Difference between revisions of "Name Ionic Compounds"
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== Steps == | == Steps == | ||
=== Basic Ionic Compounds === | === Basic Ionic Compounds === | ||
| − | #Write down the formula of the ionic compound. Let's say the ionic compound you're working with is ''NaCl.''<ref>http://www.youtube.com/watch?v=7Lfc6jjp1WQ</ref> | + | #Write down the formula of the ionic compound. Let's say the ionic compound you're working with is ''NaCl.''<ref name="rf1">http://www.youtube.com/watch?v=7Lfc6jjp1WQ</ref> |
#Write the name of the metal, or the cation.This is the positively charged ion in the compound, and it is always written first in ionic compound formulas. ''Na'' is sodium. So, write ''Sodium.'' | #Write the name of the metal, or the cation.This is the positively charged ion in the compound, and it is always written first in ionic compound formulas. ''Na'' is sodium. So, write ''Sodium.'' | ||
#Write the name of the nonmetal, or the anion, with the "-ide" ending. ''Cl'' is chlorine. To add the "ide" ending, just drop the last syllable, "-ine," and add "-ide" instead. Chlorine becomes ''chloride.'' | #Write the name of the nonmetal, or the anion, with the "-ide" ending. ''Cl'' is chlorine. To add the "ide" ending, just drop the last syllable, "-ine," and add "-ide" instead. Chlorine becomes ''chloride.'' | ||
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#*MgCl<sub>2</sub> = ''Magnesium chloride'' | #*MgCl<sub>2</sub> = ''Magnesium chloride'' | ||
=== Transition Metals === | === Transition Metals === | ||
| − | #Write down the formula of the ionic compound. Transition metals can be found in the middle of the periodic tables. They get their name because their oxidation numbers, or their charges, are constantly changing. Let's say you're working with this compound: Fe<sub>2</sub>O<sub>3</sub>.<ref | + | #Write down the formula of the ionic compound. Transition metals can be found in the middle of the periodic tables. They get their name because their oxidation numbers, or their charges, are constantly changing. Let's say you're working with this compound: Fe<sub>2</sub>O<sub>3</sub>.<ref name="rf1" /> |
#Write down the charge of the metal. You know that the metal will have a positive charge, so cross over the 3 from the ''O<sub>3</sub>'' and write that ''Fe'' has a charge of +3. (For fun, do the reverse and write that ''O'' has a charge of -2.) Sometimes, the charge will be provided for you. | #Write down the charge of the metal. You know that the metal will have a positive charge, so cross over the 3 from the ''O<sub>3</sub>'' and write that ''Fe'' has a charge of +3. (For fun, do the reverse and write that ''O'' has a charge of -2.) Sometimes, the charge will be provided for you. | ||
#Write down the name of the metal. Since you know that ''Fe'' is iron and that it has a charge of +3, you can call it ''Iron (III)''. Remember to only use the Roman numeral when you're writing out the name, not writing the formula. | #Write down the name of the metal. Since you know that ''Fe'' is iron and that it has a charge of +3, you can call it ''Iron (III)''. Remember to only use the Roman numeral when you're writing out the name, not writing the formula. | ||
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#Remember the exceptions. There are two transition metals that do have a definite charge. Those are zinc (Zn) and silver (Ag). This means that you don't have to use Roman numerals or the older naming method in describing those elements. | #Remember the exceptions. There are two transition metals that do have a definite charge. Those are zinc (Zn) and silver (Ag). This means that you don't have to use Roman numerals or the older naming method in describing those elements. | ||
=== Compounds with Polyatomic Ions === | === Compounds with Polyatomic Ions === | ||
| − | #Write the formula for the polyatomic ion. This compound will have more than two ions in it. Let's say you're working with the following compound: FeNH<sub>4</sub>(SO<sub>4</sub>)<sub>2</sub>.<ref>http://www.dummies.com/how-to/content/how-ionic-compounds-are-named.html</ref> | + | #Write the formula for the polyatomic ion. This compound will have more than two ions in it. Let's say you're working with the following compound: FeNH<sub>4</sub>(SO<sub>4</sub>)<sub>2</sub>.<ref name="rf2">http://www.dummies.com/how-to/content/how-ionic-compounds-are-named.html</ref> |
#Find the charge of the metal. You'll have to do some math to find it. First, you know that the sulfate, or the SO<sub>4</sub> ion has a charge of -2, and that there are two of them because of the 2 below the parenthesis. So, 2 x -2 = -4. Then, you know that the NH<sub>4</sub>, or the ammonia ion, has a charge of +1. Add up -4 and 1 and you get -3. This means that the iron ion, Fe, must have a charge of +3 to make up for it and to make the compound neutral. | #Find the charge of the metal. You'll have to do some math to find it. First, you know that the sulfate, or the SO<sub>4</sub> ion has a charge of -2, and that there are two of them because of the 2 below the parenthesis. So, 2 x -2 = -4. Then, you know that the NH<sub>4</sub>, or the ammonia ion, has a charge of +1. Add up -4 and 1 and you get -3. This means that the iron ion, Fe, must have a charge of +3 to make up for it and to make the compound neutral. | ||
#Write the name of the metal. In this case you can either write ''Iron (III)'' or ''ferric.'' | #Write the name of the metal. In this case you can either write ''Iron (III)'' or ''ferric.'' | ||
