Document 2517742

05_Chem_GRSW_Ch09.SE/TE 6/11/04 3:33 PM Page 79
Name ___________________________
9
Date ___________________
Class __________________
CHEMICAL NAMES AND FORMULAS
SECTION 9.1 NAMING IONS (pages 253–258)
This section explains the use of the periodic table to determine the charge of
an ion. It also defines polyatomic ion and gives the names and formulas for
the most common polyatomic ions.
Monatomic Ions (pages 253–256)
1. What are monatomic ions?
Monatomic ions are ions consisting of only one atom.
2. How is the ionic charge of a Group 1A, 2A, or 3A ion determined?
The ionic charge is numerically equal to the group number.
3. How is the ionic charge of a Group 5A, 6A, or 7A ion determined?
The charge of an ion in Groups 5A, 6A, or 7A is determined by subtracting 8 from
the group number.
4. Circle the letter of the type of element that often has more than one common
ionic charge.
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a. alkali metal
b. alkaline earth metal
c. transition metal
d. nonmetal
Stock system
5. The ______________________
of naming transition metal cations uses a Roman
numeral in parentheses to indicate the numeric value of the ionic charge.
6. An older naming system uses the suffix -ous to name the cation with the
lesser
______________________
charge, and the suffix -ic to name the cation with the
greater
______________________
charge.
7. What is a major advantage of the Stock system over the old naming system?
The Stock system gives the actual charge of the ion.
Chapter 9 Chemical Names and Formulas 79
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Class __________________
CHAPTER 9, Chemical Names and Formulas (continued)
8. Use the periodic table to write the name and formula (including charge) for
each ion in the table below.
Element
Name
Formula
Fluorine
fluoride ion
F–
Calcium
calcium ion
Ca2+
Oxygen
oxide ion
O2–
Polyatomic Ions (pages 257–258)
9. What is a polyatomic ion?
A polyatomic ion is a tightly bound group of atoms that behaves as a unit and carries
a charge.
10. Is the following sentence true or false? The names of polyatomic anions always
false
end in -ide. ______________________
11. What is the difference between the anions sulfite and sulfate?
The sulfite ion has one less oxygen atom than the sulfate ion.
12. Look at Table 9.3 on page 257. Circle the letter of a polyatomic ion that is a cation.
b. acetate
c. oxalate
d. phosphate
13. How many atoms make up the oxalate ion and what is its charge?
It is made up of 6 atoms (2 carbon atoms and 4 oxygen atoms) and it has a charge
of 2.
14. What three hydrogen-containing polyatomic anions are essential components
of living systems?
hydrogen carbonate ion
a. ____________________________________________
hydrogen phosphate ion
b. ____________________________________________
dihydrogen phosphate ion
c. ____________________________________________
80 Guided Reading and Study Workbook
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a. ammonium
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Date ___________________
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15. Look at Figure 9.5 on page 257. Identify each of the ions shown below.
3
N
1
ammonium ion
a. __________________
1
P
N
phosphate ion
b. ______________________
nitrate ion
c. ______________________
SECTION 9.2 NAMING AND WRITING FORMULAS FOR
IONIC COMPOUNDS (pages 260–266)
This section explains the rules for naming and writing formulas for binary
ionic compounds and compounds containing a polyatomic ion.
Binary Ionic Compounds (pages 260–263)
property
1. Traditionally, common names were based on some ______________________
of
source
a compound or its ______________________
.
2. What is the general name for compounds composed of two elements?
They
are binary compounds.
__________________________________________________
3. When writing the formula for any ionic compound, the charges of the ions
balance
must ______________________
.
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4. What are two methods for writing a balanced formula?
finding the least common multiple of the charges
a. ____________________________________________________________________
using the crisscross method
b. ____________________________________________________________________
5. What are the formulas for the compounds formed by the following pairs of ions?
FeCl2
a. Fe2, Cl ______________________
Cr2O3
b. Cr3, O2 ______________________
Na2S
c. Na, S2 ______________________
6. What are the formulas for these compounds?
LiBr
a. lithium bromide ______________________
Cu3N2
b. cupric nitride ______________________
MgCl2
c. magnesium chloride ______________________
7. The name of a binary ionic compound is written with the name of the
cation
anion
______________________
first followed by the name of the ______________________
.
