The learning outcomes for this unit are described below. These outcomes are built from the learning activities in lectures, tutorials, laboratory and independent study. Important attributes are:
- the ability to apply scientific knowledge and critical thinking to identify, define and analyse problem and create solutions: you will be expected to demonstrate these outcomes on problems drawn from the material presented in the course and to novel situations.
- the ability to evaluate your own performance and development and to recognize gaps in your knowledge: keep a portfolio of your progress using the 'self assessment tool'
- Generic Attributes
By the end of this topic, you should be able to
- apply scientific knowledge and critical thinking to identify, define and analyse problems, create solutions, evaluate opinions, innovate and improve current practices
- gather, evaluate and deploy information relevant to a scientific problem
- disseminate new knowledge and engage in debate about scientific issues
- recognize the rapid and sometimes major changes in scientific knowledge and technology, and to value the importance of continual growth in knowledge and skills
- use a range of computer software packages in the process of gathering, processing and disseminating scientific knowledge
- make value judgements about the reliability and relevance of information in a scientific context
- evaluate your own performance and development, to recognize gaps in knowledge and acquire new knowledge independently
- set achievable and realistic goals and monitor and evaluate progress towards these goals
- appreciate sustainability and the impact of science within the broader economic, environmental and socio-cultural context
- present and interpret data or other scientific information using graphs, tables, figures and symbols
- work independently and as part of a team and to take individual responsibility with a group for developing and achieving goals
- actively seek, identify and create effective contacts with others in a professional and social context, and maintain those contacts for mutual benefit
- recognize the importance of safety and risk management and compliance with safety procedures
- manipulative equations and measurements with due regard for significant figures and unit conventions
- Laboratory Skills
By the end of this topic, you should be able to
- perform careful and safe experiments
- accurately report scientific observations
- work as a professional scientist with due regard for personal safety and for the safety of those around you
- interpret observations in terms of chemical models with appropriate use of chemical equations and calculations
- perform calculations containing concentrations, moles and masses
- choose and use appropriate glassware for a given task
- choose and use balances accurately and appropriately
- present and interpret data or other scientific information using graphs, tables, figures and symbols
- work as a member of a team and to take individual responsibility within a group for developing and achieving group goals
- actively seek, identify and create effective contacts with others in a professional and social context, and maintain those contacts for mutual benefit
- Nuclear and Radiation Chemistry
By the end of this topic, you should be able to
- summarise the postulates of Dalton’s Atomic theory, and put them into a modern context.
- recognise the components of a mass spectrometer, and know what it is used for.
- recognise nuclear reactions, including the major spontaneous decay mechanisms.
- define and distinguish between nucleons, nuclides and isotopes, X-rays & gamma rays, decay series and daughter isotopes.
- explain stellar nucleogenesis.
- calculate the average atomic mass from isotope information
- balance nuclear reactions
- recognise stable and unstable nuclides
- predict the decay mechanism for an unstable isotope
- calculate the activity or half-life of an unstable nuclide from appropriate data.
- calculate the age of a sample using the carbon-14 method, and know the underlying assumptions and appropriate timescale for its application.
- explain the main factors that contributes to effective radiation dose, including penetrating power, activity and energy
- explain the main mechanism of biological damage by ionizing radiation.
- explain the use of radioactive isotopes in medical imaging, and distinguish the information obtained from X-rays
- explain how isotope generators produce isotopes such as 99mTc for medical imaging, and give some examples of its use.
- explain PET, the generation of radioisotopes by a cyclotron, and know the kinds of isotopes produced.
- The Periodic Table and Periodic Trends
By the end of this topic, you should be able to
- give examples of periodic trends and chemical properties used to construct the Periodic Table.
- assign atoms to appropriate groups in the Periodic Table on the basis of their properties
- explain the historic significance of key events in the development of modern atomic structure theory, such as nuclear charge, atomic mass and the discovery of the neutron
- define ionization energy and atomic radius and know their trends in the Periodic Table.
- Wave Theory of Electrons and Atomic Energy Levels
By the end of this topic, you should be able to
- name the key experimental observations that led to the development of quantum mechanics
- convert between velocity, kinetic energy or momentum and wavelength of a free electron (or other particle of known mass)
- identify the components of the wave equation
- convert between the wavelength, frequency and energy of light
- calculate the allowed energy of a hydrogen-like atom of atomic number Z and quantum number n, and the wavelength of a transition between energy levels.
