Lecture Notes for CHEM 362 - DESCRIP INORGANIC CHEM with Dunbar at Texas A&M (A&M)

Notes Information

Material Type:Class Note
University:Texas A&M University
  • Sp2 Hybridization
  • Either...or
  • Hybridization
  • Combination
  • Sp3 Hybridization
  • Unsaturated
  • Qualitative
  • Special Case
  • No Molecules
  • Valence Shell
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B. Electron Deficient (less than an octet) e.g. BeH2 H-Be-H Be does not need an octet Total of 4 valence electrons Not the same as unsaturated systems that achieve the 8e- (octet) through the formation of multiple bonds. C. Electron Rich (greater than an octet) Valence shell expansion occurs with elements beyond the 2nd row s, p, d levels are all available 2e6e- 10e→ total of 18e- possible e.g., transition metals have expanded electron counts, typically 18ereferred to as valence shell expansion PCl5 P 5eCl 7e- x 5 = 5e35e40e- Q. What about transition metals? A. They tend to exhibit 18e- valence shells (full s, p, d levels). They form bonds to lone pairs of molecules (called ligands) until they reach the 18econfiguration. Ex. Ni2+ compounds Ni has 10 valence electrons - it needs 4 bonds to reach 18 valence electrons. - Ni(CO)4 is a compound that illustrates this point. CO valence electrons :C ≡ O: (unsaturated) 4+6 = 10eLewis structure is this one to allow for an octet CO can then act as a ligand ...

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