Metals play a vital role in the metabolism of plants and animals and, increasingly, in medicine. This book, one of two used as the main teaching material on an Open University course, provides an introduction to the metals essential to life and ligands of biological importance. It considers the uptake of metals, their transport and ultimately their storage, illustrated in particular with the story of iron in the body. It also considers Na, K and Ca ion channels and biomineralisation and covers the key roles that metals and their complexes play in living systems, for example in respiration and photosynthesis. The last section (delivered online) considers metal toxicity and deficiency and the role that metals play in medicine, looking at both diagnostics and therapy and the forefront of inorganic research.
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Eleanor Crabb is a Lecturer in Materials Chemistry at The Open University. She studied chemistry at the University of Reading where she continued to undertake a PhD in heterogeneous catalysis. She spent another 9 months at Reading as a postdoctoral research fellow before moving to the Ecole Normale Superieure de Chimie de Montpellier as a postdoctoral research fellow. In 1993, she joined The Open University and has worked on a number of science courses, producing both text based and multimedia materials. She has produced sequences introducing students to 3D molecular representations of molecules and proteins for a wide range of courses at different levels, and has produced a number of animated multimedia sequences on receptor binding. Her research interests remain in the field of heterogeneous catalysis and she is the author (or co-author) of around 20 papers in this area. She is currently seconded part-time to one of the Centres for Excellence in Teaching and Learning (CETL) awarded to The Open University. Rob Janes is a Staff Tutor at The Open University in Wales. He studied chemistry at the University of Leicester, where he remained to undertake PhD research in solid state chemistry of the silver halides. He spent one year as a visiting scientist at Eastman-Kodak, Rochester, New York, before moving to the University of Cambridge as a Post-Doctoral Research Associate, working on high-Tc superconductivity. He taught at the Manchester Metropolitan University, developing courses in inorganic chemistry, materials chemistry and imaging science. His publications record consists of around 50 papers in the field of solid-state/materials chemistry. His research interests centre on the synthetic routes to ceramics - more specifically nanosize ceramic oxides and composite oxides, inorganic pigments and phosphors and studies of the electronic and magnetic properties of solids. Elaine Moore is a Reader in Chemistry at The Open University. She studied chemistry at Oxford University, stayed on to complete a DPhil in theoretical chemistry and after a two year post-doctoral position at Southampton, she joined The Open University in 1975. She has produced OU teaching texts in chemistry and astronomy and her research interests are in theoretical chemistry applied to solid state systems and to NMR spectroscopy. She is author or co-author on over 40 papers in scientific journals. Lesley Smart is a Senior Lecturer in chemistry at The Open University. She studied chemistry at the University of Southampton where she stayed on to complete a PhD on Raman spectroscopy. She has written on many science courses and chaired the production of the second level chemistry course. Her research interests are in the areas of solid state chemistry and catalysis, and in particular, preparing and characterizing new materials and catalysts. Dr Rob Davies (Consultant Author) is Senior Lecturer at Imperial College, London. He graduated from the University of Bristol before going to St John's College Cambridge to study for his PhD. He was appointed to a three year Research Fellowship at St Catharines College Cambridge and then moved to Imperial College where he was awarded a Governors' lectureship. His research interests lie in synthetic organometallic and coordination chemistry, especially of the main group metals. Dr David Johnson (Consultant Author) is a Visiting Reader in Chemistry at The Open University. A fellow of Trinity Hall, Cambridge, he was a founding member of the Department and worked on many of the chemistry courses prior to his retirement.
Metals play a vital role in the metabolism of plants and animals and, increasingly, in medicine. The Open University has developed an undergraduate course - Metals and Life, with two books, Metals and Life and Concepts in Transition Metal Chemistry used as the main teaching material. The books and the course cover how organisms acquire metals, their transport and storage, illustrated by such diverse examples as iron in the human body, and structures such as shells and teeth. This book provides an introduction to the metals essential to life and ligands of biological importance. It considers the uptake of metals, their transport and ultimately their storage, illustrated in particular with the story of iron in the body. It also considers Na, K and Ca ion channels and biomineralisation and covers the key roles that metals and their complexes play in living systems, for example in respiration and photosynthesis. The last section (delivered online) considers metal toxicity and deficiency and the role that metals play in medicine, looking at both diagnostics and therapy and the forefront of inorganic research.