Chapter 9 Chemical Names and Formulas 81
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Date ___________________
Class __________________
CHAPTER 9, Chemical Names and Formulas (continued)
8. How can you tell that cobalt(II) iodide is a binary ionic compound formed
by a transition metal with more than one ionic charge?
The name includes a Roman numeral representing the ionic charge of the transition
metal cation.
9. Write the names for these binary ionic compounds.
a. PbS
lead(II) sulfide
__________________________________
magnesium chloride
b. MgCl2 __________________________________
aluminum selenide
c. Al2Se3 __________________________________
Compounds with Polyatomic Ions (pages 264–266)
10. What is a polyatomic ion?
A polyatomic ion contains more than one element.
11. How do you write the formula for a compound containing a polyatomic ion?
Write the symbol for the cation followed by the formula for the polyatomic ion
and balance the charges.
12. Why are parentheses used to write the formula Al(OH)3?
13. Complete the table for these ionic compounds containing polyatomic ions.
Cation
Anion
Name
Formula
NH4+
S2
ammonium sulfide
(NH4)2S
Fe3+
CO32–
iron(III) carbonate
Fe2(CO3)3
Ag+
NO3
K+
CN–
82 Guided Reading and Study Workbook
silver nitrate
potassium cyanide
AgNO3
KCN
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The parentheses indicate how many polyatomic ions are needed in the formula.
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Name ___________________________
Date ___________________
Class __________________
SECTION 9.3 NAMING AND WRITING FORMULAS FOR
MOLECULAR COMPOUNDS (pages 268–270)
This section explains the rules for naming and writing formulas for binary
molecular compounds.
Naming Binary Molecular Compounds (pages 268–269)
1. Circle the letter of the type(s) of elements that form binary molecular compounds.
a. two nonmetallic elements
b. a metal and a nonmetal
c. two metals
2. Is the following sentence true or false? Two nonmetallic elements can combine
false
in only one way. ______________________
3. What method is used to distinguish between different molecular compounds
Prefixes are used.
that contain the same elements? _________________________________________
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Match the prefix with the number it indicates.
c
_______
4. octa-
a. 4
a
_______
5. tetra-
b. 7
b
_______
6. hepta-
c. 8
d
_______
7. nona-
d. 9
8. What are the names of the following compounds?
boron trifluoride
a. BF3 ____________________________________________
dinitrogen tetroxide
b. N2O4 ____________________________________________
tetraphosphorus heptasulfide
c. P4S7 ____________________________________________
Writing Formulas for Binary Molecular Compounds (page 270)
9. What are the formulas for the following compounds?
CBr4
a. carbon tetrabromide ______________________
NI3
b. nitrogen triiodide ______________________
ICl
c. iodine monochloride ______________________
I4O9
d. tetraiodine nonaoxide ______________________
Chapter 9 Chemical Names and Formulas 83
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Name ___________________________
Date ___________________
Class __________________
CHAPTER 9, Chemical Names and Formulas (continued)
Reading Skill Practice
Writing a summary can help you remember the information you have read. When you write a
summary, include only the most important points. Write a summary of the information in Section 9.3
on pages 268–269. Your summary should be shorter than the text on which it is based. Do your work
on a separate sheet of paper.
Students’ summaries should focus on the main points of each subsection and include the information
given in Table 9.4.
SECTION 9.4 NAMING AND WRITING FORMULAS
FOR ACIDS AND BASES (pages 271–273)
This section explains the three rules for naming acids and shows how these
rules can also be used to write the formulas for acids. Names and formulas
for bases are also explained.
Naming Common Acids (pages 271–272)
hydrogen
1. Acids produce ______________________
ions when dissolved in water.
2. When naming acids, you can consider them to be combinations of
anions
hydrogen
______________________
connected to as many ______________________
ions
as are necessary to create an electrically neutral compound.
4. What are the components of phosphorous acid? What is its formula?
hydrogen ion and phosphite ion; H3PO3
Writing Formulas for Acids (page 272)
5. Use Table 9.5 on page 272 to help you complete the table about acids.
Acid Name
Formula
Anion Name
acetic acid
HC2H3O2
acetate
carbonic acid
H2CO3
carbonate
hydrochloric acid
HCl
chloride
nitric acid
HNO3
nitrate
phosphoric acid
H3PO4
phosphate
sulfuric acid
H2SO4
sulfate
84 Guided Reading and Study Workbook
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HBr
3. What is the formula for hydrobromic acid? ______________________
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Date ___________________
Class __________________
Names and Formulas for Bases (page 273)
hydroxide ions
6. A base is a compound that produces ______________________
when dissolved
in water.
