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Electronic Configuration Chemical Bonding Coordination

Electronic Configuration Chemical Bonding Coordination. Electronic Configuration of the Elements. www.nutrisci.wisc.edu/NS623/ electronic .pdf What determines how electrons are distributed? Pauli Exclusion Principle Hund’s Rule

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Electronic Configuration Chemical Bonding Coordination

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  1. Electronic ConfigurationChemical BondingCoordination

  2. Electronic Configuration of the Elements • www.nutrisci.wisc.edu/NS623/electronic.pdf • What determines how electrons are distributed? • Pauli Exclusion Principle • Hund’s Rule • Good web site: http://www.science.uwaterloo.ca/~cchieh/cact/c120/eleconfg.html

  3. Transition Elements

  4. Information on Transition Elementsor Why do we care? • http://library.thinkquest.org/3659/pertable/trametal.html

  5. Oxidation of Iron • Fe +2 Fe +3 • Ferrous Ferric • Reduced Oxidized • Reduction is the gain of electrons • Oxidation is the loss of electrons

  6. Bonding in minerals • Ionic • Covalent • Metallic • Van der Waals • Polar

  7. Ionic Bonding • NaCl (halite or rock salt) • Na+ and Cl- have noble gas configuration • Electrostatic attraction bonds them together • Minerals with ionic bonds have moderate H and G, have high melting points and are poor conductors of electricity and heat • Strength is proportional to the electronic attraction • Bond is non-directional

  8. Covalent • Sharing of electrons • Strongest of chemical bonds • Do not yield ions in solution • Bonds are directional • Example: diamond C

  9. Si-O bond • Is about 50% covalent and 50% ionic • Electronegativity—power of an atom to attract. Compounds made of elements with very different values of electronegativity are more ionic than compounds made of elemts clost to each other in electronegativity

  10. y = 1 - exp(-0.25 * x2) (Pauling, 1948)

  11. Metallic Bond • Many electrons owe no allegiance to any particular nucleus and are free to “drift” • Good conductors • Usually low hardness and melting points • Examples include native metals such as Cu, Ag, and Au • Minerals may have qualities of several types of bonds: galena ionic and metallic

  12. Van der Waals • Dipoles of molecules • Usually found in gases and liquids, rare in minerals • Example is graphite C

  13. Polar Bonding or Hydrogen Bonding Examples include micas

  14. Coordination Number C.N. • # of anions that can fit around a cation • NaCl 6 • CaF2 8

  15. Radius Ratio • This is the ratio of the radius of the cation to that of the anion • This ratio usually determines the CN of the cation

  16. Coordination Number vs Radius Ratio Make sure you remember to give examples on the board

  17. Let’s calculate one of the radius ratios • Use triangular coordination • Handout or on board!

  18. Some words you need to know • CN=4 tetrahedral • CN=6 octahedral • CN=8 cubic

  19. Pauling’s Rules • http://www.tulane.edu/~sanelson/eens211/paulingsrules.htm

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