1. Rules for Naming Compounds and Writing Formulas

2. Naming Binary Ionic Compounds
Determine whether the element would lose or gain electrons when bonding to get a full outer energy level and determine the charge the ion would have resulting from losing or gaining electrons. (practice problems Ch 6 #2, 16-17)
Positive ions are called cations and negative ions are called anions. (practice problems #18-19)
Cations names are taken straight from the periodic table. For Anions names, the end of the name on the periodic table is replaced with “ide”. (practice problems #1, 8-9, 22-23)
When cations and anions come together to make a compound, the cation is always written first and capitalized and the anion is written second (practice problems #26-27)

3. Writing Binary Ionic Compound Formulas
Determine the charge of each element in the compound (can use pgs ).
Make the charges equal zero by adding the correct number of atoms for each element.
Write the cation first and anion second. (practice problems 24-25)
Ex: Oxygen O2- Sodium Na1+
Na2O

4. Naming Ternary Ionic Compounds
Use Polyatomic Ions, which are tightly bound groups of atoms that behave as a unit and carry a charge.
Most end in “ite” or “ate” and are listed in a table on pg 147.
Cations are written first and anions are written second just like binary ionic compounds. (practice problems and #12 in Ch 15)

5. Writing Ternary Ionic Compound Formulas
Follow the same rules as binary compounds except if you need more than one polyatomic atom.
Parentheses are used around polyatomic atoms when you need more than one to balance the charges. (Practice problem #28-29 and #11 in Ch 15)
Ex: Magnesium Mg2+ nitrate NO31-
Mg(NO3)2

6. Naming Molecular Compounds
Composed of molecules (covalent bonds), so ionic charges are not used to assign formulas or names to them.
When two non metallic compounds come together, they can form more than one compound. Ex: CO and CO2
Prefixes are therefore used to indicate these different compounds.
Mono-1 Tetra-4 Hepta Deca-10
Di-2 Penta-5 Octa-8
Tri-3 Hexa-6 Nona-9

7. Naming Acids
Acids are compounds that produce hydrogen ions when dissolved in water.
Acids are an anion connected to a hydrogen ion.
If it a monatomic anion, then you add “hydro” on the front, end it with “ic” and then add acid. Ex: HCl  Hydrochloric acid
If it is a polyatomic anion that end with “ate”, change ending to “ic” and add acid. Ex: H2SO4  Sulfuric acid.
If it is a polyatomic anion that ends with “ite”, change ending to “ous” and add acid. Ex: HNO2  Nitrous acid

8. Use flow charts on pg 161 and 162 to help you with naming and writing formulas