7. How are bases named?
Name the cation first followed by the anion (hydroxide ion).
SECTION 9.5 THE LAWS GOVERNING FORMULAS
AND NAMES (pages 274–279)
This section uses data to demonstrate that a compound obeys the law of
definite proportions. It also explains how to use flow charts to write the
name and formula of a compound.
The Laws of Definite and Multiple Proportions (pages 274–275)
1. What is the law of definite proportions?
In different samples of the same chemical compound, the masses of the elements
are always present in the same proportions.
2. Circle the whole-number mass ratio of Li to Cl in LiCl. The atomic mass of Li is
6.9; the atomic mass of Cl is 35.5.
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a. 42 : 1
b. 5 : 1
c. 1 : 5
3. Circle the whole-number mass ratio of carbon to hydrogen in C2H4. The
atomic mass of C is 12.0; the atomic mass of H is 1.0.
a. 1 : 6
c. 1 : 12
b. 6 : 1
d. 12 : 1
4. In the compound sulfur dioxide, a food preservative, the mass ratio of sulfur to
oxygen is 1 : 1. An 80-g sample of a compound composed of sulfur and oxygen
contains 48 g of oxygen. Is the sample sulfur dioxide? Explain.
No; If the sample contains 48 g of oxygen, it contains 32 g of sulfur. The ratio 32 : 48
is equivalent to 2 : 3, not 1 : 1.
5. What is the law of multiple proportions?
When two elements form more than one compound, the different masses of one
element that combine with the same mass of the other element are in a ratio of
small whole numbers.
Chapter 9 Chemical Names and Formulas 85
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Name ___________________________
Date ___________________
Class __________________
CHAPTER 9, Chemical Names and Formulas (continued)
6. Complete the table using the law of multiple proportions.
Mass of Cu
Mass of Cl
Mass Ratio
Cl : Cu
Whole-number
Ratio of Cl
Compound A
8.3 g
4.6 g
0.55
1
Compound B
3.3 g
3.6 g
1.1
2
Practicing Skills: Naming Chemical Compounds (pages 276–277)
7. How can a flowchart help you to name chemical compounds?
It gives step-by-step directions for naming a compound.
8. Use the flowchart in Figure 9.20 on page 277 to write the names of the
following compounds:
a. CsCl
cesium chloride
___________________________________
b. SnSe2
tin(IV) selenide
___________________________________
ammonium hydroxide
c. NH4OH ___________________________________
d. HF
hydrofluoric acid
___________________________________
e. Si3N4
trisilicon tetranitride
___________________________________
zero
a. In an ionic compound, the net ionic charge is ______________________
.
binary
b. An -ide ending generally indicates a ______________________
compound.
polyatomic
c. An -ite or -ate ending means there is a ______________________
ion that
includes oxygen in the formula.
Prefixes
d. ______________________
in a name generally indicate that the compound is
molecular and show the number of each kind of atom in the molecule.
Roman numeral
e. A ______________________
after the name of a cation shows the ionic charge
of the cation.
86 Guided Reading and Study Workbook
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9. Complete the following five rules for writing a chemical formula from a
chemical name.
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Name ___________________________
Date ___________________
Class __________________
Practicing Skills: Writing Chemical Formulas (page 278)
10. Fill in the missing labels from Figure 9.22 on page 278.
Name of Compound
Contains
prefixes?
Molecular
compound
yes
Uses prefixes to
write formula.
no
Ionic
compound
Identify symbols
Group A
elements
Roman
numerals
Polyatomic
ions
Use Table 9.1
for charges.
Give charges
for cations.
Use Table 9.3
for charges.
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Balance
charges
Use crisscross method. Add parentheses
for any multiple polyatomic ions.
11. Use the flowchart in Figure 9.22 to write the formulas of the following
compounds:
K2SiO3
a. potassium silicate ______________________
PCl5
b. phosphorus pentachloride ______________________
MnCrO4
c. manganese(II) chromate ______________________
LiH
d. lithium hydride ______________________
I 2O5
e. diiodine pentoxide ______________________
Chapter 9 Chemical Names and Formulas 87
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Name ___________________________
Date ___________________
Class __________________
CHAPTER 9, Chemical Names and Formulas (continued)
GUIDED PRACTICE PROBLEMS
GUIDED PRACTICE PROBLEM 2 (page 256)
2. How many electrons were lost or gained to form these ions?
a. Fe3
b. O2
c. Cu
Step 1. Determine the number of electrons based on the size of the charge.
