THE UNIVERSITY OF MANCHESTER School of Chemistry Programme Unit Specification Part III Chemistry Course Unit Directory 71 THE UNIVERSITY OF MANCHESTER School of Chemistry Programme Unit Specification 1. GENERAL INFORMATION Title Introductory Chemistry Unit code CM1101 Credit rating 30 credits Level Pre-requisite units Co-requisite units Member of staff responsible Prof J Christopher Whitehead 2. AIMS The programme unit aims to: To provide an introduction to the fundamental principles underlying all chemical phenomena, and establish a sound basis for the further study of all branches of Chemistry . 3. CONTENT Semester 1: Week 1 Introduction to Chemistry (Heads of the Teaching Sections) 3 lectures illustrating the place of Chemistry in the Modern World introduction to the e-learning tutorial support for this course Weeks 2-6 Foundations of Chemistry (Dr J P Day and Prof R E P Winpenny) the invention of the Periodic Table – Lavoisier to Mendeleev sub-atomic structure – Thompson to Schrödinger the quantum mechanical description of multi-electron atoms bonding and diatomic molecules common simplifications to describe bonding in polyatomic molecules Weeks 7-9 Molecular Structure, Reactivity and Functionality (Dr T W Wallace and Dr A C Regan) alkanes and cycloalkanes, conformation stereoiomerism mechanisms of reactions, electron movement and distribution curly arrows polarisation, inductive and resonance effects acidity, pKa; stability of anions haloalkanes, synthesis and uses; substitution and elimination reactions ethers, alcohols and amines alkenes, electrophilic addition; stability of carbocations alkynes; comparison with nitriles aldehydes and ketones, carboxylic acids; interconversion between alcohols, aldehydes ketones and carboxylic acids by oxidation and reduction; carboxylic acid derivatives: esters and amides Weeks 10-12 Properties of Gases. The Quantum World and Spectroscopy, Thermochemistry (Prof M W Anderson and Prof J C Whitehead, 8 lectures) the gas laws perfect gases, real gases and gas mixtures Maxwell distribution of speeds and Maxwell-Boltzmann van der Waals equation of state consequences of Schrödinger for spectroscopy absorption and emission spectra Beer-Lambert law infra-red spectra and the harmonic oscillator selection rules fluorescence, phosphorescence and lasers energy and enthalpy specific heats enthalpy changes of reactions calorimetry Hess’s Law phase changes 72 THE UNIVERSITY OF MANCHESTER School of Chemistry Programme Unit Specification 4. LEARNING OUTCOMES Category of outcome Students should/will (please delete as appropriate) be able to: Knowledge and trace the historical origin of the subject and appreciate the role played by experiment in understanding the development of chemical understanding describe an electron in an orbital for any element in terms of the four quantum numbers, n, l, m and s give the electronic configuration for any element or ions of elements in the periodic table appreciate how chemical principles apply to reactions of organic compound know the reactions of simple functional groups understand and apply the gas laws understand the meaning of the terms: heat, work energy and enthalpy understand how energy is stored by molecules understand the thermochemistry of phase transitions Intellectual skills produce molecular orbitals for homonuclear and heteronuclear diatomics of the first short period, using terms such as σ-orbitals, π-orbitals, bonding, antibonding and non- bonding orbitals derive the structures of small molecules such as valence-shell electron pair repulsion (VSEPR define: ionisation energy, electron affinity, electronegativity, covalent and ionic bonding understand the structure and reactivity of simple organic compounds in terms of functional groups distinguish between different types of spectroscopy predict the appearance of some basic spectra be able to calculate enthalpies for simple chemical processes such as reactions and combustion be able solve quantitative problems in basic chemistry, manipulating equations and applying formulae Practical skills Transferable skills and personal qualities 5. LEARNING AND TEACHING PROCESSES 6. ASSESSMENT METHOD 3 Course Tests (30%) 3 hour written examination in January (70%) 7. RECOMMENDED TEXTS C Housecroft and E Constable, Chemistry: An Introduction to Organic, Inorganic and Physical Chemistry, (3rd Ed) Prentice Hall, 2006 8. STUDY BUDGET Lectures Practicals Tutorials Self Study Revision Total Hours 48 24 12 158 58 300 73 THE UNIVERSITY OF MANCHESTER School of Chemistry Programme Unit Specification 1. GENERAL INFORMATION Title Basic Physical Chemistry Unit code CM1212 Credit rating 10 Level 1 Pre-requisite units None Co-requisite units None School responsible Chemistry Member of staff responsible Dr J J W McDouall 2. AIMS The programme unit aims to: ° Provide an introduction to the physical principles underlying all chemical phenomena. ° Lay the foundations of a knowledge and understanding of physical chemistry which will permit rapid progress to advanced topics in subsequent years of the course. ° Introduce and develop those aspects of physical chemistry related to quantum mechanical models of bonding and spectroscopy and the thermodynamic and kinetic governance of chemical processes. ° Develop practical physical chemistry skills in the associated laboratory course. 