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無 機 化 學 ( ㄧ )
2009 化學系 黃建和
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1-1 What is Inorganic Chemistry
limitless area
1-2 Contracts with Organic Chemistry
delta bond
bridging H and alkyl group
higher coordination numbers
aromatic ring-metal bond
carbon in metal cluster cpds
fullerene
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1-3 Genesis of the elements and formation of the earth: the big bang theory
hydrogen burning
helium burning
the carbon-nitrogen cycle
1-4 Nuclear reaction and radioactivity
fission of U and Pu
fusion of H
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• 1-5 Distribution of elements on earth according to the solubility in water and
magma
• 1-6 The history of inorganic chemistry before alchemy alchemy radioactivity Werner, Ziegler biological activity
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Chap. 2
• 2.1 Historical development of atomic theory
2.2.1 The periodic table
2.2.2 discovery of subatomic particles and the Bohr atom
hydrogen emission spectrum quantum number Heisenberg’s uncertainty principle
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Chapter 2 p17
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Chapter 2 p20
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Chap. 2
• 2.2 The Schrodinger equation
2.2.1 the particle in a box
2.2.2 quantum numbers and atomic wave functions
2.2.3 the Aufbau principle
2.2.4 Shielding: Slater rule
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Chapter 2 p23
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Chapter 2 p26
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Chapter 2 p26
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Chapter 2 p27
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Chapter 2 p31
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Chapter 2 p31
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Chapter 2 p35
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Chap. 2
• 2.3 periodic properties of atoms
2.3.1 ionization energy
2.3.2 electron affinity
2.3.3 covalent and ionic radii
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Chap. 3
• 3.1 Lewis electron-dot diagrams
3.1.1 resonance
3.1.2 expanded shells
3.1.3 formal charge
3.1.4 multiple bonds in Be and B compounds
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Chapter 3 p55
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Chapter 3 p56
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Chap. 3
• 3.2 valence shell electron pair repulsion theory
3.2.1 lone pair repulsion
3.2.2 multiple bonds
3.2.3 electronegativity and atomic size effects
3.2.4 ligand close-packing
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Chapter 3 p58
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Chapter 3 p61
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Chapter 3 p64
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Chap. 3
• 3.3 polar molecules
dipole moment
dispersion forces
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Chap. 3
• 3.4 Hydrogen bonding
ammonia
clathrates
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Chapter 3 p70
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Chapter 3 p71
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Chapter 4
• 4.1 symmetry elements and operations
identity
rotation
reflection
inversion
improper rotation
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Chapter 4 p81
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Chapter 4
• 4.2 point groups
the point group assignment method
4.2.1 group of low and high symmetry
4.2.2 other groups
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Chapter 4 p84
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Chapter 4
• 4.3 properties and representations of groups
4.3.1 matrices
4.3.2 representation of point groups
4.3.3 character tables
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Chapter 4
• 4.4 examples and applications of symmetry
4.4.1 chirality
4.4.2 molecular vibrations
water and cis-ML2(CO)2
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Chapter 4 p102
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Chapter 4 p103
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Chapter 4 p103
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Chapter 5
• 5.1 formation of molecular orbitals from atomic orbitals
5.1.1 molecular orbitals from s orbitals
5.1.2 molecular orbitals from p orbitals
5.1.3 molecular orbitals from d orbitals
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Chapter 5 p118
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Chapter 5
• 5.2 homonuclear diatomic molecules
5.2.1 molecular orbitals
5.2.2 orbital mixing
5.2.3 homonuclear diatomic molecules
5.2.4 photoelectron spectroscopy
5.2.5 correlation diagrams
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Chapter 5 p123
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Chapter 5
• 5.3 heteronuclear diatomic molecules
5.3.1 polar bonds
5.3.2 ionic compounds and molecular orbitals
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Chapter 5 p135
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Chapter 5
• 5.4 molecular orbitals for larger molecules
FHF-
CO2
H2O
NH3
BF3
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Chapter 5 p144
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Chapter 5 p147
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Chapter 5 p148
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Chapter 5 p151
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Chapter 5 p152
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Chapter 5
• 5.5 expanded shells and molecular orbitals
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Chapter 5 p161
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Chapter 6
• 6.1 acid-base concepts and organizing concepts
6.1.1 history
from the concept of sour-bitter taste
to Table 6-1
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Chapter 6
• 6.2 major acid-base concepts
6.2.1 Arrhenius concept 6.2.2 Brønsted-Lowry concept 6.2.3 Solvent system concept 6.2.4 Lewis concept 6.2.5 frontier orbitals and acid-base reactions 6.2.6 hydrogen bonding 6.2.7 electronic spectra
