CH1IN1-Fundamentals of Atomic Structure and the Periodic Table

Module Provider: Chemistry
Number of credits: 20 [10 ECTS credits]
Level:4
Terms in which taught: Autumn / Summer term module
Pre-requisites:
Non-modular pre-requisites: A level Chemistry, or equivalent
Co-requisites:
Modules excluded: CH1FC1 Fundamental Concepts in Chemistry 1 and CH1FC3 Molecular Studies for the Life Sciences or CH1IN4 Inorganic Chemistry for Biological Sciences
Current from: 2021/2

Module Convenor: Dr Michael Piperakis
Email: m.m.piperakis@reading.ac.uk

Type of module:

Summary module description:

Develop your understanding of the fundamental principles of inorganic chemistry through lectures, workshops and tutorials. This module will provide you with solid foundations for the remainder of the course.

Aims:
The module aims to provide the students with an understanding of the fundamental principles of Inorganic Chemistry to act as a foundation for the remainder of the course.

Assessable learning outcomes:

• Students should be able to describe fundamental principles of atomic structure, give the electronic structures of atoms and their quantum numbers.


• Students should appreciate how the electronic structure of atoms leads to the build-up of the periodic table.


• Students should be able to construct and interpret simple MO diagrams for diatomics; and determine the shapes of polyatomic molecules by applying the VSEPR rules.


• Students should have an understanding of the concept of ionic bonding and the stability and structures of ionic solids.


• Students should be able to recognise and illustrate simple solid-state structures and have an understanding of interactions in ionic solids.


• Students should understand the basic types of packing as related to atoms in metallic structures and ions in the ionic solids encountered above.


• Students should be able to display a knowledge of the chemistr y of hydrogen and the property trends across the s, p and d blocks of the Periodic Table.


• Students should understand the principles pertinent to solution chemistry including acidity and basicity as well as redox chemistry.

Additional outcomes:
Students will enhance their team working skills by various related problem solving workshops and appreciate the three dimensional nature of solid state structures by model building. Students will practise and develop their oral communication skills by contributions to small group tutorials.

Outline content:

Atomic Structure

The structure of the atom. Quantum numbers and their significance. Shapes of atomic orbitals. Radial distribution functions and penetration and shielding effect. The Pauli exclusion principle. The Aufbau principle, Hund’s rule and electron configurations. The atomic spectrum of hydrogen. Ionization energies and electronegativity.

Bonding and Shapes of Molecules

The Linear Combi nation of Atomic Orbitals (LCAO) approach. Molecular orbital formation for homo and heteronuclear diatomic molecules and for triatomic molecules. Molecular orbital energy level diagrams. The concept of bond order and bond lengths. Comparison of Molecular Orbital theory with Valence bond theory. VSEPR theory and the shapes of simple molecules. Dipole moments.

Solid-State Chemistry

Structures of the metallic elements described in terms of pa cking of metal atoms, including cubic packing and close packing. The structures of ionic solids derived from cubic and hexagonal close packing. Radius ratio rules and their use in predicting structures. The ionic model and the concept of lattice energies. The Kapustinskii equation. The use of Born-Haber cycles to calculate lattice energies.

The Periodic Table

The chemical features of different blocks of the periodic table (s/p and d block s). The chemistry of hydrogen and the s- and p-block elements, with examples taken from various groups. Trends in properties across the periodic table and within individual groups. Periodicity. Ionization potentials, electron affinities and electronegativity.

Solution Chemistry

Definition of Brønsted acids and bases. Definition of Lewis acids and bases. Pauling’s rules. The definition of pH, pKa. Electron-deficient molecules a s Lewis acids. Donor-acceptor complexes. Non-aqueous solvents. Oxidation-reduction processes and their half equations. The electrochemical series and the definition of EO. Use of EO to determine energies and equilibrium constants.

Revision of material covered in all courses in preparation for the final exam will be given in the Summer term before the examination.

Brief description of teaching and learning methods:

Over the term: 5 x 5 lecture blocks, 5 x 1 workshops, 2 x 1 tutorials. A start-of-Spring-term test to reinforce content delivered in Autumn. Five revision workshops in the Summer term prior to the Summer exam.Ìý

Contact hours:

Ìý	Autumn	Spring	Summer
Lectures	25
Seminars			5
Tutorials	2
Practicals classes and workshops	5
Guided independent study:	83		80
Ìý	Ìý	Ìý	Ìý
Total hours by term	115	0	85
Ìý	Ìý	Ìý	Ìý
Total hours for module	200

Summative Assessment Methods:

Method	Percentage
Written exam	75
Class test administered by School	25

Summative assessment- Examinations:

2.5Ìý hours

Summative assessment- Coursework and in-class tests:

Coursework and in-class tests: 1 in class open-book test which students will complete in their own time during week 1 of spring term.

Formative assessment methods:

There will be tutorials requiring completed work to be submitted and workshops in which the students carry out problem-based learning. Both are formative.

Penalties for late submission:

The Support Centres will apply the following penalties for work submitted late:

• where the piece of work is submitted after the original deadline (or any formally agreed extension to the deadline): 10% of the total marks available for that piece of work will be deducted from the mark for each working day (or part thereof) following the deadline up to a total of five working days;
• where the piece of work is submitted more than five working days after the original deadline (or any formally agreed extension to the deadline): a mark of zero will be recorded.

The University policy statement on penalties for late submission can be found at:
You are strongly advised to ensure that coursework is submitted by the relevant deadline. You should note that it is advisable to submit work in an unfinished state rather than to fail to submit any work.

Assessment requirements for a pass:
A mark of 40% overall.

Reassessment arrangements:

Reassessment arrangements are in accordance with University policy. Reassessment of the written examination is held during the University-administered re-examination period in August. Failed coursework may be re-assessed by an alternative assignment before or during the August re-examination period.

Additional Costs (specified where applicable):

1) Required text books:Ìý None

2) Specialist equipment or materials:Ìý None

3) Specialist clothing, footwear or headgear:Ìý None

4) Printing and binding:Ìý None

5) Computers and devices with a particular specification:Ìý None

6) Travel, accommodation and subsistence:Ìý None

Last updated: 30 June 2021