Overview chemistry e

Chemistry overview for years 3 to 5 The subject-group overviews show the units taught in each year in each discipline. They include the unit title, key and related concepts, global contexts, statements of inquiry, objectives, ATL skills and the content (if any).

For years 1 and 2, please see the “Modular sciences overview”.

Year 3

Unit title and teaching hours Key concept Related

concept(s) Global context Statement of inquiry Objectives ATL skills Content

Atomic structure

15 hours

Systems Models

Evidence

Personal and cultural expression: the ways in which we discover and express ideas

Models are created and modified over time to express new ideas formed by experimental evidence.

A Thinking: critical thinking

Thinking: transfer

Communication: communication

Research: information literacy

Research: media literacy

Atomic models: Thomson, Rutherford and Bohr

Subatomic particles: the electron, proton and neutron and their characteristics

Introduction to bonding ionic, covalent, and metallic bonds. How electrons are used differently in each type of bond. Simple models to demonstrate each type

Simple quark theorywhich quarks make up neutrons and protons and the models used to demonstrate this

Simple outline of the strong interaction that operates within atomic nuclei

Electronic configurations of atoms

Energy and chemical change

15 hours

Change Interaction

Consequences

Scientific and technical innovation: the impact of scientific and technological advances on communities and environments

A change in matter is a consequence of energy differences between substances. Scientists and technicians make use of this to create a range of innovative products.

B

D

Thinking: critical thinking

Self-management: reflection

Thinking: creative thinking


Self-management: organization



The law of conservation of mass

Physical change, chemical change, reactant, product, combustion

Definition of the terms “catalyst” and “precipitate”

Writing word and symbol equations

Importance of the subscripts (and coefficients) in equations

Changes in matter in terms of physical changes and chemical changes and the types of evidence that identify a chemical change from a physical change and how this is related to energy change

Types of chemical reaction: single-/double-displacement reaction, decomposition, neutralization, synthesis, combustion reaction, endothermic and



exothermic reactions

Identify the names and formulas for common laboratory acids and alkalis.

Balancing chemical equations (Limited to simple compounds and elements or counting atoms/particles in a diagrammatic problem)

Chemistry in the automobile industry: common chemical reactions (airbags, semiconductors, catalytic converters)

Concept that chemical potential energy is stored within compounds and that it can be released in a controlled manner to do work or produce heat

Solutions

15 hours

Relationships Evidence

Form

Globalization and sustainability: the relationship between local and global processes

The formation of a solution provides evidence of a relationship between the natures of substances.

B

C


Social: collaboration



Self-management: affective


Polar molecules are electrically neutral but have a partially positive end and a partially negative end. Water, ammonia and DNA are polar molecules.

Water molecules are attracted to each other by “hydrogen bonds”, which are really just forces of attraction.

The attraction between molecules at the surface of a liquid is called surface tension.

Because “hydrogen bonds” are relatively strong, water has a high boiling point for a covalent substance.

Solutions are homogeneous mixtures that can be solid, liquid or gas. Metal alloys are solid solutions. Air is a gaseous solution. Aqueous solutions are solutions that have water as the solvent.

The substance being dissolved is called the solute; the substance doing the dissolving is called the solvent.

The amount of a substance that can dissolve in a liquid (at a particular temperature) is called the solubility of the substance.

Each substance has a different solubility, which depends on its interaction with water.

Solutions are said to be saturated when no more solute can be dissolved.

Polar solvents dissolve polar and ionic solutes. Non-polar solvents (organic compounds) dissolve non-



polar solutes like dissolves like.

The concentration of a solution tells us how much solute has been dissolved in the solvent. The units of concentration are grammes of solute per millilitre of solvent. A concentrated solution contains more solute than a dilute solution.

Some gases can dissolve in water. Whether or not the gas will dissolve depends on the interaction between the gas molecules and the water molecules.

More gas can dissolve in cold water than in hot waterfor example, cold soda.

Electrolytes are solutions that can conduct electricity. They are created by dissolving a salt, acid or base in water.

A suspension is a mixture of two substances, one of which is finely divided and is dispersed in the other.

