65111 Chemistry 1

Warning: The information on this page is indicative. The subject outline for a particular semester, location and mode of offering is the authoritative source of all information about the subject for that offering. Required texts, recommended texts and references in particular are likely to change. Students will be provided with a subject outline once they enrol in the subject.

Handbook description

The study of chemistry is central to an understanding of the world around us and is relevant to all other science areas, such as physics, biology, geology and the environment at the fundamental level. This subject is designed to develop a student's understanding of the basic principles of chemistry. Topics covered are an introduction to matter, chemical reactions, atomic structure, stoichiometry, the periodic table, bonding, intermolecular forces and crystal structures, molecular geometry, introductory carbon chemistry, equilibrium, and acid-base equilibria. The subject provides the requisite knowledge and skills for 65212 Chemistry 2.

Subject objectives/outcomes

On completion of this subject students are expected to:

1. be able to describe the differences between elements, compounds and mixtures and recognise the important differences between states of matter,
2. understand the electronic structure of the atom, how ions are formed and allocate electrons to atoms in terms of energy levels,
3. understand the significance of the periodic table and predict properties of elements from their position in the periodic table,
4. balance chemical equations including redox reactions,
5. understand the mole concept and apply it to quantitative calculations,
6. draw Lewis structures for simple molecules, interconvert full and abbreviated structural formulae and electron-dot formulae,
7. apply VSEPR theory to the geometry of molecules and predict shapes of molecules from electron–dot notation,
8. identify the bonding type in compounds,
9. understand the concept of intermolecular forces and relate this to how water acts as a solvent,
10. identify functional groups in organic structures, use IUPAC rules to name simple alkanes, alkenes, alkynes, alcohols, ethers and halogen compounds and write structures for the possible constitutional isomers of a given molecular formula
11. write equations for the combustion and halogenation reactions of alkanes and cycloalkanes, and addition reactions of alkenes,
12. describe the bonding in hydrocarbons in terms of hybridisation, sigma and pi bonds and work out the degree of hydrogen deficiency (degree of unsaturation),
13. understand the concept of stereoisomerism, name alkene cis/trans isomers and identify the eclipsed and staggered conformations of alkanes and the chair conformation of cyclohexane,
14. understand the concept of reversible reactions, apply Le Chatelier’s principle and calculate equilibrium constants,
15. identify weak acids and weak bases and conjugate acid/base pairs, understand the concepts of Kw, pH and Ka and be able to calculate pH, Ka , pKa and % dissociation.

Contribution to course aims and graduate attributes

Chemistry 1 provides the student with foundational theoretical and practical discipline based knowledge required for the application of chemistry in interdisciplinary environments and provides the foundation concepts and skills essential for undertaking Chemistry 2. Professional skills are developed in the laboratory through the application of specific experimental techniques and numeracy and analytical skills are developed through data analysis and problem solving. Communication skills are developed through a communication activity early in the semester.

Teaching and learning strategies

Chemistry 1 is taught on a lecture/practical/workshop basis and includes lectures providing an introduction to key concepts, tutorial problems to support the learning from the lectures and laboratory experiments and workshop exercises to extend the theory and help the students understand the key concepts developed in the lectures. The practical component also focuses on the development of practical skills.

The teaching of this subject will be carried out in six contact hours per week comprised of:

• 3 hours lecture,
• 3 hours practical/workshop.

Content

The following topics will be covered:

• Classification of matter, ionic, molecular and macromolecular compounds.
• Brief description of the structure of atoms, relative masses and charges of basic subatomic particles.
• Writing and balancing net ionic equations for specific reactions.
• Activity series of metals and balancing redox equations.
• Atomic mass table. Mole concept. Concentration in terms of molarity. Ttitrations.
• The concept of electronic energy levels. Planck’s equation.
• Allocation of electrons into an energy level diagram. Aufbau principle, Hund’s rule, Pauli exclusion principle, quantum numbers.
• General description of the periodic table – periodicity of electron configurations, atomic and covalent radii, ionization energies, electron affinities and electronegativities.
• Descriptive account of covalent bonding in terms of sharing valence electrons, octet trend, electron pairing, electron-dot notation. Lewis formulas. Multiple bonding. Shapes of molecules and complex ions, electron pair repulsion theory. Resonance concept.
• Bond polarity, dipole moments, polar molecules, intermolecular forces, hydrogen bonding.
• Crystals and amorphous solids. Structures of ionic, molecular and macromolecular crystals.
• Covalent bonding in carbon. The functional group concept. Recognition of alkene, alkyne, haloalkane, alcohol and ether. Nomenclature of simple carbon compounds incorporating these functional groups.
• Conformations of alkanes and cycloalkanes, and their relative stabilities.
• Constitutional isomerism and alkene cis/trans stereoisomerism.
• Introduction to reactions of alkanes, alkenes and alkynes.
• Differentiation between alcohols and carboxylic acids by simple chemical tests.
• Concept of dynamic equilibrium. Equilibrium constant. Calculations and meaning of Kc and Kp. Reaction quotient (Q). Factors that affect chemical equilibrium. Le Chatelier’s principle.
• Lewis and Lowry-Brønsted theories. Dissociation constants of weak acids and weak bases. Definition of Ka , pKa and degree of dissociation.

Assumed Knowledge: basic skills in mathematics (algebra, graph plotting, properties of logarithms) and proficiency in written and spoken English are assumed.

Assessment

Assessment Item 1: Practical components

Assessment Item 2: Mid-semester quiz

Assessment Item 3: Final Exam

Minimum requirements

In order to be eligible for consideration for a pass in Chemistry 1, a student must achieve at least 40% in the final examination in this subject. If 40% is not reached, an X grade fail may be awarded for the subject, irrespective of an overall mark greater than 50.

Practical classes in subjects offered by the School of Chemistry and Forensic Science are an essential and integral part of each subject in which they run. In addition to assisting students’ understanding of concepts, practical classes develop laboratory skills and experience, including safety skills, that are essential graduate attributes desired by employers. Thus, students are expected to attend all scheduled practical classes. Failure to attend a class that is associated with an assessment item will attract a mark of zero for that assessment item unless an acceptable reason for their absence, supported by relevant documentary evidence, is provided to the subject coordinator.

Required texts

Blackman, Bottle, Schmid, Mocerino, Wille, Chemistry, 2nd ed Wiley, Australia 2012

Recommended texts

Aylward and Findlay, S.I. Data book, 6th ed Wiley Australia 2008

Zeegers et alia, Essential Skills for Science and Technology: Oxford University Press 2008

Paul Monk, Maths for Chemistry 2nd Ed Oxford University Press 2010