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CHEM 111 (69)

Main group ions, transition metal ions, paramagnetism, diamagnetism, ionic size

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CHEM 111
Dana Johnson

27 September Ch 8 problems 6, 9, 11, 20, 21, 25, 29, 33, 37, 41, 53, 54, 64, 74, 78, 86 Announcements Model assignment due Wednesday (9/29) Beginning of class 2 parts: final refined model of the atom and initial bonding Early Check Scores are incorrect Corrected scores are up now All 3 exam versions are now posted Main group ions 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 1A & 2A lose electrons 6A & 7A gain electrons Ne = 1s 2s 2p 6 2 2 6 1 2 2 6 - Na = 1s 2s 2p 3s → 1s 2s 2p + e F = 1s 2s 2p + e → 1s 2s 2p2 2 6 Light atoms in 3A, 4A, and 5A 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-) Not common, but possible These atoms tend to share electrons to gain a full set of orbitals Heavy atoms in 3A, 4A and 5A The d block alters how these atoms ionize Too many electrons to lose to get to noble gas config 10 They will lose electrons to a full d Called a “pseudo-noble gas configuration” 2 10 1 In = [Kr] 5s 4d 5p In = [Kr] 5s 4d 10 3+ 10 In = [Kr] 4d Transition metal ions Main group ions form by adding or removing electrons from the orbitals in the highest energy shell Same thi
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