Step 2. Determine whether the electrons were lost or gained based on the sign
of the charge.
Fe3 lost 3 electrons.
a. ________________________________________________
O 2 gained 2 electrons.
b. ________________________________________________
Cu lost 1 electron.
c. ________________________________________________
GUIDED PRACTICE PROBLEMS 10B AND 10C (page 263)
10. Write formulas for compounds formed from these pairs of ions.
b. Li+ , O2–
Analyze
Step 1. Do the ions combine in a 1:1 ratio?
No, the charges on the ions are not equal.
Step 2. Use the crisscross method
to balance the formula.
Li20
Write the formula. ___________
Li
Evaluate
Step 3. How do you know your formula is reasonable?
The positive and negative charges are equal.
88 Guided Reading and Study Workbook
2
O
2
1
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Solve
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Name ___________________________
Date ___________________
Class __________________
c. Ca2 , N3
Analyze
Step 1. Will the calcium (Ca2+) and nitride (N3–) ions combine in a 1 : 1 ratio?
How do you know?
No, because then the total charge would be negative, instead of neutral.
Solve
Step 2. Use the crisscross method
to balance the formula.
Ca
Ca3 N2
Write the formula. ___________
2
N
3
3
2
Evaluate
Step 3. How do you know this formula is reasonable?
The positive and negative charges are equal.
GUIDED PRACTICE PROBLEM 13B (page 265)
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13b. Write the formula for chromium(III) nitrate.
• Is the compound ionic or molecular? Explain.
It is ionic because it has no prefixes and it contains a metal.
• Use Table 9.3 on page 257 to write the formula for
NO3–
the nitrate ion. ________
• Use the crisscross method to balance the formula.
Cr(NO3)3
• Write the formula. ____________________________
Cr
3
1
(NO3)
3
Chapter 9 Chemical Names and Formulas 89
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Name ___________________________
Date ___________________
Class __________________
CHAPTER 9, Chemical Names and Formulas (continued)
GUIDED PRACTICE PROBLEM 34 (page 275)
34. Lead forms two compounds with oxygen. One compound contains 2.98 g of
lead and 0.461 g of oxygen. The other contains 9.89 g of lead and 0.763 g of
oxygen. For a given mass of oxygen, what is the lowest whole-number mass
ratio of lead in the two compounds?
Complete the following steps to solve the problem.
First compound
Step 1. Write the ratio of lead to
oxygen for each compound.
2.98 g lead
0.461 g oxygen
Step 2. Divide the numerator by
the denominator in each ratio.
6.46 g lead
Second compound
9.89 g lead
g oxygen
0.763
13.0 g lead
g oxygen
g oxygen
Step 3. Write a ratio comparing
the first compound to the second.
6.46
Step 4. Simplify. Note that this ratio
has no units.
0.497 roughly
1
g lead/g oxygen
13.0 g lead/g oxygen
1
2
90 Guided Reading and Study Workbook
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1 : 2 ___ .
The mass ratio of lead per gram of oxygen in the two compounds is ___________
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Name ___________________________
9
Date ___________________
Class __________________
CHEMICAL NAMES AND FORMULAS
Practice Problems
In your notebook, solve the following problems.
SECTION 9.1 NAMING IONS
1. What is the charge on the ion typically formed by each element?
a. oxygen
c. sodium
e. nickel, 2 electrons lost
b. iodine
d. aluminum
f. magnesium
2. How many electrons does the neutral atom gain or lose when each ion
forms?
a. Cr3
c. Li
e. Cl
b. P3
d. Ca2
f. O2
3. Name each ion. Identify each as a cation or an anion.
a. Sn2
c. Br
e. H
b. Co3
d. K
f. Mn2
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4. Write the formula (including charge) for each ion. Use Table 9.3 if necessary.