METALS AND CHEMICAL CHANGE David Johnson and Kiki Warr,
1 INTRODUCTION, 13,
2 REACTIONS OF METALS, 17,
3 METALS AND THEIR ORES, 27,
4 METALS AND THEIR EASE OF OXIDATION: A HYPOTHESIS, 37,
5 EQUILIBRIUM: A RESTATEMENT OF THE PROBLEM, 41,
6 THOMSENS HYPOTHESIS: TOWARDS A SOLUTION?, 42,
7 THE SECOND LAW OF THERMODYNAMICS: THE SOLUTION, 45,
8 THE FIRST LAW OF THERMODYNAMICS, 52,
9 ENTHALPIES OF REACTION: A DATABASE, 63,
10 ENTROPY CHANGES, 71,
11 THE GIBBS FUNCTION, 84,
12 METALS AND THEIR EASE OF OXIDATION, 91,
13 THERMODYNAMIC AND KINETIC STABILITY, 98,
14 REACTIVITY, 102,
15 THERMODYNAMICS AND THE OXIDATION OF METALS, 104,
16 ENTHALPY AND ENTROPY TERMS, 110,
17 METALS AMD THEIR ORES, 114,
18 THE BORN–HABER CYCLE, 122,
19 INTRODUCTION TO THE REMAINING SECTIONS, 128,
20 THE LATTICE ENERGY, 129,
21 ELECTROCHEMICAL CELLS AND REDOX POTENTIALS, 139,
22 IONIZATION ENERGIES OF ATOMS, 143,
23 THE CHEMISTRY OF GROUP I: THE ALKALI ELEMENTS, 148,
24 ALKALI METAL COMPOUNDS IN INDUSTRY, 154,
25 BINARY ALKALI METAL COMPOUNDS WITH NON-METALS, 160,
26 METAL IONS, LIGANDS AND COMPLEXES, 170,
27 ALKALI METAL COMPLEXES, 176,
28 THE GROUP II OR ALKALINE EARTH ELEMENTS, 184,
APPENDIX THERMODYNAMICS IN THIS BOOK, 203,
LEARNING OUTCOMES, 205,
QUESTIONS: ANSWERS AND COMMENTS, 208,
FURTHER READING, 234,
ACKNOWLEDGEMENTS, 234,
CASE STUDY: BATTERIES AND FUEL CELLS Ronald Dell and David Johnson,
1 INTRODUCTION, 237,
2 BATTERIES, 240,
3 BATTERY APPLICATIONS AND SIZES, 241,
4 CELL DISCHARGE AND CHARGE, 243,
5 BATTERY SPECIFICATION, 246,
6 DEGRADATION MODES IN BATTERIES, 255,
7 FUEL CELLS, 256,
ACKNOWLEDGEMENTS, 260,
INDEX, 261,
INTRODUCTION
In the earlier books in this series, there has been an emphasis on molecular and electronic structure — that is, on the spatial arrangement of atoms within chemical substances, and on the arrangement of electrons within atoms. Very little has been said about chemical change. But here this emphasis shifts, and we ask why chemical reactions happen. There are two conditions that must be fulfilled before a chemical reaction can occur: the equilibrium constant must be sufficiently favourable, and the rate must be sufficiently fast. This Book will be concerned with both conditions, but mainly with the first. You will meet new 'labour-saving' properties of chemical substances; these will allow us to predict whether a chemical reaction has a favourable equilibrium constant or not; the reaction does not even have to be tried out.
The units of the properties in question are mainly those of energy, and come from a branch of science called thermodynamics. To show the relevance of this subject, we shall use it to explore an important problem about the chemical behaviour of metals. Finally, when our study of this problem is complete, thermodynamics is used again, towards the end of the Book, in a systematic study of the chemistry of the alkali and alkaline earth elements — that is, of Groups I and II of the Periodic Table. Along with thermodynamics, metals are therefore a major theme in this Book, so we begin by reminding you about them, and about the way that their properties are explained by the simplest theory of metallic bonding.
1.1 Metals and their physical properties
Figure 1.1 shows a full Periodic Table, colour-coded to reveal the periodic distribution of metals, semi-metals and non-metals. Of the 114 known elements, 90 are, or are likely to be, metallic. This, and the other books in the series, concentrate on the 46 typical elements. Here, metals are not so predominant, but, even so, they still outnumber each of the other two categories.
Some metallic elements, such as bismuth and manganese, are brittle, but most, when pure, are malleable and ductile. Malleable materials are those that can be reshaped by hammering; ductile materials can be drawn out under tension into wires. Figure 1.2 shows a piece of early British gold jewellery dated 1600 BC. Such things were made by hammering out gold into sheets. This is possible because the metal is malleable, and at the same time strong.
Malleability and ductility are especially associated with those metals that possess one of the two close-packed structures discussed in The Third Dimension: Crystals.
* What are the names of these two types?
* Hexagonal close-packed and cubic close-packed.
Both close-packed structures consist of layers of atoms of the metallic element. It follows that if we can explain why such layers can slip over one another fairly easily, we can account for both malleability and ductility. Now a simple model of a metal consists of a regular array of positively charged ions in a 'pool' of freely moving electrons. The interaction between the positive ions and the negatively charged electrons, which surround the ions, holds the metal together. Let us contrast the situations in a metal and in an ionic solid, such as NaCl, when the layers are displaced relative to one another. Look first at Figure 1.3b.
* Why should such a displacement be unfavourable in an ionic solid?
* The displacement brings like charges in adjacent layers into close proximity. Repulsion between the charges will then push the layers apart.
This explains why fracture and not deformation is usually the result of beating an ionic solid. The contrast with the situation in a metal (Figure 1.3a) is obvious: all the ions are of like charge, the situation after displacement is similar to what it was before, and the freely moving electrons can adjust to the change without further disruption. Consequently, in a pure metallic crystal, layers can usually slip easily over one another, thus accounting for the properties of ductility and malleability.
You will be familiar with other properties of metals from your everyday contact with iron, aluminium, copper, silver and tin, for example. They often have a lustrous appearance, and are good conductors of heat. However, the most characteristic property of metals is their high electrical conductivity. This is explained by the free electrons that roam at random through the metallic structure. When a voltage difference is applied across two points on a piece of metal, the motion of the electrons becomes less random, there is an overall movement of electrons between the two points, and an electric current flows.
The unit of electrical conductivity is siemens per metre (Sm-1). Those elements classified as metals in Figure 1.1 have an electrical conductivity at or below room temperature of at least 3 x 105 S m-1 along any direction in a single crystal of any known form of the element. Although it is a good electrical conductor, carbon in the form of graphite does not meet this criterion. The structure of graphite is shown in Figure 1.4. It consists of sheets of carbon atoms, and each atom is bonded to three others in the same sheet. Carbon has four outer electrons in the shell structure (2, 4); in graphite, each carbon atom shares three of these with three other carbon atoms in the same sheet by forming three covalent C — C bonds. The fourth electron is mobile, just as the bonding electrons in a metal are mobile; it binds carbon atoms...
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