Free Study Guide for
Cracolice • Peters
Introductory Chemistry: An Active Learning Approach
Second Edition
www.brookscole.com/chemistry
Chapter 6
Chemical Nomenclature
Chapter 6–Assignment A: Reviewing Elements, Naming Compounds Made from
Two Nonmetals or One Nonmetal and One Metalloid
In Section 5.7, you learned the symbols of some common elements in the periodic table.
Any chemist can tell you that some elements are trickier than others. For chemistry students,
those trickier elements are the seven that exist as diatomic molecules at room temperature. In
this assignment you'll learn to write the formulas of those elements correctly. You'll also
learn to write the names and formulas of some molecules made from two different atoms.
Here are the big ideas:
1)
The names and formulas of the 35 elements in Figure 5.8 should already be in
memory. The seven diatomic elements H2 , N2 , O2 , F2 , Cl2 , Br2 , and I2 must be
learned.
2)
Two nonmetals or a nonmetal and a metalloid form chemical bonds with each other
to form binary molecular compounds. The name of a binary molecular
compound is the name of the first element followed by the name of the second
element, modified with an -ide suffix. Prefixes are used to indicate the number of
atoms of each element in the molecule.
3)
Two common binary molecular compounds with nonsystematic names are water,
H2 O, and ammonia, NH3 .
Learning Procedures
Study
Sections 6.1–6.3. Focus on Goals 1–3 as you study.
Strategy
The seven diatomic elements must be memorized. Binary molecular
compounds are named according to the rules in the Summary in Section 6.3.
Nomenclature is a learn-by-doing skill—keep practicing!
Answer
Questions, Exercises, and Problems 1–5. Check your answers with those at
the end of the chapter.
Workbook
If your instructor recommends the Active Learning Workbook, do
Questions, Exercises, and Problems 1–5.
33
Copyright © 2004 Brooks/Cole, a division of Thomson Learning, Inc.
No part of this work may be reproduced without the written permission of the publisher.
Study Guide for Introductory Chemistry: An Active Learning Approach
Chapter 6–Assignment B: Names and Formulas of Monatomic Ions
In this assignment you'll learn names and formulas of monatomic (one-atom) ions. The big
ideas follow:
1)
Ions are charged particles. A cation has a positive charge; an anion has a negative
charge.
2)
The name of a monatomic cation is the name of the element, followed by the word
ion. The name of a monatomic anion is the name of the element, changed to end in
-ide, followed by the word ion.
3)
The formula of a monatomic ion is the symbol of the element followed by its
electrical charge, written in superscript.
4)
The charge of ions formed from main-group elements corresponds to the group
number: 1A/1, 1+; 2A/2, 2+; 3A/3, 3+; 5A/15, 3–; 6A/16, 2–; 7A/17, 1–.
5)
Some transition elements commonly form more than one ion. For these ions, its
oxidation state is added to the elemental name. The oxidation state is written in
parentheses immediately after the name. For example, the formula of the iron(II) ion
is Fe2+.
6)
Three common transition elements normally form only one ion. The charges on
these ions must be memorized: nickel ion, Ni2+; zinc ion, Zn2+; silver ion, Ag+.
Learning Procedures
Study
Section 6.4. Focus on Goal 4 as you study.
Strategy
Your nomenclature skills build throughout this chapter. Learn each piece of
the system as you go, striving for mastery of each Goal. Goal 4 is divided
into three parts: main group elements, transition elements with more than one
charge, and transition elements with only one charge. Learn the system for
the main group elements: group number corresponds to charge. The charge
on three transition elements must be memorized; the charge on the others
comes from their names.
Answer
Questions, Exercises, and Problems 6–8. Check your answers with those at
the end of the chapter.
Workbook
If your instructor recommends the Active Learning Workbook, do
Questions, Exercises, and Problems 6–8.
Chapter 6–Assignment C: Acids, Oxyanions, and Acid Anions
Thus far, you can write the names and formulas of elements, binary molecular compounds,
and monatomic ions. In this assignment you'll expand your skill to acids and their
corresponding anions. Here are the main points to look for as you study:
34
Copyright © 2004 Brooks/Cole, a division of Thomson Learning, Inc.
No part of this work may be reproduced without the written permission of the publisher.
Chapter 6
Chemical Nomenclature
1)
An acid ionizes in water to give H+ and an anion. A general equation used to
describe acid ionization is HX Æ H+ + X– .
2)
Five -ic acids must be memorized: carbonic acid, H2 CO3 ; nitric acid, HNO3 ;
phosphoric acid, H3 PO4 ; sulfuric acid, H2 SO4 ; chloric acid, HClO3 .
3)
A system is used to name acids with different numbers of oxygens than the related
-ic acids. Learn the system.
4)
A system is used to name ions formed from total ionization of acids. In this system
-ic acids form -ate ions and -ous acids form -ite ions. Learn the system.
5)
Acid anions are named in the same way as oxyanions, with the term hydrogen or
dihydrogen added to indicate the number of hydrogen ions bonded to the oxyanion.
