Introductory Chemistry

CHEM10101 Introductory Chemistry 30 Semester 1 Undergraduate Level 1 Alan Brisdon Unit coordinator Department of Chemistry 1 FHEQ level (Framework for Higher Education Qualifications) ' First part HE study/Bachelors ' European Credit Transfer & Accumulation System Rating : 15.0 <div>Week 1: Introduction to Chemistry at ManchesterDr A K Brisdon and Dr F Mair<ul><li>To encourage reflection on prior learning and to aggregate existing knowledge.</li><li>To provide an introduction to the ethos of university-level learning and teaching.</li></ul>Weeks 2-5Dr A K Brisdon and Dr F Mair<ul><li>Atomic orbitals and simple wavefunctions</li><li>Introduction to molecular orbitals</li><li>Valence bond approaches to molecular structure</li><li>Application of MO and VB theory</li></ul>The module then splits into two streams: “Shape and Reactivity” and “States of Matter”Shape and ReactivityWeeks 7-11Dr C. Poree<ul><li>Molecular shape</li><li>Stereoisomerism</li><li>Fundamentals of chemical reactivity</li></ul>States of MatterWeeks 7-12Prof. M. Anderson<ul><li>Interatomic and intermolecular forces</li><li>Gases and liquids</li><li>Solids</li></ul></div> <div>Week 1: Introduction to Chemistry at Manchester/Reflection on Prior Learning(i) To encourage students to review and reflect on prior learning and to aggregate their existing knowledge;(ii) To break the ice and introduce students to the ethos of university-level learning and teaching.Weeks 2-5 (Dr Alan Brisdon)<ul><li>Atomic orbitals and simple wavefunctions</li><li>Rydberg equation and H spectrum</li><li>Atomic orbitals in pictures; quantum numbers (n, l, ml)</li><li>Basic QM approach to wavefunctions: radial and angular terms</li><li>Many electron systems</li><li>IE, Zeff, electronegativity in multi-electron systems.</li><li>Effective nuclear charge, Slater’s rules</li><li>Pauling electronegativities</li><li>Introduction to symmetry</li></ul>Molecular Orbitals<ul><li>Molecular orbital energy diagrams for homonuclear diatomic molecules and ions.</li><li>Molecular orbital energy diagrams for heteronuclear diatomic molecules and ions.</li><li>Use of SALCs for polyatomic molecules.</li></ul>Approaches to molecular structure<ul><li>Lewis structures</li><li>Hybridisation</li><li>MO/hybridisation approach to tetrahedral and square planar molecules.</li><li>Comparisons between the different models available</li></ul>Application to examples<ul><li>Orbitals of methane and XeF4 from SALC of AOs.</li><li>Metallic bonding</li><li>Reviewing electrophilic addition to an alkene using orbital considerations.</li></ul>Weeks 7-11 Shape and Reactivity (Dr C. Poree)Basic molecular shape<ul><li>Skeletal formula (rings and chains, alkanes/alkenes)</li><li>Conformational analysis in linear alkanes, cyclohexane (staggered and eclipsed bonds)</li><li>Sigma and pi bonds in organic compounds and metal complexes</li><li>Resonance/delocalisation</li><li>Inductive effects</li><li>Hyperconjugation</li></ul>Stereochemistry<ul><li>Stereoisomerism in molecules and complexes</li><li>Structural isomerism in compounds and complexes</li><li>Geometric isomerism (cis and trans, E and Z)</li><li>Optical isomerism (Absolute and relative stereochemistry, enantiomers and diastereomers, with examples drawn from prior content)</li><li>Molecular symmetry.</li></ul>Fundamentals of Reactivity<ul><li>Why do reactions happen?</li><li>Electrostatics and orbitals</li><li>Orbital description of reactivity</li><li>Curly arrow formalism - electron movement and distribution</li><li>Electrophiles and Nucleophiles</li><li>Acids and bases: pKa</li></ul>Examples:<ul><li>SN1 and SN2 – simple stereoelectronic representation, fates of reactive intermediates</li><li>Nucleophilic addition and substitution at C=O</li></ul>Weeks 7-12 States of Matter (Prof.M.Anderson)Interatomic and Intermolecular Forces<ul><li>Electric dipole moments,</li><li>Electrostatic interactions, short range repulsion  and the Lennard-Jones potential</li><li>Dispersion</li><li>Induction interactions and polarisability</li><li>Polarity</li><li>Hydrogen bonding, hydrophobic interaction</li><li>Potential energy surfaces (PES) for intermolecular forces</li><li>Determining state of matter</li></ul>Gases and Liquids<ul><li>Recap of perfect gas equation of state</li><li>Non-ideal behaviour – van der Waals equation of state</li><li>Kinetic theory of gases: collision frequency, diffusion and effusion</li><li>Maxwell-Boltzmann distribution of molecular speeds</li><li>Kinetic energy versus PE as a function of temperature: formation of liquids and solids</li><li>Simple phase diagram for gas/liquid/solid</li><li>The triple-point: sublimation and supercriticality</li><li>Development of Clausius-Clapeyron equation</li></ul>Solids<ul><li>Packing in solid state structures: crystal systems and Bravais lattices, unit cells for fcc, bcc and diamond.</li><li>Polymorphism</li><li>Packing efficiency</li><li>Lattice enthalpy and Madelung constants.