Basic Principles of Inorganic Chemistry

by Murphy, Brian; Murphy, Clair; Hathaway, Brian J.

• ISBN13: 9780854045747
• ISBN10: 0854045740
• Format: Paperback
• Copyright: 1998-12-01
• Publisher: Royal Society of Chemistry

Summary

General chemistry textbooks are usually lengthy and present chemistry to the student as an unconnected list of facts. In inorganic chemistry, emphasis should be placed on the connections between valence shell electron configuration and the physical and chemical properties of the element. Basic Principles of Inorganic Chemistry: Making the Connections is a short, concise book that emphasises these connections, in particular the chemistry of the Main Group compounds. With reference to chemical properties, Lewis Structures, stoichiometry and spider diagrams, students will be able to predict or calculate the chemistry of simple polyatomic compounds from the valence shell configuration and will no longer be required to memorise vast amounts of factual chemistry. This book is ideal for students taking chemistry as a subsidiary subject as well as honours degree students.

Table of Contents

Chapter 1 Moles and Molarity	1	(13)
Aims and Objectives	1	(1)
States of Matter	1	(1)
Elements, Atoms and Molecules	1	(1)
Elements, Mixtures and Compounds (Molecules)	2	(1)
Simple Chemical Names	3	(1)
Cations and Anions	3	(1)
Types of Chemical Formula	4	(1)
Atomic Weight	4	(1)
Avogadro's Number	5	(1)
Empirical Formula	5	(1)
Chemical Equations	6	(1)
Balancing Chemical Equations	7	(1)
Molar Solutions	8	(1)
Volumetric Reactions	9	(1)
Volumetric Titrations	10	(1)
Limiting Reactions	11	(1)
Worked Example No. 1	11	(2)
Worked Example No. 2	13	(1)
Chapter 2 The Structure of the Atom, Electron Configuration and the Build-up to the Periodic Table	14	(17)
Aims and Objectives	14	(1)
The Structure of the Atom	14	(3)
Bohr Model of the Atom	17	(10)
The Build-up Process for the Periodic Table	27	(4)
Chapter 3 The Physical Properties of the Elements and the Periodic Table	31	(8)
Aims and Objectives	31	(1)
The Periodic Table	31	(3)
Variation in the Atomic Radii	34	(1)
Variation in the Ionisation Potentials	34	(3)
Variation in the Electron Affinities or Attachment Enthalpies	37	(1)
Summary	38	(1)
Chapter 4 Chemical Properties of the Elements and the Periodic Table	39	(22)
Aims and Objectives	39	(1)
Introduction	39	(2)
Characteristic or Group Oxidation Numbers	41	(2)
Oxidation Numbers	43	(1)
Rules for the Determination of Oxidation Numbers	44	(1)
Main Group Variable Valence	44	(2)
Transition Metal Variable Valence	46	(3)
Chemical Stoichiometry	49	(4)
The Calculation of Chemical Stoichiometry Factors -- Worked Examples	51	(1)
Redox Reactions	52	(1)
Covalent Bonds	53	(3)
Polyatomic Covalent Molecules	54	(2)
Molecular Orbital Theory of Diatomic Molecules	56	(4)
Bond Order	60	(1)
Chapter 5 The Lewis Structures of Molecules, Cations and Anions, Including Oxyanions	61	(27)
Aims and Objectives	61	(1)
Introduction	61	(3)
The Working Method for Drawing Lewis Structures	64	(10)
Example 1: Methane (CH(4)) and Carbon Tetrachloride (CCl(4))	65	(1)
Example 2: The Ammonium Cation (NH(4)(+)) and the Tetrafluorborate Anion (BF(4)(-))	66	(2)
Example 3: Ammonia (NH(3)) and Water (OH(2))	68	(1)
Example 4: Beryllium Dihydride (BeH(2)) and Boron Trifluoride (BF(3))	69	(1)
Example 5: Phosphorus Pentchloride (PCl(5)) and Sulfur Hexafluoride (SF(6))	70	(1)
Example 6: 1, 1, -Dichloromethanone (Cl(2)CO) and Ethene (C(2)H(4))	71	(2)
Example 7: Ethyne (C(2)H(2))	73	(1)
The Oxyacids and Oxyanions of the Main Group Elements	74	(5)
The Position of the Hydrogen Atoms in the Oxyacids	74	(2)
The Free Valence of the Terminal Oxygen Atoms	76	(2)
Resonance in the Structures of the Oxyanions	78	(1)
The Application of the Working Method to the Lewis Structures of the Oxyanions	79	(5)
Example 1: Carbonic Acid, H(2)CO(3)	79	(2)
Example 2: Sulfuric Acid, H(2)SO(4)	81	(3)
The Use of Formal Charges	84	(2)
Summary	86	(2)
Chapter 6 Shape and Hybridisation	88	(19)
Aims and Objectives	88	(1)
The Shapes of Covalent Molecules	88	(4)
The Working Method for Using VSEPR Theory	92	(2)
Deviations from Regular Shapes	94	(1)
The Advantages of VSEPR Theory	95	(1)
The Disadvantages of VSEPR Theory	95	(1)
The Shape of Dinuclear Molecules	95	(4)
Hybridisation of Atomic Orbitals	99	(5)
Hybridisation in Polynuclear Molecules	104	(2)
Summary	106	(1)
Chapter 7 A Features of Interest Approach to Systematic Inorganic Chemistry	107	(37)
Aims and Objectives	107	(1)
Introduction	107	(2)
The Preparation of Simple Compounds from the Elements	109	(4)
The Reactions of Simple Compounds	113	(3)
Reaction with Water	113	(1)
Volumetric Reactions	114	(1)
The Effect of Heat	115	(1)
Features of Interest of Simple Compounds -- Working Method The Application of the Working Method to a Selection of Simple Compounds	116	(3)
Example 1: Methane, (CH(4))	119	(11)
Example 2: Hydrochloric Acid (HCl)	120	(1)
Example 3: Sodium Chloride (NaCl)	121	(1)
Example 4: Phosphorus Pentachloride (PCl(5))	122	(1)
Example 5: Copper (II) Oxide, (CuO)	123	(1)
Example 6: Iron (II) Chloride (FeCl(2))	124	(1)
Example 7: Iron (II) Sulfate Hexahydrate ([Fe(OH(2))(6)]SO(4))	125	(1)
Example 8: Carbonic Acid (H(2)CO(3))	126	(2)
Writing an Essay or Report from a Spider Diagram	128	(2)
Conclusions	130	(1)
Suggested Ways Forward	130	(14)
Phase II -- Features of Interest	130	(1)
Phase III -- Features of Interest	131	(8)
The Advantages of the Features of Interest Approach	139	(1)
The Disadvantages of the Features of Interest Approach	139	(5)
Appendices	144	(4)
Periodic Table of the Elements	148	(1)
Subject Index	149