General Chemistry-1

Class Head: Dr. L.J. Farrugia

Course Documentation

 


Title:		Atoms, Molecules and Moles - the Chemists' Toolkit
Duration:	11 hours (lectures/workshops)
Lecturer:	Dr. Kenneth C. Campbell

Aims:	To consider the fundamental building units of matter - atoms, molecules and ions, 
and the mole concept as a convenient measuring standard.

Objectives:
Understand the classification of matter into elements, compounds and mixtures and be familiar with 
the physical states of matter.
Understand the use of chemical symbols to represent atoms, molecules and ions, and the use of 
formulae in chemical equations.
Use the concept of the MOLE as a counting unit for molecules, etc. and to apply it to determining 
relative reacting masses of substances taking part as reactants, or being formed as products in 
chemical reactions.
Know the common types of chemical reactions in aqueous solutions.
Know how to express the concentration of a solution, and be able to use numerical values of 
concentration in titrimetric analysis.
Use the ideal gas equation,  PV = nRT in calculations

Outline:	To investigate states of matter and chemical interactions in the context of chemical 
structure at a molecular level.

These topics are broadly covered in Chang, Chapters 1-5



Title:		The Elements and the Periodic Table 
Duration:	14 hours (lectures/workshops)
Lecturers:	Drs. Diane Stirling and Ronald J. Cross

Aims:		To review elements and their compounds, their occurrence and importance.  To look 
for generalisations about behaviour and properties of elements using the Periodic Table.  To discuss 
ionic and covalent bonding in compounds, and relate this to the position of the elements involved and 
to chemical reactivity.

Objectives:	
Know the names and symbols for elements of groups 1, 2, 12, 13, 14, 15, 16, 17, 
and 18, and of the first transition series (Sc-Cu):  know the names and formulae of the ions NH4+, 
NO3-, CO32-, SO42-, OH-, and CN-.

Understand the concept of oxidation levels of the elements above when in their common compounds, 
and be able to derive them.

Be able to derive the electronic configuration of the elements and the ions formed from them.

Know the basis of the periodic table in terms of electronic structures of the atoms:  be able to use the 
periodic table to rationalise or predict the properties of elements and compounds:  know which 
elements are metals, semi-metals and non-metals.

Know how ionisation energy, electron affinity, and electronegativity of elements vary across the 
periodic table.

Understand how sharing pairs of electrons can lead to single, double or triple covalent bonds between 
atoms:  that sharing electron-pairs between atoms of different electronegativity can lead to polar 
covalent bonds:  in the limiting case, transfer of electrons from one element to another can lead to 
ionic bonds.  Be able to relate the position of constituent elements of simple compounds to the type of 
bonding (ionic, covalent or metallic) encountered.

Understand how the properties and structures of compounds are dependent on the types of bonding 
involved.  Be able to derive the structures of simple covalent molecules.  Be able to write Lewis 
structures for covalent molecules.

Know the common properties of simple, binary molecules (e. g. chlorides, oxides, hydrides).

Be able to balance redox equations.

Outline:	After an initial survey of the Periodic Table, the electronic structure of atoms will be 
presented and related to each element's position. The relationship of element position to the nature 
and bonding of the compounds it forms will then be described.

These topics are broadly covered in Chang, chapters 7, 8, and 9.



Title:		Metals & their Compounds: Complexes and Corrosion
Duration: 	10 hours (Lectures & worshops)
Lecturer:	Dr. Louis J. Farrugia

Aims:	To consider the chemistry of the metallic elements, with emphasis on their 
reactivity in relation to their position in the Periodic Table, and their corrosion processes. To 
understand the concept of coordination chemistry and how it results in diverse behaviour of metal 
ions.

Objectives:
Know where metals, semi-metals and non-metals occur in the Periodic Table 

List the characteristic properties of metals and non-metals

Understand what is meant by coordination number and unit cell

Draw the structures of some metals and simple ionic compounds in terms of FCC, BCC or HCP unit 
cells.

Appreciate close packing, octahedral and tetrahedral holes

Understand the chemical processes involved in the corrosion of metals, and understand how corrosion 
can be prevented.

Write down the first row transition series elements and know their common oxidation states. Be able 
to determine the oxidation state of transition metals in their complexes.

Define coordinate bond, coordination compound complex ion, chelation compound, ligand, 
polydentate ligand, geometrical isomers. 