a. carbonate ion
c. sulfate ion
e. chromate ion
b. nitrite ion
d. hydroxide ion
f. ammonium ion
5. Name the following ions. Identify each as a cation or an anion.
a. CN
c. PO43
e. Ca2
b. HCO3
d. Cl
f. SO32
SECTION 9.2 NAMING AND WRITING FORMULAS
FOR IONIC COMPOUNDS
1. Write the formulas for these binary ionic compounds.
a. magnesium oxide
c. potassium iodide
e. sodium sulfide
b. tin(II) fluoride
d. aluminum chloride
f. ferric bromide
2. Write the formulas for the compounds formed from these pairs of ions.
a. Ba2, Cl
c. Ca2, S2
e. Al3, O2
b. Ag, I
d. K, Br
f. Fe2, O2
3. Name the following binary ionic compounds.
a. MnO2
c. CaCl2
e. NiCl2
g. CuCl2
b. Li3N
d. SrBr2
f. K2S
h. SnCl4
Chapter 9 Chemical Names and Formulas
221
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Name ___________________________
Date ___________________
Class __________________
4. Write formulas for the following ionic compounds.
a. sodium phosphate
c. sodium hydroxide
e. ammonium chloride
b. magnesium sulfate
d. potassium cyanide
f. potassium dichromate
5. Write formulas for compounds formed from these pairs of ions.
a. NH4, SO42
c. barium ion and hydroxide ion
b. K, NO3
d. lithium ion and carbonate ion
6. Name the following compounds.
a. NaCN
c. Na2SO4
e. Cu(OH)2
b. FeCl3
d. K2CO3
f. LiNO3
7. Name and give the charge of the metal cation in each of the following
ionic compounds.
a. Na3PO4
c. CaS
e. FeCl3
b. NiCl2
d. K2S
f. CuI
SECTION 9.3 NAMING AND WRITING FORMULAS
FOR MOLECULAR COMPOUNDS
1. Name the following molecular compounds.
a. PCl5
c. NO2
e. P4O6
g. SiO2
b. CCl4
d. N2F2
f. XeF2
h. Cl2O7
2. Write the formulas for the following binary molecular compounds.
c. sulfur dioxide
b. dichlorine monoxide
d. dinitrogen tetrafluoride
SECTION 9.4 NAMING AND WRITING FORMULAS
FOR ACIDS AND BASES
1. Name the following compounds as acids.
a. HNO2
b. H2SO4
c. HF
d. H2CO3
2. Write the formulas for the following bases.
a. calcium hydroxide
c. aluminum hydroxide
b. ammonium hydroxide
d. lithium hydroxide
SECTION 9.5 THE LAWS GOVERNING FORMULAS AND NAMES
1. Write the formulas for these compounds.
222
a. potassium sulfide
e. hydrobromic acid
i. sulfur hexafluoride
b. tin(IV) chloride
f. aluminum fluoride
j. magnesium chloride
c. hydrosulfuric acid
g. dinitrogen pentoxide
k. phosphoric acid
d. calcium oxide
h. iron(III) carbonate
l. nitric acid
Core Teaching Resources
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a. nitrogen tribromide
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Name ___________________________
Date ___________________
Class __________________
2. Complete this table by writing correct formulas for the compounds formed by
combining positive and negative ions.
SO42
NO3
OH
PO43
Ca2
Al3
Na
Pb4
3. Name the following compounds.
a. K3PO4
c. NaHSO4
e. N2O5
g. PI3
b. Al(OH)3
d. HgO
f. NBr3
h. (NH4)2SO4
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4. Explain the difference between the law of definite proportions and the law of
multiple proportions.
Chapter 9 Chemical Names and Formulas
223
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Name ___________________________
9.1
Date ___________________
Class __________________
NAMING IONS
Section Review
Objectives
• Determine the charges of monatomic ions by using the periodic table and write
the names of the ions
• Define a polyatomic ion and write the names and formulas of the most common
polyatomic ions
• Identify the two common endings for the names of most polyatomic ions.
Vocabulary
• monatomic ions
• polyatomic ions
Part A Completion
Use this completion exercise to check your understanding of the concepts and terms
that are introduced in this section. Each blank can be completed with a term, short
phrase, or number.
1
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Ions that consist of a single atom are called
Metallic elements tend to
3
2
ions.
1.
electrons. Group 1A ions have a
4
charge, whereas Group 2A metals form ions with a
charge, and Group 3A metals form ions with a
5
charge.
The charge of a Group A nonmetal ion is determined by
subtracting
6
8
Many of the
10
.
9
system
naming system.
Ions containing more than one atom are called
or
13
.
6.
8.
9.
10.
11
The names of most common polyatomic ions end in either
12
4.
7.
have more than one common ionic
charge. These ions are named using either the
or the
7
3.
5.
from the group number. For example, the
Group 7A elements form ions with a charge of
2.
ions.
