SALTERS CHEMISTRY.
UNITS OF WORK. 12A
AS Module 2848: Chemistry of Natural Resources
UNIT 3 Minerals to Elements (Ken)
Module 2
Recommended Prior Knowledge
From Key Stage 4 Science Double Award
bonding (ionic compounds)
Useful products from metal ores and rocks
Quantitative chemistry;
The Periodic Table (halogens).
DATE
From other teaching modules in the course:
Atomic structure (EL);
Amount of substance (EL and DF);
Bonding (EL);
The Periodic Table (EL).
Learning outcomes
TuA x2
23-11
Show awareness of the economic importance of bromine
and chlorine and their compounds.
FrA
26-11
Write ionic equations to represent precipitation reactions
and other reactions involving ionic compounds.
Describe the hydration of ions in aqueous solution.
Describe the structure of an ionic lattice, e.g. sodium
chloride.
Write ionic equations to represent precipitation reactions
and other reactions involving ionic compounds.
TuB X2
30-11
FrB
3-12
TuA X 2
7-12
2004-5
Explain the redox changes occurring in the extraction of
bromine from sea water;
Interpret flow diagrams showing the sequence of
operations in a chemical process;
Module 1 test – Mock 75mins
ACTIVITY
HOMEWORK DUE IN
1st
Test
Lesson
Read SL pg 45 –
52, Assign. 1 - 5
Theory C.I. 5.1 Ionic bonding
Act. M1.1(P) soln.
of ions,
Theory C.I. 9.1
read CI 5.1
30-11
Qu. 2, 3, 5,
read CI 9.1
30-11
7-12
Write up
7-12
read CI 2.4
14-12
Page 1 of 5
DATE
Learning outcomes
ACTIVITY
HOMEWORK DUE IN
FrA
10-12
Use conventions for representing the distribution of
electrons in atomic orbitals (no treatment of the shapes of
atomic orbitals is expected);
Recall the classification of elements into s, p and d blocks;
Deduce (given the atomic number) the electronic
configuration of atoms from hydrogen to krypton in
terms of main energy levels and s, p and d atomic orbitals;
Assign oxidation states to the elements in a compound;
Use oxidation states to decide which species have
been oxidised and which reduced in a redox reaction;
Describe redox reactions of s- and p-block elements in
terms of electron transfer, using half-equations to
represent the oxidation and reduction reaction
Explain the redox changes which take place when
chlorine, bromine and iodine react with other halide
ions; Compare the relative reactivity of the halogens;
Recall the reaction between halide ions and silver ions;
Recall the following physical properties of the halogens:
appearance and state at room temperature, volatility, and
solubility in water and organic solvents.
Show awareness of the scale and importance of mineral
extractive industries and discuss the environmental
implications of mineral extraction
Describe and explain the major stages in the extraction of
a pure metal from its ore.
Interpret flow diagrams showing the sequence of
operations in a chemical process;
Show awareness of the health and safety precautions
needed in industry when hazardous chemicals are being
stored, transported and used
Theory CI 2.4
questions Read
CI 11.4
14-12
Act M1.2
Write up,
18-1
CI 11.4 p-block,
Gp 7
Even Qus
18-1
Act M1.3 (P)
Halogens
Write up,
25-1
Read SL
M2(pages 53 – 58)
do Assign 6 – 8
Ass for M2
25-1
Act M 1.4, M 1.5
theory sheets,
Complete
1-2
TuB
x2
14-12
FrB
14-1
TuA X2
18-1
FrA
21-1
TuB x2
25-1
2004-5
Page 2 of 5
DATE
Learning outcomes
ACTIVITY
HOMEWORK DUE IN
FrB
28-1
TuA x2
1-2
Use the concept of amount of substance to perform
calculations involving concentrations of solutions
Recap CI 1.5,
All Quests
Describe and explain he major stages in the extraction of
a pure metal from its ore.
Act M2.1 (P), M2.2
(P)
FrA
4-2
Recognise from the balanced equation for a reaction
whether it Is an acid-base, redox, or precipitation reaction.
Recall that acid-base reactions involve proton transfer;
identify the proton donor and proton acceptor in an acidbase reaction;
Describe and explain the major stages in the extraction of
a pure metal from its ore.
Interpret flow diagrams showing the sequence of
operations in a chemical process;
Recall the procedure for vacuum filtration
Describe examples of giant covalent (network)
structures, such as diamond and silicon(IV) oxide;
Interpret differences in the physical properties of CO2
and SiO2 in terms of their different structures.
Recall the procedure for carrying out an acid-alkali
titration and be able to work out the results;
CI 8.1 Acid/base
TuB X2
8-2
FrB
11-2
TuA
22-2
x2
FrA
25-2
Describe examples of giant covalent (network) structures,
such as diamond and silicon (IV) oxide.
Interpret differences in the physical properties of CO2 and
SiO2 in terms of their different structures.
TuB X2
1-3
Preparation for coursework. (EUT next lesson)
2004-5
1-2
8-2
Even Qu.Read
CI 5.2
8-2
Begin Act M 2.3(P) Assign 9-10
(2 lessons needed)
Complete SL pg
58 - 60
22-2
CI 5.2 molecules
Even Qu
22-2
Complete Act.
M2.3 (P) –
Titration end
Act M2.6 Check
notes M3
write up M2.3
Read CI 8.1
1-3
Act M2.5
1-3
Act M 2.4 (P)
Write up
4-3
Page 3 of 5
DATE
Learning outcomes
FrB
4-3
TuA x2
8-3
FrA
11-3
TuB x2
15-3
FrB
18-3
TuA X2
22-3
TuB X2
12-4
FrB
15-4
TuA X2
19-4
FrA
22-4
TuB X2
26-4
FrB
29-4
EUT , We begin coursework 2 -3 weeks
2004-5
ACTIVITY
HOMEWORK DUE IN
Page 4 of 5
DATE
Learning outcomes
ACTIVITY
HOMEWORK DUE IN
TuA X2
3-5
FrA
6-5
TuB X2
10-5
FrB
13-5
TuA X2
17-5
FrB
20-5
TuA X2
24-5
FrA
27-5
2004-5
Page 5 of 5