Presentation7_061009

Presentation7_061009 - Chem 6A Presentation #7 Overview...

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Chem 6A Presentation #7 2006-10-09 1 Overview Fundamentals D: Nomenclature of Compounds Naming ions and ionic compounds Naming covalent/molecular compounds Fundamentals E: Moles and molar masses
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2 Naming ions and ionic compounds Name of simple binary ionic compounds = { cation name} { anion name} {cation name} = {element name} {anion name} = {element root}+ide For example: sodium fluoride: NaF zinc sulfide: ZnS If the cation can have more than one charge, the charge is indicated in parentheses after the cation element name, e.g.: iron(III) oxide: Fe 2 O 3
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3 Naming ions and ionic compounds Cations are typically formed from metallic elements.
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4 Naming ions and ionic compounds Monoatomic anions are typically formed from nonmetals.
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5 Naming ions and ionic compounds Anions have a corresponding acid: H + {anion} The atoms of polyatomic anions are joined by covalent bonds.
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6 Naming ions and ionic compounds Anions have a corresponding acid: H + {anion}
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7 Naming ions and ionic compounds Hydrates: ionic compounds whose crystals contain a definite proportion of water molecules, e.g.: Copper(II) sulfate pentahydrate: CuSO 4 ·5H 2 O
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Presentation7_061009 - Chem 6A Presentation #7 Overview...

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