PICNIC POINT HIGH SCHOOL
2014
CHEMISTRY
Weekly Outline
Syllabus Outcomes
GLOSSARY
8.2 THE CHEMICAL EARTH
8.2
The Chemical Earth
Contextual Outline
The Earth includes a clearly identifiable biosphere, lithosphere, hydrosphere and atmosphere. All of
these are mixtures of thousands of substances and the use of this pool of resources requires the
separation of useful substances. The processes of separation will be determined by the physical and
chemical properties of the substances.
In order to use the Earth’s resources effectively and efficiently, it is necessary to understand the
properties of the elements and compounds found in mixtures that make up earth materials. Applying
appropriate models, theories and laws of chemistry to the range of earth materials allows a useful
classification of the materials and a better understanding of the properties of substances.
This module increases students’ understanding of the nature, practice, applications and uses of
chemistry.
Assumed Knowledge
Domain: knowledge and understanding
Refer to the Science Years 7–10 Syllabus for the following:
5.7.1a) describe features of and the location of protons, neutrons and electrons in the atom
5.7.2a) identify the atom as the smallest unit of an element and distinguish between atoms and
molecules
5.7.2b) describe some relationships between elements using the Periodic Table
5.7.3a) identify that a new compound is formed by rearranging atoms rather than by creating
matter
5.7.3b) classify compounds into groups based on common chemical characteristics
5.7.3c) construct word equations from observations and written descriptions of a range of
chemical reactions
5.7.3d) identify a range of common compounds using their common names and chemical
formulae
5.7.3e) qualitatively describe reactants and products in the following chemical reactions:
vi) decomposition.
1. The living and
non-living
components of the
Earth contain
mixtures
Students learn to:
Students:

1.2a.construct word and balanced
formulae equations of chemical
reactions as they are encountered


1.2b. identify the difference
between elements, compounds and
mixtures in terms of particle theory
1.3a. gather and present information
from first-hand or secondary
sources to write equations to
represent all chemical reactions
encountered in the Preliminary
course


1.2c. identify that the biosphere,
lithosphere, hydrosphere and
atmosphere contain examples of
mixtures of elements and
compounds
1.3b.identify data sources, plan,
choose equipment and perform a
first-hand investigation to separate
the components of a naturally
occurring or appropriate mixture
such as sand, salt and water

1.2d. identify and describe
procedures that can be used to
separate naturally occurring
mixtures of:
- solids of different sizes
- solids and liquids
- dissolved solids in liquids
- liquids
- gases

1.3c. gather first-hand information
by carrying out a gravimetric
analysis of a mixture to estimate its
percentage composition

1.3d. identify data sources, gather,
process and analyse information
from secondary sources to identify
the industrial separation processes
used on a mixture obtained from the
biosphere, lithosphere, hydrosphere
or atmosphere and use the evidence
available to:
- identify the properties of the
mixture used in its separation
- identify the products of
separation and their uses
- discuss issues associated with
wastes from the processes used

1.2e. assess separation techniques
for their suitability in separating
examples of earth materials,
identifying the differences in
properties which enable these
separations

1.2f. describe situations in which
gravimetric analysis supplies useful
data for chemists and other
scientists

1.2g. apply systematic naming of
inorganic compounds as they are
introduced in the laboratory

1.2h. identify IUPAC names for
carbon compounds as they are
encountered
2. Although most
elements are found
in combinations on
Earth, some
elements are found
uncombined
Students learn to:
Students:

2.2a. explain the relationship
between the reactivity of an element
and the likelihood of its existing as
an uncombined element


2.2b. classify elements as metals,
non-metals and semi-metals
according to their physical
properties
2.3a. plan and perform an
investigation to examine some
physical properties, including
malleability, hardness and electrical
conductivity, and some uses of a
range of common elements to
present information about the
classification of elements as metals,
non-metals or semi-metals

2.2c. account for the uses of metals
and non-metals in terms of their
physical properties

2.3b. analyse information from
secondary sources to distinguish the
physical properties of metals and
non-metals

2.3c. process information from
secondary sources and use a
Periodic Table to present
information about the classification
of elements as:
- metals, non-metals and semimetals
- solids, liquids and gases at 25˚C
and normal atmospheric pressure
3. Elements in Earth
materials are
present mostly as
compounds because
of interactions at
the atomic level
Students learn to:
Students:

3.2a. identify that matter is made of
particles that are continuously
moving and interacting


