1. Naming Chemical Compounds Binary Compounds of Metals with Fixed Charges (Ionic Compounds) Covalent Compounds of Nonmetals: The Greek System Binary Compounds of Cations with Variable Charges: Stock System

2. Naming Chemical Compounds Binary Compounds of Cations with Variable Charges: Common Name System Polyatomics Acids Hydrates

3. Binary Compounds of Metals with Fixed Charges Name the cation first then the anion Use the cation’s fixed charge directly from the periodic table (eg. Ca +2 is Calcium) Name the anion using the root of the element’s name plus the suffix “ide” (eg. S -2 would be Sulfide) Examples: CaS would be Calcium Sulfide Na 2 O would be Sodium Oxide Potassium Chloride would be KCl

4. Covalent Compounds of Nonmetals: The Greek System Name the first element: if there are two or more, add a prefix to match the subscript Name the second element also using a prefix to match the subscript (including “mono-” for one) Prefixes: one=“mono-”, two=“di-”, three=“tri-”, four=“tetra-”, five=“penta”, six=“hexa-”, seven=“hepta-”, eight=“octa-”, nine=“nona-”, ten=“deca-”

5. The Greek System Example 1: N 2 O Subscript for 2 is “di-” so it is dinitrogen Subscript for O is 1 so the name is dinitrogen monoxide Example 2: N 2 O 5 Subscript for nitrogen is 2 so it is dinitrogen Subscript is 5 for oxygen or pentaoxide The name is dinitrogen pentaoxide (pentoxide is also acceptable)

6. Binary Compounds of Cations with Variable Charges: The Stock System Named for German chemist Alfred Stock Cations involved have at least two charges Anion has one charge Uses parentheses and roman numerals Example: FeCl 2 is iron(II) chloride

7. The Stock System Name the cation’s element first Determine the charge by multiplying the anion’s charge by it’s subscript; then divide this by the cation’s subscript Example 1: Name CuCl 2 Chloride anion’s charge is -1 times it’s subscript 2 equals 2 (Ignore sign of -2) Divide by Copper’s subscript of 1 equals 2 The result is Copper(II) chloride

8. The Stock System Example 2: Name Fe 2 O 3 Oxide anion’s charge is -2 times it’s subscript 3 equals -6 Divide by Iron’s subscript of 2 equals 3 The result is iron(III) oxide Example 3: Give the formula for manganese(IV) oxide The cation’s charge is given from the formula +4 Oxide’s charge is -2; Since the charge of the final formula must be zero, two oxides or 2 times -2 equals -4 gives zero net charge The result is MnO 2

9. Binary Compounds of Cations with Variable Charges: The Common Name System Proposed by Lavoisier “Father of Modern Chemistry” Uses the Latin root of the cation plus –ous or –ic suffix to indicate oxidation state (-ous is lowest, -ic is highest)

10. The Common Name System Find the root name of the first element Iron=“ferr-“, chromium="chrom-“, lead="plumb-”, tin="stann-“, copper="cupr-“, cobalt="cobalt-“, gold="aur-“, manganese="mangan-“, mercury="mercur-“ Multiply the charge of the anion by its subscript (Ignore the sign) Divide by the cation’s subscript The lower of 2 values gives –ous; the higher -ic

11. The Common Name System Example 1: Fe 2 O 3 Multiply oxide’s -2 times the subscript 3 equals 6 (ignore the sign) Divide 6 by iron’s subscript by 2 equals 3 The result is ferric oxide (iron exists as +2 or +3) Example 2: Cu 2 S Multiply sulfide’s -2 times the subscript 1 equals 2 (ignore the sign) Divide by copper’s subscript 2 equals 1 The result is cuprous sulfide

12. The Common Name System Example 3: Ferrous Oxide Ferrous means +2 Oxide is -2 Use charge balance or criss-cross method to solve Fe +2 O -2 yields FeO Example 4: Stannic Phosphide Stannic means Sn +4 Phosphide is P -3 Sn +4 P -3 yields Sn 3 P 4

13. Polyatomics Naming can be either fixed or variable charges When more than one polyatomic ion is required, parenthesis must be used Example 1: Fe(NO 3 ) 2 Decide if the cation has a variable charge (iron does so you must determine the roman numeral) NO 3 has a -1 charge so iron must be +2 The name is iron(II) nitrate or ferrous nitrate

14. Polyatomics Example 2: Fe(OH) 3 Determine the charge of iron: Hydroxide is -1 so iron must be +3 The compound is iron(III) hydroxide or ferric hydroxide Example 3: Aluminum Phosphate Aluminum is a fixed-charge of +3 Phosphate ion is PO 4 -3 The formula is AlPO 4

15. Binary Acids Binary acids are hydrogen with a non-metal (binary acids include: HCl, HF, HBr, HI) “hydro-” STEM “-ic” is used (STEM comes from the anion) The word acid is added at the end Examples: HCl is hydrochloric acid (STEM is chlor) HF is hydrofluoric acid HBr is hydrobromic acid

16. Oxy (Ternary) Acids Contains hydrogen and a polyatomic ion Change the “ate” ending to “ic” and the “ite” ending to “ous” and add the word acid Polyatomic ion that ends in “ate” STEM –ic acid Example HClO 3 = chloric acid Polyatomic ion that ends in “ite” STEM –ous acid Example HClO 2 = chlorous acid

17. Oxy (Ternary) Acids Polyatomic ion with prefix “hypo” Hypo- STEM –ous acid Example HClO hypochlorous acid Polyatomic ion with prefix “per” Per- STEM –ic acid Example HClO 4 perchloric acid

18. Hydrates Compounds that have water in them General Formula AB. xH 2 O Name the compound (AB) and add the number of water molecules present (x equals the coefficient) Examples: CuSO 4. 5 H 2 O is copper(II) sulfate pentahydrate MgSO 4. 9 H 2 O is magnesium sulfate nonahydrate

19. Reference See these web sites for practice!!! http://dbhs.wvusd.k12.ca.us/webdocs/Nomencl ature/Nomenclature.htmlhttp://dbhs.wvusd.k12.ca.us/webdocs/Nomencl ature/Nomenclature.html http://www.woodrow.org/teachers/chemistry/lin ks/chem1/NamingComp.htmlhttp://www.woodrow.org/teachers/chemistry/lin ks/chem1/NamingComp.html