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