Teaching-Learning Program: Chemistry 2A/BCHE
WEEK
UNIT CONTENT
CHEMISTRY 2A/2B
TEXT
OTHER
2013
STAWA
Resources
Expts/probs
SEMESTER ONE: 2A
Atomic structure and bonding
1-2
Atomic structure and Periodic Table







compare the relative charge and relative
masses of protons, neutrons and electrons
identify elements using their atomic number
(Z)
explain isotopes using their atomic number
(Z) and mass number (A)
use the energy level or shell model of
electron structure to write the electron
configurations for the first twenty elements
(Na 2, 8, 1)
explain the relationship between position on
the Periodic Table and number of valence
electrons of elements in groups 1, 2 and
13–18
explain the relationship between the
number of valence electrons and chemical
properties of elements in groups 1, 2 and
13–18
explain the formation of positive and
negative ions for elements in groups 1, 2
and 13–18.
Other
References
ESSChem
(lucarelli)
Exploring
Chemistry Stage 2
Chemistry
for WA 1
(Pearson/
Heinemann)
E = Experiment
I = Investigation
Set = Problems
Chapter 1
Set 1
SET 2
1.1 - 1.4
Set 4
TASK 1
H/O
1.5, 1.6
Assign 1
Atomic
Structure
Review
Formula
etc
Set 5
1.7
(Extension)
E7
Chapter 2
2.1 - 2.5
3-6
Bonding



describe and explain the formation and
characteristics of metallic bonds and
metallic substances
write and interpret formulae of metallic
elements
describe and explain the relationships
between properties and structures of
metallic substances
2.6 - 2.7
(extension)
Chapter 3
3.1-3.8
H/O
ESSAY
(Task 1)






describe and explain the formation and
characteristics of ionic bonds and ionic
substances
write and interpret formulae of ionic
compounds (from the Appendix 1)
describe and explain the relationships
between properties and structures of ionic
substances
draw representations of ionic substances
using electron dot (octet only) or Lewis
SET 8
Set 6
Chapter 4
4.1 - 4.6
4.7
Set 7
SET 9
structure diagrams.




describe and explain the formation and
characteristics of covalent bonds covalent
molecular substances
write and interpret formulae of covalent
molecular elements and compounds
describe and explain the relationships
between properties and structures of
covalent molecular substances
draw representations of molecular
substances using electron dot (octet only)
or Lewis structure diagrams.
Chapter 5
5.1-5.3
TASK 2
5.4





write the chemical formulae for molecular
compounds
based on the number of atoms of each
element present as inferred from the
systematic names
write the molecular formulae of commonly
encountered molecules that have nonsystematic names
describe and explain the formation and
characteristics of covalent bonds covalent
network substances
write and interpret formulae of covalent
network elements and compounds
describe and explain the relationships
between properties and structures of
covalent network substances
SET 7
(extension)
Chapter 6
( completion
of set tasks
atomic
structure and
bondins)
SET 10
Sets
8-11
SET 11
SET 12
TASK 3
6.1-6.8
Applied chemistry

describe the relationships between
properties and uses
of ionic, metallic, covalent network and
covalent molecular substances found in
and around the home
E8
E9
I4
TEST 1
Atomic Structure and Bonding
Stoichiometry

7-8
perform simple calculations: 
1. molar mass
2. mole to mole
3. mass to mole
4. mass to mass
5. percentage composition
Chapter 7
7.1-7.5
(Qualitative
only)
Set 12
I5
I6
E 11
SET 13
SET 14
Macroscopic properties of
matter
Kinetic Theory

9-10
use the Kinetic Theory of Matter to explain
1. relationship between heat and
temperature
2. change of phase
3. vapour pressure and factors
9.8
Set 3
SET 1
that affect vapour pressure
4. effect on gases of changes in
pressure, temperature and
volume
5. the characteristics of gases


predict the effect on gases of changes in
pressure, temperature and volume
(qualitative only)
explain the boiling point of a liquid.
Stoichiometry

perform simple calculations: 
1. mass to volume (gases at
S.T.P)
2. volume to volume
3. volume (at S.T.P) to moles

use molar volume of gases at STP in
calculations involving the evolution of gases
predict the effect on gases of changes in
pressure,
temperature
and
volume
(qualitative only)
explain the boiling point of a liquid.


