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

2. Nomenclature Chapter 5 1

3. CHEMISTRY 100 Dr. Jimmy Hwang Sections 5 and 7 Tu & Th 9:30a. m
CHEMISTRY 100 Dr. Jimmy Hwang Sections 5 and 7 Tu & Th 9:30a.m.-10:45a.m.
Textbook: Zumdahl, Introductory Chemistry, 5th Edition
Office Hours: by appointment
Ext (voic )

4. Overview In Chapter 5, our goals are for the students to:
1. Understand why it is important to have a system for naming compounds.
2. Learn how to name binary compounds of a metal and a nonmetal.
3. Learn how to name binary compounds containing only nonmetals.
4. Review the naming of Type I, Type II, and Type III binary compounds.
5. Learn the names of common polyatomic ions and how to use them in naming compounds.
6. Learn how the anion composition determines the acid’s name.
7. Learn names of common acids.
8. Learn to write the formula of a compound given its name.

5. Common Names - Exceptions
H2O = water, steam, ice
NH3 = ammonia
CH4 = methane
NaCl = table salt
C12H22O11 = table sugar 2

6. Naming Starts with Classifying Compounds
Binary Compounds = only 2 elements
Compounds containing polyatomic ions
Acids = formula often starts with H 3

7. Classifying Binary Compounds
Compounds containing a metal and a nonmetal are binary ionic
Type I and II
Compounds containing two nonmetals
Type III
Compounds containing H and a nonmetal = Acids 4

8. Binary Ionic Made of metal cation and nonmetal anion
Name by naming the ions 5

9. Metal Cations Type I Type II
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 6

10. Type I Binary Ionic Compounds
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 7

11. CaCl2 = calcium chloride
Naming Compounds
Binary Ionic Compounds (Type I):
1. Cation first, then anion
2. Monatomic cation = name of the element
Ca2+ = calcium ion
3. Monatomic anion = root + -ide
Cl = chloride
CaCl2 = calcium chloride

12. Memorize Table 5.1

13. Principle of Electrical Neutrality
The principle that, in any ionic compound, the total positive charge must equal the total negative charge, i.e., a chemical compound must have a net charge of zero.

14. Determining the Charge on a Cation – Au2S3 using the Principle of Electrical Neutrality
Determine the charge on the anion
Au2S3 - the anion is S, since it is in Group 6A, its charge is -2
Determine the total negative charge
since there are 3 S in the formula, the total negative charge is -6
Determine the total positive charge
since the total negative charge is -6, the total positive charge is +6
Divide by the number of cations
since there are 2 Au in the formula & the total positive charge is +6, each Au has a +3 charge 9

15. 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 8

16. Figure 2.22: The common cations and anions

17. Monatomic Ions 2. Transition metal cations (Figure 2.22)
Memorize the charge of other metals in Figure 2.8. It is easy to remember the charges of the metal ions in the figures as follows:
+1: all alkali metals, Ag+, Cu+, Hg22+
+3: Al3+, Co3+, Cr3+, Fe3+, Mn3+ (AC2FM)
+4: Sn4+ , Pb4+
+2: everything else
Note that some metals have two charges (Type II).

18. Principle of Electrical Neutrality
The principle that, in any ionic compound, the total positive charge must equal the total negative charge, i.e. a chemical compound must have a net charge of zero.
iron(II) chloride
2 Cl- -2 so Fe is +2
FeCl2
iron(III) chloride
FeCl3
3 Cl- -3 so Fe is +3
Cr2S3
3 S2- -6 so Cr is +3 (6/2)
chromium(III) sulfide

20. Naming Compounds (continued)
Binary Ionic Compounds (Type II):
 metal forms more than one cation
 use Roman numeral in name
PbCl2
Pb2+ is cation
PbCl2 = lead (II) chloride

22. QUESTION

23. ANSWER
Class Prep CD: Table 5.1, Figure 5.1, Figure 5.2

24. 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 10

25. (not used on first nonmetal)
Prefixes
octa- 8
hepta- 7
hexa- 6
penta- 5
tetra- 4
tri- 3
di- 2
mono-
(not used on first nonmetal) 1
Prefix
Subscript
Drop last “a” in the prefix if the name begins with vowel 11

26. Molecular Compounds NF3 nitrogen trifluoride SO2 sulfur dioxide N2Cl4
dinitrogen tetrachloride
TOXIC!
NO2
nitrogen dioxide
N2O
dinitrogen monoxide
Laughing Gas
2.7

27. Figure 5.1: A flow chart for naming binary compounds.

28. QUESTION

29. ANSWER
Class Prep CD: Table 5.3, Table 5.4

30. 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 12

31. 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
ClO3- = chlorate  BrO3- = bromate
If the polyatomic ion starts with H, add hydrogen- before the ions name and add 1 to the charge
CO32- = carbonate  HCO3- = hydrogen carbonate 13

32. Patterns for Polyatomic Ions
-ate ion
chlorate = ClO3-
-ate ion plus 1 O  same charge, per- prefix
perchlorate = ClO4-
-ate ion minus 1 O  same charge, -ite suffix
chlorite = ClO2-
-ate ion minus 2 O  same charge, hypo- prefix, -ite suffix
hypochlorite = ClO- 14

34. Figure 5.2: Overall strategy for naming chemical compounds.

35. Acids Contain H+ cation and anion
Binary acids have H+ cation and a nonmetal anion
Oxyacids have H+ cation and a polyatomic anion 15

36. Memorize

37. Memorize

38. Figure 5. 3: A flow chart for naming acids
Figure 5.3: A flow chart for naming acids. The acid is considered as one or more H+ ions attached to an anion.

39. Memorize Acid Anion Name HClO4 perchlorate perchloric acid
HClO3 chlorate chloric acid
HClO2 chlorite chlorous acid
HClO hypochlorite hypochlorous acid

40. QUESTION

41. ANSWER
Class Prep CD: Table 5.2, Figure 5.1, Figure 5.2

42. QUESTION

43. ANSWER
Class Prep CD: Figure 5.1, Figure 5.2, Tables 5.2, 5.4, and 5.6

44. 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 16

45. Naming Exercise Al2(C2O4)3 P4O10 Cu(NO2)2 NaMnO4 CS2 Fe2(CrO4)3 Hg2Cl2
NH4BrO2
Ca(ClO4)2
Aluminum oxalate
Tetraphosphorous decaoxide
Copper(II) nitrite
Sodium permanganate
Carbon disulfide
Iron(III) chromate
Mercury(I) chloride
Ammonium bromite
Calcium perchlorate