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Chapter 6 p179
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Chapter 6
• 6.3 hard and soft acids and bases
6.3.1 theory of hard and soft acids and bases
class (a) is hard class (b) is soft 6.3.2 quantitative measures Drago and Wayland system
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Chapter 6 p183
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Chapter 6 p184
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Chapter 6 p185
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Chapter 6 p191
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Chapter 6• 6.4 acid and base strength
6.4.1 measurement of acid-base interactions 6.4.2 thermodynamic measurements 6.4.3 proton affinity 6.4.4 acidity and basicity of binary hydrogen compounds 6.4.5 inductive effects 6.4.6 strength of oxyacids 6.4.7 acidity of cations in aqueous solution 6.4.8 steric effects 6.4.9 solvation and acid-base strength 6.4.10 nonaqueous solvents and acid-base strength 6.4.11 superacids
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Chapter 6 p202
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Chapter 6 p203
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Chapter 7
• 7.1 formulas and structures
7.1.1 simple structures
cubic, body-centered cubic,
close-packed structures,
metallic crystals, properties of metals,
diamond
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Chapter 7
• 7.1.2 structures of binary compounds sodium chloride cesium chloride zinc blend wurtzite fluorite NiAs rutile
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Chapter 7 p214
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Chapter 7 p214
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Chapter 7 p216
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Chapter 7 p216
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Chapter 7 p216
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Chapter 7 p216
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Chapter 7 p217
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Chapter 7 p217
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Chapter 7
• 7.1.3 more complex compounds
• 7.1.4 radius ratio
Table 7-1 radius ratio limiting values
0.414
0.732
1.00
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Chapter 7
• 7.2 thermodynamics of ionic crystal formation
7.2.1 lattice energy and Madelung constant
7.2.2 solubility, ion size, and HSAB
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Chapter 7 p221
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Chapter 7
• 7.3 molecular orbitals and band structure
p- and n-type semiconductors
7.3.1 diodes, the photovoltaic effect, and light-emitting diodes (LED)
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Chapter 7 p223
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Chapter 7 p225
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Chapter 7
• 7.4 superconductivity
7.4.1 low-temperature superconducting alloys
7.4.2 the theory of superconductivity
(Cooper pairs)
7.4.3 high-temperature superconductors
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Chapter 7 p228
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Chapter 7 p230
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Chapter 7
• 7.5 bonding in ionic crystals
• 7.6 imperfections in solids
vacancies and self-interstitials
substitutions
dislocations
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Chapter 7
• 7.7 silicates
silica: quartz, tridymite, and cristobalite
silicate: chain, double chain, ring, sheet, and 3-D array
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Chapter 7 p237
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Chapter 8
• 8.1 general trends in main group chem.
8.1.1 physical properties
8.1.2 electronegativity
8.1.3 ionization energy
8.1.4 chemical properties
redox reactions
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Chapter 8 p241
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Chapter 8 p243
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Chapter 8
• 8.2 hydrogen
Table 8-2
hydrogen, deuterium, and tritium
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Chapter 8
• 8.3 group 1: the alkali metals
8.3.1 the elements
8.3.2 chemical properties
crown ether
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Chapter 8 p251
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Chapter 8 p253
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Chapter 8 p253
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Chapter 8
• 8.4 group 2: alkaline earths
8.4.1 the elements
8.4.2 chemical properties
BeCl2 Grignart reagent
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Chapter 8
• 8.5 group 13
8.5.1 the elements boron diborane 8.5.2 other chemistry of the group 13 ele
ments inorganic benzene
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Chapter 8 p258
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Chapter 8 p261
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Chapter 8
• 8.6 group 14
8.6.1 the elements
8.6.2 compounds
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Chapter 8 p264
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Chapter 8 p268
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Chapter 8
• 8.7 group 15
8.7.1 the elements
8.7.2 compounds
hydrides
nitrogen oxides and oxyions
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Chapter 8 p277
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Chapter 8
• 8.8 group 16
8.8.1 the elements
the viscosity of sulfur is due to the tendency of S-S bonds to break and to reform at high temperature
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Chapter 8 p283
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Chapter 8
• 8.9 group 17
8.9.1 the elements
Table8-14
polyatomic ions
interhalogens
pseudohalogens
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Chapter 8
• 8.10 group 18
8.10.1 the elements
8.10.2 chemistry
clathrates
xenon compounds
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Chapter 8 p293