2AB+Chemistry


 * ** Week ** ||= ** Content - 2A Chemistry ** ||
 * 1–3 || ** Macroscopic properties **

** Classifying material **
 * describe the characteristics of homogeneous and heterogeneous mixtures
 * distinguish between pure substances, homogeneous mixtures and heterogeneous mixtures.

** Kinetic Theory ** ** Solutions **
 * use the Kinetic Theory of Matter to explain
 * relationship between heat and temperature
 * change of phase
 * vapour pressure and factors that affect vapour pressure
 * effect on gases of changes in pressure, temperature and volume
 * the characteristics of gases
 * predict the effect on gases of changes in pressure, temperature and volume (qualitative only)
 * explain the boiling point of a liquid.
 * identify, explain and give examples of saturated, unsaturated and supersaturated solutions
 * apply solubility rules to predict if a precipitate will form when two dilute ionic solutions are mixed (see data sheet)
 * use the colour of ions (see data sheet) to identify reactants and the products in chemical processes
 * explain the effect of concentration on vapour pressure, melting point and boiling point of a solution
 * describe the characteristics and give examples of strong, weak and non-electrolytes
 * explain the differences between concentrated and dilute solutions of strong and weak electrolytes.

** Applied chemistry **
 * describe and give examples of solutions and their uses in and around the home
 * explain concentration units used in household mixtures (g 100g-1,mL L-1, g mL-1, percentage composition)
 * calculate concentration (mixtures (g 100g-1,mL L-1, g mL-1,) ||
 * 4 - 7 || ** Atomic structure and Periodic Table **
 * compare the relative charge and relative masses of protons, neutrons and electrons
 * identify elements using their atomic number (Z)
 * explain isotopes using their atomic number (Z) and mass number (A)
 * use the energy level or shell model of electron structure to write the electron configurations for the first twenty elements (Na 2, 8, 1)
 * explain the relationship between position on the Periodic Table and number of valence electrons of elements in groups 1, 2 and 13–18
 * explain the relationship between the number of valence electrons and chemical properties of elements in groups 1, 2 and 13–18
 * explain the formation of positive and negative ions for elements in groups 1, 2 and 13–18.

** Bonding **
 * describe and explain the formation and characteristics of:
 * ionic bonds and ionic substances
 * metallic bonds and metallic substances
 * covalent bonds
 * covalent network and molecular substances
 * describe and explain the relationships between properties and structures of ionic, metallic, covalent network and covalent molecular substances
 * draw representations of molecular and ionic substances using electron dot (octet only) or Lewis structure diagrams.

** Applied chemistry ** > > > ** Applied chemistry ** > ** Reaction rates ** > > > ** Applied chemistry ** > selection of the appropriate units of measurement of quantities such as volume and time. || ** stoichiometry **
 * describe the relationships between properties and uses of ionic, metallic, covalent network and covalent molecular substances found in and around the home ||
 * 8 - 11 || ** Energy effects **
 * use the Law of Conservation of Energy to explain endothermic and exothermic reactions
 * apply the concepts of system and surroundings to energy transfer
 * explain enthalpy (H) in terms of stored chemical energy
 * explain endothermic and exothermic reactions in terms of bond breaking and bond making
 * interpret and explain enthalpy diagrams and equations that include the heat lost or gained (ΔH).
 * describe and explain common examples of endothermic and exothermic reactions or processes in and around the home e.g. combustion, hot packs, change of phase
 * describe the rate of a reaction in terms of rate of change of a measurable quantity with time
 * identify and apply the factors affecting rates of reaction:
 * concentration
 * catalysts
 * temperature
 * state of sub-division
 * apply the collision theory to explain the factors affecting rates of reaction
 * draw and interpret energy profile diagrams to show the transition state, activation energy, uncatalysed and catalysed pathways and the heat of reaction
 * explain the relationship between collision theory, kinetic energy distribution graphs and the rate of a reaction.
 * describe and explain examples where rates of reaction have been altered in and around the home
 * investigate real world problems in a laboratory setting with appropriate teacher direction, considering:
 * sources of uncertainty in experimental measurements
 * 12 - 15 || ** Reactions and equations **
 * write and interpret formulae of elements and compounds
 * describe, write equations and predict observations for precipitation reactions
 * write equations that show only the species involved in the reaction