- appreciate how the wave nature of an electron leads to discrete energy levels
- Shape of Atomic Orbitals and Quantum Numbers
By the end of this topic, you should be able to
- identify the key features of waves in 1-3 dimensions - displacement, amplitude, nodes
- explain the meaning of the orbital quantum numbers, n, l, m, and the designation of orbitals such as 1s, 3d, 4p, 4f..
- recognize the representations of waves as cross-sectional graphs, contour plots and lobes
- recognise the shapes of atomic orbitals in these representations
- understand how the wavefunction relates to electron charge density
- explain why the spatial extent of the electron increases with energy
- Filling Energy Levels in Atoms Larger than Hydrogen
By the end of this topic, you should be able to
- draw out the electron configuration for atoms in the s-and p-blocks of the Periodic Table, including unpaired electrons
- explain why the orbitals with the same principal quantum number but different angular momentum quantum numbers have different energies in multi-electron atoms
- explain periodic trends in atomic radii and ionization energies in terms of quantum theory
- define electron affinity and explain some features of its periodic trends in terms of electronic configurations derived from quantum theory.
- Atomic Electronic Spectroscopy
By the end of this topic, you should be able to
- explain the difference between core and valence electrons
- distinguish between absorbance and emission spectra
- explain how atomic absorption spectroscopy (AAS) works
- convert experimental data between transmission, absorbance, and concentration if given appropriate information
- calculate the minimum wavelength of Bremsstrahlung radiation
- explain how the elements in stars and other celestial objects can be identified and their abundances measured from visible and X-ray spectrometry
- Material Properties (Polymers, Liquid Crystals, Metals, Ceramics)
By the end of this topic, you should be able to
- explain complementary colours
- explain the origins of discrete and continuous spectra
- relate wavelength of a photon to energy difference
- describe the qualitative differences between atomic and molecular electronic spectra
- define conductivity, paramagnetism and diamagnetism
- recognise conductors and insulators by their conductivity
- define an allotrope
- define UV-A -B, and -C radiation.
- Bonding in H2 - MO theory
By the end of this topic, you should be able to
- explain the reason for bond formation being due to energy lowering of delocalised electrons in molecular orbitals
- describe a molecular orbital
- recognise sigma bonding, sigma* antibonding and non-bonding orbitals
- assign the (ground) electron configuration of a diatomic molecule.
- define HOMO and LUMO, and homonuclear and heteronuclear diatomic molecules
- Bonding in O2, N2, C2H2 and C2H4
By the end of this topic, you should be able to
- distinguish between various types of bonding, anti-bonding and non-bonding orbitals
- distinguish between polar and apolar bonds in diatomic molecules and relate it to electron attraction of a nucleus
- draw out ground state electronic configurations for molecules and molecular ions given their allowed energy levels
- calculate bond order from molecular electronic configurations
- relate Electronic Absorbance Spectra to electronic structure
- Band Theory - MO in Solids
By the end of this topic, you should be able to
- explain how band structure in insulators, semiconductors and metals arise from delocalised orbitals
- describe the characteristics of natural and doped semiconductors, including band-gap energy
- explain how semiconductors are used in solar energy collection and conversion
- describe chemical vapour deposition, and how it can be used to build up layers of different composition.