3.2b. describe qualitatively the
energy levels of electrons in atoms
3.3a. analyse information by
constructing or using models
showing the structure of metals,
ionic compounds and covalent
compounds

3.3b. construct ionic equations
showing metal and non-metal atoms
forming ions

3.2c. describe atoms in terms of
mass number and atomic number

3.2d. describe the formation of ions
in terms of atoms gaining or losing
electrons

3.2e. apply the Periodic Table to
predict the ions formed by atoms of
metals and non-metals

3.2f. apply Lewis electron dot
structures to:
- the formation of ions
- the electron sharing in some
simple molecules

3.2g. describe the formation of
ionic compounds in terms of the
attraction of ions of opposite charge

3.2h.describe molecules as particles
which can move independently of
each other

3.2i. distinguish between molecules
containing one atom (the noble
gases) and molecules with more
than one atom

3.2j. describe the formation of
covalent molecules in terms of
sharing of electrons

3.2k. construct formulae for
compounds formed from:
- ions
- atoms sharing electrons
4. Energy is required
to extract elements
from their
naturally occurring
sources
Students learn to:
Students:

4.2a. identify the differences
between physical and chemical
change in terms of rearrangement of
particles


4.2b. summarise the differences
between the boiling and electrolysis
of water as an example of the
difference between physical and
chemical change
4.3a. plan and safely perform a
first-hand investigation to show the
decomposition of a carbonate by
heat, using appropriate tests to
identify carbon dioxide and the
oxide as the products of the reaction

4.3b. gather information using firsthand or secondary sources to:
- observe the effect of light on
silver salts and identify an
application of the use of this
reaction
- observe the electrolysis of
water, analyse the information
provided as evidence that water
is a compound and identify an
application of the use of this
reaction

4.3c. analyse and present
information to model the boiling of
water and the electrolysis of water
tracing the movements of and
changes in arrangements of
molecules

4.2c. identify light, heat and
electricity as the common forms of
energy that may be released or
absorbed during the decomposition
or synthesis of substances and
identify examples of these changes
occurring in everyday life

4.2d. explain that the amount of
energy needed to separate atoms in
a compound is an indication of the
strength of the attraction, or bond,
between them
5. The properties of
elements and
compounds are
determined by
their bonding and
structure
Students learn to:
Students:

5.2a. identify differences between
physical and chemical properties of
elements, compounds and mixtures


5.2b. describe the physical
properties used to classify
compounds as ionic or covalent
molecular or covalent network
5.3a. perform a first-hand
investigation to compare the
properties of some common
elements in their elemental state
with the properties of the
compound(s) of these elements (eg
magnesium and oxygen)

5.3b. choose resources and process
information from secondary sources
to construct and discuss the
limitations of models of ionic
lattices, covalent molecules and
covalent and metallic lattices

5.3c. perform an investigation to
examine the physical properties of a
range of common substances in
order to classify them as metallic,
ionic or covalent molecular or
covalent network substances and
relate their characteristics to their
uses

5.2c. distinguish between metallic,
ionic and covalent bonds

5.2d. describe metals as
three-dimensional lattices of ions in
a sea of electrons

5.2e. describe ionic compounds in
terms of repeating threedimensional lattices of ions

