Inorganic Chemistry CHEM 3010
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This 2 page Class Notes was uploaded by Vesta Rippin on Monday October 12, 2015. The Class Notes belongs to CHEM 3010 at Georgia College & State University taught by Julia Metzker in Fall. Since its upload, it has received 7 views. For similar materials see /class/221954/chem-3010-georgia-college-state-university in Chemistry at Georgia College & State University.
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Date Created: 10/12/15
CHEM 3010 Name Fall 05 Final Exam Study Guide List of wordstopics you may encounter on the final exam Some of these things have not been discussed in lecture Introduction Atomic amp Bonding Theories CH 1 CH 3 H a Quantum numbers b Orbitals 0 Electron configurations d DiamagneticParamagnetic e Isoelectronic f Molecular shape Bond angle 2 S mmetry Group Theory amp Molecular Orbital Theory CH 4 CH 5 a Polarity b Molecular orbital diagram 0 Bond order d DiamagneticParamagnetic e HOMOLUMO f Frontier orbitals g Isolobal h Point group i Symmetry element j Spectroscopic State 3 Acid Base Chemistry amp The Solid State CH 6 CH 7 a Stoichiometry b Lattice energy Born Haber cycle 0 Band theory semiconductor conductor insulator d Acid Base definitions Bronsted Lewis Solvent e HSAB theory f Keq 4 Coord39nation Chemistry CH 9 CH 10 a Electrochemistry oxidant reductant b Oxidation state c Chiral d Isomers e J ahn Teller distortion f Ligand field amp Crystal Field theory g Magnetic moment h Inert complex i Labile ligands j Chelate effect k Oxidative addition 1 NMR IR 5 Main Group Chemistry CH 8 a Acidic oxides b Halides c Nitrides Dr J Metzker 3010ACSFinalReViewdoc Page 1 of 3 CHEM 3010 Name Fall 05 Final Exam Study Guide Study Guide from last year 1 9 94 0 gt1 9 Dr J Metzker 3010ACSFinalReview doc Define and give an example for the following terms a chelate effect b isoelectronic c isolobal d paramagnetic e diamagnetic f semiconductor g Lewis acid h Lewis base Draw the molecular orbital splitting diagram for a homonuclear diatomic Is 02 expected to be paramagnetic or diamagnetic a Give the electronic configuration for 02 02 02 b order these species in order of increasing O O bond length Review the MO diagram planar and pyramidal CH3 Give the stoichiometry of an ionic solid with the following unit cells a rock salt b perovskite c wurtzite Review the concept of lattice energy The exam does not ask you to calculate lattice energy You need to know what properties of a solid give it a low or high lattice energy to be able to answer the question which solid has the highest molar lattice energy a Which enthalpy in the born haber cycle provides the greatest contribution to the stability of an ionic solid How would the resistivity of the following solids change with increasing temperature a metallic b semiconductor c superconductor Read the following paragraph and use these ideas to answer the questions below Soft acids are defined as electron pair acceptors Lewis acids in which the acceptor atom has a zero or low positive charge and a relatively large size These characteristics give rise to low electronegativity and high polarization of valence electrons meaning soft acids are easily oxidized Hard acids have the opposite characteristics that result in low polarization of valence electrons Soft bases are electron pair donors Lewis bases in which the donor atom similar to a soft acid has a high polarizability Hard bases have a donor atom with the opposite characteristics a Define the trends for hardsoft acids in terms of the periodic table b Define the trends for hardsoft bases in terms of the periodic table Page 2 of3