> > ** Applied chemistry ** Semester 2
 * perform simple gravimetric calculations:
 * molar mass
 * mole to mole
 * mass to mole
 * mass to mass
 * calculate concentration (mixtures (g 100g-1,mL L-1, g mL-1,)
 * percentage composition
 * write the chemical formulae for molecular compounds based on the number of atoms of each element present as inferred from the systematic names
 * write the molecular formulae of commonly encountered molecules that have non-systematic names
 * explain conservation of mass, atoms and charge during a chemical reaction ||
 * 16 ||= ** Revision for exam ** ||
 * 17 - 19 ||= ** Semester 1 examination ** ||

describe electro-winning and electro-refining || >> ** Applied chemistry ** >> empirical formula calculations using percentage composition, mass composition and combustion data ||
 * = **Week** ||= ==**Content - 2B Chemistry**== ||
 * = 1 - 4 ||< ** Acids and bases in aqueous solutions **
 * describe, explain and apply an understanding of the Arrhenius and Brønsted-Lowry models of acids and bases
 * describe and explain the difference between strong acids, including HCl, H2SO4, HNO3 and weak acids including CH3COOH and H3PO4
 * identify acids by:
 * indicator colour
 * pH scale value
 * reaction with:
 * metal carbonates and hydrogen carbonates
 * metals such as magnesium and iron
 * metal oxides
 * metal hydroxides
 * describe and explain the difference between strong bases, including group 1 and group 2 hydroxides and weak bases including NH3 and Na2CO3
 * identify bases by:
 * indicator colour
 * pH scale value
 * reaction with:
 * acids
 * ammonium salts
 * write equations for the reactions of acids showing only the species involved, using state symbols where appropriate
 * describe, write equations and predict observations for the following reactions:
 * acid-base
 * acid-carbonate
 * acid-metal
 * write equations for the successive ionisation of polyprotic acids
 * qualitatively apply the pH scale
 * describe properties and reactions of non-metal and metal oxides e.g. reaction of SO2 with water
 * perform stoichiometric problems that interrelate mass, molar mass, number of moles of solute, and concentration and volume of solution
 * mass to volume (gases at STP)
 * limiting reagent ||
 * = 5 - 8 ||< **Oxidation and reduction**
 * explain oxidation and reduction as an electron transfer process
 * calculate oxidation numbers
 * identify and name oxidants and reductants in equations
 * identify oxidation-reduction reactions using oxidation numbers
 * describe, write equations for and interpret observations for:
 * metal displacement reactions
 * halogen displacement reactions
 * write balanced simple redox equations (metal/metal ion, metal/hydrogen ion and halogen/halide ion)
 * describe and explain how an electric current is conducted in an electrolytic cell
 * describe and explain the following during the operation of an electrolytic cell:
 * anode processes
 * cathode processes
 * role of the electrolyte
 * direction of ion migration
 * direction of electron flow in external circuit
 * electrode product prediction for molten metal halides only
 * predict and name the electrode products for the electrolysis of molten metal halides only
 * Applied chemistry **
 * = 9 -13 ||< ** Organic chemistry **
 * describe the bonding capacity of carbon
 * explain the diversity of carbon based compounds
 * Alkanes:
 * name and draw straight and simple branched to C8
 * observations and equations for:
 * substitution reactions
 * combustion reactions
 * draw and name structural isomers
 * Alkenes:
 * name and draw straight and simple branched to C8 (only one double bond per structure)
 * write observations and equations for:
 * addition reactions with halogens and hydrogen
 * combustion reactions
 * draw and name structural and geometric isomers
 * Cycloalkanes and cycloalkenes:
 * draw and name simple structures to C8
 * write observations and equations for:
 * substitution and combustion reactions for cycloalkanes
 * addition and combustion reactions for cycloalkenes
 * Benzene:
 * explain the unique structure and reactivity of benzene
 * write equations for:
 * catalysed substitution reactions with halogens
 * combustion reactions
 * describe and explain the sources and uses of hydrocarbons e.g. fuels
 * determine molecular formulae (organic or inorganic) from empirical formula and molar mass
 * = 14 ||= **Revision for exam** ||
 * = 15 - 17 ||= ** Task 12 Semester 2 Examination ** ||

