2. Naming Ionics Stepwise Method for Naming Ionic Compounds 1.Name the metal first (ie. NaCl, sodium chloride) 2. The name of the nonmetal has -ide added (ie: NaCl sodium chloride) 3. If the metal has more than one possible charge, we must indicate which oxidation state (charge) is present using the Stock Method. Indicate the ion by writing the charge in roman numerals (ie: FeCl 2 Iron (II) chloride).

3. Examples using the Stock Method CompoundStock Method FeF 2 iron (II) fluoride FeF 3 iron (III) fluoride Hg 2 Br 2 mercury (I) bromide HgBr 2 mercury (II) bromide

4. Polyatomics Using a Polyatomic Ion to Determine the Charge on a Metal Consider Fe(OH) 2 1. Use the polyatomic ion to determine the charge of the metal, OH - is -1, 2 OH - ‘s in the formula therefore Fe must be +2 2. Name the metal using Stock Method, iron (II) (Fe) 3. Name the anion, hydroxide (OH - ) 4. Name the compound, iron (II) hydroxide Name of Ion FormulaCharge cyanideCN - sulfateSO 4 -2 -2 phosphat e PO 4 -3 -3 carbonat e CO 3 -2 -3 chromateCrO 4 -

5. Hydrates (this is new! Please copy) Many ionic compounds also have water molecules attached to the formula; these do not affect the name of the ionic compound; however we must have a way to account for them within the name. We refer to them as hydrates. We use the covalent prefixes to indicate the number of H 2 O molecules present in a hydrate. You will see this on the CSI sheet you got last day! NumberPrefix 1mono- 2di- 3tri- 4tetra- 5penta- 6hexa- 7hepta- 8octa- 9nona- 10deca- Consider CuSO 4. 5H 2 O copper (II) sulfate pentahydrate

6. Covalent Molecules ***Covalent molecules are typically made up of two or more non- metals and we cannot determine the number of atoms in a covalent compound simply by naming the first and second element.*** For example: carbon (C) and oxygen (O) can combine to form CO and CO 2 (also CO 3 2- but we will neglect this for the time being). If we were to use the ionic naming system we would get for each case carbon oxide, which does not tell the two molecules apart. To this end we need to use the prefixes: mono, di, tri, tetra etc. To name covalent compounds use the following method prefix + first element + prefix + root of second element + ide (the prefix "mono" is assumed, and therefore dropped)

7. Covalent Compounds To name covalent compounds use the following method prefix + first element + prefix + root of second element + ide Examples 1. SO 2 (sulfur dioxide) 2. Si 3 P 6 (trisilicon hexaphosphide) 3. BF 3 (boron trifluoride) 4. CO 2 (carbon dioxide) 5. S 5 F (pentasulfur fluoride) Exceptions: 1. H 2 O is water, not dihydrogen oxide. 2.NH 3 is ammonia, not nitrogen trihydride. 3. CO is carbon monoxide and N 2 O is dinitrogen monoxide but in all other cases, the mono is dropped.

8. Covalent Molecules PCl 5, phosphorus pentachloride BF 3, boron trifluoride S 4 N 4, tetrasulfur tetranitride

10. Naming Acids - copy An acid is a special kind of compound. When it is dissolved in water, an acid releases a hydrogen ion (H + ) into solution. Even though many acids are made from two non-metals (H and F, Cl, Br, I) we treat them as ionic compounds. We can tell a compound is an acid by indicating its state: o HCl (g) is hydrogen chloride gas o HCl (aq) is hydrochloric acid because (aq) means aqueous or dissolved in water

11. Naming Acids - copy Rule 1 - To name an acid if it is binary (having hydrogen and either F-, Cl-, Br- or I-) hydro ________ic acid (fluor, chlor, brom, iod) HBr (aq) is hydrobromic acid Rule 2 - To name an acid with a polyatomic ion Replace the suffix “ate” with “ic” and add “acid” to complete the name Replace the suffix “ite” with “ous” and add “acid” to complete the name HNO 3 (aq) (hydrogen nitrate, becomes “nitric acid”) HNO 2 (aq) (hydrogen nitrite becomes “nitrous acid”)