Chemistry3 : introducing inorganic, organic and physical chemistry
著者
書誌事項
Chemistry3 : introducing inorganic, organic and physical chemistry
Oxford University Press, 2017
3rd ed
- : pbk
- タイトル別名
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Chemistry : introducing inorganic, organic and physical chemistry
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注記
Includes index
Other authors: John Holman, Andrew Parsons, Gwen Pilling, Gareth Price
内容説明・目次
内容説明
Chemistry is widely considered to be the central science: it encompasses concepts from which other branches of science are developed. Yet, for many students entering university, gaining a firm grounding in chemistry is a real challenge. Chemistry(3) responds to this challenge, providing students with a full understanding of the fundamental principles of chemistry on which to build later studies.
Uniquely amongst the introductory chemistry texts currently available, Chemistry(3) is written by a team of chemists to give equal coverage of organic, inorganic and physical chemistry - coverage that is uniformly authoritative. The approach to organic chemistry is mechanistic, rather than the old-fashioned 'functional group' approach, to help students achieve a fuller understanding of the underlying principles.
The expertise of the author team is complemented by two specialists in chemistry education, who bring to the book a wealth of experience of teaching chemistry in a way that students enjoy and understand, and who understand the challenges of the transition from school to university. The result is a text that builds on what students know already from school and tackles their misunderstandings and misconceptions, thereby providing a seamless transition from school to undergraduate study.
The authors achieve unrivalled accessibility through the provision of carefully-worded explanations and reminders of students' existing knowledge; the introduction of concepts in a logical and progressive manner; and the use of annotated diagrams and step-by-step worked examples. Students are encouraged to engage with the text and appreciate the central role that chemistry plays in our lives through the unique use of real-world context and photographs.
Chemistry(3) tackles head-on two issues pervading chemistry education: students' mathematical skills, and their ability to see the subject as a single, unified discipline. Instead of avoiding the maths, Chemistry(3) provides structured support, in the form of careful explanations, reminders of key mathematical concepts, step-by-step calculations in worked examples, and a Maths Toolkit, to help students get to grips with the essential mathematical element of chemistry.
Frequent cross-references highlight the connections between each strand of chemistry and explain the relationship between the topics, so students can develop an understanding of the subject as a whole.
目次
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 Enthalpy and enthalpy changes13.3 Enthalpy changes in chemical reactions 13.4 Variation of enthalpy with temperature 13.5 Internal energy and the First Law of thermodynamics 13.6 Measuring energy changes14 Entropy and Gibbs energyProtein folding14.1 What are spontaneous processes? 14.2 Entropy and the Second Law of thermodynamics 14.3 The Third Law and absolute entropies14.4 Entropy changes in chemical reactions 14.5 Gibbs energy 14.6 Variation of Gibbs energy with conditions15 Chemical equilibriumEquilibria in the oceans15.1 Gibbs energy and equilibrium 15.2 The direction of a reaction: the reaction quotient15.3 Gibbs energy and equilibrium constants 15.4 Calculating the composition of a reaction at equilibrium 15.5 Effect of conditions on reaction yields and K 15.6 Applying the thermodynamics in Chapters 13, 14, and 1516 Electrochemistry Electrical energy on the move16.1 What is electrochemistry? 16.2 Ions in solution 16.3 Electrochemical cells16.4 Thermodynamics of electrochemical cells16.5 Electrolysis17 Phase equilibrium and solutions Supercritical fluids17.1 Phase behaviour of single components 17.2 Quantitative treatment of phase transitions 17.3 Intermolecular interactions 17.4 Phase behaviour in two-component systems18 Isomerism and stereochemistryBitter isomers in beer18.1 Isomerism 18.2 Conformational isomers 18.3 Configurational isomers: E- and Z-isomers 18.4 Configurational isomers: isomers with chiral centres19 Organic reaction mechanismsAntidotes for nerve agentsBox 19.1 The birth of organic reaction mechanisms 19.1 Fundamental concepts of organic reaction mechanisms19.2 Classification of organic reaction mechanisms 19.3 Reaction selectivity20 Halogenoalkanes: substitution and elimination reactionsAlternative pesticides to bromomethane20.1 Structure and reactivity of halogenoalkanes 20.2 Preparation of halogenoalkanes 20.3 The mechanisms of nucleophilic substitution reactions 20.4 The mechanisms of elimination reactions 20.5 Substitution versus elimination reactions21 Alkenes and alkynes:electrophilic addition and pericyclic reactions The citric acid cycle21.1 Structure and reactivity of alkenes and alkynes 21.2 Preparation of alkenes and alkynes 21.3 Electrophilic addition reactions of alkenes 21.4 Pericyclic reactions of alkenes 21.5 Electrophilic addition reactions of alkynes22 Benzene and other aromatic compounds: electrophilic substitution reactionsAzo dyes: the start of the rainbow22.1 The structure of benzene and other aromatic compounds 22.2 Electrophilic substitution reactions of benzene 22.3 Reactivity of substituted benzenes in electrophilic substitutions22.4 The synthesis of substituted benzenes23 Aldehydes and ketones: nucleophilic addition and -substitution reactions Rhodopsin and vision23.1 The structure and reactions of aldehydes and ketones 23.2 Nucleophilic addition reactions of aldehydes and ketones23.3 -Substitution reactions of aldehydes and ketones 23.4 Carbonyl-carbonyl condensation reactions24 Carboxylic acids and derivatives: nucleophilic acyl substitution and -substitution reactions PET plastics24.1 Structure and reactions of carboxylic acids and derivatives24.2 Nucleophilic acyl substitution reactions24.3 -Substitution and carbonyl-carbonyl condensation reactions25 HydrogenThe planet Jupiter25.1 Elemental hydrogen 25.2 Compounds of hydrogen 25.3 Hydrogen bonding 25.4 Isotope effects26 s-Block chemistry Biominerals26.1 The Group 1 elements26.2 Group 1 compounds Box 26.1 Why is sodium peroxide more stable to heating than lithium peroxide? 26.3 Group 1 ions in solution 26.4 Group 1 coordination chemistry 26.5 Reaction of Group 1 metals with liquid ammonia26.6 The Group 2 elements 26.7 Group 2 compounds 26.8 Group 2 coordination chemistry 26.9 Lithium and beryllium as exceptional elements 26.10 Organometallic compounds 26.11 Diagonal relationships27 p-Block chemistryPhotochemical smog27.1 General aspects and trends in the p block27.2 Group 13: boron, aluminium, gallium, indium,and thallium27.3 Group 14: carbon, silicon, germanium, tin, and lead27.4 Group 15: nitrogen, phosphorus, arsenic, antimony,and bismuth27.5 Group 16: oxygen, sulfur, selenium, tellurium,and polonium27.6 Group 17: fluorine, chlorine, bromine, iodine,and astatine27.7 Group 18: helium, neon, argon, krypton, xenon,and radon27.8 p-Block organometallic chemistry28 d-Block chemistry Colouring with metal pigments28.1 The d-block elements 28.2 Chemistry of the first row d-block elements 28.3 Coordination chemistry 28.4 Crystal field theory 28.5 Filling the d orbitals 28.6 Colour in coordination compounds 28.7 Magnetic properties28.8 Aqueous chemistry of the first row d-block ionsMaths ToolkitAppendix
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