Set 18
Set 19
Chapter 8
TASK 4
Investigatio
n: I3 or I6
8.1-8.8
TEST 2 Part1
STOICHIOMETRY and KINETIC
THEORY
Set 2
Solutions

11-12
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
describe the characteristics of
homogeneous and heterogeneous
mixtures
distinguish between pure substances,
homogeneous mixtures and
heterogeneous mixtures.
identify, explain and give examples of
saturated, unsaturated and supersaturated
solutions
apply solubility rules to predict if a
precipitate will form when two dilute ionic
solutions are mixed (see data sheet)
use the colour of ions (see data sheet) to
identify reactants and the products in
chemical processes
explain the effect of concentration on
vapour pressure, melting point and boiling
point of a solution
describe the characteristics and give
examples of strong, weak and nonelectrolytes
explain the differences between
concentrated and dilute solutions of strong
and weak electrolytes.
Set 15
Chapter 9
9.1 - 9.6
SET 19
E3
E4
E5
I2
I3
SET 20
9.7
(extension)
Stoichiometry

12-13
perform simple calculations involving
concentration
calculations (moles per Litre, grams per
Litre)
Applied chemistry
SET 21
E 12
I7

TASK 5
describe and give examples of solutions
and their uses in and around the home
explain concentration units used in
household mixtures (g 100g-1, mL L-1, g mL1, percentage composition)

STAWA Calc
Sets
Test
Sample
EXAM WEEK 15/16
Chemical reactions
Reactions, equations and
stoichiometry

write equations for simple chemical
reactions (molecular or ionic) using state
symbols where appropriate.
explain conservation of mass, atoms and
charge during a chemical reaction.
perform stoichiometric problems that
interrelate mass,
molar mass, number of moles of solute,
and concentration and volume of solution.


SET 6
Chapter 10
TASK 6
Test
SET 17
10.1 - 10.5
SET 22
Applied chemistry
 investigate a biological, environmental or
industrial process applicable to a chosen
context e.g. chemicals in the garden,
kitchen chemistry or chemistry of cleaning.
Include:
1. a description of the chosen process
2. an explanation of relationships between
the chosen process and chemical
models and theories
3. where appropriate:
 safe handling and disposal of
any materials or specific
chemicals involved in the
process
 discussion of sustainability of
the process
Chapter 11
11.1 - 11.3
TASK 7
Report:
E 14
E 15
TASK 8
TEST 2 Part 2
SOLUTIONS & STOICHIOMETRY
Investigatio
n: Rates of
Reaction:
Clock
Reaction.
(Or
selection I8
– I10)
Energy effects
1719



use the Law of Conservation of Energy to
explain endothermic and exothermic
reactions
apply the concepts of system and
surroundings to energy transfer
explain enthalpy (H) in terms of stored
Unit 2A
I8
E 16
E 17
E 18
SET 15


chemical energy
explain endothermic and exothermic
reactions in terms of bond breaking and
bond making
interpret and explain enthalpy diagrams
and equations that include the heat lost or
gained
Revision
Applied chemistry

describe and explain common examples of
endothermic and exothermic reactions or
processes in and around the home e.g.
combustion, hot packs, change of phase
TASK 9
Practical
Test 1
TASK 10
I 8- I 11
(selection)
Reaction rates





describe the rate of a reaction in terms of
rate of change of a measurable quantity
with time
identify and apply the factors affecting
rates of reaction:
1. concentration
2. catalysts
3. temperature
4. state of sub-division
apply the collision theory to explain the
factors affecting rates of reaction
draw and interpret energy profile diagrams
to show the transition state, activation
energy, uncatalysed and catalysed
pathways and the heat of reaction
explain the relationship between collision
theory, kinetic energy distribution graphs
and the rate of a reaction.
SET 16
TASK 11
TASK 12
Practical
Reports
(Due on
completion
of each
experiment)
Applied chemistry
 describe and explain examples where rates
of reaction have been altered in and
around the home
 investigate real world problems in a
laboratory setting with appropriate teacher
direction, considering:
1. sources of uncertainty in experimental
measurements
2. selection of the appropriate units of
measurement of quantities such as
volume and time
TEST 3
ENERGY AND RATES OF REACTION
SEMESTER TWO: 2B
19-20
Chemical reactions
Chapter 12
Reactions, equations and stoichiometry

write equations that show only the species involved in
the reaction
perform calculations involving limiting reagent.
empirical formula
molecular formula



