Nomenclature

1. Nomenclature Learn to name binary compounds of a metal and a nonmetal. Learn how to name binary compounds containing only nonmetals. Learn the names of common polyatomic ions and how to use them in naming compounds. Learn names for common acids and how the anion composition determines the acids name. Learn to write the formula of a compound, given its name.

2. Naming compounds • Common names are Epsom salts, milk of magnesia, laughing gas, and many more • There are over 4 million different compounds and more are discovered all the time • Memorizing the common names would be impossible so we have a system

3. Binary compounds • Compounds composed of 2 elements • Two types: • Compounds that contain a metal and nonmetal • Compounds that contain 2 nonmetals

4. Naming Compounds That Contain a Metal and a Nonmetal To learn to name binary compounds of a metal and a nonmetal.

5. Binary Ionic Compound • Contain a positive ion (cation) and a negative ion (anion) • Two types of binary ionic compounds • Type I: contain elements with only one ion • Na+, Cs+, Ca+2, etc • Type II: contain elements with 2 or more ions • Cr+2 or Cr+3, Cu+ or Cu+2

6. Type I Binary Ionic Compounds • The cation is always named 1st • The cation is named as the element name • Na+ is sodium • The anion is named by taking the 1st part of the element name and adding –ide • Cl- is chloride

7. NaI sodium iodide CaO calcium oxide NaCl sodium chloride KI potassium iodide CaS calcium sulfide CsBr cesium bromide MgO magnesium oxide CsF cesium fluoride AlCl3 aluminum chloride MgI2 magnesium iodide Rb2O rubidium oxide SrI2 strontium iodide K2S potassium sulfide Type I Binary Ionic Compounds

8. Type II Binary Ionic Compounds • Some metals can produce 2+ ions • When this happens, we use Roman Numerals • The Roman numerals only tell us the charge, not how many of that ion there are in the compound • You do not need to use Roman numeral for metals that form only 1 cation

9. Type II Binary Ionic Compounds • What is FeCl2 made of? • Fe+2 and two Cl- • What would we name it? • Iron (II) chloride • What is PbO2 made of and what is its name? • Pb+4 and 2 O-2 called lead (IV) oxide

10. Type II Binary Ionic Compounds • Write out the following and give their name • CuCl • copper (I) chloride • HgO • mercury (II) oxide • Fe2O3 • iron (III) oxide • MnO2 • manganese (IV) oxide • PbCl4 • lead (IV) chloride

11. Review Type I and II • CoBr2 • Co+2 + Br- cobalt (II) bromide • CaCl2 • Ca+2 + Cl- calcium chloride • Al2O3 • Al+3 + O-2 aluminum oxide • CrCl3 • Cr+3 + Cl- chromium (III) chloride

12. Naming Binary Compounds That Contain Only Nonmetals (Type III) To learn how to name binary compounds containing only nonmetals.

13. The 1st element in the formula is named 1st and the full element name is used. The 2nd element is named as though it were an anion. Prefixes are used to indicate the # of atoms present The prefix mono- is never used for the 1st element Prefixes for Type III mono- 1 di- 2 tri- 3 tetra- 4 penta- 5 hexa- 6 hepta- 7 octa- 8 Rules for naming Type III

14. Type III • BF3 • notice they are both nonmetals • Name the 1st element – boron • Name the 2nd as an anion – fluoride • Add prefixes • boron trifluoride

15. NO nitrogen monoxide N2O3 dinitrogen trioxide CCl4 carbon tetrachloride NO2 nitrogen dioxide IF3 iodine trifluoride I2O7 diiodine heptoxide CO2 carbon dioxide CF4 carbon tetrafluoride NH3 nitrogen trihydride PCl3 phosphorous trichloride Practice Problems

16. Naming Binary Compounds: A Review To review the naming of Type I, II, and III binary compounds.

17. Naming binary compounds Binary Compound? Yes Metal Present? No Yes Type III: Use prefixes Does the metal form more than one cation? Yes No Type II: Determine the charge of the cation; use a Roman numeral after the cation Type I: Use the element name for the cation