11.
12.
13.
Chapter 9 Chemical Names and Formulas
211
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Name ___________________________
Date ___________________
Class __________________
Part B True-False
Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT.
________ 14. The names of polyatomic ions end in -ite or -ate.
________ 15. In polyatomic ions for which there is an -ite/-ate pair, the -ite ending will
always indicate one less oxygen atom than the -ate ending.
________ 16. Polyatomic ions are anions.
________ 17. The charge on Group A metal ions is determined by subtracting the
group number from 8.
________ 18. The Group 6A ions have a charge of 2.
Part C Matching
Match each description in Column B to the correct term in Column A.
Column A
Column B
a. negatively charged ions
________ 20. polyatomic ions
b. ions formed from single atoms
________ 21. cations
c. a traditional way of naming transition metal cations
________ 22. anions
d. positively charged ions
________ 23. classical naming system
e. ions formed from groups of atoms
Part D Questions and Problems
Answer the following in the space provided.
24. What is the charge on a typical ion for each of the following groups?
a. 1A
c. 7A
b. 6A
d. 2A
25. Write the name of each of the following polyatomic ions.
a. HCO3
c. MnO4
b. NH4
d. OH
26. How many electrons does the neutral atom gain or lose to form each of the
following ions?
212
a. Ca2
c. I
b. S2
d. Mn3
Core Teaching Resources
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________ 19. monatomic ions
05_CTR_ch09 7/9/04 3:29 PM Page 213
Name ___________________________
Date ___________________
Class __________________
NAMING AND WRITING FORMULAS
FOR IONIC COMPOUNDS
9.2
Section Review
Objectives
• Apply the rules for naming and writing formulas for binary ionic compounds
• Apply the rules for naming and writing formulas for compounds with
polyatomic ions
Vocabulary
• binary compound
Part A Completion
Use this completion exercise to check your understanding of the concepts and terms
that are introduced in this section. Each blank can be completed with a term, short
phrase, or number.
Binary ionic compounds are named by writing the name of
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the
1
followed by the name of the
binary compounds end in
3
2
1.
. Names of
4
. For example, NaI is
2.
.
5
When a cation has more than one ionic charge, a
4.
is used in the name.
5.
Compounds with polyatomic ions whose names end in -ite
or -ate contain a polyatomic
6
that includes
7
.
In writing the formula of an ionic compound, the net ionic charge
must be
8
3.
6.
7.
8.
.
Part B True-False
Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT.
________ 9. The systematic name for baking soda (NaHCO3) is sodium
bicarbonate.
________ 10. In writing a formula for an ionic compound, the net ionic charge of
the formula must be zero.
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213
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Name ___________________________
Date ___________________
Class __________________
________ 11. Anions that contain oxygen end in -ite or -ate.
________ 12. The cation name is placed first when naming ionic compounds.
Part C Matching
Match each description in Column B to the correct term in Column A.
Column A
Column B
________ 13. binary compounds
a. ions that consist of a single atom
________ 14. monatomic ions
b. ionic compounds composed of two elements
________ 15. polyatomic ions
c. Group B metals, many of which have more than one
common ionic charge
________ 16. transition metals
d. ions that consist of more than one atom
Part D Questions and Problems
Answer the following in the space provided.
17. Name the following compounds and tell what type of compound they are
(binary ionic or ionic with a polyatomic ion).
a. FeBr3
b. KOH
18. Write the formulas for the following compounds.
a. sodium chlorate
b. lead(II) phosphate
c. magnesium hydrogen carbonate
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c. Na2Cr2O7
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Name ___________________________
9.3
Date ___________________
Class __________________
NAMING AND WRITING FORMULAS
FOR MOLECULAR COMPOUNDS
Section Review
Objectives
• Interpret the prefixes in the names of molecular compounds in terms of their
chemical formulas
• Apply the rules for naming and writing formulas for binary molecular compounds
Part A Completion
Use this completion exercise to check your understanding of the concepts and terms
that are introduced in this section. Each blank can be completed with a term, short
phrase, or number.
1
Binary molecular compounds are composed of two
2
elements. The name of this type of compound ends in
Prefixes are used to show how many
3
of each element
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are present in a molecule of the compound. For example,
the name of As2S5 is
4
1.
.
2.
3.
4.
.
Part B True-False
Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT.
________ 5. Binary molecular compounds contain carbon.
________ 6. Charges must be balanced when writing formulas for molecular
compounds.
