Chemistry for Biosciences and Experimentation
ΒΒ0103 | ECTS: 6
Theory: 3 hours/week | Practicals: 2 hours/week
Learning Outcomes
This course provides an introduction to the fundamental principles of Chemistry, a scientific field that enables us to gain an in-depth understanding of the processes occurring in the world around us.
Upon successful completion of the course, students are expected to be able to:
- identify atomic numbers, mass numbers and isotope symbols, and convert between moles, atomic/molecular mass and number of atoms;
- relate wavelength, frequency and radiation energy, and link quantum numbers to the corresponding orbitals and electronic transitions;
- write electron configurations for atoms and ions, and construct atomic and molecular orbital diagrams;
- draw Lewis structures and use them to predict molecular geometry;
- understand and apply the concepts of internal energy, enthalpy, entropy and Gibbs free energy to predict the direction of a spontaneous chemical process;
- meet the requirements of teaching in the biosciences, a field that forms part of the professional prospects of the Department’s graduates;
- calculate the concentration of a substance in a solution or mixture, prepare solutions, use laboratory equipment, and integrate laboratory techniques.
Analytical Description of the Course
- Atomic Structure: Fundamental constituents of the atom; atomic nucleus; isotopes; Rutherford atomic model; Bohr atomic model; modern quantum-mechanical description of the atom; Schrödinger equation; quantum numbers; atomic orbitals.
- Periodic Table of the Elements: Electronic structure and properties of atoms; ionisation energy; electronegativity; atomic radius.
- Chemical Bonding: Ionic bonding; quantum-mechanical interpretation of covalent bonding; molecular orbitals; molecular geometry; VSEPR theory; molecular dipole moment; metallic bonding.
- Intermolecular Forces: London dispersion forces; dipole–dipole interactions; hydrogen bonding.
- States of Matter: Evaporation; vapour pressure; boiling and freezing points; sublimation; phase diagrams; types of crystalline solids; ionic and metallic crystals; X-ray diffraction by crystals.
- Solution Properties: Enthalpy of dissolution and solubility; solution concentrations; vapour pressure; boiling and freezing points of solutions; osmosis; colloids.
- Thermodynamics and Thermochemistry: Thermodynamic systems; extensive and intensive properties; internal energy; first law of thermodynamics; enthalpy; heat capacity; standard state; entropy; second law of thermodynamics; third law of thermodynamics; Gibbs free energy; phase equilibria; chemical potentials; chemical equilibrium; reaction quotient and equilibrium constant; Le Chatelier’s principle; van ’t Hoff equation
- Chemical Kinetics: Rate laws and reaction order; methods for determining rate laws; temperature dependence of rate constants; Arrhenius equation; transition state theory; diffusion-controlled reactions; catalysis.
- Oxidation–Reduction: Galvanic cells; standard reduction potential; Nernst equation; electrolysis; batteries.
- Environmental Chemistry: Earth’s atmosphere; human activities and the atmosphere; human activities and water quality; Green Chemistry.
- Experimental Teaching Methodology: Approaches to the teaching of laboratory experimentation, in the context of bioscience-related courses.
Laboratory Exercises
- Safety regulations in the chemistry laboratory; reagents and laboratory glassware; preparation of solutions.
- Measurement of pH.
- Buffer solutions
- chemical equilibrium.
- Introduction to chemical analysis; acid–base titration
- Spectrophotometry; construction of a calibration (standard) curve.
- Determination of chemical equilibrium constant.
- Enthalpy changes in simple chemical reactions; Hess’s law.
Student Performance Evaluation
Students are assessed in the theoretical component of the course through the end-of-semester examination, which includes multiple-choice questions, and problem-solving exercises.
Assessment in the laboratory component is based on:
a short pre-laboratory quiz (multiple-choice) prior to the conduct of each experiment; and
submission of a laboratory report after the experiment.
The laboratory report includes experimental measurements (presented in tables and graphical formats), conclusions, and identification and discussion of potential sources of error in the experimental work.
Suggested Bibliography
- General Chemistry, 1st Edition, Robinson Jill K., McMurry John Ε., Fay Robert C.
- General Chemistry, 13rd Edition, Brown T. – LeMay E. – Burste B. – Murphy C. – Woodward P. – Stoltzfus M.
- Modern General Chemistry, 10th International Edition, Darrell Ebbing, Steven Gammon
Teaching Material / E-class
Lecturers
Maria Kontou (Course Coordinator)
Anastasia Kantsadi
Persephoni Giannouli