A colloid is a type of mixture intermediate between a homogeneous mixture (also called a solution) and a heterogeneous mixture and also has properties that are intermediate between the two.

An emulsion is a suspension of two liquids that do not usually mix together.

Acids and bases

20 hours

Relationships Function Fairness and development: rights and responsibilities

The strength of acids and bases is related to the function of the degree of dissociation and determines how they should be used and disposed of.

A

B

C









Definitions of acids and bases (Arrhenius and Brønsted−Lowry)

pH scale

Indicators (litmus, universal, phenolphthalein)

Conductivity

Concentrated, diluted, strong and weak acids and bases

Household detergents



Environmental cycles

15 hours

Relationships Balance

Transformation

Scientific and technical innovation: the impact of scientific and technological advances on communities and environments

Scientific and technological advances are impacting upon the naturally balanced relationships provided by the effective transformations in environmental cycles.

D Thinking: critical thinking







Importance of carbon, nitrogen and water

Water cycle

Treatment and recycling of water

Carbon cycle

Nitrogen cycle

Nitrogen-fixing

Year 4



Periodic trends

15 hours

Relationships Change

Form

Function

Orientation in space and time: discoveries

The form of the periodic table is evolving due to knowledge-challenging discoveries, thus enhancing its function of showing trends in the physical and chemical properties of the elements.


Thinking: transfer




The periodic table shows the positions of metals, non-metals and metalloids.

Metals tend to lose electrons and so they form cations. Non-metals tend to gain electrons so they form anions.

Elements in a group have the same oxidation state and therefore similar chemical properties.

Shielding is the decrease in attraction between an electron and the nucleus in any atom with more than one electron shell.

• As the number of electron shells increases, shielding increases.

• No change occurs as you move across a period.

Effective nuclear charge is the positive charge experienced by the electrons due to the charges in the nucleus.



• No change occurs as you move down a group.

• The charge increases from left to right across a period because protons are being added to the nucleus.

Vertical and horizontal trends in the periodic table exist for atomic radius, ionization energy and electronegativity.

Atomic radius is the distance between the nuclei of two atoms of the same element, or the size of an atom. The atomic radius:

• increases as you move down a group because more electron shells are being added that are further away from the nucleus

• decreases as you move across a period.

Ionization energy is the amount of energy it takes to remove the most loosely held electron from an atom. The ionization energy:

• decreases as you move down a group because of shielding

• increases as you move across a period because the electrons are more tightly held to the nucleus due to the effective nuclear charge.

Electronegativity is the tendency of an atom in a bond to pull electrons towards itself. The electronegativity:

• decreases as you move down a group because the atom has a weaker ability to accept electrons

• increases as you move across a period because the charge on the nucleus becomes stronger and so the atom can attract more electrons.

Properties of fluorine and its use in municipal water



Stoichiometry

20 hours

Systems Balance

Conservation

Scientific and technical innovation: how humans use their understanding of scientific principles

The scientifically constructed systems for balancing chemical equations require the numbers and types of atoms to be conserved.

B

C





Communication: collaboration



Communication: media literacy

Concept of the mole

Avogadro’s number

Relative molecular mass and relative atomic mass

Empirical and molecular formula

Percentage composition

Stoichiometric calculations

Solutions and problems involving concentrations

Gas laws

10 hours

Relationships Movement

Conditions


Humans can manipulate the conditions impacting upon gas particles, thereby determining their movement.

C Thinking: critical thinking

Thinking: reflection



Kinetic molecular theory

Conversions for temperature and pressure

Dalton’s law

Boyle’s law

Charles’ law

Ideal gas law

Graphing and calculations

Standard temperature and pressure

Redox reactions

20 hours

Systems Transfer

Balance


Designers use the balanced systems maintained by the transfer of electrons in redox reactions to develop a range of products.

B

C

D







Definition of oxidation and reduction (electron transfer)

Rules for assigning oxidation numbers

Definition of oxidising agent and reducing agent

Half reactions

Electrochemistry (The study of the interchange of chemical and electrical energy)

Electrochemical cells: voltaic cells (spontaneous)

Reactivity series

Factors (for example, concentration, types of





electrode) that effect cell voltage

Electrolysis reactions

Electrolytic cells and factors (for example, concentration of solutions, temperature, types of solutions) that effect electrolysis reactions

Applications of redox reactions (for example, batteries, purification of metals, galvanizing)

Food chemistry

15 hours

Change Culture

Influences

Balance

Conditions

Identities and relationships: personal health

A person’s health is influenced by cultural and conditional changes to his or her diet.