- Ionic Bonding
By the end of this topic, you should be able to
- explain the origin of ionic bonding as a limiting case of MO theory
- explain why ionic interactions lead to crystals rather than small molecules
- define the Madelung constant, and explain its relevance to the stability of an ionic crystal
- explain how ionic radii influence crystal structure, and why they differ from atomic radii
- Lewis Structures
By the end of this topic, you should be able to
- draw out plausible Lewis structures for simple polyatomic molecules
- assign bond orders based on sharing of electron pairs and resonance structures
- identify carbon-carbon single, double and triple bonds, as well as aldehyde, alcohol and nitrile functional groups and their bonding
- VSEPR
By the end of this topic, you should be able to
- assign molecular shapes based on Lewis structures
- recognise four functional groups: aldehyde, alcohol, ketone and nitrile
- recognise the following functional groups in organic molecules: aldehyde, alcohol, ketone, nitrile, ether, ester, carboxylic acid, amine, amide, acid chloride and alkyl halide, as well as benzene and alkanes, alkenes, and alkynes
- Liquid Crystals
By the end of this topic, you should be able to
- describe lyotropic, nematic and smectic A & C thermotropic liquid crystals
- explain the general features of the liquid crystal state
- describe how liquid crystals can be used to generate displays
- relate intermolecular forces to boiling points and surface tension
- Thermochemistry
By the end of this topic, you should be able to
- define system, surroundings and universe for simple thermodynamic processes
- explain the difference between heat and temperature
- use the First Law of Thermodynamics to calculate the change in internal energy accompanying heating and expanding an ideal gas
- relate temperature and heat change using specific and molar heat capacities
- calculate internal energy changes using the bomb calorimeter
- Enthalpy
By the end of this topic, you should be able to
- define the difference between internal energy and enthalpy
- draw enthalpy diagrams for endothermic and exothermic processes
- obtain the enthalpy change using a coffee-cup calorimeter
- define the enthalpy change for phase changes and for the formation, atomization and combustion of compounds
- use Hess's Law
- estimate atomization energies from bond enthalpies
- define standard states
- combine enthalpies of formation to work out the enthalpy change for chemical reactions
- combine enthalpies of reactions to work out the enthalpies of formation
- explain the advantages and disadvantages of solid, petroleum, hypergolic and cryogenic fuels
- work out the efficiency of fuels
- Entropy
By the end of this topic, you should be able to
- explain the thermodynamic concept of spontaneity
- define entropy as the tendency of energy to spread out in a spontaneous process
- predict the relative entropy of solids, liquids and gases and how entropy is affected by temperature, molecular size and complexity
- define and use the Second Law of Thermodynamics
- relate the entropy change of the universe to the Gibbs free energy
- use Gibbs free energy to predict spontaneous and non-spontaneous processes
- Nitrogen Chemistry and Compounds
By the end of this topic, you should be able to
- explain the difference between a fuel and an explosive
- explain the concept of activation energy
- work out the oxidation number of nitrogen in its compounds
- work out the shapes and the number of unpaired electrons on nitrogen oxides and halides
- discuss the NOx cycle in the atmosphere
- explain the formation of PAN and acid rain
- calculate the temperature of a planet without a greenhouse effect
- comment on the evidence for global warming and the most important greenhouse gases
- Equilibrium
By the end of this topic, you should be able to
- explain what reactions are spontaneous and under what conditions
- explain the dynamic nature of equilibrium processes
- write the equilibrium constant for any reaction or process
- use initial, change, equilibrium (ICE) tables and the small 'x' approach to work out equilibrium concentations
- convert between the equilibrium constant in terms of partual pressures, Kc, and in terms of concentrations, Kp
- calculate the value of the equilibrium constant for a reverse reaction from its value for a forward reaction, and if the stoichiometry is changed
- calculate the equilibrium constant for a reaction obtained by combining two other reactions
- explain the difference between the equilibrium constant, K, and the reaction quotient, Q
- write down the reaction quotient and use it to predict the direction of change
- use Le Chatelier's principle to predict the response of a system at equilibrium to changes in temperature, pressure and composition
- explain how catalysts effect chemical reactions without changing the equilibrium concentrations
- Equilibrium and Thermochemistry in Industrial Processes
By the end of this topic, you should be able to
- explain the main processes used industrially to extract metals from their ores
- use Ellingham diagrams to predict which metals can be extracted using coke at different temperatures
- discuss the role of the chemical industry in the modern world and Australia with particular regard to the Top Ten chemicals
- outline the thermodynamic principles behind the industrially optimized routes to sulfuric acid and ammonia
- Electrochemistry
By the end of this topic, you should be able to
- relate the sign of the electrode potential to the direction of spontaneous change
- combine half cells to produce balanced redox reactions and to calculate cell potentials
- identify the species which are being oxidzied and those being reduced in a redox reaction
- write down the cell notation for a Galvanic cell including ones involving inert electrodes
- use the Nernst equation to calculate the effect of concentration on the cell potential
- relate the electrode potential and the reaction quotient
- relate the standard electrode potential and the equilibrium constant
- Electrolytic Cells
By the end of this topic, you should be able to
- identify the processes and species formed at the anode and cathode of Galvanic and electrolytic cells
- identify the direction of electron flow in Galvanic and electrolytic cells
- identify what can be electroysed and the role of over-potential in the electrolysis of water and in the production of NaOH and Cl2
- use Faraday's Laws of Electrolysis to relate the amount of product to the electric current applied
- Types of Intermolecular Forces
By the end of this topic, you should be able to
- describe the different kinds of intermolecular forces that exist
- identify which intermolecular forces are present and which are more important between different molecules
- relate variations in melting and boiling points in related compounds to their intermolecular forces