| -ate Polyatomic Ions: Formulas and Charges | ||||||||||||
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| IIIA/13 | IVA/14 | VA/15 | VIA/16 | VIIA/17 | ||||||||
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Click on the X in the Formula for the #oxygens |
Click on the Y- in the Formula for the charge |
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Intro To Polyatomic Ions The Problem -ite Rule -ide Rule Taylor's 3/4 -ate Rule Taylor's Charge Rule |
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Other -ate Polyatomic Ions Acetate Ion Hydrogen carbonate Ion Hydrogen phosphate Ion Hydrogen sulfate Ion Chromate Ion Dichromate Ion Dihydrogen phosphate Ion Permanaganate Ion |
Polyatomic Ion Charts from Textbooks McMurray: Table 3.2 Silverberg: Table 2.5 Corwin: Table 7.03 Tillery: Table 9.3 Kotz: Table 3.1 Hill: Table 5.04 -ite & -ide Rule |
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Taylor's 3/4 Oxygen Rule O-All Border Three Rule: 0 1 2 3 4 5 6 7 8 9 Block of 4/6 Rule: 6-Both 1 2 3 4 5 6 6-All O-Both 5 6 O-None Transitional Metal O4 Rule: 0 1 2 3 4 5 6 7 8 T-All Dot Structures T-Both |
Taylor's Charge Rule O-All Single Bond Rule: 0 1 2 3 4 5 6 7 8 9 Double Bond Rule: 6-All 1 2 3 4 5 6-Both Hydrogen Rule: T-Both 1 2 3 O-None Transitional Metal -2 Rule: 0 1 2 3 4 5 6 7 8 T-All |
You should begin to see a relationship between the # of oxygens in the formula, and the position of the -ate ion on the periodic table. Continue clicking the #s 1-7 for three oxygens in Taylor's 3/4 Oxygen Rule to the left! Borate, Carbonate, Nitrate, and Chlorate each have three oxygens in the formula! Let's examine Group VIIA! (Click on #5 under Border 3 to the left) |
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