CH1401 – Introductory Inorganic and Physical Chemistry
Lecturers:
Dr P. Kilian, Professor R. E. Morris, Dr D. G. Pinto and Dr R. M. Smith.
Module Convenor: Dr R. T. Baker
Aims:
To provide, via lectures, tutorials and coursework assignments, a firm foundation for the further study of Inorganic and Physical Chemistry, developed using both descriptive and quantitative approaches.
Nuclear and Electronic Structure, Atoms and the Periodic Table – Professor R. E. Morris
Duration:
12 hours
Aims:
To understand the structure of atoms.
To give elementary descriptions of the electronic structure of atoms leading to an understanding of the structure of the Periodic Table of the elements; of the properties of atoms and ions; and of the properties of simple ionic solids and of molecular compounds. To lay foundations of MO theory. To discuss the processes that have led to the range of elements that we see in the Universe and on Earth today.
Objectives:
1. To revise basic aspects of atomic structure and to understand the concept of electrons as waves.
2. To know of the basic nuclear reactions.
3. To know of the Big Bang synthesis of the lighter elements.
4. To understand concepts surrounding atomic structure and quantisation.
5. To know the allowed values of the quantum numbers n, l, m and s for multi-electron atoms, and to relate n, l and m to the shapes and multiplicities of atomic orbitals.
6. To know the relative energies of atomic orbitals and their filling order, and so to be able to derive, and write down, electronic configurations for atoms up to Kr.
7. To know and understand the structure of the Periodic Table in terms of the filling of atomic orbitals.
8. To understand the concept of electrons as waves and how it applies to atomic orbitals (including phases and nodes).
9. To begin to appreciate the way atomic orbitals can be combined to give molecular orbitals in simple diatomic systems.
10. To understand the notation associated with MO theory
Nuclear and Electronic Structure, Atoms and the Periodic Table – Professor R. E. Morris
Duration:
12 hours
Aims:
To understand the structure of atoms.
To give elementary descriptions of the electronic structure of atoms leading to an understanding of the structure of the Periodic Table of the elements; of the properties of atoms and ions; and of the properties of simple ionic solids and of molecular compounds. To lay foundations of MO theory. To discuss the processes that have led to the range of elements that we see in the Universe and on Earth today.
Objectives:
1. To revise basic aspects of atomic structure and to understand the concept of electrons as waves.
2. To know of the basic nuclear reactions.
3. To know of the Big Bang synthesis of the lighter elements.
4. To understand concepts surrounding atomic structure and quantisation.
5. To know the allowed values of the quantum numbers n, l, m and s for multi-electron atoms, and to relate n, l and m to the shapes and multiplicities of atomic orbitals.
6. To know the relative energies of atomic orbitals and their filling order, and so to be able to derive, and write down, electronic configurations for atoms up to Kr.
7. To know and understand the structure of the Periodic Table in terms of the filling of atomic orbitals.
8. To understand the concept of electrons as waves and how it applies to atomic orbitals (including phases and nodes).
9. To begin to appreciate the way atomic orbitals can be combined to give molecular orbitals in simple diatomic systems.
10. To understand the notation associated with MO theory
Thermodynamics – Dr D. G. Pinto
Duration:
8 hours
Aims:
Discuss Units and temperature. Cover Ideal Gas Law. Introduce the basic concepts of thermodynamics and three of the most important terms enthalpy, entropy and Gibbs energy. These will be used to predict whether a chemical reaction will occur or not under given conditions and to determine the position of chemical equilibrium for reactions which do not proceed to completion.
Objectives:
1. Discuss units, temperature and the Ideal Gas Law, PV = nRT.
2. To introduce the basic terms and concepts used in thermodynamics – e.g., energy, heat and work.
3. To introduce the first law of thermodynamics, the internal energy (U) and the enthalpy (H).
4. Define the standard state.
5. Use Hess’s Law to calculate changes in enthalpy (ΔH) for phase transition and chemical reactions. To define and use the standard enthalpy of formation (ΔfH).
6. To introduce the second law of thermodynamics. To define the concepts of disorder, entropy (S) and spontaneous changes and explain their relevance to chemical systems.
7. Define Gibbs energy (G) and its relationship to enthalpy and entropy.
8. Define ΔG and its relationship to ΔG0 and K (equilibrium constant).
Chemical Kinetics – Dr D. G. Pinto
Duration:
4 hours
Aims:
Introduce Chemical Kinetics as the Rate at which a thermodynamically favourable reaction can occur and equilibrium achieved.
