Lacey_Che131_F2011_Lect-27p

Lacey_Che131_F2011_Lect-27p - Lec Lec-27: Resonance &...

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Lec-27: Resonance & Formal Charge Lec 27: Resonance & Formal Charge Roy A. Lacey, Stony Brook University; Che 131, Fall 2011 1 Recap Roy A. Lacey, Stony Brook University; Che 131, Fall 2011 2
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Drawing Lewis Structures Hydrogen and the halogens bond once Additional handy rules ± Hydrogen and the halogens bond once. ± The oxygen group bonds twice. ± The nitrogen group bonds three times. So does boron. The carbon group bonds four times ± The carbon group bonds four times. Roy A. Lacey, Stony Brook University; Che 131, Fall 2011 3 Drawing Lewis Structures NO 2 + #valence electrons = 16 i) Draw skeletal structure ii) Satisfy octet rule [ ] ONO + == Roy A. Lacey, Stony Brook University; Che 131, Fall 2011 4
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A. 1 nonbonding pair on carbon B 2 nonbonding pairs on nitrogen #ve = 10 B. C. 1 nonbonding pair on nitrogen D. 2 nonbonding pairs on carbon 5 Roy A. Lacey, Stony Brook University; Che 131, Fall 2011 Bond Types Electrons are shared equally only in pure covalent bonds Roy A. Lacey, Stony Brook University; Che 131, Fall 2011 6
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Electronegativity ` Electronegativity is a measure of an element’s ability Electronegativity is a measure of an element s ability to attract bonding electrons. It is used for predicting the degree to which bonding pairs of electrons are shared unequally. Roy A. Lacey, Stony Brook University; Che 131, Fall 2011 7 Electronegativity Increase se Increa Note the periodic trend of electronegativity Roy A. Lacey, Stony Brook University; Che 131, Fall 2011 8
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Electronegativity ` Changes in electronegativity are related to increasing atomic size.
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This note was uploaded on 11/18/2011 for the course CHE 131 taught by Professor Kerber during the Spring '08 term at SUNY Stony Brook.

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Lacey_Che131_F2011_Lect-27p - Lec Lec-27: Resonance &...

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