3. CONTENT Quantum Mechanics and Molecular Structure (Dr J J W McDouall, 8 Lectures) ° Introduction to Molecular Orbital Theory ° Homonuclear Diatomic Molecules ° Heteronuclear Diatomic Molecules ° Polyatomic Molecules ° Bonding in Solids ° Interaction of Molecules with Light ° Particle in a Box Model ° Harmonic Oscillator Model ° Rigid Rotor Model Thermodynamics (Dr S L M Schroeder, 8 Lectures) ° Recapitulation of the 1st Law and of Thermochemistry ° The 2nd Law: Entropy and Spontaneous Processes ° The 2nd Law: The Gibbs Energy (Free Enthalpy) ° The Chemical Potential ° Electrochemical Potentials: The Nernst Equation ° Introductory Thermodynamics of Mixtures ° Thermodynamic Description of Chemical Equilibria, with Examples Kinetics (Dr R H Henchman, 8 Lectures) ° The Nature of Transformations in Chemistry. ° Reaction Rates. Reaction Order, Rate Laws, Activation Energy, Collision Theory. ° Reaction Mechanisms. Molecularity, Energy Profile, Reaction Coordinate, Transition State. ° Measurement And Prediction. Spectroscopic Detection, Transition State Theory. ° Catalysis. Enzymes, Inhibitors. 4. LEARNING OUTCOMES Category of outcome Students should be able to: Knowledge and understanding ° Discuss the electronic structure of small molecules using the principles of molecular orbital theory. ° Discuss the physical origins and quantum mechanical models of UV/Vis, infrared and microwave spectroscopies. ° Discuss thermodynamic state functions and their influence and control of chemical processes. ° Discuss the notions of rate laws, rate constants, reaction order, molecularity and the Arrhenius equation in chemical kinetics. Intellectual skills ° Understand physical principles underlying most chemical phenomena. 74 THE UNIVERSITY OF MANCHESTER School of Chemistry Programme Unit Specification ° Handle mathematical models of the physical world. ° Understand and manipulate units. Practical skills ° The use of laboratory equipment pertinent to physical chemistry experiments. ° The analysis of experimentally derived data and the treatment of errors. Transferable skills and personal qualities ° Analytical skills ° Problem identification 5. LEARNING AND TEACHING PROCESSES 24 lectures 12 week laboratory course (1 day per week) Recommended Texts: (i) P W Atkins and J de Paula, The Elements of Physical Chemistry, 4th Edition, 2005, Oxford University Press. (ii) C E Housecroft and E C Constable, Chemistry, 2nd Edition, 2002, Pearson 6. ASSESSMENT Assessment task Length Weighting within unit (if relevant) Written examination in May/June 1 hour 45 minutes 100% Date of current version 25/5/2005 75 THE UNIVERSITY OF MANCHESTER School of Chemistry Programme Unit Specification 1. GENERAL INFORMATION Title Basic Inorganic Chemistry Unit code CM1312 Credit rating 10 Level 1 Pre-requisite units None Co-requisite units None Member of staff responsible Dr. Stephen Godfrey 2. AIMS The programme unit aims to: Build a solid knowledge base in all fundamental areas of basic inorganic chemistry across the periodic table. Aspects of nuclear chemistry, transition metal chemistry, solution chemistry, redox chemistry and main-group chemistry (the s- and p-block elements). Highlight the importance of many of these materials in industrial and/or biological systems. 3. CONTENT Nuclear Chemistry (Dr. Francis Livens 4 lectures) The chart of the nuclides, the atomic nucleus Radioactive decay Binding energies and the model of the atomic nucleus Solution Chemistry (Dr. Francis Mair 4 lectures) Metal ions in solution, Lewis acids and bases, speciation. Equilibrium Constants and enthalpy and entropy effects Hard/Soft concepts and stability effects. Transition Metal Chemistry (Dr. Sarah Heath 8 lectures) Electronic Configurations and oxidation states Ligands and donor atoms, coordination numbers. Formulae and nomenclature, isomerism d-configurations, spin states, d-orbital shape and symmetry. Crystal Field Theory, octahedral/tetrahedral/square planar geometries Jahn-Teller distortion and redox chemistry. Main-Group Chemistry (Dr. Stephen Godfrey 8 lectures) Isolation of the elements from their compounds. The reactivity of s-and p-block with common reagents Structures adopted