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Chemistry

Author: Allan Blackman
Publisher: Milton, Qld. : John Wiley & Sons Australia, Ltd, 2016.
Edition/Format:   eBook : Document : English : 3rd editionView all editions and formats
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Genre/Form: Electronic books
Textbooks
Additional Physical Format: Print version:
Blackman, Allan (Allan G.).
Chemistry.
Milton, Qld. : John Wiley & Sons Australia, Ltd, 2016
(OCoLC)903004834
Material Type: Document, Internet resource
Document Type: Internet Resource, Computer File
All Authors / Contributors: Allan Blackman
ISBN: 9780730328353 073032835X
OCLC Number: 967841417
Notes: Includes index.
Description: 1 online resource (xx, 1159 pages) : color illustrations
Contents: 1 The atom --
1.1 Atoms, molecules, ions, elements and compounds --
1.2 The atomic theory --
1.3 The structure of the atom --
Chemical Connections Imaging atoms --
Atomic mass --
Chemical Connections Saving lives with isotopes --
1.4 The periodic table of the elements --
The modern periodic table --
Naming the elements --
1.5 Electrons in atoms --
Summary --
Key concepts and equations --
Key terms --
Review questions --
Review problems --
Additional exercises --
2 The language of chemistry --
2.1 Measurement --
SI units --
Non-SI units --
Dimensional analysis --
Precision and accuracy --
Uncertainties and significant figures --
Chemical Connections The National Measurement Institute --
2.2 Representations of molecules and reactions --
Chemical formulae --
Structural formulae --
Three-dimensional structures --
Mechanistic arrows in chemical reactions --
2.3 Nomenclature --
Chemical Connections IUPAC --
Naming inorganic compounds --
Naming organic compounds --
Chemical Connections Bosutnib --
Summary --
Key concepts and equations --
Key terms --
Review questions --
Review problems --
Additional exercises --
Maths for chemistry --
3 Chemical reactions and stoichiometry --
3.1 Chemical equations --
Specifying states of matter --
3.2 Balancing chemical equations --
3.3 The mole --
3.4 Empirical formulae --
Chemical Connections Elemental analysis at the Campbell Microanalytical Laboratory --
Mole ratios from chemical formulae --
Determination of chemical formulae --
Determination of empirical formulae --
3.5 Stoichiometry, limiting reagents and percentage yield --
Mole ratios in chemical reactions --
Limiting reagents --
Percentage yield --
3.6 Solution stoichiometry --
The concentration of solutions. Applications of solution stoichiometry --
Stoichiometry of solutions containing ions --
Summary --
Key concepts and equations --
Key terms --
Review questions --
Review problems --
Additional exercises --
4 Atomic energy levels --
4.1 Characteristics of atoms --
4.2 Characteristics of light --
Wave-like properties of light --
Particle properties of light --
Chemical Connections The Australian Synchrotron --
Absorption and emission spectra --
Atomic spectra --
Quantisation of energy --
Energy level diagrams --
4.3 Properties of electrons --
The Heisenberg uncertainty principle --
4.4 Quantisation and quantum numbers --
Principal quantum number (n) --
Azimuthal quantum number (l) --
Magnetic quantum number (ml) --
Spin quantum number (ms) --
The Pauli exclusion principle --
4.5 Atomic orbital electron distributions and energies --
Orbital electron distributions --
Orbital energies --
4.6 Structure of the periodic table --
The Aufbau principle and order of orbital filling --
Valence electrons --
4.7 Electron configurations --
Electron-electron repulsion --
Orbitals with nearly equal energies --
Configurations of ions --
Magnetic properties of atoms --
Excited states --
4.8 Periodicity of atomic properties --
Atomic radii --
Ionisation energy --
Electron affinity --
Sizes of ions --
4.9 Ions and chemical periodicity --
Cation stability --
Anion stability --
Metals, nonmetals and metalloids --
s-block elements --
p-block elements --
Summary --
Key concepts and equations --
Key terms --
Review questions --
Review problems --
Additional exercises --
5 Chemical bonding and molecular structure --