5.2f. explain why the formula for an
ionic compound is an empirical
formula

5.2g. identify common elements
that exist as molecules or as
covalent lattices

5.2h. explain the relationship
between the properties of
conductivity and hardness and the
structure of ionic, covalent
molecular and covalent network
structures
Glossary
AC- (alternating current) electric current alternating in direction
analysis- process of identifying parts of a sample
anion- a negative ion
atmosphere- layer of gas around the Earth
atomic number- unique number for each element; equal to the number of protons in the
nucleus
atomic weight- weight of an atom compared with the weight of a carbon-12 atom taken to be
exactly 12
binary compound- made up of two elements only
biosphere- parts of the Earth where life is found
boiling- liquid changing to gas rapidly
BP- (boiling point) temperature at which liquid changes to gas
bond energy- energy absorbed to break a bond or energy released when a bond forms
bonding- strong forces of attraction
brittle- cracks or breaks easily when deformed
catalyst- substance which, although not consumed, reduces the energy of activation of a
reaction
cation- positive ion
chemical change- chemical reaction; at least one new substance produced and is not easily
reversed
chemical property- property of a substance reacting with another chemical
chemiluminescence- chemical reaction emitting light without heating
compound- pure substance formed by the combination of two or more different elements in a
fixed ratio
compressibility- ability to be pressed into a smaller space
condensation- change from gas to liquid
condenser- cooling equipment used to change gas to liquid
conductivity- ability to allow passage of electricity/heat
configuration- arrangement
covalent bond- bond formed by two atoms sharing a pair of electrons
crystal- piece of solid with some regular shape
crystallization- separation of solid crystals from impurities and from solution
decomposition- reaction in which one substance forms two or more substances
density- mass of substance per unit volume
DC- (direct current) electric current moving in one direction only
distillation- process in which a more volatile substance is separated from a less volatile
substance
ductility- ability to be drawn into a wire without breaking; property of many metals
electrode- material transferring electrons to or from a liquid or a solution
electrolysis- chemical reaction requiring electrical energy
electrolyte- liquid or solution containing ions
electrolytic cell- arrangement of chemicals for changing electrical energy to chemical energy
electron- negatively charged subatomic particle with effectively no mass
electron configuration- arrangement of electrons in shells around the nucleus of an atom going
from innermost shell to outermost valence shell eg. 2.8.8.1 for potassium
element- pure substance made up of only one type of atom
empirical formula- formula giving the simplest whole number ratio of particles in a compound
enzyme- biological catalyst
evaporation- changing of liquid to gas below the BP
filtrate- clear solution that passes through a filter
galvanic cell- ‘battery’; arrangement of chemicals for changing chemical energy to electrical
energy
gravimetric analysis- quantitative analysis using weighing
group- vertical column of the Periodic Table
hardness- ability to resist applied pressure
hydrocarbon- compound of hydrogen and carbon only
hydrosphere- layer of water around the Earth
inert- does not readily react with other chemicals
inference- a conclusion reached on the basis of evidence and reasoning
inorganic- non-living origin
ion- charged particle formed from an atom or group of atoms (polyatomic ion)
ionic bond- bond formed between oppositely charged ions
IUPAC- International Union of Pure and Applied Chemistry
joule- metric unit of energy, symbol is J
justify- support an argument or conclusion
Kelvin- unit of temperature = Celsius degree, symbol is K (0°C=273°K and 0°K= -273°C)
lattice- arrangement of particles in a crystal
liquefaction- changing a gas to liquid eg. production of liquefied petroleum gas (LPG),
compressed natural gas (CNG) or liquid nitrogen from atmospheric nitrogen
lithosphere- rigid outer layer of the Earth that includes the Earth's crust
malleability- ability to be shaped without breaking
mass number- total number of protons and neutrons in the nucleus of an atom
melting- changing of solid to liquid
MP- (melting point) temperature at which solid changes to liquid
mineral- useful element or compound from the earth
mixture elements and/or compounds mixed together
mole- large number (6 x 1023) of particles. Also the atomic mass of an element or molecule or
compound expressed in grams- ie one mole of carbon weighs 12 grams and has 6x1023 atoms of
carbon in it.
molecule- particle that can move independently of other particles
neutron- neutral subatomic particle in the nucleus of an atom than weighs one atomic mass
unit (AMU)
nucleus- central core of an atom containing protons and neutrons
