Additional Higher Level Syllabus
Topic 12: The Mass Spectrometer (1hr)
12.1.1 State the principles of a mass spectrometer and outline the main stages in its operation.
12.1.2 Describe how the mass spectrometer may be used to determine relative isotopic, atomic and molecular masses, using the 12C scale.
12.2 Electronic Configuration of Atoms (3hr)
12.2.1 State and explain how the evidence from first and successive ionization energies accounts for the existence of main energy levels and sub-levels.
12.2.2 State how orbitals are labeled. n<5
12.2.3 State the relative energies of s, p, d and f orbitals.
12.2.4 State the number of orbitals at each energy level.
12.2.5 Draw the shapes of px, py and pz orbitals.
12.2.6 State the Aufbau principle.
12.2.7 Apply the Aufbau notation for electronic configurations (up to Z=54). Exceptions not expected.
12.2.8 Relate the electronic configuration of an atom to its position in the Periodic Table.
13.1 Periodic trends Na --> Ar
13.1.1 Explain the physical properties of the chlorides and oxides of the elements (Na to Ar), in terms of their bonding and structure.
13.1.2 describe the chemical trends for the chlorides and oxides referred to in 13.1.1 include relevant questions
13.2 d-block Elements (first row) (2hr)
13.2.1 List the characteristic properties of transitions elements.
13.2.2 Identify which elements are considered typical of the d-block.
13.2.3 Describe the existence of variable oxidation states in d-block elements.
13.2.4 Define the term ligand.
13.2.5 Describe how complexes of d-block elements are formed
13.2.5 Explain why some complexes of the d-block element are colored .
13.2.6 Describe the catalytic behavior of d-block elements and their compounds. MnO2 in decomposition of peroxides, V2O5 in the contact process, Fe in the Haber process, Ni in conversions of alkenes to alkanes. Mechanisms are not required.
13.2.7 Outline the catalytic behavior of d-block elements and their compounds.
14.1 Shapes of molecules and ions (1hr)
14.1.1 State and predict the shape and bond angles using the Valence Shell Electron pair Repulsion (VSEPR) theory for 5 and 6 negative charge centers.
14.2 Hybridization (2hr)
14.2.1 Describe sigma and pi bonds.
14.2.2 State and explain the meaning hybridization the term hybridization.
14.3.2 Predict the types of hybridization
14.3 Delocalization of electrons (2hr)
14.3.1 State what is meant by the delocalization of pi electrons and explain how this can account for the structures of some substances.
14.4.1 Structures of Allotropes of Carbon (1hr)
14.4.1 describe and explain the structures and properties of diamond, graphite and fullerene.
15.1 Standard enthalpy changes of reaction (1hr)
15.1.1 Define and use the terms 'standard state' and 'standard enthalpy change of formation'. Use 101 kPa and 298 K
15.1.2 Calculate the enthalpy change of a reaction using standard enthalpy changes of formation
15.2 Lattice enthalpy (2hr)
15.2.1 Define the term 'lattice enthalpy'.
15.2.2 Compare the effect of both the relative size and charges of ions on the lattice enthalpies of different ionic compounds
15.2.3 Construct a Born-Haber cycle and use it to calculate the enthalpy change.
15.2.4 Analyze theoretical and experimental lattice enthalpy values
15.3 Spontaneity of a Reaction (1hr)
15.3.1 Calculate the standard entropy change for a reaction using values of absolute entropies
15.3.2 Calculate D G° for a reaction using the equation D G° = D H° - TDS° or by using values of the standard Gibbs free energy change of formation.D G°f
.
16.1 Rate expression (3hr).
16.1.1 Define the terms 'order of a reaction' and 'rate constant'.
16.1.2 Derive the rate expression for a reaction from data
16.1.3 Draw and analyze graphical representations for zero, first, and second order reactions.
16.1.4 define the term half-life and calculate the half-life for 1st order reactions
16.2 Reaction mechanisms(1hr)
16.2.1 Define the terms 'rate determining step' , 'molecularity' and 'activated complexes'.
16.2.2 Describe the relationship between mechanism, order, rate determining step and activated complex.
16.3 Activation Energy (2hr)
16.3 describe qualitatively the relationship between the rate constant (k) and temperature (T)
16.3.2 describe how the Arrhenius equation can be used to determine the activation energy and the Arrhenius constant (A)