Understand the concepts of Lewis acids and Lewis bases as applied to metal complexes, and 
appreciate the hard/soft acid/base concept. Be able to clearly identify Lewis acids and Lewis bases 
and hard and soft acids and bases.
 
Outline:  The position of metals in the Periodic Table, and their physical and chemical properties. 
Concepts of close packing, oxidation and reduction and coordination complexes.

These topics are covered in Chang Chapters  8.6, 11.4 - 11.6,  16.8 - 16.10, 18.1 - 18.3 & 20.7






Title:		How Fast and How Far ?: Chemical Kinetics and Equilibrium

Duration:	14 hours (lectures/workshops/prelects)

Lecturer:	Drs. Malcolm Kadodwala & Ken Muir

Aims:	To consider the various factors that determine how fast and how far chemical reactions may 
go - basic kinetics and equilibrium thermodynamics, and their applications.

Objectives:
Explain in simple molecular terms why the rate of a reaction may depend on physical factors such as 
size, shape, form, and temperature of the reactants.
Write down expressions showing how the rates of chemical reactions might depend on concentrations 
of reactants, and define what is meant by a "rate constant".
Understand and use exponential/logarithmic forms of first order rate equations. Know what is meant 
by higher order kinetics, rate determining step (but equations not required.)
Describe concepts such as "reaction coordinate", "transition states", and "activation energy", and use 
the Arrhenius equation to relate rate constants to temperature.
Define catalysis and explain the various ways it might come about (surface, acid, base, enzymes).
Describe possible mechanisms of chain reactions, explosions, etc.
Explain why reactions eventually stop (reach equilibrium) and appreciate that, in the real world, most 
things have not yet reached equilibrium.
Define reaction quotient, Q, and equilibrium constant, K. Show how K follows from consideration of 
dynamic, steady-state equilibrium.
Use Q and K to predict in which direction a reaction may proceed, and what the final equilibrium 
concentrations might be.
Understand how Q and K may be expressed alternatively as "Gibbs free energy change", DG = DGO  
+ RTlnQ , and DGO  = - RTlnK.
Understand the relative roles of enthalpy (DH) and entropy (DS) of reaction in determining DG (= 
DH - T.DS), and use this to calculate effects of temperature on equilibrium.
Appreciate the connection between DG and work, and know what is meant by the first and second 
laws of thermodynamics. Explain in simple molecular terms why the rate of a reaction may depend on 
physical factors such as size, shape, form, and temperature of the reactants. 

Outline: Starting from simple molecular and everyday concepts, the various factors that control how 
fast chemical reactions may go (kinetics) and how far they may go before reaching equilibrium 
(thermodynamics) will be considered.

Covered in Chang Chapters  15, 19 & 21.




Title:		Aqueous Solutions				
Duration:	10 hours (lectures/workshops)  
Lecturer:	Dr.  J. Kelvin Tyler

Aims:	To consider the general nature of aqueous solutions of all types and to introduce 
simple quantitative ideas for some of their properties.

Objectives:
Appreciate the special nature of water as a solvent, its polarity, and its ability to 'solvate' molecules 
and ions.
Learn about hydrogen bonding and its great significance in nature.
Be able to distinguish electrolytes from non-electrolytes in aqueous solution through conductivities 
and number of particles. Understand the significance of the van't Hoff i factor.
Understand the function of membranes and the origin of osmotic pressure. Be able to do simple 
calculations with P = icRT. Appreciate the nature and stabilities of colloidal solutions in terms of 
particle sizes and charges.
Be familiar with the qualitative and simple quantitative aspects of ionic equilibria in aqueous media. 
These include concepts of acids and bases, hydrogen ion concentrations, pH and its measurement.
Also, weak acids/bases and their salts, water as an electrolyte, Ka, Kb, Kw and pKa, etc., buffer 
solutions, acid-base titration curves, the use of pH indicators. Be able to handle simple calculations of 
pH, etc. for acid/base systems.
Appreciate how the extent of protonation of species in solution varies wth pH.
Understand simple concepts relating to solubility such as, pH dependence for weak acids and bases, 
and the solubility product.

Outline:	To highlight the unique nature of water as a solvent and to consider some of the 
special properties of aqueous solutions and their general significance in nature. To introduce ideas 
relating to electrolytes in solution, membranes and osmotic pressure, colloidal solutions, acid-base 
phenomena, and the solubilities of substances in water. Simple quantitative treatments will be given 
when appropriate.

