Editing Naming Ionic Compounds With Cation With More Than One Charge
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<center><b>Chemistry - Naming Ionic Compounds with Cation Ions of More than One Charge</b></center><br> <b>A. Chemical Name to Chemical Formula</b><br> 1. Write down the symbol(s) and charge of cation (look at Roman numeral for charge), then the anion. <br> 2a. The number of positive ions has to equal the number of negative ions. <br> 2b. Determine the number of each ion to make the charges equal. <br> 3. To get correct chemical formula **Each number of ions will be the subscript of the ion in the final chemical formula. **When writing chemical formula, never shows charges of ions. <i>Example: Chromium (III) sulfate</i><br> Step 1 Cr<sup>3+</sup> <nowiki>SO</nowiki><sub>4</sub><sup>2-</sup><br> Step 2 Need two cations, Cr<sup>3+</sup>, Cr<sup>3+</sup> and three anions,<nowiki>SO</nowiki><sub>4</sub><sup>2-</sup>, <nowiki>SO</nowiki><sub>4</sub><sup>2-</sup>, <nowiki>SO</nowiki><sub>4</sub><sup>2-</sup><br> Step 3 Cr<sub>2</sub><nowiki>(SO</nowiki><sub>4</sub>)<sub>3</sub><br> <i>More Examples:</i> Iron (III) nitride, Cobalt (IV) sulfite {Answer: Fe<sub>1</sub>N<sub>1</sub>, Co<sub>1</sub>(<nowiki>SO</nowiki><sub>3</sub>)<sub>2</sub>}<br> <b>B. Chemical Formula to Chemical Name</b><br> 1a.Write down the chemical name for the cation.<br> 1b. To determine the Roman numeral, need to determine the charge on the cation.<br> 1c. Figure out the anion charge, then find total negative charge (also total positive charge) and divide by the number of cations.<br> 2. Write down the chemical name for the anion.<br> <i>Example</i>: Sn<sub>1</sub><nowiki>(CO</nowiki><sub>3</sub>)<sub>2</sub><br> Step 1a Tin <br> Step 1b&c <nowiki>CO</nowiki><sub>3</sub> has 2- charge, there are 2 so -4 total charge=+4 charge, only one cation, therefore each Sn has 4+ charge<br> Step 2 Tin (IV) carbonate<br> <i>More Example</i>: Fe<sub>1</sub><nowiki>(OH</nowiki>)<sub>3</sub> (Answer: Iron (III) hydroxide)<br>
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