- Häftad (Paperback)
- Antal sidor
- OUP Oxford
- Holman, John / Parsons, Andrew / Pilling, Gwen / Price, Gareth
- 277 x 219 x 50 mm
- Antal komponenter
- 2860 g
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Introducing inorganic, organic and physical chemistry609Skickas inom 10-15 vardagar.
Fri frakt inom Sverige för privatpersoner.Chemistry establishes the fundamental principles of all three strands of chemistry; organic, inorganic and physical. By building on what students have learned at school, using carefully-worded explanations, annotated diagrams and worked examples, it presents an approachable introduction to chemistry and its relevance to everyday life.
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Dr Rossana Wright, University of Nottingham It is a great textbook for first year courses with really good use of visual aids and excellent provision of worked examples to illustrate the concepts and their applications. It is a perfect transition from A-Level to Higher Education Chemistry.
Dr Gareth Owen, University of South Wales Chemistry3 is the best introductory chemistry textbook currently available. It is well written, excels in clarity of presentation, and is an outstanding book from the student learning perspective. All of the concepts covered are well explained and supported by excellent artwork. This is a book that all first and second year chemistry undergraduates should have.
Dr Loretta M. Murphy, Bangor University This is an exemplar modern chemistry resource with a very rounded pedagogical approach to engaging students and supporting staff in delivering key chemical concepts and supporting facts. It is a one stop shop for mainstream chemistry fundamentals.
Adam Stubbs, student at Newcastle University A fantastic all-round reference for university-level chemistry. It is a perfect way to bridge between school and university.
Christian Nichol J. Geronimo, student at Dublin Institute of Technology Chemistry3 is the best university chemistry text book for first and second year science students. It is comprehensive and contains all the fundamentals for chemists to know- from analytical to organic chemistry. It is also a student friendly book with tons of pictures and applications of chemistry in the real world.
Rebecca Snelgrove, student at Keele University This material is fantastic and should be used alongside courses. The level of detail is exactly right for undergraduate courses and the colour coding of the boxes for worked examples and summaries make them really easy to find. There are lots of questions for you to have a go at which makes it easy to practice the new skills the book is helping to teach.
Jelte van der Valk, student at the University of Groningen, the Netherlands Plenty of facts and figures are scattered throughout the text which makes reading not solely an educational, but also a fun activity. The examples of real life chemistry applications maintain the connection between theory and practice. The interdisciplinary approach provides a broader chemical understanding while not losing the comprehensiveness of the book. In short, a good all-in-one textbook for first-year students in chemistry.
Michelle Rasmussen, student at the University of Roskilde, Denmark The topics are very thoroughly explained and are at exactly the right level for the student. There are many great examples illustrating the topics. It is a great book to read and study from as a student starting university. This is definitely a book I would buy, read and return to, when I needed an explanation for some basic chemistry.
Dr Andrew Burrows, Department of Chemistry, University of Bath Professor John Holman, Professor of Science Education, Director of the National Science Learning Centre, University of York Dr Andrew Parsons, Department of Chemistry, University of York Dr Gwen Pilling, Formerly of the Science Education Group, University of York Dr Gareth Price, Department of Chemistry, University of Bath
A message to readers Getting the most from Chemistry3 Acknowledgements1 Fundamentals What do chemists do?1.1 Chemistry: the central science 1.2 Measurement, units, and nomenclature 1.3 Atoms and the mole 1.4 Chemical equations 1.5 Working out how much you have 1.6 Energy changes in chemical reactions1.7 States of matter and phase changes 1.8 Non-covalent interactions1.9 Chemical equilibrium: how far has a reaction gone?2 The language of organic chemistryDesigner medicines for treating high blood pressure: an ACE approach2.1 Why are organic compounds important? 2.2 Drawing organic compounds 2.3 Carbon frameworks and functional groups 2.4 Naming organic compounds 2.5 Hydrocarbons 2.6 Functional groups containing one or more heteroatoms 2.7 Functional groups containing carbonyl groups2.8 Naming compounds with more than one functional group3 Atomic structure and propertiesImaging atoms3.1 The classical picture of the atom 3.2 Electromagnetic radiation and quantization 3.3 Atomic spectra and the Bohr atom 3.4 The nature of the electron 3.5 Wavefunctions and atomic orbitals 3.6 Many-electron atoms 3.7 Atomic properties and periodicity 3.8 Nuclear chemistry4 Diatomic moleculesMolecules in space4.2 The Lewis model 4.3 Electronegativity 4.4 Valence bond theory and molecular orbital theory 4.5 Valence bond theory 4.6 Molecular orbital theory 4.7 Molecular orbitals in hydrogen (H2) 4.8 Molecular orbital energy level diagrams 4.9 Linear combinations of p orbitals 4.10 Bonding in fluorine (F2) and oxygen (O2) 4.11 s-p mixing 4.12 Heteronuclear diatomics5 Polyatomic molecules Xenon compounds5.1 The Lewis model 5.2 Valence shell electron pair repulsion theory 5.3 Bond polarity and polar molecules 5.4 Valence bond theory for polyatomic molecules 5.5 Resonance 5.6 A molecular orbital approach to the bonding in polyatomic molecules 5.7 Partial molecular orbital schemes6 Solids Zeolites6.1 Covalent network structures Box 6.1 Graphene, nanotubes, and nanotechnology Box 6.2 Superconductors 6.2 Structures based on the packing of spheres 6.3 Metallic bonding Box 6.3 CD writers and re-writers 6.4 Structures of compounds Box 6.4 X-ray crystallography Box 6.5 Self-cleaning windows 6.5 The ionic model 6.6 Calculating lattice energy Box 6.6 Determining the Madelung constant 6.7 Predicting bond types7 Acids and bases Acids and bases in the garden7.1 Bronsted-Lowry acids and bases 7.2 The strengths of acids and bases 7.3 Buffer solutions 7.4 pH changes in acid-base titrations 7.5 Indicators 7.6 Oxoacids 7.7 Acidic and basic oxides 7.8 Lewis acids and bases8 Gases Breathing under water8.1 The gas laws: an empirical approach 8.2 Using the ideal gas equation 8.3 Mixtures of gases 8.4 Kinetic molecular theory and the gas laws 8.5 The speeds of molecules in a gas8.6 Real gases9 Reaction kinetics Methane in the troposphere9.1 Why study reaction kinetics? 9.2 What is meant by the rate of a reaction? 9.3 Monitoring the progress of a reaction 9.4 Elementary reactions 9.5 Complex reactions: experimental methods 9.6 Complex reactions: reaction mechanisms 9.7 Effect of temperature on the rate of a reaction 9.8 Theories of reactions 9.9 Catalysis10 Molecular spectroscopy Searching for life on Mars10.1 Introduction to molecular spectroscopy 10.2 Molecular energies and spectroscopy 10.3 General principles of spectroscopy 10.4 Rotational spectroscopy10.5 Vibrational spectroscopy 10.6 Electronic spectroscopy 10.7 Spin resonance spectroscopy11 Analytical chemistryDrugs and the Olympics11.1 Carrying out an analysis 11.2 Electrochemical methods of analysis 11.3 Chromatography 11.4 Spectroscopic methods of analysis 11.5 Atomic spectrometry12 Molecular characterizationUsing isotope ratios to analyse orange juice12.1 Mass spectrometry 12.2 Infrared spectroscopy 12.3 Nuclear magnetic resonance spectroscopy 12.4 Structure determination using a combination of techniques13 Energy and thermochemistryLaunching the Space Shuttle13.1 Energy changes in chemistry: heat and work 13.2 Entha