5.1 Fundamentals of bonding --
The hydrogen molecule --
Bond length and bond energy --
Other diatomic molecules: F2 --
Unequal electron sharing --
Chemical Connections Electromagnetic radiation and cancer --
5.2 Ionic bonding --
5.3 Lewis structures. The conventions --
Building Lewis structures --
Resonance structures --
5.4 Valence-shell-electron-pair repulsion (VSEPR) theory --
Two sets of electron pairs: linear geometry --
Three sets of electron pairs: trigonal planar geometry --
Four sets of electron pairs: tetrahedral geometry --
Five sets of electron pairs: trigonal bipyramidal geometry --
Six sets of electron pairs: octahedral geometry --
5.5 Properties of covalent bonds --
Dipole moments --
Bond length --
Bond energy --
Chemical Connections Making use of the energy stored in covalent bonds --
Summary of molecular shapes --
5.6 Valence bond theory --
Orbital overlap --
Conventions of the orbital overlap model --
Hybridisation of atomic orbitals --
Multiple bonds --
5.7 Molecular orbital theory: diatomic molecules --
Molecular orbitals of H2 and He2 --
Molecular orbitals of O2 --
Homonuclear diatomic molecules --
Heteronuclear diatomic molecules --
Summary --
Key concepts and equations --
Key terms --
Review questions --
Review problems --
Additional exercises --
6 Gases --
6.1 The states of matter --
6.2 Describing gases --
Pressure (p) --
The gas laws --
The ideal gas equation --
6.3 Molecular view of gases --
Molecular speeds --
Speed and energy --
Average kinetic energy and temperature --
Rates of gas movement --
Ideal gases --
6.4 Gas mixtures --
Dalton's law of partial pressures --
Describing gas mixtures --
6.5 Applications of the ideal gas equation --
Determination of molar mass --
Determination of gas density --
6.6 Gas stoichiometry --
Summary of mole conversions --
6.7 Real gases --
The halogens --
Properties of real gases --
The van der Waals equation --
Melting and boiling points --
6.8 Intermolecular forces --
Dispersion forces --
Dipolar forces --
Hydrogen bonds --
Binary hydrogen compounds --
Chemical Connections Atmospheric carbon dioxide --
Summary. Key concepts and equations --
Key terms --
Review questions --
Review problems --
Additional exercises --
7 Condensed phases: liquids and solids --
7.1 Liquids --
Properties of liquids --
Vapour pressure --
7.2 Solids --
Magnitudes of forces --
Molecular solids --
Network solids --
Metallic solids --
Ionic solids --
7.3 Phase changes --
Phase diagrams --
Chemical Connections Chemistry and cool jackets --
7.4 Order in solids --
Close-packed structures --
The crystal lattice and the unit cell --
Cubic structures --
Ionic solids --
7.5 X-ray diffraction --
7.6 Amorphous solids --
7.7 Crystal imperfections --
7.8 Modern ceramics --
Properties of ceramics --
Applications of advanced ceramics --
High-temperature superconductors --
Chemical Connections Fast trains on superconductors --
Summary --
Key concepts and equations --
Key terms --
Review questions --
Review problems --
Additional exercises --
8 Chemical thermodynamics --
8.1 Introduction to chemical thermodynamics --
8.2 Thermodynamic concepts --
Heat and temperature --
System, surroundings and universe --
Units --
(SE (BX: the change in X --
State functions --
(SE (BG and spontaneity --
8.3 The first law of thermodynamics --
Heat capacity and specific heat --
Determination of heat --
8.4 Enthalpy --
Standard enthalpy of reaction --
Chemical Connections Cold fusion --
a nuclear reaction at room temperature --
Hess's law --
Standard enthalpy of formation --
Standard enthalpy of combustion --
Bond enthalpies --
Chemical Connections The thermodynamics of steam burns --
8.5 Entropy --
Entropy and probability --
Entropy and entropy change --
Factors that affect entropy --
8.6 The second law of thermodynamics --
8.7 The third law of thermodynamics --
Chemical Connections Airconditioning and the second law of thermodynamics --
8.8 Gibbs energy and reaction spontaneity --
The sign of (SE (BG --
Standard Gibbs energy change.
Responsibility: Allan Blackman [and ten others].

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