1. Naming Chemical Compounds Chemical Nomenclature From the Latin: Nomen – name calare – to call 10 million known chemicals

2. Naming Ionic Compounds Naming Rules Cations Rule 1: Cations formed from metal ions have the same name as the metal.( positive ion) Write the name of the first element Example K + potassium Zn 2+ zinc

3. Rule 2: Cations that form can form different charges, use a Roman numeral Example Fe 2+ iron(II) Fe 3+ iron(III) Use the table on p364 in your text book!

4. Anions Rule 3: Anions( negative ion) drop the ending of the elemental name and add ------- ide. Example H - hydride O 2- oxide Rule 4: Polyatomic anions containing oxygen have names ending in -----ate or -------ite Use the table on p366 in text book (you do not have to memorize these) Example NO 3 - nitrate Remove 1 oxygen atom NO 2 - nitrite a.k.a. oxyanions

5. Naming the Ionic Compound Cation - Anion BaBr 2 Al(NO 3 ) 3 Al(NO 2 ) 3 CuSO 4 Mg(ClO 4 ) 2 Fe(HCO 3 ) 3 barium bromide aluminum nitrate aluminum nitrite copper(II) sulfate magnesium perchlorate iron(III) hydrogen carbonate

6. Let’s Go The Other way potassium sulfide calcium hydrogen phosphate nickel(II) hypochlorite sodium peroxide strontium nitride sodium oxide ammonium sulfide K2SK2S CaHPO 4 Ni(ClO) 2 Na 2 O 2 Sr 3 N 2 Na 2 O (NH 4 ) 2 S

7. Special Cases for oxygenated halogens Add 1 extra oxygenClO 4 - perchlorate BaseClO 3 - chlorate Less 1 oxygenClO 2 - chlorite Less 2 oxygenClO - hypochlorite ****Use for FO 3 -, ClO 3 -, BrO 3 -, and IO 3 -

8. Rule 6: Adding H + to an oxyanions. CO 3 2- carbonate HCO 3 - hydrogen carbonate PO 4 3- phosphate HPO 4 2- hydrogen phosphate H 2 PO 4 - dihydrogen phosphate H + reduces the charge

9. Naming Inorganic Acids Acid – A substance which yields hydrogen ions(H + ) when dissolve in water. All acids will begin with an “H” as the first element. Example: HNO 3 HCl

10. Rule 1: Acids based on anions whose name ends in -------ide uses hydro as a prefix and -----ic as a suffix Example HCl hydrochloric acid H 2 S hydrosulfuric acid ***These types of acids are called binary acids.

11. Rule 2: Acids based on anions whose names in -----ate uses -----ic as a suffix Example HClO 3 chloric acid H 3 PO 4 phosphoric acid Rule 3: Acids based on anions whose name ends in -----ite uses -----ous as a suffix Example HClO 2 chlorous acid H 2 SO 3 sulfurous acid

12. Naming Binary Molecular Compounds ( covalently bonded atoms-nonmetals) Rules 1.The first shown element is named as the element( example-CO---carbon is the first element) 2.The name of the second element is given an -----ide ending. 3. The second element always carries a prefix indicating the # of times it is present-example CO 2 dioxide. 4. The amount of the first element is only shown if it is present more than once.

13. 4. Greek prefixes are used to indicate the number of atoms of each element mono1 di2 tri3 tetra4 penta5 hexa6 hepta7 octa8 nona9 deca10

14. 5.The prefix “mono” is never used with the first element. 6. When a prefix ends in “a” or “o” and the name of the second element begins with a vowel, the “a” or “o” is often dropped.

15. Examples OCl 2 NF 3 P 4 S 10 SO 2 PCl 5 N2O3N2O3 The other way Silicon tetrabromide Disulfur dichloride Triphosphorus monoxide Oxygen dichloride Nitrogen trifluoride Tetraphosphorus decasulfide Sulfur dioxide Phosphorus pentachloride Dinitrogen trioxide SiBr 4 S 2 Cl 2 P3OP3O