Chemistry | FP015Module SummaryWith an emphasis on the development of students’ scientific skills, this module will focus on competences such as evidence based reasoning, the application of quantitative analysis to interpret chemical data and the evaluation of experimental design. Chemistry is an evidence based science discipline and there will be a strong experimental element to this module. In this progressive module students will also look at how Chemical applications can be used to solve societal problems. Students undertaking this module will develop the academic experience required for a range of undergraduate science programmes, including chemistry and chemical engineering.

Module ObjectivesThe Module will:1. Develop the students’ understanding of

chemistry concepts and processes such that they become confident in their use and application

2. Develop the students’ ability to reason logically and recognise incorrect reasoning, to become aware of the way ideas develop and evolve in chemistry

3. Develop the students’ ability to link chemistry concepts to real-world scenarios and appraise how they can be used to solve problems

4. Develop an awareness of the relevance of chemistry to other fields of study, particularly the natural sciences and engineering, and to be able to communicate effectively

Learning OutcomesBy the end of the module, students will have:1. Construct and present arguments through

appropriate use of logical deduction physical principles and experimentation

2. Use chemistry principles in the analysis and solution of real world problems in the sciences and engineering

3. Exhibit a range of key competences including time management, team-work, communication skills and presentation skills, research skills (including information retrieval, interpretation and citation) and critical analysis

Assessment Methods

Verbal presentation 20%

Practical assessment 15%

Practical assessment 15%

Two hour examination 50%

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Course ContentCourse Content

Part 1: Atomic Structure Protons, neutrons and electrons, location in atom

and relative charge Electrons in shells + successive ionisation

energies up to Z = 36 in terms of levels and sub-levels (orbitals) s, p and d

Electron configurations using electrons in shells and spd notation.

Relative atomic/molecular and isotopic mass. The principles of a simple mass spectrometer,

limited to ionisation, acceleration, deflection and detection

Interpret simple mass spectra of elements and calculate relative atomic mass from isotopic abundance, limited to mononuclear ions

How do ionisation energies in Period 3(Na – Ar) and in Group 2 (Be – Ba) give evidence for electron arrangement in sub-levels and in levels?

Part 2: Chemical Bonds The ionic bond, Dot/cross diagrams The covalent bond to include dative bond Shapes of simple molecules, to include

biologically important molecules Polar bonds Polar molecules

Part 3: Formulae, balanced equations and mole amounts Balanced equationsMole quantities and Avogadro’s numberMole to mass conversionsMoles in solution Reacting mass calculations Empirical formulaMolecular formulae

The relationship between, empirical and molecular formulae

The ideal gas equation Structural formulae to include skeletal formulae

Part 4: Redox equations Oxidation and reduction in terms of electron

transfer Oxidising and reducing agents Balancing half and redox equations

Part 5: Intermediate forces Permanent dipole attractions London forces Hydrogen bonds

Part 6: Equilibria Dynamic equilibria Factors affecting equilibrium composition Le Chatelier’ s Principle

Part 7: Kinetics Collision theory for reactions Factors affecting rates of reaction Enzymes as catalysts Competitive and non-competitive inhibitionMichaelis-Menten constant Effect of temperature, pH and heavy metal ions

of activity Enzymes in biotechnology

Part 8: Energetics Exothermic and endothermic changes Calculations to determine enthalpy of reaction

using (mean) bond energies Using Hess’s Law to perform simple calculations

Chemistry | FP015

Find out more at:Warwick.ac.uk/ifp ifp@warwick.ac.uk facebook.com/warwickifp @warwickifp

Course Content

Part 9: Rates Use the rate equations of the form Rate = k[A]

m [B]n where m and n are the orders of reaction with respect to reactants A and B

Derive the rate equation for a reaction from data relating initial rate to the concentrations of the different reactants

The effect of changes in temperature on the rate constant k

The rate determining/limiting step of a reaction

Part 10: Thermodynamics Define and apply the terms enthalpy of

formation, ionisation enthalpy, enthalpy of atomisation of an element and of a compound, bond dissociation enthalpy, electron affinity, lattice enthalpy

The effect of temperature on the position of equilibrium from the sign of DH for the forward reaction

The balance between entropy and enthalpy and the feasibility of a reaction; ∆G = ∆H – T∆S

Determine how ∆G varies with temperature Determine the temperature at which a reaction

is feasible

Part 11: Organic Chemistry Systematic naming limited to alkanes, alkenes,

alcohols, aldehydes, ketones, Carboxylic acids and amine Functional groups and tests to identify functional

groups within a molecule Isomerism to include structural, geometrical

(+ E/Z) optical Combinatorial Chemistry in drug designMechanisms to include addition reactions

Part 12: Acids, Bases and Buffers Bronsted-Lowry definitions Conjugate acid-base pairs Calculating Ka and pKa pH, calculations and indicators Buffers especially as applied to

biological systems

Part 13: Spectroscopy The production of infrared spectra Use infrared spectra to identify particular

functional groups and to identify impurities Identify the difference between 13C and 1H

spectra Be able to use the n +1 rule to deduce the

spin–spin splitting patterns of adjacent, non-equivalent protons, limited to doublet, triplet and quartet formation in simple aliphatic compounds

Use NMR 1H spectra to provide information about the structure of a compound

Identify the limitations of Infrared spectra