observation- what you detect with your senses
ohm- unit of electrical resistance represented by Ω
ore- matter from the earth worth extracting a mineral from
organic- from living things
phase- change change between states of matter
period- horizontal row of the Periodic Table
periodic- reoccurring at regular intervals
Periodic Table- arrangement of chemical elements in order of atomic number so that elements
with similar properties occur at fixed intervals
physical change- change where the identity of the substance does not change eg. phase change
or solution and is reversible
physical property- property of a substance such as hardness, density, viscosity etc.
picometre- unit of length; 10-12m; symbol is pm
prefix- part with a fixed meaning put at the beginning of a word eg. bi for two, kilo for thousand
proton- positive subatomic particle that weighs one atomic mass unit(AMU)
qualitative- analysis finding out what elements are in a sample
quantitative- analysis finding out how much of each element is in a sample
radioactive decay- change involving protons and neutrons in the nucleus of an atom releasing
energy
reactive- tends to react with other chemicals
reciprocal- opposite in trend; reciprocal of a is 1/a
reliable- trustworthy with results able to be repeated
residue- solid that collects on a filter
resistance (electrical)- resistance to flow of electricity
semiconductor- substance that is not a good conductor but conducts if small amounts of certain
elements are added or the temperature is changed
semi-metal- element intermediate in properties between metals and non-metals
solidification- freezing; liquid changes to solid
solute- substance that dissolves
solution- mixture of solute and solvent
solvent- liquid able to dissolve another substance
spreadsheet- computer program for processing numbers arranged in table form
subatomic- smaller in size than an atom such as protons and neutrons
supernova- explosion that occurs towards the end of a large star's life; the star collapses to a
dense core then explodes creating heavier atoms
synthesis- building up a substance from simpler substances
synthetic- made by synthesis- not naturally occuring
thermal- heat
URL- uniform resource locator; the address of a document on the internet
valence/valency- used to describe the outer electrons of an atom that determine reactivity and
bonding with other atoms
valence/valency shell- outer electron shell of an atom
valid- leading to effective results and worthwhile conclusions
volatile- describing something that easily becomes vapour
voltameter- equipment used to measure electrolytic decomposition
volume- amount of space
volumetric analysis- quantitative analysis using volumes
Preliminary Chemistry
8.2 The Chemical Earth Weekly Outline
Fortnight
Pre-reading
Chemical Context 1
(2nd Ed)
1.1
1.2
1.1 & 1.2
1.3
1.4
1.5
2.1
1.3
1.4, 1.6
1.7
2.2
2.3
2.4
2.1, 2.2
2.3
2.4
2.5
3.1
2.6
2.7
3.1
3.4
3.5
3.2, 3.4
3.5,
3.2
4.1
4.1
4.2
4.3
4.2, 4.3
4.4
Topic
Introduction to Preliminary Chemistry
Hand out textbooks – Pre Test
Particle Theory, atoms, elements, compounds,
mixtures; separation techniques
Practical 8.2.1 Separate sand and water
Earth materials and Separation Techniques
Practical 8.2.2 Gravimetric Analysis
Practical 8.2.3 Industrial Separation Processes –
Library – Hand out assignment
Elements
Practical 8.2.4 Physical Properties of Elements
Practical 8.2.5 Physical Properties of metals and
non-metals and semi-metals
Atoms, Molecules, atomic number, molecular
weight and the periodic table
Energy levels of electrons, Ionic Compounds
Ionic Equations, Formula and naming
Review Homework – Catch up lesson
Formation of Covalent Compounds and Naming
Practical 8.2.6 Models of Ionic Compounds and
covalent
Practice time for naming ionic compounds.
Chemical and Physical Changes
Practical 8.2.7 Modelling Boiling and Electrolysis of
Water
Balancing Equations
Bond Energy and Reactions
Homework
Syllabus
Q’s 1.1 and 1.3
1.2b, d
Write-up
Q’s 1.2 and 1.4
Write-up +DA 1.4
Q’s 1.5 + DA 1.5 +
Checkpoint Revision 1
1.3b
1.2c,e, f
1.3c, f
1.3d
Write-up + Q’s 2.1
DA2.2 + DA2.3
2.2a, 2.3a
2.2b, 2.3b, c
Q’s 3.1
3.2a, c, h, i
Q’s 3.2
3.2b, d, e, f, g
3.3b
DA 3.1 + Q’s 3.3
Write up + Checkpoint
Revision 2
3.2 j, k
3.3a, 5.3b
Write up + DA 4.4 + Q’s 4.1
4.2a, b,
4.3b, c
Write up + DA 4.5 + Q’s 4.2
1.2a
4.2c, d,
4.3a,b
Register
8.2 The Chemical Earth Weekly Outline
Fortnight
Pre-reading
Chemical Context 1
(2nd Ed)
4.4
4.5
4.6
5.1
5.2
3.7
5.3
3.6
4.6
4.7
Topic
Practical 8.2.8 Decomposition of a Carbonate and
silver salts
Review Homework – Catch up lesson
Physical and Chemical Properties
Practical 8.2.9 Properties of Elements and their
Compounds
Types of Bonds in metals, Ionic and molecular
covalent and covalent lattices.
Calculating Empirical Formula of ions
8.2.10 Properties of compounds
Module Revision
Module Revision
Homework
Syllabus
Q’s 5.1
Write-up
5.2a, b
5.3a
5.2i
5.2 c, d, e, j, g,
h
5.2f
5.3c
Write-up + DA 5.3 + Q’s 5.2
Library Lesson Write-up
Register