Objectives:
1. Define units of rate and how rate can be measured.
2. To discuss the rate law as the dependence of rate upon reactant concentration.
3. Via the rate law, introduce the concepts of order of reaction.
4. To treat first order processes mathematically.
5. To analyse the temperature dependence of rate in terms of the Arrhenius equation, activation energy and pre-exponential factor.
6. To discuss briefly theories of rate processes.
Mathematical Tools for CH1401 – Dr R. M. Smith
Duration:
3 hours
Aims:
To revise and/or introduce the mathematical concepts encountered in CH1401 only.
Objectives:
For chemical applications, students should be able to understand and use:
1.1 Numbers, rounding, significant figures, decimal places, operators & BODMAS
1.2 Algebra, indices, roots or powers, infinity and magnitude
1.3 Units or quantity calculus, SI base units, scientific and prefix notation
2.1 Clear workings for calculations
2.2 Polynomials
2.3 Plot a graph with linear fit
2.4 Differentiation basics
2.5 Integration basics
3.1 Utilise properties of exponentials and logarithms
Properties of Solutions – Dr R. M. Smith
Duration:
6 hours
Aims:
To introduce the concept of chemical equilibrium and investigate the behaviour of different solution equilibrium systems, including acid- base and redox equilibria. To apply concepts of chemical equilibrium to real-world applications.
Objectives:
Students should have an understanding of the following:
1. Chemical equilibrium – Response of equilibrium to change. The equilibrium constant. The concept of activity.
2. Solubility – including the behaviour of ionic solutes in solution and equilibrium constant expressions such as Ksp, Kw.
3. Acids and bases – Arrhenius, Brønsted-Lowry, Lewis, strong, weak and conjugate acids/bases. Acid dissociation constant Ka and base association constant Kb. Interpreting acid-base titration data. Predicting the pH of salt and buffer solutions. Characteristic components of buffer solutions including some physiological buffers. Interpreting acid-base titration data.
4. Introductory electrochemistry – Describing electrochemical cells using oxidation/reduction half cells and using schematic representations. Difference between galvanic and electrolytic cells. The importance of reference half cells especially standard hydrogen electrode in generating standard reduction potentials. From standard reduction potential, determining cell potentials and hence predicting the spontaneity and feasibility of redox reactions.
Shapes and Properties of Molecules / Chemistry of the Elements – Dr P. Kilian
Duration:
12 hours
Aims:
To gain understanding how electronic structure of atoms affects the physical properties and reactivity of elements and simple compounds. To appreciate the differences in chemistries of main group elements from various Groups of the Periodic Table.
Objectives:
1. To understand how periodic trends in electronegativity and ionization energy determine nature of the bonding (metallic, covalent) in the solid state.
2. To understand how periodic trends in electronegativity and ionization energy determine nature (ionic, covalent) of binary compounds.
3. To understand and be able to determine oxidation numbers in compounds. To understand the concept of oxidation and reduction.
4. To know common oxidation states across the s- and p-block. To be able to predict which hydrides, oxides and halides exist.
5. To understand and know limitations of the octet rule. To know and understand how size of the central atom determines maximum coordination number in simple molecules.
6. To draw Lewis structures for simple covalent molecules and ions, and to understand and apply the VSEPR method for the prediction of molecular shape.
7. To know some main group descriptive chemistry of alkali metals, halides, oxides and hydrides. To know chemical transformations and processes involved in the manufacture of selected industrially important inorganic compounds.
Introductory Inorganic and Physical Chemistry (Laboratory)
Duration:
12 hours
Aims:
The laboratory class consists of a series of experiments designed to be completed in one session. Post-laboratory assessments will focus on notable features of each task. The course is designed to illustrate and reinforce concepts related to basic analytical techniques and observational skills. The skills acquired will be valuable for all students who advance to CH1601 and level 2000 laboratory courses.
Objectives:
To perform four experiments that are intended as an introduction to basic observation skills and analytical techniques. Aspects of “Good Laboratory Practice” (GLP) and safety and chemical calculations relevant to laboratory work will be covered in self- study exercises.
Introduction to analytical techniques:
1. Separation and solubility exercise
2. Acid-base titrations with a selection of indicators 3. Analysis of group 2 carbonates
4. Introduction to chromatography