________ 7. CO2 is named monocarbon dioxide.
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Name ___________________________
Date ___________________
Class __________________
Part C Matching
Match each description in Column B to the correct term in Column A.
Column A
Column B
________ 8. binary molecular
compound
a. used to indicate the relative number of atoms of an
element in a molecular compound
________ 9. prefix
b. prefix indicating one atom of an element in a molecule
________ 10. mono-
c. prefix indicating four atoms of an element in a molecule
________ 11. tetra-
d. nonionic compound containing atoms of two elements
Part D Questions and Problems
Answer the following in the space provided.
12. Name each of the following compounds.
a. PCl5
b. SO2
c. P4S10
13. Write formulas for the following compounds.
a. carbon tetrabromide
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b. dinitrogen tetroxide
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Name ___________________________
9.4
Date ___________________
Class __________________
NAMING AND WRITING FORMULAS
FOR ACIDS AND BASES
Section Review
Objectives
• Apply three rules for naming acids
• Apply the rules in reverse to write formulas of acids
• Apply the rules for naming bases
Vocabulary
• acid
• base
Part A Completion
Use this completion exercise to check your understanding of the concepts and terms
that are introduced in this section. Each blank can be completed with a term, short
phrase, or number.
1
© Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved.
An acid is a compound that contains one or more
2
atoms and produces
1.
when dissolved in water. There
2.
are rules for naming acids. For example, HBr is called
3
acid, whereas HNO3 is called
A base is a(n)
5
4
3.
acid.
4.
6
compound that produces
when
dissolved in water. Ionic compounds that are bases are named
in the same way as other
of the
8
7
compounds, that is, the name
is followed by the name of the
9
.
5.
6.
7.
8.
9.
Part B True-False
Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT.
________ 10. A compound that contains hydrogen atoms will be an acid when
dissolved in water.
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217
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Name ___________________________
Date ___________________
Class __________________
________ 11. An acid contains one or more hydroxide ions.
________ 12. Chemists have a special system for naming bases.
Part C Matching
Match each description in Column B to the correct term in Column A.
Column A
Column B
________ 13. acid
a. a compound containing hydrogen that ionizes to yield
hydrogen ions in solution
________ 14. base
b. a solution in which the solvent is water
________ 15. aqueous solution
c. a compound that produces hydroxide ions in water
Part D Questions and Problems
Answer the following in the space provided.
16. Write the formula for each acid or base.
a. magnesium hydroxide
b. hydrofluoric acid
d. lithium hydroxide
17. Name each acid or base.
a. KOH
b. HI
c. H2SO4
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c. phosphoric acid
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Name ___________________________
9.5
Date ___________________
Class __________________
THE LAWS GOVERNING FORMULAS
AND NAMES
Section Review
Objectives
• Define the laws of definite proportions and multiple proportions
• Apply the rules for writing chemical formulas by using a flowchart
• Apply the rules for naming chemical compounds by using a flowchart
Vocabulary
• law of definite proportions
• law of multiple proportions
Part A Completion
Use this completion exercise to check your understanding of the concepts and terms
that are introduced in this section. Each blank can be completed with a term, short
phrase, or number. [Use Figure 9.20 to complete this exercise.]
© Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved.
The law of
1
states that in samples of any chemical
1.
compound, the masses of the elements are always in the same
2.
2
3
. The law of
states that whenever the same two
3.
elements form more than one compound, the different masses
4.
of one element that combine with the same mass of the other
5.
4
6.
element are in the ratio of
H3PO4 is a(n)
CCl4 is not a(n)
5
numbers.
6
. It is called
7
.
7.
. It contains two elements, so it is a
8.
8
compound. It does not contain a metal, so it is a binary
9.
9
compound. The compound is called
Pb(C2H3O2)2 is not a(n)
12
11
.
10.
. It contains more than two
. C2H3O2 is a polyatomic
metal. The compound is called
10
13
15
.
. Pb is a Group
14
11.
12.
13.
14.
15.
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219
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Name ___________________________
Date ___________________
Class __________________
Part B True-False
Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT.
________ 16. Roman numerals are used when naming Group B metal cations.
________ 17. Names of compounds containing polyatomic anions end in -ide.
________ 18. Prefixes are used when naming binary ionic compounds.
________ 19. Compounds containing two elements are called binary compounds.
Part C Questions and Problems
Answer the following in the space provided.
