Chem 201 - 8.29.07

Chem 201 - 8.29.07 - Naming Binary Ionic Compounds –...

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CHEM 201 – August 29, 2007 Covalent Bonds – atoms that share electrons to form a molecule; always two non-metals Structural Formulas – O=C=O (Carbon Dioxide) Elements that exist as Molecules: N 2 O 2 F 2 Cl 2 Br 2 I 2 H 2 Ionic Bonding – atoms donate or accept an electron to form a salt (MgBr 2 – Magnesium Bromide) Polyatomic Ions – MEMORIZE Table 2.3 – covalently bonded atoms that are charged Acids – provide Hydrogen cation (H + ) in water Bases – provide a Hydroxide anion (OH - ) in water Naming Molecular Compounds – two non-metals name cation first name anion second (with –ide) add prefixes o mono-, di-, tri-, tetra-, penta-, hexa-, septa-, octa-, nona-, deca-
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Unformatted text preview: Naming Binary Ionic Compounds – Figure 2.11 Group 1A: +1 ions Group 2A: +2 ions Group 3A: +3 ions Group 4A: +2 ions or +4 ions Group 5A: -3 ions Group 6A: -2 ions Group 7A: -1 ions Transition Metals – name includes a roman numeral with column 4A All Molecules must have a charge equal to zero 1. cation keeps its name 2. anion gets an “ide” 3. metals with unknown cation get a roman numeral Charge on the M + are determined by the anion ClO – Hypochlorite ClO 2 – chlorite ClO 3 – chlorate ClO 4 – Perchlorate Naming Common Acids – Pure – HF – Hydrogen Flouride Aqueous – HF – Hydrofluoric Acid...
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This note was uploaded on 04/07/2008 for the course CHEM 201 taught by Professor Harris during the Fall '07 term at Bucknell.

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Chem 201 - 8.29.07 - Naming Binary Ionic Compounds –...

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