Catch Up Chemistry : For the life and medical sciences / Mitch Fry and Elizabeth Page.

By:

Fry, Mitch

Contributor(s):

Page, Elizabeth

Material type: Text

TextPublication details: Bloxham, Oxfordshire : Scion Publishing Ltd., c.2005.Description: x, 190 p. : ill. ; 24 cmISBN:

9781904842101 (pbk.)

Other title:

Chemistry : for the life and medical sciences

Subject(s):

DDC classification:

540 FRY

Holdings
Item type	Current library	Call number	Copy number	Status	Date due	Barcode
Standard Loan	Moylish Library Main Collection	540 FRY (Browse shelf(Opens below))	1	Available		39002100331702

Enhanced descriptions from Syndetics:

Many students now begin life and medical science degrees with far less knowledge of chemistry than they need - and they struggle as a result. "Catch Up Chemistry" brings students up to speed with the subject quickly and easily. The book puts the essential chemistry into real biological context and is written in an extremely student-friendly manner: the text is concise and to the point; the equations are clearly laid out and explained.
Key Features: Provides all the core chemistry required for a medical sciences degree
Numerous examples to demonstrate the relevance to biology and medicine
Test Yourself questions at the end of each chapter to help the reader practise what they have learned
Student-friendly format and price
"

Includes index.

Table of contents provided by Syndetics

Preface (p. ix)
About the authors (p. x)
1 Elements, atoms and electrons (p. 1)
1.1 Isotopes (p. 2)
1.2 Electrons (p. 3)
1.3 Summing up (p. 8)
1.4 Test yourself (p. 8)
Taking it further: Isotopes in biology (p. 9)
Taking it further: The periodic table (p. 13)
2 Bonding, electrons and molecules (p. 19)
2.1 What is a covalent bond? (p. 19)
2.2 Non-bonding electrons - lone pairs (p. 21)
2.3 Pi molecular orbitals (p. 22)
2.4 Coordinate bonds (p. 23)
2.5 Electronegativity and polar covalent bonds (p. 24)
2.6 What effect does electronegativity have on covalent bonds? (p. 25)
2.7 Ionic bonds (p. 26)
2.8 The concept of the chemical bond (p. 27)
2.9 Summing up (p. 27)
2.10 Test yourself (p. 28)
Taking it further: The peptide bond (p. 28)
3 Interactions between molecules (p. 35)
3.1 Hydrogen bonding (p. 35)
3.2 Charge-charge interactions (p. 38)
3.3 Short range charge-charge interactions (p. 39)
3.4 Hydrophobic interactions (p. 40)
3.5 Summing up (p. 41)
3.6 Test yourself (p. 41)
Taking it further: Solubility in water (p. 42)
4 Counting molecules (p. 49)
4.1 Moles (p. 49)
4.2 Molecular mass (p. 51)
4.3 Moles and molarity (p. 51)
4.4 A note on units (p. 53)
4.5 Dilutions (p. 54)
4.6 Percent composition solutions (p. 54)
4.7 Summing up (p. 55)
4.8 Test yourself (p. 56)
Taking it further: Confidence with moles (p. 57)
5 Carbon - the basis of biological life (p. 61)
5.1 The electronic structure of carbon (p. 61)
5.2 Hybridisation (p. 62)
5.3 The tetravalency of carbon (p. 63)
5.4 Shapes of molecules (p. 64)
5.5 Carbon in chains and rings - delocalisation of electrons (p. 65)
5.6 Aromaticity (p. 68)
5.7 Summing up (p. 69)
5.8 Test yourself (p. 69)
Taking it further: Carbon structures (p. 69)
6 The same molecule but a different shape (p. 73)
6.1 Isomers (p. 73)
6.2 Optical isomerism (p. 73)
6.3 Geometric isomerism (p. 77)
6.4 Isomers as a problem (p. 79)
6.5 Summing up (p. 80)
6.6 Test yourself (p. 81)
7 Water - the solvent of life (p. 83)
7.1 Bonding in the water molecule (p. 84)
7.2 The dissociation (auto-ionisation) of water (p. 85)
7.3 Acids and bases (p. 86)
7.4 Using pH as a measure of acidity (p. 87)
7.5 Calculating the pH of water (p. 88)
7.6 The dissociation of weak acids and weak bases in water (p. 89)
7.7 Buffers and buffered solutions (p. 90)
7.8 Calculating the pH of buffer systems using the Henderson-Hasselbach equation (p. 91)
7.9 Life in water (p. 92)
7.10 Amino acids (p. 94)
7.11 Controlling cellular pH (p. 95)
7.12 Summing up (p. 96)
7.13 Test yourself (p. 97)
Taking it further: Biological buffers (p. 97)
8 Reacting molecules and energy (p. 101)
8.1 Energy from molecules (p. 101)
8.2 Getting molecules to react (p. 103)
8.3 Energy, heat and work: some basic terms of thermodynamics (p. 104)
8.4 Enthalpy (p. 105)
8.5 Entropy (p. 106)
8.6 Gibbs free energy and work (p. 106)
8.7 Energy changes in biological reactions (p. 108)
8.8 Summing up (p. 109)
8.9 Test yourself (p. 110)
Taking it further: Free energy and metabolic pathways (p. 111)
9 Reacting molecules and kinetics (p. 117)
9.1 Rate equations (p. 118)
9.2 Reaction routes or mechanisms (p. 120)
9.3 The rate-limiting step (p. 120)
9.4 Considering the activation energy (p. 120)
9.5 Equilibrium (p. 121)
9.6 The equilibrium position can change (p. 124)
9.7 Free energy and equilibrium (p. 125)
9.8 Free energy change is zero at equilibrium (p. 126)
9.9 Summing up (p. 126)
9.10 Test yourself (p. 127)
10 Energy and life (p. 129)
10.1 Oxidation and reduction (p. 129)
10.2 Half-reactions (p. 130)
10.3 Redox potential (p. 132)
10.4 Free energy and redox potentials (p. 134)
10.5 Obtaining energy for life (p. 134)
10.6 What happens to this free energy? (p. 136)
10.7 Summing up (p. 137)
10.8 Test yourself (p. 138)
Taking it further: Further oxidation (p. 138)
11 Reactivity of biological molecules (p. 141)
11.1 Addition reactions (p. 142)
11.2 Substitution reactions (p. 143)
11.3 Elimination reactions (p. 143)
11.4 Free radical reactions (p. 144)
11.5 Pi bonds and addition reactions (p. 145)
11.6 Functional groups link molecules together (p. 146)
11.7 Enzyme-catalysed reactions (p. 150)
11.8 Summing up (p. 151)
11.9 Test yourself (p. 151)
Taking it further: Enzyme catalysis (p. 152)
Answers to "test yourself" questions (p. 159)
Appendices
1 Some common chemical formulae (p. 165)
2 Common anions and cations (p. 166)
3 Common functional groups (p. 167)
4 Notations, formulae and constants (p. 168)
5 Glossary (p. 172)
Index (p. 187)