18. AsF3 arsenic trifluoride Al2S3 aluminum sulfide SnBr4 tin (IV) bromide CS2 carbon disulfide CdS cadmium sulfide AgCl silver chloride KI potassium iodide NO nitrogen monoxide P2O5 diphosphorous pentoxide FeCl3 iron (III) chloride Type I, II, III

19. Naming compounds with polyatomic ions • Simply write the name of the polyatomic ion • No change is needed • What would NH4C2H3O2 be called? • Look at the table • NH4 – ammonium • C2H3O2 – acetate • Put the them together in the same order as the formula • Ammonium acetate

20. Naming compounds with polyatomic ions • If using a cation with more than one charge, use Roman numerals • Fe(NO3)3 • The 2nd 3 tells us that there are 3 NO3 in the formula • Looking on our chart we see NO3 has a charge -1 • If they’re totaled, that makes our total charge -3 • Fe must be +3 to cancel it out • Iron (III) nitrate

21. Na2SO4 sodium sulfate KH2PO4 potassium dihydrogen phosphate Mn(OH)2 Manganese (II) hydroxide Na2SO3 sodium sulfite Cu(NO3)2 Copper (II) nitrate PbCO3 Lead (II) carbonate KHSO4 potassium hydrogen sulfate NH4I ammonium iodide NaCN sodium cyanide Polyatomic Practice

22. Naming Chemical Compounds Binary Compound? Yes No Metal Present? Polyatomic Ion or Ions Present? Yes No No Yes Type III: Use prefixes Does the metal form more than one cation? We will learn this procedure later. Name the compound similar to naming binary compounds but use the polyatomic chart for their names No Yes Type I: Use the element name for the cation Type II: Determine the charge of the cation; use a Roman numeral after the cation

23. Na2CO3 FeBr3 PCl3 CsClO4 CuSO4 NaHCO3 BaSO4 CsClO4 BrF5 NaBr KOCl Zn3(PO4)2 Ca(HCO3)2 MgI2 KMnO4 Sb2O3 Fe(OH)2 Name the following chemical compounds to be turned in for a grade

24. Na2CO3sodium carbonate FeBr3iron (III) bromide PCl3phosphorous trichloride CsClO4 cesium perchlorate CuSO4 copper (II) sulfate NaHCO3 sodium hydrogen carbonate BaSO4 barium sulfate CsClO4 cesium perchlorate BrF5 bromine pentafluoride NaBr sodium bromide KOCl potassium hypochlorite Zn3(PO4)2 zinc (II) phosphate Ca(HCO3)2 calcium hydrogen carbonate MgI2 magnesium iodide KMnO4 potassium permanganate Sb2O3 antimony (III) oxide Fe(OH)2 iron (II) hydroxide

25. Naming Acids To learn how the anion composition determines the acid’s name To learn names for common

26. Acids • A molecule w/ one or more H+ ions attached to an anion • The rules for naming acids depend on whether it has oxygen

27. Rules for naming acids • If no oxygen is present • Add prefix hydro- and suffix –ic to the root word and the word acid to the end • HCl • hydro + chlorine + ic + acid • hydrochloric acid

28. Rules for naming acids • If oxygen is present • Named after the anion present • When anion ends in –ate • Add suffix –ic and the word acid • H2SO4 • sulfate becomes sulfuric acid • When anion ends in –ite • Add suffix –ous and the word acid • HNO2 • nitrite becomes nitrous acid

29. Naming Acids Does the anion contain oxygen? No Yes hydro- +anion root + -ic hydro(anion root)ic acid Check the ending of the anion name -ite -ate anion or element root + -ous (root)ous acid anion or element root + -ic (root)ic acid

30. Acid Practice • HF • Hydrofluoric acid • H3PO3 • Phosphorous acid • HNO3 • Nitric acid • HBrO3 • Bromic acid • H2S • Hydrosulfuric acid

31. Writing Formulas from Names To learn to write the formula of a compound, given its name

32. Formulas from names • So far you were given a name and you gave the formula • A lot of times the reverse is also necessary • calcium hydroxide • Ca+2 OH- • You will need 2 hydroxide ions to cancel out the +2 charge of Ca • Ca(OH)2 • iron (II) oxide • Fe+2 O-2 • The +2 and -2 cancel each other out • FeO