CHEM 111 Lecture Notes - Transition Metal, Noble Gas, Electron Configuration

58 views3 pages
10 Mar 2014
School
Department
Course
Professor

Document Summary

2 parts: final refined model of the atom and initial bonding. Remember, there is stability in sets of full orbitals. The noble gases are unreactive for this very reason. Main group ions form to be isoelectric with (have the same electron configuration as) the noble gases. Mainly involves groups 1a, 2a, 6a, and 7a. Ionization to noble gas configuration involves a lot of energy. C group ions (4+ or 4-) almost never form. B group ions (3+) and n group (3-) These atoms tend to share electrons to gain a full set of orbitals. The d block alters how these atoms ionize. Too many electrons to lose to get to noble gas config. They will lose electrons to a full d10. Main group ions form by adding or removing electrons from the orbitals in the highest energy shell. Same thing is true here, even though we have a partially filled d block. First, remove electrons in the n s orbital.