A

D




Thinking: transfer




Determining caloric values of food

Macromolecules and enzymes

Colour and flavour

Shelf life

Additives

Food technology

Year 5



Chemical nomenclature

15 hours

Systems Patterns

Development

Models

Globalization and sustainability: the interconnectedness of human-made systems and communities

Systems for explaining the world are constructed by observing patterns.


Thinking: transfer



Chemical formula review

Naming of simple compounds

Naming of ionic compounds

Naming of positive ions

Naming of negative ions

Naming of polyatomic ions

Naming of acids: organic and inorganic

IUPAC nomenclature

Naming of organic compounds (aliphatic and



aromatic hydrocarbons, alkanes, alkenes)

Bonding

15 hours

Relationships Interactions

Nature

Models

Globalization and sustainability: the interconnectedness of human-made systems and communities

Scientists use bonding models to explain the nature of interactions between different types of particles.

A

D









Bonds are formed to achieve stability.

Positive ions (cations) form by metals losing valence electrons.

Negative ions (anions) form by non-metals gaining electrons.

The number of electrons lost or gained is determined by the electron configuration of the atom.

The ionic bond is due to electrostatic attraction between oppositely charged ions.

A covalent bond is the electrostatic attraction between a shared pair of electrons and the positively charged nuclei.

Single, double and triple covalent bonds involve one, two and three shared pairs of electrons, respectively.

Lewis (electron dot) structures show all the valence electrons in a covalently bonded species.

The ‘octet rule’ refers to the tendency of atoms to gain a valence shell with a total of eight electrons.

Some atoms have incomplete octets of electrons, for example Be and B.

Carbon and silicon form giant covalent/network covalent/macromolecular structures.

Intermolecular forces include London dispersion, dipole−dipole forces and hydrogen bonding.

A metallic bond is the electrostatic attraction between a lattice of positive ions and delocalized electrons

Alloys usually contain more than one metal and have enhanced properties.

Thermochemistry

20 hours

Change Energy

Process


Physical and chemical processes involve energy changes that can be used to create a range of

B

C

D



Thinking: transfer

Energy changes (transformation)

Temperature and heat

Temperature as the measure of the average kinetic energy of particles in a system

Describing the difference between physical and



products and solutions that impact on humankind and the environment.





chemical changes in terms of energy

Qualitative and quantitative measurements.

Units of energy

Exothermic and endothermic processes

Combustion as an exothermic reaction

Difference between complete and incomplete combustion

The role of fossil fuels in our modern society

Bond breaking as an endothermic and bond making as an exothermic process

Different types of insulators

Heat capacity and specific heat capacity

Using calorimetry to measure changes in heat (enthalpy) and determine the enthalpy change for a chemical process

Calculating energy change in chemical reactions per unit mass or mole of substance using experimental data

Concept of equipment accuracy

Kinetics and equilibrium

20 hours

Relationships Balance

Reaction

Scientific and technical innovation: the natural world and its laws

Equilibrium is the state of balance attained when opposing reaction rates become equal.

A

B

C



Thinking: transfer





Reaction rate and collision theory

Factors affecting the rate of reaction: nature of reactants, concentration, surface area, catalyst, temperature

Equilibrium

• Physical • Chemical • Le Chatelier’s principle: concentration,

temperature and pressure changes, effect of a catalyst



Organic chemistry

10 hours

Change Form (Structure)

Energy

Orientation in space and time: turning points in humankind

In order for structure and energy to continue driving change, finite fossil fuels will need to be replaced by renewable raw materials.

B Thinking: critical thinking





Identification of the following: alkane, alkene, alkyne, alcohol, aldehyde, ketone, carboxylic acid

Nomenclature for straight-chain organic molecules

Combustion reactions

Fossil fuels

Overview chemistry e

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