20. Name the following compounds.
a. Pb(C2H3O2)4
b. HF
c. P2O5
d. LiBr
21. Write formulas for the following compounds.
a. phosphorus pentachloride
b. iron(II) oxide
d. potassium chloride
e. calcium nitrate
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c. nitric acid
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Name ___________________________
9
Date ___________________
Class __________________
INTERPRETING GRAPHICS
Use with Section 9.1
Group
1A
8A
1
2
H
He
Hydrogen
3
Helium
2A
3A
4A
5A
6A
7A
4
5
6
7
8
9
10
Li
Be
B
C
N
O
F
Ne
Lithium
Beryllium
Boron
Carbon
Nitrogen
Oxygen
Fluorine
Neon
11
12
13
14
15
16
17
18
Na
Mg
Al
Si
P
S
Cl
Ar
Sodium
Magnesium
Aluminum
Silicon
Phosphorus
Sulfur
Hydrogen
Argon
19
20
K
Ca
Potassium
Calcium
Use the abbreviated periodic table above to answer the following questions.
1. Which group on the periodic table contains magnesium (Mg)?
2. How many electrons does a magnesium atom lose to form a
magnesium cation?
4. How many electrons does a magnesium cation contain?
5. Which group on the periodic table contains fluorine (F)?
6. How many electrons does a fluorine atom gain to form a fluoride anion?
7. How many electrons does a neutral fluorine atom contain?
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3. How many electrons does a neutral magnesium atom contain?
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Name ___________________________
Date ___________________
Class __________________
8. How many electrons does a fluoride anion contain?
9. How many electrons does a sodium cation contain?
10. How many electrons does an oxide anion contain?
11. How many electrons does each of the following ions contain?
a. S2
b. Ca2
c. K
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d. Cl
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Name ___________________________
9
Date ___________________
Class __________________
CHEMICAL NAMES AND FORMULAS
Vocabulary Review
Match the correct vocabulary term to each numbered statement. Write the letter of the
correct term on the line.
Column A
Column B
a. anion
________ 2. an ionic compound that produces hydroxide ions
when dissolved in water
b. law of multiple
proportions
________ 3. any atom or group of atoms that has a positive charge
c. base
________ 4. compounds composed of metal cations and nonmetal
anions
d. ionic compounds
________ 5. composed of two elements and can be either ionic or
molecular
e. binary compound
________ 6. an ion consisting of a single atom with a positive or
negative charge
f. monatomic ion
________ 7. Whenever two elements form more than one
compound, the different masses of one element that
combine with the same mass of the other element are
in the ratio of small whole numbers.
g. cation
________ 8. a tightly bound group of atoms that behaves as a unit
and carries a charge
h. polyatomic ion
________ 9. In samples of any chemical compound, the masses of
the elements are always in the same proportions.
i. acids
________ 10. any atom or group of atoms that has a negative charge
j. law of definite
proportions
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________ 1. compounds that contain one or more hydrogen atoms
and produce hydrogen ions in solution
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Name ___________________________
9
Date ___________________
Class __________________
CHEMICAL NAMES AND FORMULAS
Chapter Quiz
Fill in the word(s) that will make each statement true.
1.
9.1
2.
9.3
3
3. A(n)
is any atom or group of atoms with a
negative charge.
3.
9.1
4
4. The law of
states that in any chemical compound,
the elements are always combined in the same proportion
by mass.
4.
9.5
5. The charge on an ion of a Group A nonmetal is determined
5
by subtracting 8 from
.
5.
9.1
6.
9.1
7.
9.1
8.
9.1
9.
9.3
10. What is the formula for iron(II) chloride?
10.
9.2
11. Name the compound whose formula is SnS2.
11.
9.2
12. Name the compound N2O5.
12.
9.3
13. Name the compound NaHCO3.
13.
9.2
14. Write the formula for copper(II) hydroxide.
14.
9.2
15. Name the compound HNO3 as an acid.
15.
9.4
1.
1
tend to lose electrons when they react to form
compounds.
2
2. The formula for phosphorus pentachloride is
6. The metals in Groups 1A, 2A, and 3A
when they form ions.
6
.
electrons
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7. The two common polyatomic ions whose names end in -ide
7
are the cyanide ion and the
ion.
8
8. The formula for the dihydrogen phosphate ion is
9. The systematic name for laughing gas (N2O) is
9
.
.
Write your answer in the space provided.
Chapter 9 Chemical Names and Formulas
227