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PICNIC POINT HIGH SCHOOL
2014
CHEMISTRY
Weekly OutlineSyllabus Outcomes
GLOSSARY
8.2 THE CHEMICAL EARTH
8.2 The Chemical EarthContextual OutlineThe 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 KnowledgeDomain: 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 atom5.7.2a) 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
matter5.7.3b) classify compounds into groups based on common chemical characteristics5.7.3c) construct word equations from observations and written descriptions of a range of
chemical reactions5.7.3d) identify a range of common compounds using their common names and chemical
formulae5.7.3e) qualitatively describe reactants and products in the following chemical reactions:
vi) decomposition.
Students learn to: Students:
1. The living and non-living components of the Earth contain mixtures
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
1.3b.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
1.3c. 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
1.2c. identify that the biosphere, lithosphere, hydrosphere and atmosphere contain examples of mixtures of elements and compounds
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
1.2e. 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
Students learn to: Students:
2. Although most elements are found in combinations on Earth, some elements are found uncombined
2.2a. explain the relationship between the reactivity of an element and the likelihood of its existing as an uncombined element
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
2.3b. 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 semi-
metals- solids, liquids and gases at 25˚C
and normal atmospheric pressure
2.2b. classify elements as metals, non-metals and semi-metals according to their physical properties
2.2c. account for the uses of metals and non-metals in terms of their physical properties
Students learn to: Students:
3. Elements in Earth materials are present mostly as compounds because of interactions at the atomic level
3.2a. identify that matter is made of particles that are continuously moving and interacting
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
3.2b. describe qualitatively the energy levels of electrons in atoms
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
Students learn to: Students:
4. Energy is required to extract elements from their naturally occurring sources
4.2a. identify the differences between physical and chemical change in terms of rearrangement of particles
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 first-hand 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
4.2b. summarise the differences between the boiling and electrolysis of water as an example of the difference between physical and chemical change
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
Students learn to: Students:
5. The properties of elements and compounds are determined by their bonding and structure
5.2a. identify differences between physical and chemical properties of elements, compounds and mixtures
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
5.2b. describe the physical properties used to classify compounds as ionic or covalent molecular or covalent network
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 three-dimensional 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 Chemistry8.2 The Chemical Earth Weekly Outline
Fortnight Pre-readingChemical Context 1 (2nd Ed)
Topic Homework Syllabus Register
1.1 Introduction to Preliminary ChemistryHand out textbooks – Pre Test
1.2 1.1 & 1.2 Particle Theory, atoms, elements, compounds, mixtures; separation techniques
Q’s 1.1 and 1.3 1.2b, d
1.3 1.3 Practical 8.2.1 Separate sand and water Write-up 1.3b1.4 1.4, 1.6 Earth materials and Separation Techniques Q’s 1.2 and 1.4 1.2c,e, f1.5 1.7 Practical 8.2.2 Gravimetric Analysis Write-up +DA 1.4 1.3c, f2.1 Practical 8.2.3 Industrial Separation Processes –
Library – Hand out assignmentQ’s 1.5 + DA 1.5 + Checkpoint Revision 1
1.3d
2.2 2.1, 2.2 Elements2.3 2.3 Practical 8.2.4 Physical Properties of Elements Write-up + Q’s 2.1 2.2a, 2.3a2.4 2.4 Practical 8.2.5 Physical Properties of metals and
non-metals and semi-metalsDA2.2 + DA2.3 2.2b, 2.3b, c
2.5 3.1 Atoms, Molecules, atomic number, molecular weight and the periodic table
Q’s 3.1 3.2a, c, h, i
2.6 3.2, 3.4 Energy levels of electrons, Ionic Compounds Q’s 3.2 3.2b, d, e, f, g2.7 3.5, Ionic Equations, Formula and naming 3.3b3.1 Review Homework – Catch up lesson3.4 Formation of Covalent Compounds and Naming DA 3.1 + Q’s 3.3 3.2 j, k3.5 Practical 8.2.6 Models of Ionic Compounds and
covalentWrite up + Checkpoint Revision 2
3.3a, 5.3b
3.2 Practice time for naming ionic compounds.4.1 4.1 Chemical and Physical Changes
Practical 8.2.7 Modelling Boiling and Electrolysis of Water
Write up + DA 4.4 + Q’s 4.1 4.2a, b,4.3b, c
4.2 4.2, 4.3 Balancing Equations 1.2a4.3 4.4 Bond Energy and Reactions Write up + DA 4.5 + Q’s 4.2 4.2c, d,
4.3a,b
8.2 The Chemical Earth Weekly OutlineFortnight Pre-reading
Chemical Context 1 (2nd Ed)
Topic Homework Syllabus Register
Practical 8.2.8 Decomposition of a Carbonate and silver salts
4.4 Review Homework – Catch up lesson4.5 5.1 Physical and Chemical Properties Q’s 5.1 5.2a, b4.6 5.2 Practical 8.2.9 Properties of Elements and their
CompoundsWrite-up 5.3a
5.2i3.7 5.3 Types of Bonds in metals, Ionic and molecular
covalent and covalent lattices.Write-up + DA 5.3 + Q’s 5.2 5.2 c, d, e, j, g,
h3.6 Calculating Empirical Formula of ions Library Lesson Write-up 5.2f
8.2.10 Properties of compounds 5.3c4.6 Module Revision4.7 Module Revision