16.3.3 Draw and explain enthalpy level diagrams for reactions with and without catalysts
16.3.4 Distinguish between homogeneous and heterogeneous catalysts.
17.3.5 Outline the use of homogeneous and heterogeneous catalysts.
17.1 Phase equilibrium (2hr)
17.1.1 State and explain the equilibrium established between a liquid and its own vapor.
17.1.2 State and explain the qualitative relationship between vapor pressure and temperature.
17.1.3 State and explain the relationship between enthalpy of vaporization, boiling point and intermolecular forces.
17.2 The Equilibrium Law (2hr)
17.2.1 Solve homogeneous equilibrium problems using the expression for Kc
18.1 Bronsted-Lowry Acids and Bases (2hr)
18.1.1 define acids and bases according to the Bronsted-Lowry theory
18.1.2 Identify whether or not a compound could act as a Bronsted_Lowry acid or base
18.1.3 Identify the conjugate acid-base pairs in a given acid-base reaction.
18.1.4 Determine the structure for the conjugate acid (or base) of any Bronsted-Lowry base (or acid)
18.2 Lewis theory (1hr)
18.2.1 Define and use the terms 'Lewis acid' and 'Lewis base"
18.3 Calculations Involving Acids and Bases (5hr)
18.3.1 State the expression for the ionic product constant of water Kw
18.3.2 Deduce [H+] and [OH-] for water at different temperatures given Kw values.
18.3.3 Define pH, pOH, and pKw
18.3.4 Calculate the pH, pOH, [H+(aq)] and [OH-(aq)] from specified concentrations
18.3.5 State the equation for the reaction of any acid or base with water and hence derive the ionization constant expression for any weak acid or base in water.
18.3.6 Derive the expression Ka X Kb =Kw and use it to solve problems for any weak acid and its conjugate base and for any weak base and its conjugate acid
18.3.7 State and explain the relationship between Ka and pKa and Kb and pKb.
18.3.8 determine the relative strengths of acids and their conjugate bases from Ka or pKa values.
18.3.9 Apply Ka or pKa in calculations.
18.3.10 Calculate the pH of a specified buffer system.
18.4 Salt Hydrolysis (1hr)
18.4.1 State and explain whether salts form acidic, alkaline or neutral aqueous solutions.
18.5 Acid-base Titrations (1hr)
18.5.1 Draw and explain the general shapes of graphs showing pH against volume of titrant for titrations involving monoprotic acids and bases.
18.6 Indicators (1hr)
18.6.1 Describe qualitatively how an acid-base indicator works.
coulour A ...................coulour B
18.6.2 Sketch and explain how the pH range of an acid-base indicator relates to its pKa.
18.6.3 determine an appropriate indicator for a titration, given the equivalence point of the titration and Ka (or pKa) values for possible indicators.
Topic 19 - Oxidation and Reduction
19.1 Redox equations (2hr)
19.1.1 Balance redox equations in acidic solution.
19.2 Standard electrode potentials (3hr)
19.1.1 Describe the standard hydrogen electrode.
19.2.2 Define the term standard electrode potential and explain the measurement of standard electrode potential to produce the electrochemical series.
19.2.3 Define the term 'cell potential' and calculate cell potentials using standard electrode potentials
19.2.4 Predict whether a reaction will be spontaneous, by using standard electrode potentials.
193 Electrolysis (2hr)
19.3.1 List and explain the factors affecting the products formed in the electrolysis of aqueous solutions.
19.3.2 List the factors affecting the amount of product formed during electrolysis
19.3.3 determine the relative amounts of products forms during the electrolysis of aqueous solutions.
20.1 Determination of Structure (4hr)
20.1.1 State that the structure of a compound can be determined by using information from a variety of spectroscopic and chemical techniques.
20.1.2 describe and explain hoe information from an infrared spectrum can be used to identify functional groups in a compound.
20.1.3 describe and explain how information from a mass spectrum can be used to determine the structure of a compound.
20.1.4 Describe and explain how information from a H NMR spectrum can be used to determine the structure of a compound.
20.2 Hydrocarbons (2hr)
20.2.1 State and explain how the poor reactivity of alkanes in terms of inertness of C-H and C-C bonds.
21.2.2 State and explain that alkanes can react with halogens and explain the difference between homolytic and heterolytic fission.
21.2.3 Describe and explain the structure of benzene, using chemical and physical evidence.
20.3 Nucleophilic Substitution reactions (2hr)
20.3.1 Distinguish between primary, secondary and tertiary halogenoalkanes.
20.3.2 Describe and explain the Sn1 and Sn2 mechanisms in nucleophilic substitution.
20.3.3 Describe and explain the molecularity for the Sn1 and Sn2 mechanisms.
20.3.4 Describe how the rate of nucleophilic substitution in halogenoalkanes depends on both the identity of the halogen and whether the halogenoalkane is primary, secondary tertiary.
20.4 Alkanols (1hr)
20.4.1 Describe the dehydration reaction of alcohols to form alkenes.
20.4.2 Determine the products of the oxidation of primary, secondary and tertiary alkanols using acidified dichromate(VI) solution.