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 the following areas in Chemistry:

Basic concepts. Classification of matter - mixtures, units and measurements, handling numbers; Atoms molecules and ions - atomic and mass number, isotopes, molecules, formulae, naming compounds, ionic compounds, molecular compounds, polarity; Mass relationships - law of conservation of mass, average atomic mass, Avogadro’s number, molecular mass, the mole concept, empirical formula, writing chemical equations, balancing chemical equations; Stoichiometry - mole method, limiting reagents and reaction yield; concentrations of solutions, molarity; Classification of common inorganic reactions; Gases – the gas laws, ideal gas equation.

Chemistry in Solution. Acid and Base Reactions: Bronsted-Lowry 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.

Atoms, Molecules and Physical Trends in the Periodic Table. The topics covered are: Historical development of atomic structure; Bohr theory; Schrödinger equation; Shapes of orbitals; Pauli principle, electron spin and Hund's rules; Atomic quantum numbers; Aufbau principle; Electronic basis of the Periodic Table; Groups, periods and blocks; Atomic and ionic sizes, ionisation energy, electron affinity, electronegativity: Basic chemistry of the elements based on the electronic structures of atoms; Simple concepts of chemical bond formation (ionic/covalent bonds); Variation in the type of compound formed across the table - some relationships between position on the periodic table and bond strength; Lewis model; Valence shell electron-pair repulsion (VSEPR) theory.

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