</li><li>Octahedral and tetrahedral holes interstitial sites in close-packed structures.</li><li>Structures of simple compounds – rocksalt, zincblende.</li></ul></div><p style="-webkit-text-stroke-width:0px;color:rgb(60, 60, 60);font-family:Arial,sans-serif;font-size:12px;font-variant:normal;letter-spacing:normal;orphans:2;text-align:left;text-indent:0px;text-transform:none;white-space:normal;word-spacing:0px;">   <div> To provide an introduction to the fundamental principles underlying all chemical phenomena, to engage prior knowledge and understanding, to introduce new concepts and establish a sound basis for further units of study.This unit will include aspects of structure, bonding, molecular shape and reactivity, the distribution of energy in microscopic and macroscopic terms, and an introduction to the important physical parameters which describe the states of matter (solid, liquid and gaseous phases).</div>  On successful completion of the course students should be able to:Predict the shape, structure and bonding of small molecules, complexes and compounds based on orbitals and electron density. Interpret the states of different kinds of matter based on the consideration of the molecular or atomic structure of the constituents and simple interatomic and intermolecular interaction potentials between the constituent species  <div> The following transferable skills will need to be used by students in order to complete this unit successfully: <ul> <li> Problem solving – the application of problem solving skills to analyse given data, propose solutions to authentic chemical problems and draw appropriate conclusions.</li> <li> Communication skills – the ability to effectively and concisely convey answers using the appropriate chemical terminology/technical language, through discussion with peers, oral presentations and written work.</li> <li> Teamworking skills – Through discussion of authentic chemical problems in workshops, tutorials and PASS sessions.</li> <li> Numeracy and mathematical skills – the ability to handle and manipulate data using simple algebra, functions and calculus, the ability to correctly handle and convert data in different scientific units;</li> <li> Investigative Skills – to be able to read and extract key information from scholarly texts, given information and the internet, and to be able to assess/critique the quality of the information sourced.</li> <li> Analytical skills – the ability to interpret and critically evaluate data (and information).</li> <li> Time management/organisational skills – the development of an ability to work to schedules and meet deadlines by working efficiently and effectively.</li> </ul></div>  1 Written exam 100% GeneralThe course is delivered in a way which allows students to regularly receive feedback on their work through a variety of teaching activities. This is achieved through i) a significant amount of content being delivered as worked problems in lecture, and ii) through regular workshops each week of the course and during tutorials. These sessions allow for provision of formative feedback through material which is designed to help guide students in their own conceptualization and approach to solving problems.WorkshopsWorkshops offer opportunities for both facilitator and peer feedback by:Providing opportunities for students to work with and master concepts introduced in lectures, and apply these concepts to unseen material.Encouraging development of thinking skills (with a focus on critical thinking, analysis, evaluation and application, rather than simple reproduction of knowledge/process)Providing opportunities for teamwork and collaboration (and the development of skills associated with this) and including time for students to reflect upon their own learning.TutorialsWeekly tutorials in Semester 1 provide opportunities for more personalised tutor feedback on submitted work and topics discussed and for informal peer feedback in a collaborative, small-group environment.E-learningCHEM10101 is supported by a set of weekly online quizzes which provide an opportunity for students to evaluate their own progress during the module. CHEM10520 Co-Requisite Compulsory CHEM10600 Practical Chemistry Co-Requisite Compulsory A-level Chemistry or equivalent qualification.Basic numeracy and literacy (to GCSE or equivalent) standard.Basic laboratory experience, including an awareness of units and errors. BSc(Hons) Chemistry BSc(Hons) Chemistry First Year Mandatory N J. Keeler and P. Wothers, Chemical Structure and Reactivity: An Integrated Approach (2nd edition), OUP, Oxford, 2013 (ISBN 978-0199604135).P. Atkins and J. de Paula, Atkins’ Physical Chemistry (10th edition), OUP, Oxford, 2014 (ISBN 978-0199697403).J. Clayden, N. Greeves and S. Warren, Organic Chemistry (2nd edition), OUP, Oxford, 2012 (ISBN 978-0199270293).C. Housecroft and A. G. Sharpe, Inorganic Chemistry (4th edition), Pearson, 2012 (ISBN 978-0273742753)  Assessment written exam 2 Lectures 200 Practical classes & workshops 90 Tutorials 10 0 0