Chapter 10

Chapter 10 - Chapter 10 Lewis theory Bonding of valence...

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Chapter 10 Lewis theory - Bonding of valence e- - ALWAYS A FULL ARROW regardless of no. of e moved - Electrons are transferred (ionic bonds) but mostly covalent - Full shell of 8 (octet) - Most ionic bonds form an ionic crystal Covalent bonding COORDINATE COVALENT? - nonmetals - Hydrogen only needs 2 electrons in its shell - Where a single atom contributes both electrons to the pair, once the bond is formed it is indistinguishable from the rest - Hydrogen-carbon IS NOT A POLAR BOND - More bonds = stronger - HALF FILLED D/ P SHELLS HAVE A SPECIAL STABILITY Polar covalent bonds/electrostatic potential maps - Electrons are closer to the nonmetal (more IE) - Bigger on the partial negative (nonmetal) side - Electronegativity is related to IE and EA (SAME DIRECTION); an atoms ability to compete for electrons w/ other atoms, high EN = nonmetal and vice versa - Big EN differ = ionic, small = covalent Writing Lewis structures - Valence e-/paired e/8 electrons (except H)/multiple bonds if needed - Hydrogen is always TERMINAL atoms - CENTRAL atoms are those with lowest EN - Carbon is always a central atom
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Chapter 10 - Chapter 10 Lewis theory Bonding of valence...

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