chem notes 11-9 - -highest energy e ALWAYS leaves 1 st-X E...

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November 9, 2007 Dr. Stevens Gen. Chem. 1 Periodic Trends -radius -based on PT location -trend goes down a group -shell # increases -trend across a period -same n across -the further right, the smaller the radius -increase to the right, increase to the left -largest radius = Fr -smallest radius = He -ionic radius -compare ions to parent neutrons for size -X+ is ALWAYS smaller atom -b/c same + nuclear q, which needs to pull in less e- -isoelectronic -Na+ Ne -Na+ < Ne -Na+ has more pos. nucleus trying to pull in same # e- -X- islarger radius, b/c same nuclear charge can’t pull in extra e- -ionization energy -energy needed to remove an e- from a gaseous atom in its ground state
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Unformatted text preview: -highest energy e- ALWAYS leaves 1 st-X + E e- + X+-IE strongly radius dependent-as radius increases, IE decreases-IE is opposite of radius-Fr has smallest IE-Fl has largest-Why is IE of B slightly less than Be?-Be 2s2-Be+ 2s1-B 2s2 2p1-B+ 2s2-Boron stabilized and Beryllium became unstable-lower stability = more energy-Why is IE of O slightly less than N?-same reason as B and Be-O makes it easier to lose e- b/c going to half-full state is easy-Electron Affinity-the negative E charge that occurs when an e- is accepted by an atom to form the anion-X + e- X-...
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This note was uploaded on 04/23/2008 for the course CH 151 taught by Professor Stevens during the Fall '08 term at Whitworth University.

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