FIFTH EDITION by Steven S. Zumdahl
University of Illinois
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Mifflin Company. All rights reserved.
1

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2

•
H
2
O = water, steam, ice
•
NH
3
= ammonia
•
CH
4
= methane
•
NaCl = table salt
•
C
12
H
22
O
11
= table sugar
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3

Naming Starts with Classifying Compounds
•
Binary Compounds = only 2 elements
• Compounds containing polyatomic ions
•
Acids = formula often starts with H
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4

•
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
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5

•
Made of metal cation and nonmetal anion
•
Name by naming the ions
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•
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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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
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•
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
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11

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
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12

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 monoon the first element
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Subscript
1
5
6
7
8
2
3
4
Prefix mono-
(not used on first nonmetal) ditritetrapentahexaheptaocta-
• Drop last “a” in the prefix if the name begins with vowel
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15

•
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
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16


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
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17

•
-ate ion
– chlorate = ClO
3
-
• -ate ion plus 1 O
 same charge, perprefix
– perchlorate = ClO
4
-
• -ate ion minus 1 O
 same charge, ite suffix
– chlorite = ClO
2
-
• -ate ion minus 2 O
 same charge, hypoprefix, ite suffix
– hypochlorite = ClO -
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19

CO
3
2= carbonate:
CaCO
3
= calcium carbonate
Na
2
CO
3
= sodium carbonate
NO
3
= nitrate:
Ca(NO
3
)
2
= calcium nitrate
NaNO
3
= sodium nitrate
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20

•
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

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
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