
Week 15
08.01.202412.01.2024
3.6. Nitrogen
compounds
3.6.2.Phenylamine and azo
compounds
Describe the
preparation of
phenylamine via the
nitration of benzene to
form nitrobenzene
followed by reduction with
hot Sn/concentrated HCl,
followed by NaOH(aq).
Describe and
explain the relative
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Oral assessment
Quiz
basicities of aqueous
ammonia, ethylamine and
phenylamine.
Week 16
15.01.202419.01.2024
3.7.Polymerisation
3.6.3. Amides
Describe the
reactions of amides:
(a) hydrolysis with
aqueous alkali or
aqueous acid
(b) the reduction of the
CO group in amides with
LiAlH4 to form an amine.
3.6.4. Amino acids
Describe the acid /
base properties of amino
acids and the formation of
zwitterions, to include the
isoelectric point.
Describe the formation of
amide (peptide) bonds
between amino acids to
give di- and tripeptides.
Describe the
formation of polyesters:
(a) the reaction between
a diol and a dicarboxylic
acid or dioyl chloride
(b) the reaction of a
3.7.1. Condensation
Polymerisation
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Practical work
hydroxycarboxylic acid.
Deduce the repeat
unit of a condensation
polymer obtained from a
given monomer or pair of
monomers.
3.7.2. Predicting the type of
polymerisation
Week 17
22.01.202426.01.2024
Free day:
24.01.2024
3.7.Polymerisaytion
3.7.3. Degradable polymers
Predict the type of
polymerisation reaction
for a given monomer or
pair of monomers.
Deduce the type of
polymerisation reaction
which produces a given
section of a polymer
molecule.
Recognise that
poly(alkenes) are
chemically inert and can
therefore be difficult to
biodegrade.
Recognise that
some polymers can be
degraded by the action of
light.
Recognise that
polyesters and
polyamides are
biodegradable by acidic
and alkaline hydrolysis.
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Oral assessment
Quiz
3.8.1. Organic synthesis
3.8.Organic
synthesis
Week 18
29.01.202402.02.2024
Week 19
05.02.202409.02.2024
3.8.Organic
synthesis
Revision for 3rd
Chapture-Quiz II
(q4)
Unit 4. Analytical
techniques
Devise multi-step
synthetic routes for
preparing organic
molecules using the
reactions in the syllabus.
3.8.1. Organic synthesis
4.1. Thin-layer
chromatography
Analyse a given
synthetic route in terms of
type of reaction and
reagents used for each
step of it, and possible
by-products.
Describe and
understand the terms
(a) stationary phase, for
example aluminium oxide
(on a solid support)
(b) mobile phase; a polar
or non-polar solvent
(c) Rf value
(d) solvent front and
baseline.
Explain the
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Quiz
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Quiz
differences in Rf values in
terms of interaction with
the stationary phase and
of relative solubility in the
mobile phase.
4.2. Gas / liquid
chromatography
Week 20
12.02.202416.02.2024
4. Analytical
techniques
4.3. Carbon-13 NMR
spectroscopy
Describe and
understand the terms:
(a) stationary phase; a
high boiling point nonpolar
liquid (on a solid
support)
(b) mobile phase; an
unreactive gas
(c) retention time.
Interpret gas /
liquid chromatograms in
terms of the percentage
composition of a mixture
Analyse and
interpret a carbon-13
NMR spectrum of a
simple molecule to
deduce:
(a) the different
environments of the
carbon atoms present
(b) the possible structures
for the molecule
Predict or explain
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Practical work
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Oral assessment
Quiz
the number of peaks in a
carbon-13 NMR spectrum
for a given molecule.
4.4. Proton (1H) NMR
spectroscopy
Analyse and
interpret a proton (1H)
NMR spectrum of a
simple molecule to
deduce:
(a) the different
environments of proton
present using chemical
shift values
(b) the relative numbers
of each type of proton
present from relative
peak areas
(c) the number of
equivalent protons on the
carbon atom adjacent to
the one to which the
given proton is attached
from the splitting pattern,
using the n + 1 rule
(limited to singlet,
doublet, triplet, quartet
and multiplet)
(d) the possible structures
for the molecule.
Describe the use
of tetramethylsilane,
TMS, as the standard for
chemical shift
measurements.
Revision for 4th
Chapture-Quiz II
(q5)
HOLIDAY
17.02.2024 – 25.02.2024
4th Module
Week 21
26.02.202402.03.2024
Week 22
05.03.202409.03.2024
Week 23
12.03.202416.03.2024
Week 24
19.03.202423.03.2024
Week 25
26.03.202430.03.2024
Revision
Week
Revision
Past Papers
Revision
Past Papers
Revision
Past Papers
Revision
Past Papers
Revision
Past Papers
30.03.2024 –
End of
Teaching for
Grades 10 to
12)
Week 26
01.04.202405.04.2024
Final Exams
Week
Week 27
08.04.202412.04.2024
(08.04.202410.04.2024 Free days for
Ramadan
Bayram)
Week 28
15.04.202419.04.2024
Speaking and
Practical
Exams week
Week 29
22.04.2024 26.04.2024
26.04.2024 First written
examination
for
Cambridge
International
Exams
HOLIDAY
27.04.2024 – 07.05.2024
5th Module
Week 30
08.05.202410.05.2024
Week 31
13.05.202417.05.2024
Week 32
20.05.202424.05.2024
Week 33
27.05.202431.05.2024
Week 34
03.06.202407.06.2024
Week 35
10.06.202414.06.2024
13.06.2024 Last day of
written
examination
for
Cambridge
International
Exams
Week 36
17.06.202421.06.2024
(Free days
17.06 - 20.06
- Kurban
Bayram)
Specifications
1. Teachers must plan according to the lates Cambridge Syllabus for their subject, not according to the
textbook, since it may be outdated
2. Teaching new content should be done by the end of March, leaving enough room for revision
3. After beginning of written examinations, teachers should schedule revision classes to support students for
their exams
4. All exams should be done from past papers available on Cambridge School Support Hub
5. Teachers should also focus on teaching students about exam skills and time management appropriate for
their subject, not only delivering the content of the syllabus
6. For subjects with practical examinations, practical skills should be planned and taught throughout the
year, for each unit.