Inorganic chemistry. (2018)
- Record Type:
- Book
- Title:
- Inorganic chemistry. (2018)
- Main Title:
- Inorganic chemistry
- Further Information:
- Note: Catherine E. Housecroft & Alan G. Sharpe.
- Authors:
- Housecroft, Catherine E, 1955-
Sharpe, A. G - Contents:
- 1 Basic concepts: atoms; 1.1 Introduction; Inorganic chemistry: it is not an isolated branch of chemistry; The aims of Chapters 1 and 2; 1.2 Fundamental particles of an atom; 1.3 Atomic number, mass number and isotopes; Nuclides, atomic number and mass number; Relative atomic mass; Isotopes; 1.4 Successes in early quantum theory; Some important successes of classical quantum theory; Bohr's theory of the atomic spectrum of hydrogen 1.5 An introduction to wave mechanicsThe wave-nature of electrons; The uncertainty principle; The Schrodinger wave equation; 1.6 Atomic orbitals; The quantum numbers n, l and ml; The radial part of the wavefunction, R (r); The radial distribution function, 4 r2R(r)2; The angular part of the wavefunction, A. ; .; Orbital energies in a hydrogen-like species; Size of orbitals; The spin quantum number and the magnetic spin quantum number; The ground state of the hydrogen atom; 1.7 Many-electron atoms; The helium atom: two electrons; Ground state electronic configurations: experimental data Penetration and shielding1.8 The periodic table; 1.9 The aufbau principle; Ground state electronic configurations; Valence and core electrons; Diagrammatic representations of electronic configurations; 1.10 Ionization energies and electron affinities; Ionization energies; Electron affinities; 2 Basic concepts: molecules; 2.1 Bonding models: an introduction; A historical overview; Lewis structures; 2.2 Homonuclear diatomic molecules: valence bond (VB) theory; Uses of1 Basic concepts: atoms; 1.1 Introduction; Inorganic chemistry: it is not an isolated branch of chemistry; The aims of Chapters 1 and 2; 1.2 Fundamental particles of an atom; 1.3 Atomic number, mass number and isotopes; Nuclides, atomic number and mass number; Relative atomic mass; Isotopes; 1.4 Successes in early quantum theory; Some important successes of classical quantum theory; Bohr's theory of the atomic spectrum of hydrogen 1.5 An introduction to wave mechanicsThe wave-nature of electrons; The uncertainty principle; The Schrodinger wave equation; 1.6 Atomic orbitals; The quantum numbers n, l and ml; The radial part of the wavefunction, R (r); The radial distribution function, 4 r2R(r)2; The angular part of the wavefunction, A. ; .; Orbital energies in a hydrogen-like species; Size of orbitals; The spin quantum number and the magnetic spin quantum number; The ground state of the hydrogen atom; 1.7 Many-electron atoms; The helium atom: two electrons; Ground state electronic configurations: experimental data Penetration and shielding1.8 The periodic table; 1.9 The aufbau principle; Ground state electronic configurations; Valence and core electrons; Diagrammatic representations of electronic configurations; 1.10 Ionization energies and electron affinities; Ionization energies; Electron affinities; 2 Basic concepts: molecules; 2.1 Bonding models: an introduction; A historical overview; Lewis structures; 2.2 Homonuclear diatomic molecules: valence bond (VB) theory; Uses of the term homonuclear; Covalent bond distance, covalent radius and van der Waals radius The valence bond (VB) model of bonding in H2The valence bond (VB) model applied to F2, O2 and N2; 2.3 Homonuclear diatomic molecules: molecular orbital (MO) theory; An overview of the MO model; Molecular orbital theory applied to the bonding in H2; The bonding in He2; Li2 and Be2; The bonding in F2 and O2; What happens if the s-p separation is small?; 2.4 The octet rule and isoelectronic species; The octet rule: first row p-block elements; Isoelectronic species; The octet rule: heavier p-block elements; 2.5 Electronegativity values; Pauling electronegativity values, P Mulliken electronegativity values, MAllred-Rochow electronegativity values, AR; Electronegativity: final remarks; 2.6 Dipole moments; Polar diatomic molecules; Molecular dipole moments; 2.7 MO theory: heteronuclear diatomic molecules; Which orbital interactions should be considered?; Hydrogen fluoride; Carbon monoxide; 2.8 Molecular shape and the VSEPR model; Valence-shell electron-pair repulsion model; Structures derived from a trigonal bipyramid; Limitations of the VSEPR model; 2.9 Molecular shape: stereoisomerism; Square planar species; Octahedral species; Trigonal bipyramidal species … (more)
- Edition:
- Fifth edition
- Publisher Details:
- Harlow, United Kingdom : Pearson Education Limited
- Publication Date:
- 2018
- Extent:
- 1 online resource (1297 pages)
- Subjects:
- 546
Chemistry, Inorganic
Chemistry, Inorganic -- Problems, exercises, etc
Chemistry, Inorganic
Chimie inorganique
Chimie inorganique -- Problèmes et exercices
inorganic chemistry
Chemistry, Inorganic
Problems and Exercises
Electronic books
exercise books
Problems and exercises
Problems and exercises
Problèmes et exercices - Languages:
- English
- ISBNs:
- 9781292134161
9781292204963
1292204966 - Related ISBNs:
- 129213416X
9781292134147
1292134143
9781292139913
1292139919 - Notes:
- Note: Includes bibliographical references and index.
Note: Print version record. - Access Rights:
- Legal Deposit; Only available on premises controlled by the deposit library and to one user at any one time; The Legal Deposit Libraries (Non-Print Works) Regulations (UK).
- Access Usage:
- Restricted: Printing from this resource is governed by The Legal Deposit Libraries (Non-Print Works) Regulations (UK) and UK copyright law currently in force.
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- Available online (eLD content is only available in our Reading Rooms) ↗
- Physical Locations:
- British Library HMNTS - ELD.DS.725069
- Ingest File:
- 14_047.xml