Nomenclature  We will be presenting this chapter a bit Chapter 6: different than the text book does. The Language of information is the same, so reading the text is still a good idea. But take a careful look at Chemistry the online notes for this chapter. (Nomenclature)  Check the nomenclature handout on my website (next to the Ch. 6 label – left side) CHM 130 GCC Chemistry  PRACTICE, PRACTICE, PRACTICE

Terms and Definitions Naming Flowchart

 Ionic compound = metal + nonmetals Is the compound ionic, covalent, or acid?  Covalent compound = nonmetals only, (aka molecular) Ionic: metal + nonmetal Covalent: 2 or more Acid:  Monoatomic ion = one atom w/charge nonmetals H…(aq) Is the metal a + - 2+ Is the Use prefixes to HCl(aq)  Na , Cl , Ca transition metal? nonmetal a identify how many of HBr(aq) poly- each element. atomic HF(aq)  Polyatomic ion = two or more atoms w/charge ion? Use Roman HNO3(aq) numerals to identify (listed on your Periodic Table – become familiar H2CO3(aq) the charge on the metal (except Ag+, H2SO4(aq) with them) Zn2+, Cd2+) 3- - 2-  PO4 , OH , CO3

Covalent/Molecular Compounds Examples

 Compounds with only nonmetals  CO2 is carbon dioxide  These are neutral compounds that do NOT have a charge. Name the following:  Use prefixes  CO • mono (1)  penta (5) • di (2)  hexa (6)  P O • tri (3)  hepta (7) 2 5 • tetra (4)  octa (8)  PF3  Prefix + 1st nonmetal; prefix + 2nd nonmetal + “ide”  IF7 Don’t use mono- if there’s only 1 of the 1st element  H2O

1 Practice Covalent/Molecular Naming Element Names

 Br3O8  Know the names for elements 1-20 AND

 P4S7 Iron: Fe Silver: Ag  SO 3 Cobalt: Co Tin: Sn  iodine hexafluoride Nickel: Ni Iodine: I Copper: Cu Barium: Ba  dichlorine pentaoxide Zinc: Zn Gold: Au

 P2I4 Bromine: Br Mercury: Hg Strontium: Sr Lead: Pb

Ionic Compounds Oxidation States  We’ll start by learning charges of ions and  Oxidations states are determined similar to how to write formulas for ionic compounds. charges of ions.  Remember that ionic compounds are made of  All elements have a charge of zero when they ions, and ions have a charge. are alone (elemental state - ex: Zn(s), H2(g), Br2(l))  The sum of the charges must equal zero.  Elements have a charge only have they react and lose or gain electrons!  Some elements have a fixed charge – only one possibility (e.g., Na+, Cl-, etc.)  Other elements have variable charge – several possibilities (e.g., Fe 2+ and Fe3+)

Metal Cations (+) Nonmetal Anions (-)  Metals lose electrons to become cations (+)  Nonmetals gain electrons to become anions (-)  Charges (learn these)  Charges (learn these) • Column IA is always +1 (alkali metals) • Column 5 is usually –3 • Column IIA is always +2 (alkaline earth metals) • Column 6 is usually –2 • Column 7 is usually –1 (F always) • Column IIIA is often +3 (Al3+ always) • Column 8 is 0 Why??? • Zn and Cd always +2 • Noble gases are already happy with 8 outer valence • Silver always +1 electrons (He has 2 v. e.), so they don’t need to form bonds. • Other metals can vary from +1 to +9 so use Roman They don’t easily gain or lose electrons!!! Numeral to tell the difference; Cu+2 is copper(II), Fe+3 is iron(III), Pb+4 is lead(IV)

2 6.3 Polyatomic Ions Formulas of Ionic Compounds  Check out information on your periodic table  Compounds MUST be neutral – lower left corner.  Need enough cations and anions to have an  Keep these atoms together as a group, think overall zero charge of them as a group, a single unit.  Combine Na and N  Na is +1; N is –3 so we need three Na’s for one N  LEARN THESE. Be familiar with them  Na N is the formula (formulas and names). 3  Practice: Write the formula for ions of Rb and 2- 2- 3- -  Examples: CO3 , SO4 , PO4 , OH S.  Start by writing the charge of each ion.

Formulas of Ionic Compounds Formulas with Polyatomic Ions What will the formulas be when the following What will the formulas be when the following ions are combined? ions are combined? • Na and S • Mg and OH- • Mg and O 3- • K and PO4 • K and Br 2- • Ag and SO4 • Ca and N • Ca and NO - • Al and Cl 3 • Cu(II) and CO 2- • Zn and I 3 • Cu(II) and O • Pb(IV) and O

Naming Ionic Compounds Ionic Compounds: Fixed Charge Cation

 Now that we can write ionic compound  For a fixed charge metal, like Na, it can only formulas, we can name them. have one possible charge so we don’t use Roman numerals  Naming the cation (metal) depends on whether  Metal name + nonmetal-“ide” it has a fixed or variable charge. • NaCl sodium chloride  Naming the anion (nonmetal) depends on • Name the following: whether it is a single atom ion or polyatomic • KBr ion. • MgO • CaF2  Metal + nonmetal (NO prefixes: the charges on • Li S ions determines how many we need.) 2 • AgCl

3 Ionic Compounds: Variable Charge Cation Ionic Compounds: Polyatomic Ions  For a variable charge metal, like Cu, the charge  Do NOT change the polyatomic ion name can vary so we do use Roman numerals • NaNO3  Metal (Roman #) + nonmetal-“ide”  YOU must figure out charge on transition metal • Name the following: • Name CuCl 2 • K3PO4 • Name the following: • Ca(OH)2 • PbO2 • ZnSO4 • FeBr3 • CoS • HgBr • CoN

Ionic Compounds: Review Ionic Compounds: Review  YOU must be able to figure out the formula  Prefixes are ONLY with covalent compounds AND the name for ionic compounds.  Roman Numerals are ONLY with variable  Example: K and O charged metal compounds (in ionic • What is the correct formula? compounds) • What is the correct name?  Transition metals (except Zn2+, Cd2+, Ag+) 2+ 4+ 2+ 4+  You need to practice writing formulas from  Main group metals (except Pb / , Sn / ) names and names from formulas; this applies  Polyatomic ions NEVER change their name to covalent and ionic compounds. OR CHARGE

Naming Acids What does  Compounds that lower pH in water by producing H+ ions. (aq) mean?  Acids are always dissolved in water = (aq)  You need to know these 6 acids: • HCl(aq) hydrochloric acid • HF(aq) hydrofluoric acid

• H2SO4 (aq) sulfuric acid

• H3PO4 (aq) phosphoric acid

• HNO3 (aq) nitric acid

• H2CO3 (aq) carbonic acid

4 Nomenclature Practice: 3 minutes! Ch. 6 Self Test, p. 187 Try 3, 4, 6, 9, 11  BaCl2 Answers in Appendix J  NO2

 Fe3(PO4)2 •Do the chapter 6 worksheet posted on my and  diiodine tetraoxide Dr. Kim’s web pages  silver sulfate •Seriously – JUST DO IT  nickel(III) sulfide http://web.gccaz.edu/~kimld88531/rev130_files /Nomenclature.pdf

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