1. Copyright©2004 by Houghton Mifflin Company. All rights reserved. 1 Introductory Chemistry: A Foundation FIFTH EDITION by Steven S. Zumdahl University of Illinois

2. Copyright©2004 by Houghton Mifflin Company. All rights reserved. 2 Nomenclature Chapter 5

3. Copyright©2004 by Houghton Mifflin Company. All rights reserved. 3 Common Names - Exceptions H 2 O = water, steam, ice NH 3 = ammonia CH 4 = methane NaCl = table salt C 12 H 22 O 11 = table sugar

4. Copyright©2004 by Houghton Mifflin Company. All rights reserved. 4 Naming Starts with Classifying Compounds Binary Compounds = only 2 elements Compounds containing polyatomic ions Acids = formula often starts with H

5. Copyright©2004 by Houghton Mifflin Company. All rights reserved. 5 Classifying Binary Compounds Compounds containing a metal and a nonmetal are binary ionic –Type I: The metal forms only one type of ions –Type II: The metal can form two (or more) cations that have different charges Compounds containing two nonmetals –Type III Compounds containing H and a nonmetal = Acids

6. Copyright©2004 by Houghton Mifflin Company. All rights reserved. 6 I. Binary Ionic Made of metal cation and nonmetal anion Name by naming the ions

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8. 8 Metal Cations Type I –Metals that can only have one possible charge –Determine charge by position on the Periodic Table Type II –Metals that can have more than one possible charge –Determine metal cation’s charge from the charge on anion

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10. 10 Rules for Naming Type I Binary Ionic Compounds NaCl Contain Metal Cation + Nonmetal Anion Metal listed first in formula & name ¶Name metal cation first, name nonmetal anion second ¶Simple metal cation name is the metal name –simple metals are Groups 1A, 2A and Al, Ga & In ¶Nonmetal anion named by changing the ending on the nonmetal name to -ide

11. Copyright©2004 by Houghton Mifflin Company. All rights reserved. 11 Rules for Naming Type II Binary Ionic Compounds Contain Metal Cation + Nonmetal Anion Metal listed first in formula & name ¶Name metal cation first, name nonmetal anion second ¶Metal cation name is the metal name followed by a Roman Numeral in parentheses to indicate its charge –Determine charge from anion charge –Common Type II cations in Table 5.2 ¶Nonmetal anion named by changing the ending on the nonmetal name to -ide

12. Copyright©2004 by Houghton Mifflin Company. All rights reserved. 12 Determining the Charge on a Cation – FeCl 2 ¬Determine the charge on the anion the anion is Cl, since it is in Group 7A, its charge is -1 ­Determine the total negative charge since there are 2 Cl atoms in the formula, the total negative charge is -2 ®Determine the total positive charge since the total negative charge is -2, the total positive charge is +2 ¯Divide by the number of cations since there is 1 Fe in the formula & the total positive charge is +2, Fe has a +2 charge

13. Copyright©2004 by Houghton Mifflin Company. All rights reserved. 13 Rules for Naming Type III - Binary Compounds of 2 Nonmetals Name first element in formula first, use the full name of the element Name the second element in the formula as if it were an anion –However, remember these compounds do not contain ions! Use a prefix in front of each name to indicate the number of atoms Never use the prefix mono- on the first element

14. Copyright©2004 by Houghton Mifflin Company. All rights reserved. 14 Prefixes Drop last “a” in the prefix if the name begins with vowel octa-8 hepta-7 hexa-6 penta-5 tetra-4 tri-3 di-2 mono- (not used on first nonmetal) 1 PrefixSubscript

15. Copyright©2004 by Houghton Mifflin Company. All rights reserved. 15 Naming Binary Compounds: Summary

16. Copyright©2004 by Houghton Mifflin Company. All rights reserved. 16 II. Compounds Containing Polyatomic Ions Polyatomic ions are charged entities that contain more than one atom –Must memorize name, formula and charge –Look for Patterns!! Polyatomic compounds contain one or more polyatomic ions Name polyatomic compounds by naming cation and anion –Non-polyatomic ions named like Type I and II Polyatomic Acids contain H + and a polyatomic anion

17. Copyright©2004 by Houghton Mifflin Company. All rights reserved. 17 Patterns for Polyatomic Ions ¬Elements in the same column on the Periodic Table form similar polyatomic ions –same number of O’s and same charge ClO 3 - = chlorate  BrO 3 - = bromate ­If the polyatomic ion starts with H, add hydrogen- before the ions name and add 1 to the charge CO 3 2- = carbonate  HCO 3 - = hydrogen carbonate

18. Copyright©2004 by Houghton Mifflin Company. All rights reserved. 18 Patterns for Polyatomic Ions -ate ion –chlorate = ClO 3 - -ate ion plus 1 O  same charge, per- prefix –perchlorate = ClO 4 - -ate ion minus 1 O  same charge, -ite suffix –chlorite = ClO 2 - -ate ion minus 2 O  same charge, hypo- prefix, - ite suffix –hypochlorite = ClO -

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20. Copyright©2004 by Houghton Mifflin Company. All rights reserved. 20 Examples CaCO 3 = calcium carbonate Ca(NO 3 ) 2 = calcium nitrate CO 3 2- = carbonate: Na 2 CO 3 = sodium carbonate NO 3 - = nitrate: NaNO 3 = sodium nitrate

21. Copyright©2004 by Houghton Mifflin Company. All rights reserved. 21 III. Acids Contain H + cation and anion Binary acids have H + cation and a nonmetal anion Oxyacids have H + cation and a polyatomic anion

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24. Copyright©2004 by Houghton Mifflin Company. All rights reserved. 24 Naming Acids: Summary

25. Copyright©2004 by Houghton Mifflin Company. All rights reserved. 25 Writing the Formulas from the Names For Type III compounds, use the prefixes to determine the subscripts For Type I, Type II, polyatomic Compounds and Acids –Determine the ions present –Determine the charges on the cation and anion –Balance the charges to get the subscripts