INTRODUCTION TO PHYSICAL CHEMISTRY - 2017/8
Module code: CHE1036
RIDGE K Dr (Chemistry)
Number of Credits
FHEQ Level 4
Module cap (Maximum number of students)
Overall student workload
Independent Study Hours: 83
Lecture Hours: 33
Tutorial Hours: 4
Laboratory Hours: 36
|Assessment type||Unit of assessment||Weighting|
|Examination||EXAM - 1.5 HOURS||60%|
|Coursework||PRACTICAL WORK LABS AND REPORTS||30%|
No alternative to Examination and tutorial exercises Failure of practical unit of assessment will be required to attend during the Late Summer Assessment period and complete a defined practical course.
Prerequisites / Co-requisites
This module gives an introduction to fundamental laws that govern the behaviour of matter through an understanding of the properties of matter at molecular, atomic and subatomic level.
To provide an understanding of the principles underlying elementary quantum theory and their experimental foundation.
To introduce the basic principles of molecular spectroscopy.
To provide a basic understanding of thermodynamics and kinetics and their relevance to chemistry in the real world.
|Understand the underlying concepts and principles of the Kinetic Theory of Gases||KCT|
|Understand the underlying concepts and principles of quantisation||KCT|
|Understand the underlying concepts and principles of chemical thermodynamics||KCT|
|Understand the underlying concepts and principles of reaction kinetic||KCT|
|Interpret and present simple data for a range of processes and appreciate different approaches to solving practical and theoretical problems.||CT|
|Carry out a range of appropriate experiments, interpret the results and draw conclusions, communicating the outcomes in written form with a structured and coherent scientific argument.||CPT|
C - Cognitive/analytical
K - Subject knowledge
T - Transferable skills
P - Professional/Practical skills
Indicative content includes:
Black body radiation. Planck distribution. 1-D Schrodinger equation. Born. Quantization. Quantum numbers. Bohr. Wave function. Probability density. Atomic orbitals. Eigen functions. Radial wave functions. Radial distribution functions. Atomic spectra (hydrogen) and energy levels. Ionization energies and electron affinities. Aufbau. Hybridisation. Bonding and antibonding orbitals. Bond order. Duality of matter and the de Broglie hypothesis. Heisenberg uncertainty principle. Particle in a box model.
Colour of conjugated molecules. Rigid rotor and microwave spectra of diatomic molecules. Harmonic oscillator. Gas-phase IR spectra of simple diatomic molecules. Electronic excitation and the fate of excited species. Degeneracy. Vibrational motion. Singlet and triplet states. Selection rules. Multiplicity. Diatomic molecules. Electron spin. Effect of magnetic fields. Populations, intensity and widths of spectral lines.
Kinetic theory of gases. Motion of gases. Chemistry in space. ZAB collision frequency. Molecular velocity RMS velocity. Nature of kinetics. Simple and complex reactions. Reaction rates and rate constants, orders, molecularity and mechanisms. Rate laws. Differential rate equations. Integrated rate equations and half-life equations for 0, 1 and 2nd order reactions. Arrhenius and the effect of temperature on reaction rates. Experimental techniques for measurement of rate, rate constant and activation energy.
Equations of state. Ideal gas. Gas laws. Molar volume. Avogadro’s constant. Thermodynamic variables: intensive and extensive. Partial pressures. Conservation of energy. Laws of thermodynamics. ΔU. Cp. Cv. ΔH. ΔHo. Calorimetry. ΔrH, ΔrS, ΔrG, Le Chatelier’s Principle. Van’t Hoff equation. Adiabatic processes. Hess’ law. T-dependence of ΔH. Kirchoff law. Joule-Thompson effect. Chemical equilibria involving gases and solids, and in solution. Spontaneous reactions.
Methods of Teaching / Learning
The learning and teaching strategy is designed to:
present the theory and foster enquiry and consolidation through discussion,
enhance problem solving skills,
enhance practical (laboratory) skills including the ability to write scientific reports
give a comprehensive understanding of the standards required for successful completion of the module
The learning and teaching methods include:
28 hours formal lectures and 6 hours of pre-practical lectures
36 hours of practical classes
4 hours of tutorials
The assessment strategy is designed to provide students with the opportunity to demonstrate that they have successfully met the learning outcomes of the module (see above).
Thus, the summative assessment for this module consists of
Coursework (30 % of the module): Assessment of practical (experimental) skills and the ability to write scientific reports (LO2, LO3)
Coursework (10 % of the module): Written solutions to set problems (LO1, LO2)
Examination (60 % of the module): Assessing LO1 and LO2
Formative assessment is provided for all types of summative assessment mentioned above. Thus two of the six experimental sessions and the laboratory reports related to them are formatively assessed.
Formative assessment is also provided both in tutorials and also in lectures aiming to enhance the ability to solve problems, as well as the understanding of what constitutes a full and well-structured answer. Thus, the work for two of the four tutorials is formatively assessed and opportunities for problem-solving during ‘lecture-time’ allow group work and discussion.
Feedback is provided orally throughout the duration of the module in every opportunity (lecture, tutorial, practical session) including one-to-one meetings arranged on student’s request.
Feedback is provided in writing
After completion of each of the first two laboratory reports and
After completion of work set for each of the first two tutorials
Reading list for INTRODUCTION TO PHYSICAL CHEMISTRY : http://aspire.surrey.ac.uk/modules/che1036
Please note that the information detailed within this record is accurate at the time of publishing and may be subject to change. This record contains information for the most up to date version of the programme / module for the 2017/8 academic year.