Introductory Inorganic Chemistry

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Introductory Inorganic Chemistry
What is Inorganic Chemistry?
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As 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p3
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For more information about these periodic tables
visit the site where I obtained the pictures
http//chemlab.pc.maricopa.edu/periodic/default.ht
ml
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Classes of Inorganic Substances
Elements Ionic Compounds Covalent Compounds
Atomic/Molecular Gases Ar, N2 Simple (binary) NaCl Simple (binary) NH3, H2O, SO2
Molecular Solids P4, S8, C60 Complex (polyatomic ions) Na2(SO4) Complex (polyatomic) As(C6H5)3, organometallic compounds
Network Solids diamond, graphite (C?) red phosphorus (P?) Network ions Mg3(Si2O5)(OH)2 (talc) DNA Network Solids SiO2, polymers
Solid/Liquid Metals Hg, Ga, Na, Fe, Mg
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Elements
Atomic/Molecular Gases Ar, N2, O2 , Br2
Molecular Solids P4, S8, C60
Network Solids diamond, graphite (C?) red phosphorus (P?)
Solid/Liquid Metals Hg, Ga, Fe, Na, Mg
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Ionic Compounds
Simple (binary) NaCl
Complex (polyatomic ions) Na2(SO4), Na2Mg(SO4)2
Network ions Mg3(Si4O10)(OH)2 (talc) DNA

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Covalent Compounds
Simple Molecular (binary) NH3, H2O, CO2, SO2
Complex Molecular As(C6H5)3, organometallic compounds
Network Solids SiO2, polymers

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Review of Concepts
Thermochemistry Standard state 298.15 K, 1
atm, unit concentration Enthalpy Change,
DH DH SHproducts - SHreactants Entropy
Change, DS Free Energy Change, DG DG DH
- TDS At STP DG DH - (298.15 K)DS
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Standard Enthalpy of Formation, DHf DH for the
formation of a substance from its constituent
elements Standard Enthalpy of Fusion,
DHfus Na(s) ? Na(l) Standard Enthalpy of
Vapourization, DHvap Br2(l) ? Br2(g) Standard
Enthalpy of Sublimation, DHsub P4(s) ?
P4(g) Standard Enthalpy of Dissociation, DHd
½ Cl2(g) ? Cl(g) Standard Enthalpy of
Solvation, DHsol Na(g) ? Na(aq)
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Why should we care about these enthalpies? They
will provide us information about the strength
of bonding in both molecules and extended solids.
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Free Energy Change, DG DH - TDS At STP DG
DH - (298.15 K) DS The two factors that
determine if a reaction is favourable If it
gives off energy (exothermic) DH SHproducts -
SHreactants DH lt 0 If the system becomes more
disordered DS SSproducts - SSreactants DS gt
0 If DG lt 0, then reaction is thermodynamically
favourable
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DG lets us predict where an equilibrium will lie
through the relationship DG -RT ln K
So if DG lt 0, then K gt 1 and equilibrium lies to
the right. There are three possible ways that
this can happen with respect to DH and DS.
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If both enthalpy and entropy favour the
reaction i.e. DH lt 0 and DS gt 0 then DG lt
0. S(s) O2(g) ? SO2(g) DH -292.9
kJ/mol TDS 7.5 kJ/mol DG
-300.4 kJ/mol If enthalpy drives the
reaction i.e. DH lt 0 and DS lt 0, but DH gt
TDS, then DG lt 0. N2(g) 3 H2(g) ? 2
NH3(g) DH -46.2 kJ/mol TDS -29.5
kJ/mol DG -16.7 kJ/mol If entropy
drives the reaction i.e. DH gt 0 and DS gt 0, but
DH lt TDS, then DG lt 0. NaCl(s) ? Na(aq)
Cl-(aq) DH 1.9 kJ/mol TDS 4.6
kJ/mol DG -2.7 kJ/mol