Exploring Chemistry Stage 2

 * = Term ||= Week ||= Strand ||= Set ||= Title || Page Numbers ||
 * = 1 ||= 1 ||= Macroscopic Properties of Matter ||= 1, 2 ||< * Mixtures
 * Solutions || 34 -35 ||
 * =  ||= 2 ||   ||= 3 ||< * Kinetic theory || 36 ||
 * =  ||= 3 || Atomic Structure and Bonding ||= 4 ||< * Atoms and isotopes || 49 ||
 * =  ||= 4 ||   ||= 5 ||< * Atomic structure and the periodic table || 51 ||
 * =  ||= 5 ||   ||= 6 ||< * Bonding || 52 ||
 * =  ||= 6 ||   ||= 7 ||< * Uses, properties and structure || 54 ||
 * =  ||= 7 || Chemical Reactions ||= 8 ||< * Elements and compounds || 94 ||
 * =  ||= 8 ||   ||= 9 ||< * Molar mass || 97 ||
 * =  ||= 9 ||   ||= 10 ||< * Moles, particles and mass || 99 ||
 * =  ||= 10 ||   ||= 11 ||< * Interpretation of formulae || 101 ||
 * = 2 ||= 1 ||  ||= 12 ||< * Percentage composition || 103 ||
 * =  ||= 2 ||   ||= 13 ||< * Ionic equations || 105 ||
 * =  ||= 3 ||   ||= 14 ||< * Stoichiometry and gas volumes || 107 ||
 * =  ||= 4 ||   ||= 15 ||< * Solution concentrations || 110 ||
 * =  ||= 5 || Acids and Bases ||= 22 ||< * Solution of acids and bases || 153 ||
 * =  ||= 6 ||   ||= 23 ||< * Acid and base reaction stoichiometry || 156 ||
 * =  ||= 7 || Chemical Reactions ||= 16 ||< * Empirical formulae || 113 ||
 * =  ||= 8 ||   ||= 17 ||< * Limiting reagents || 117 ||
 * =  ||= 9 ||   ||= 18 ||< * Gas volumes || 120 ||
 * =  ||= 10 ||   ||= 19 ||< * Stoichiometry || 122 ||
 * = 3 ||= 1 ||  ||= 20 ||< * Reacting masses and gaseous and solution volumes || 124 ||
 * =  ||= 2 ||   ||= 21 ||< * Equations and observations || 127 ||
 * =  ||= 3 ||   ||=   ||<   ||   ||
 * =  ||= 4 ||   ||=   ||<   ||   ||
 * =  ||= 5 || Oxidation and Reduction ||= 24 ||< * Oxidation number (ON) || 174 ||
 * =  ||= 6 ||   ||= 25 ||< * Balancing half equations || 176 ||
 * =  ||= 7 ||   ||= 26 ||< * Balancing overall redox equations || 177 ||
 * =  ||= 8 ||   ||=   ||<   ||   ||
 * =  ||= 9 || Organic Chemistry ||= 27 ||< * Naming and drawing hydrocarbons || 188 ||
 * =  ||= 10 ||   ||= 28 ||< * Reactions of hydrocarbons || 194 ||
 * = 4 ||= 1 ||  ||= 29 ||< * Calculations involving hydrocarbons || 198 ||