Lecture 11

Lecture 11 - CHM 115 Lecture 11 Lecture Reading was: KTT:...

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CHM 115 Lecture 11 Reading was: KTT: Sections 8.2, 8.4 - 8.6 Lecture 12: Section 8.9 Lecture 13: Section 8.6 Lecture
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2 Lewis Electron-dot Structures Number of dots = number of outer (valence) electrons Leave a maximum number unpaired. This is NOT the arrangement in some isolated atoms Rules: Depicting Valence Electrons in Main Group Atoms
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3 Non-metals (Groups 6A and 7A) Metals (Groups 1A and 2A) Li Mg Li + Mg 2+ [He]2s 1 [He] [Ne]3s 2 [Ne] [He]2s 2 2p 5 [He]2s 2 2p 6 = [Ne] [Ne]3s 2 3p 4 [Ne]3s 2 3p 6 = [Ar] Closed Shells Most atoms possess filled outer shells when bonded. In Ionic Compounds: : : . F : . . S : : F : : S 2–
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4 Ionic Bonding A tendency to form closed shells is observed during electron transfer Na [Ne] 3s 1 + Cl [Ne] 3s 2 3p 5 Na + [Ne] + Cl - [Ar] Na Cl Na + Cl - + or, in terms of Lewis electron dots
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5 Buddy Question #1 Let’s see what you remember about bonds between atoms. Covalent bonds can
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Lecture 11 - CHM 115 Lecture 11 Lecture Reading was: KTT:...

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