Chemistry : the molecular nature of matter and change /
Martin Silberberg ; consultants, L. Peter Gold . . . [et al.].
- Boston : McGraw-Hill/WCB, c1996.
- xxxiv, (various pagings) : ill. (some col.) ; 27 cm.
Contents;
1 Keys to the study of chemistry 1.1 Some fundamental definitions 1.2 Chemical arts and the origins of modern chemistry 1.3 The scientific approach: Developing a model 1.4 Chemical problem solving 1.5 Measurement in scientific study 1.6 Uncertainty in measurement: Significant figures
2 The components of matter, 2.1 Elements, compounds and mixtures: An atomic overview 2.2 The observations that led to an atomic view of matter 2.3 The observations that led to the nuclear Atom model 2.4 The Atomic theory today 2.5 Elements: A first look at the periodic table etc.
3 Stoichiometry; Mole mass relationships in chemical systems 3.1 The mole 3.2 Determining the formula of an unknown compound 3.3 Writing and balancing chemical equations 3.4 Calculating the amounts of reactant and product 3.5 Fundamentals of solution stoichiometry
4 The major classes of chemical reactions 4.1 Types of chemical reactions: An accounting of reactants and products 4.2 The role of water as a solvent 4.3 Some important aqueous ionic reactions;writing ionic equations 4.4 Oxidation-reduction ( redox)reactions 4.5 Reversible reactions: An introduction to chemical equilibrium
5 Gases and the kinetic-molecular theory 5.1 An overview of the physical states of matter 5.2 Measuring the pressure of a gas 5.3 The Gas laws and their experimental foundations 5.4 Further applications of the ideal Gas law 5.5 The ideal Gas Law and reaction stoichiometry etc.
6 Thermochemistry: Energy flow and chemical change 6.1 Forms of energy and their interconversion 6.2 Enthalpy: Heats of reaction and chemical change 6.3 Calorimetry:Laboratory measurement of heats of reaction 6.4 Stoichiometry of thermochemical equations etc.
7 Quantum theory and atomic structure 7.1 The nature of light 7.2 Atomic spectra and the Bohr model of the atom 7.3 The wave-particle duality of matter and energy 7.4 The quantum-mechanical model of the atom etc.
8 Electron configuration and chemical periodicity 8.1 Characteristics of many -electron atoms 8.2 The quantum-mechanical atom and the periodic table 8.3 Trends in some key periodic atomic properties 8.4 The connection between atomic structure and chemical reactivity etc.
9 Models of chemical bonding 9.1 Atomic properties and chemical bonds 9.2 The ionic bonding model 9.3 The covalent bonding model 9.4 Between the extremes: Electronegativity and bond polarity etc.
10 Molecular shape and theories of covalent bonding 10.1 Valence-shell electron-pair repulsion 10.2 Molecular shape and molecular polarity 10.3 Valence bond (VB) theory and orbital hybridization 10.4 Molecular orbital (MO)theory and electron delocalization etc.
11 Intermolecular forces: Liquids, solids and changes of state 11.1 An overview of physical states and phase 11.2 Types of intermolecular forces 11.3 Properties of the liquids state 11.4 Properties of the solid state etc.
12 The Properties 0f Mixtures: Solutions and Colloids 12.1 Types of Solutions: Intermolecular Forces and the Prediction of Solubility 12.2 Energy Changes in the solution process 12.3 Solubility as an Equilibrium process 12.4 Quantitative Ways of Expressing Concentration 12.5 Colligative Properties of Solutions etc