CHEM1602: Chemistry For Biology Students
Course Organizer: Prof A Sella (email: firstname.lastname@example.org)
Lecturers: Dr Daren Caruana, Prof P F McMillan, Dr K Holt, Prof A Sella
Normal prerequisite: A-level Chemistry or equivalent
Units: 1/2 unit
Twitter feed: #UCLChem160x
Moodle page: https://moodle.ucl.ac.uk/course/view.php?id=4979
The aim of this course is to provide students with the basic foundation in structural and physical chemistry needed to develop an understanding of biological systems at a molecular level. This course is not recommended for anyone continuing in Biochemistry, Pharmacology, and Molecular Biology as it does not include coverage of organic and bio-organic chemistry. It cannot be used as a pre-requisite for further chemistry courses.
- to understand the structure and bonding in simple molecules and the fundamental principles of biological self-assembly
- to use UV/Vis, infrared, and NMR spectroscopy to identify simple organic molecules
- to understand pH and its measurement
- to understand equilibrium and the factors which determine it (enthalpy, entropy, and the Gibbs energy)
- to understand the factors affecting reaction rate and methods by which reaction mechanisms can be investigated.
- Lectures: 25
- Tutorials: 0
- Workshops: 6
- Labs: 3 + 3 summarizing workshops.
- Exam: 60% (2 hours normally held in May)
- Lab: 20% (in lab assessment and open book online test)
- Coursework: 20% (3 online MCQ tests)
Practical course organizer:
- Dr K Holt email:email@example.com
- Burrows, Holman, et al. "Chemistry^3", Oxford University Press
- Any first year General Chemistry text. Browse around in the library where there are also custom texts "Chemistry for Biologists" used in the past for this course.
Reading for Rainy Days
- P Levi, "The Periodic Table", Abacus Books
- B Selinger, "Chemistry in the Marketplace" Harcourt Brace
- P Ball, "H2O The Biography of Water"
- P Ball, "Nature's Patterns: A Tapestry in Three Parts" Oxford UP 2009 (3 vols. Shapes, Flow, Branches)
- H McGee, "On Food and Cooking - Science and Lore of the Kitchen", Prentice Hall, 1997
The course is divided into a series of five 5-lecture blocks, each of which includes revision sections either as a separate session or embedded into the course.
There will be an Induction Lecture on the first Thursday of term at 0900 in the Chemistry Auditorium.
The course has an associated Moodle Headquarters - requires enrolment key.
A: Structure, Bonding, and Self-Assembly of Biological Structures (Holt)
- Electron configuration of atoms, Pauli principle, Hund's rule. Covalent bonding in simple molecules - principally made up of C, O, H, N, S, P - using electron-sharing arguments (Lewis structures). Single and multiple bonds, and bond order.
- Geometry of covalently bonded molecules based on valence shell electron pair repulsion (VSEPR). Orbital overlap and hybridisation models for bonding (Valence Bond Theory). Sigma and pi bonds, rationalised using diagrams for orbital overlap.
- Basic Molecular Orbital Theory, as an alternative representation of bonding in molecules. Electronegativity, and its relation to bond polarity, and ionic vs. covalent bonding.
- The role of non-covalent interactions between molecules in determining the properties of condensed-phase and biological materials. The interaction between charges, dipoles, and induced dipoles in varying combinations. How molecular liquids behave as solvents, in particular their differing polarity.
- The properties of water as nature's solvent, in particular the dissociation and hydration of ionic species in water. The hydrogen bonding within bulk water, between water and solute molecules, and within and between other molecules. The origin of hydrophobic interactions which cause the aggregation of non-polar moieties in water. Solvation of non-polar molecules.
- The concept of self-assembly, building from the non-covalent interactions studied previously. Examples to include: self-assembly of lipids into membranes, protein folding, membrane proteins, viruses, cytoskeleton, liposomes.
B: Seeing Biomolecules - Spectroscopy and Quantification (McMillan)
- The nature of light and how it interacts with molecules
- Vibrations of molecules : basic theory
- Infrared (IR) spectroscopy of organic molecules and functional groups
- UV-visible spectroscopy and electronic structure
- Atomic and molecular orbitals and energy levels : a review
- UV-vis spectra of organic molecules and species
- Nuclear Magnetic Resonance (NMR) spectroscopy : basic concepts
- Proton (1H) NMR spectra : shielding and chemical shifts
- High resolution 1H NMR spectra : coupling patterns
- Interpreting NMR spectra of organic molecules
C: Chemical Equilibrium and Chemical Thermodynamics (Sella)
This section will build fundamental thermodynamic ideas from the fundamental unit of human energy, the McVities Digestive Biscuit.
- Definition of energy, kinds of energy, units,
- Energy consumption and power output - comparisons across different organisms
- The First Law - Conservation of Energy
- Heat and Work as mechanisms of energy transfer - Temperature difference as the driver of heat.
- The Second Law - The Quality of Energy
- Spontaneous vs Irreversible change - Free Energy as a criterion.
- The idea of deltaG ATP as fundamental biological energy unit.
- Simple introduction to Boltzmann's ideas
- Excursion into energy flows. Dissipative structures or Protein Folding
D: Concentrations, pH and Equilbria (Caruana)
- Revision of acids and bases. Strong and weak acids. Multiple ionisation.
- Buffers. Buffering capacity.
- Titration curves. Indicators.
- Revision of electrochemistry. Galvanic cells.
- Standard potentials and Free Energy.
- Chemical potential and extent of reaction.
- Equilibria in Redox reactions.
- Nernst equation. Application of the Nernst equation.
- Membrane potentials.
- Reference electrodes and applications in biology.
E: The Speed of Life - Chemical and Biological Kinetics (Sella)
- Nature and scope of kinetics.
- Meaning and definition of rate of reaction.
- Factors influencing rate of reaction.
- Concept of order of reaction. Examples of reactions with simple orders. Pseudo-order reactions. Order and stoichiometry. Integrated rate equations for first and second order processes.
- Experimental methods in kinetics. Determination of reaction order and rate coefficients. Kinetics and reaction mechanism. Concepts of elementary processes and molecularity. The steady state approximation.
- Enzyme kinetics as an example of the application of the steady state approximation. The Michaelis-Menten equation for reactions involving one intermediate.
- Effect of temperature on reaction rate - the Arrhenius equation. Theories of reaction rates: collision theory and transition state theory. Catalysts.
- An excursion into biological pattern formation.