Covered in Chang , Chapters 16 & 1




Title:		Carbon Compounds-I
Duration:	14 hours (lectures/workshops)
Lecturer:	Dr. John Carnduff

Aims:	to discuss the distinctive characteristics, structures, shapes, naming, reactions, 
applications and natural occurrence of organic molecules and to interpret their reactions and bonding 
using general principles

Objectives:
Appreciate the unique ability of carbon to form elaborate molecules (many of which are found in 
living things), the nature of the covalent bond and the limitations on bond angles and lengths
Understand the importance of charge and polarity in determining properties, solubility, intermolecular 
interactions and chromatography
Draw molecules using various conventions and interpret molecular models
Understand structural isomers, geometric isomers and chirality and appreciate the importance of lone 
pairs for shape and reactivity; understand the concept of nucleophiles and electrophiles
Know the sources, uses and nomenclature of alkanes
Understand what is meant by "functional groups"; recognise functional groups and correlate these 
with names of types of compound and of single compounds
Understand the structure of alkenes, know examples of additions reactions and their use in industrial 
synthesis, understand the addition-polymerisation of alkenes and know some examples of such 
polymers
Understand the inertness and uses of polyhalogen compounds
Know examples of important alcohols and relate structures to water solubility.
Understand the oxidation and metabolism of alcohols leading to aldehydes, ketones, acids and carbon 
dioxide
Understand the structure and hydrolysis of esters and fats
Know the applications of various alcohols, esters, ketones, acids, etc. and predict products of reactions 
of alcohols, esters, ketones and acids and devise syntheses 
Appreciate the uses of phosphate and sulphate esters and understand the mode of action of detergents 
and their biodegradation

Outline:	Carbon and its compounds, natural and synthetic.  Alkanes, isomers, naming, fuels, 
lubricants, cracking.  Alkenes, polymers, unsaturated fats, addition reactions,  Halogen compounds.  
Alcohols, oxidation to acids, vinegar, esters, detergents.

Covered ( only partially) in Chang Chapter 13.





Title:		Carbon Compounds-2 Polymers & the basis of Life
Duration:	10 hours (lectures/workshops)
Lecturer(s):	Dr. David D. MacNicol

Aims:	To consider the chemistry of some more complex organic molecules and polymers 
and their uses and to illustrate how their properties depend on their structures and electron 
distributions.

Objectives:
Understand the relationship between amines and ammonia, the naming of amines and their basicity.  
Illustrate the importance of lone pairs for the hydrogen bonding, basicity and shape of amines.
Appreciate the factors involved in drug transport.  Identify imines including oximes, semicarbazones, 
etc.); understand their formation from carbonyl compounds and their importance in certain biological 
reactions.
Write the structures of several aminoacids.  Understand the formation of zwitterions and the meaning 
of 'isoelectronic point'.  Select reagents for synthesis of amides and predict the products of hydrolysis 
of amides.
Write the structures of some anaesthetics and explain how they act.
Understand the water solubility, shape, neutrality and biological role of urea.  Give experimental 
evidence for delocalisation in amides.
Appreciate the importance of chirality; draw enantiomers; identify asymmetric centres; understand the 
terms: optical resolution, racemate and racemisation.
Understand the nature and preparation of various linear and cross linked condensation polymers.  
Explain what is meant by the primary structure of proteins and identify peptide linkages and chiral 
centres.  Understand (in simple terms) how enzymes operate and explain the role of 	sidechain 
functional groups.
Draw chair conformations of a and b glucose.  Understand the formation of polysaccharides and the 
effect of stereochemistry on water solubility and biodegradability.
State clearly the experimental evidence for delocalisation of electrons in benzene.  Know that 
substitution reactions of benzenes and subsequent modifications can lead to a variety of substituted 
benzenes (e.g. -NO2, -SO3H, -NH2, -SO2NH2).  Understand the acidity and reactions of phenols.
Understand the mode of action of certain sulphonamide drugs.
Appreciate why certain organic molecules are coloured, define the term chromophore and give 
examples.  Give examples of dyes and their use.

Outline:	This part of the organic element of the course is designed to illustrate how the 
chemical functionality controls the molecular properties.  Examples range from drug transport to the 
properties of amino acids.

Covered (only partially) in Chang Chapter 14