Courses / Module

Toggle Print

Module GENERAL CHEMISTRY

Module code: CH101
Credits: 7.5
Semester: 1
Department: CHEMISTRY
International: Yes
Overview Overview
 

Introduction and stoichiometry; Chemistry in aqueous solutions; Atoms, molecules and the Periodic Table; Atomic structure and shapes of atomic orbitals; Bond formation, ionic and covalent bonds; Lewis structures, VSEPR theory and geometry predictions for polyatomic molecules; Physical trends in the Periodic Table.

This module covers four important areas in chemistry:
(i) Introduction to Chemistry. Elements and their physical characteristics. Introduction to Atomic Theory - physical mixtures versus chemical compounds. Covalent and Ionic bonding, the naming of chemical compounds, expression of chemical reactions. The mole concept. The chemical equation. Relative atomic mass. Stoichiometric calculation and balancing chemical equations using mole quantities. The ideal gas equation and units. Empirical and molecular formulae of compounds from elemental analysis. The determination of relative atomic mass from chemical reaction data. Solutions, concentration, molarity. Calculations using titrimetric data. Stoichiometric calculations for reactions involving solid, dissolved and gaseous reagents. (ii) Chemistry in Solution. Acid and base reactions: Lowry-Brønsted theory of acids and bases; Strong and weak acids; pH of strong and weak acids/bases; Titration curves; Indicators; Buffer Solutions; pH of salt solutions. Redox reactions: Concept of oxidation state and reactions involving a change in oxidation state.
(iii) Atoms, Molecules and the Periodic Table. The topics covered in this section are: Historical development of atomic structure; Bohr theory; Ionization potentials; Atomic quantum number; Aufbau principle; Electronic basis of the Periodic Table; Groups, periods and blocks; Basic chemistry of the elements based on the electronic structures of atoms; Electronegativities; Wave mechanical theory of the H-atom; Schrödinger''s equation (angular and radial functions, radial distribution functions); Shapes of orbitals; Pauli principle, electron spin and Hund''s rules; Simple concepts of chemical bond formation (ionic/covalent bonds); Lewis model; Valence shell electron-pair repulsion (VSEPR) theory; Orbital hybridisation and the prediction of geometries for polyatomic molecules.
(iv) Metatheses reactions and solubility rules.
(v) Physical Trends in the Periodic Table. Atomic and ionic sizes, ionisation energy, electron affinity, electronegativity; Variation in the type of compound formed across the table - some relationships between position on the periodic table and bond strength.

Open Learning Outcomes
 
Open Teaching & Learning methods
 
Open Assessment
 
Open Autumn Supplementals/Resits
 
Open Timetable
 
Back to top Powered by MDAL Framework © 2022
V5.3.3 - Powered by MDAL Framework © 2022