21-23
Acids and bases in aqueous solutions

describe, explain and apply an understanding of the
Arrhenius and Brønsted-Lowry models of acids and
bases
describe and explain the difference between strong
acids including HCl, H2SO4, HNO3 and weak acids
including CH3COOH and H3PO4
identify acids by:
1. indicator colour
2. pH scale value
3. reaction with:
o metal carbonates and hydrogen
carbonates
o metals such as magnesium and
iron
o metal oxides
o metal hydroxides
describe and explain the difference between strong
bases including group 1 and group 2 hydroxides and
weak bases including NH3 and Na2CO3
identify bases by
1. indicator colour
2. pH scale value
3. reaction with:
o acids
o ammonium salts
write equations for the successive ionisation of
polyprotic acids
describe, write equations and predict observations for
the following reaction types:
1. acid-base
2. acid-carbonate
3. acid-metal
qualitatively apply the pH scale
describe properties and reactions of non-metal and
metal oxides e.g. reaction of SO2 with water.
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Set 16
12.1-12.5
Set 17
Chapter 13
13.1 - 13.8
TASK 4
E 19, 20
Assign Acids
/Bases
Set 21
Set 22
E21 – 24
(selection)
TASK 1
Investigation:
(Selection:
I11 – I13)
Set 23
I 12 – I 13
(selection)
Applied chemistry
describe and explain the formation and impact of acids in
the environment e.g. rain, acid rain, soil acidification in
agriculture or acidification of ground water by mineral
sulfides.
TASK 3
TEST 4
ACIDS, BASES, STOICHIOMETRY
24-27
Oxidation and reduction

explain oxidation and reduction as an electron transfer
process
Chapter 14
14.1 - 14.4
Set 24


calculate oxidation numbers
identify and name oxidants and reductants in
equations
 identify oxidation-reduction reactions using oxidation
numbers
 describe, write equations for and interpret
observations for:
o metal displacement reactions
o halogen displacement reactions
 write balanced simple redox equations (metal/metal
ion, metal/hydrogen ion and halogen/halide ion)
 describe and explain how an electric current is
conducted in an electrolytic cell
 describe and explain the following during the
operation of an electrolytic cell:
o anode processes
o cathode processes
o role of the electrolyte
o direction of ion migration
o direction of electron flow in external circuit
o electrode product prediction for molten metal
o halides only.
TASK 2
Assign Redox
Set 25
E 25
E 26
Chapter 15
Set 26
15.1 - 15.5
E 27
Applied chemistry
 predict and name the electrode products for the
electrolysis of molten metal halides only.
 describe electro-winning and electro-refining
 investigate real world problems in a laboratory setting
with appropriate teacher direction, considering:
o sources of uncertainty in experimental
measurements
o selection of the appropriate units of
measurement of quantities such as volume and
time
60
61
TASK 6
Test
62
TEST 5
REDOX AND ELECTROLYSIS
Chapter 16
28-30
TASK 5
Assign Org
Organic chemistry


16.1-16.2
describe the bonding capacity of carbon
explain the diversity of carbon based compounds
Alkanes:
 name and draw straight and simple branched to C8
 observations and equations for:
o substitution reactions
o combustion reactions
 draw and name structural isomers
Alkenes:
 name and draw straight and simple branched to C8
(only one double bond per structure)
E 29
E 30
16.3
Set27


write observations and equations for:
o addition reactions with halogens and
hydrogen
o combustion reactions
draw and name structural and geometric isomers
Cycloalkanes and Cycloalkenes:
 draw and name simple structures to C8
 write observations and equations for:
o substitution and combustion reactions for
cycloalkanes
o addition and combustion reactions for
cycloalkenes
Benzene:
 explain the unique structure and reactivity of
benzene
 write equations for:
o catalysed substitution reactions with
halogens
o combustion reactions
16.4
16.5
Set 28
Set 29
16.6
TASK 7
Investigation:
I14 (Chemical
composition
of Rocks
31-32
TASK 8
Applied chemistry

describe and explain the sources and uses of
hydrocarbons e.g. fuels

perform calculations involving empirical formula
calculations using percentage composition, mass
composition and combustion data

investigate a biological, environmental or industrial
process applicable to the context/s chosen e.g.
catalytic cracking of hydrocarbons, electroplating,
electrowinning or chemistry in agriculture. Include:
o a description of the chosen process
o an explanation of the relationships between
the chosen process and chemical models
and theories
o where appropriate:
 safe handling and disposal of any
materials or specific chemicals
involved in the process
 discussion of sustainability of the
Practical Test
2
REACTIONS
TASK 9
Test

process
discussion of the environmental
impact of the process.
TEST 6
ORGANIC CHEMISTRY
33
REVISION
(Due on
completion of
each
experiment)
34
EMISTRY
TASK 11
Practical
Reports
END OF YEAR EXAM 2A/B
TASK 10