Handbook : Unit informationEdith Cowan University

Faculty of Health, Engineering and Science

School: Natural Sciences

This unit information may be updated and amended immediately prior to semester. To ensure you have the correct outline, please check it again at the beginning of semester.

• Unit Title

  General Chemistry

• Unit Code

  SCC1111

• Year

  2015

• Enrolment Period

  1

• Version

  2

• Credit Points

  15

• Full Year Unit

  N

• Mode of Delivery

  On Campus
  

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Description

This is a unit which develops students' understanding of important chemical concepts and principles in physical and inorganic chemistry. The unit illustrates the applications of chemistry worldwide. A WACE chemistry background is assumed.

Prerequisite Rule

Must have received a mark of over 50 in WACE Chemistry 2A/2B or 3A/3B

Learning Outcomes

On completion of this unit students should be able to:

1. Demonstrate competency in written communication.
2. Demonstrate key laboratory skills including team work, time management and negotiation of roles.
3. Demonstrate problem solving skills in evaluating appropriate experimental approaches for analyses.
4. Demonstrate safe handling and appropriate use and disposal of chemicals.
5. Explain and apply fundamental concepts, principles and theories of physical and inorganic chemistry.
6. Identify and describe some important applications of chemistry in key industries worldwide.
7. Perform mathematical calculations relating to the gas laws, solutions, reaction stoichiometry, chemical equilibria and pH.

Unit Content

1. Acids and Bases Acids, bases and salts, neutralisation, strong and weak acids and bases, water as a weak electrolyte, Kw, pH, indicators, acid-base titrations, buffer solutions. Acid ionisation constants, Henderson-Hasselbach equation, hydrolysis constants; calculation of [H+], [OH-] and pH for weak acids and bases, buffer solutions; titration curves.
2. Atomic Structure, Bonding and the Solid State Quantum theory, Bohr atom, quantum mechanical atom, quantum mechanics, quantum numbers, atomic orbitals and their energies, Pauli exclusion principle, Hunds rule, Aufbau principle. Development of the periodic table, periodic variation in physical and chemical properties, ionisation energy, electron affinity, electronegativity, main group chemistry. Chemical bonding; metallic, ionic and covalent bonding, Lewis structures. Molecular geometry and shape, Valence Shell Electron Pair Repulsion Theory, Valence Bond Theory, hybridisation. Intermolecular forces: dispersion, dipole-dipole, and hydrogen bonding.
3. Chemical Reactions Energy changes accompanying chemical reactions, exothermic and endothermic processes. Sources of energy, energy conservation. Rates of reaction, factors affecting reaction rate, reaction profile diagrams. Equilibria in chemical reactions, characteristics of equilibrium, Le Chatelier's Principle, reaction quotient and equilibrium constant. Calculating the equilibirium. Solubility equilibria and problems involving solubility products.
4. Gases Review of gas laws, Kinetic Theory of Gases, Avogadro's Hypothesis, mole-gas volume calculations; ideal gas equation, non-ideality, van der Waals equation.
5. Review of Chemical Fundamentals Element symbols, chemical formulae, chemical equations, stoichiometry, mass-mass calculations; limiting reagent, oxidation reduction.
6. Water and the Liquid State Changes of state, cooling curves, vapour pressure, simple phase diagrams. Solutions, common aqueous solutions, concentration of solutions in mol L-1, percentage composition, molality and mole fraction. Colligative properties. Electrolyte solutions; strong, weak and non-electrolytes, relationship to conductivity.

Additional Learning Experience Information

Lectures, pre-laboratory activities and briefings, and laboratory work. Lectures provide students with the theoretical background in chemistry. Laboratory work gives students opportunity to put into practice lecture material, learn chemical laboratory skills and recording of observations. The pre-laboratory activities require students to identify risk and hence appropriate handling of chemicals. The pre-lab briefings discuss appropriate handling and disposal of chemicals in terms of personal safety and environmentally sustainable practice.

Assessment

GS1 GRADING SCHEMA 1 Used for standard coursework units

Students please note: The marks and grades received by students on assessments may be subject to further moderation. All marks and grades are to be considered provisional until endorsed by the relevant Board of Examiners.

Due to the professional competency skill development associated with this Unit, student attendance/participation within listed in-class activities is compulsory. Students failing to meet participation standards as outlined in the unit plan may be awarded an I Grade (Fail - incomplete). Students who are unable to meet this requirement for medical or other reasons must seek the approval of the unit coordinator.

Text References

• ^ Mahaffey, P., Bucat, R., Tasker, R., Kotz, J., Treichel, P., Weaver, G., & McMurry, J. (2014). Chemistry: Human activity, chemical reactivity. Toronto: Nelson.
• Brown, T.L., LeMay, H.E., Bursten, B.E., Langford, S., Sagatys, D. & Duffy, N. (2009). Chemistry, The central science: A broad perspective (2nd ed.). NSW: Pearson Education Australia.
• Blackman, A., Bottle, S., Schmid, S., Mocerino, M., & Wille, W. (2008). Chemistry (2nd ed.). QLD: Wiley and Sons Australia Ltd.
• Chang, R. (2010). Chemistry (10th ed.). Sydney: McGraw-Hill.

^ Mandatory reference

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