Learning Procedures
Study
Sections 6.5 and 6.6. Focus on Goals 5 and 6 as you study.
Strategy
This is a long, challenging assignment. Take the time to learn it thoroughly.
You will not be able to succeed in the goals that appear later in this chapter
without mastering this assignment. Start by memorizing the five -ic acids.
Learn them inside and out. Do not learn them by grouping them into a
system. For each name, you need to be able to immediately write the formula
and vice versa. Once you've memorized the -ic acids, learn the system by
which other acids are named. Follow your learning by lots of practice.
Answer
Questions, Exercises, and Problems 9–14. Check your answers with those at
the end of the chapter.
Workbook
If your instructor recommends the Active Learning Workbook, do
Questions, Exercises, and Problems 9–14.
Chapter 6–Assignment D: Names and Formulas of Ionic Compounds
In this assignment, you'll combine cation and anion naming skills to name ionic compounds
called salts. Look for these high points:
1)
The ammonium ion is NH4 +; the hydroxide ion is OH– .
2)
To write the formulas for ionic compounds, write the symbol for the cation, then the
anion. Use subscripts to indicate the number of each ion needed so that the total
charge of the compound is zero.
3)
To name ionic compounds, name the cation, then the anion.
4)
Hydrates are ionic compounds that exist with a definite number of water molecules
in their crystal structure. Waters of hydration are indicated by the “ •”!symbol
before the number of water molecules.
35
Copyright © 2004 Brooks/Cole, a division of Thomson Learning, Inc.
No part of this work may be reproduced without the written permission of the publisher.
Study Guide for Introductory Chemistry: An Active Learning Approach
Learning Procedures
Study
Sections 6.7–6.11. Focus on Goals 7–11 as you study.
Strategy
In this assignment, you draw on your skills from the previous assignments
in this chapter. If you have trouble, you probably need to review the material
earlier in the chapter. The more you practice this material, the better you'll be
at doing it. A word of warning: Many instructors will incorporate
nomenclature into problems for the remainder of the course. In other words,
deriving a formula from a name will become the first step in many later
problems. The skills you learn in Chapter 6 will be used over and over again.
Learn these skills now!
Answer
Questions, Exercises, and Problems 15–25. Check your answers with those
at the end of the chapter.
Workbook
If your instructor recommends the Active Learning Workbook, do
Questions, Exercises, and Problems 15–25.
Chapter 6–Assignment E: Summary and Review
Sometimes to know what to do, you also have to know what not to do. Here's a list of the
most frequent student nomenclature errors.
1)
Students have not learned the formulas of the diatomic elements. To remember the
seven elements that form diatomic molecules, first notice the position of the elements
N, O, F, Cl, Br, and I on the periodic table. They form the shape of the number 7.
Add hydrogen and you have the seven diatomics. Also remember the sentence:
Horses Need Oats For Clear Brown Iz. The first letter or two of each word is the
symbol for the elements that form diatomic molecules, in order of increasing atomic
number. This will even help you get the symbol of fluorine correct; it's F, not Fl.
2)
In naming binary molecular compounds, the Greek prefixes for number must be
used before the name of the element that contributes more than one atom to the
molecule. The prefix mono- may be used if only one atom of an element is present;
in the absence of a prefix, one atom is understood.
3)
Students try to memorize all the formulas or names, or even ions. That's a waste of
time, if not impossible. Learn the system and limit your memorization to the few
essential starting points.
4)
You must memorize the five -ic acids. Learn these “cold”; that is, do not make up
some system for learning them as a group. You need to be able to instantly go
between name and formula for these five acids.
5)
Some students fail to appreciate the importance of Table 6.3. This summarizes the
nomenclature system for acids and their ions, on which the names of many ionic
compounds are based. This table should be the focal point of your memorization
efforts.
36
Copyright © 2004 Brooks/Cole, a division of Thomson Learning, Inc.
No part of this work may be reproduced without the written permission of the publisher.
Chapter 6
Chemical Nomenclature
The entire system is summarized in Table 6.9. Everything you need is here. With this
knowledge and a periodic table you can write the names and formulas of thousands of
compounds. After learning the system, practice, practice, practice. Tables 6.12 and 6.13 in
the Questions, Exercises, and Problems section offer a good opportunity for practice. Don't
neglect to answer Questions 26 to 40, which are an assortment of questions from the whole
chapter.
Avoid the temptation to always capitalize chemical names. When you write a chemical name,
there is no need to capitalize the first letter unless grammar dictates it should be a capital
letter.
Learning Procedures
Review
your lecture and textbook notes.
the Chapter in Review and the Key Terms and Concepts, and read the Study
Hints and Pitfalls to Avoid.
Answer
Concept-Linking Exercises 1–4. Check your answers with those at the end
of the chapter.
Questions, Exercises, and Problems 26–40. Check your answers with those
at the end of the chapter.
Workbook
If your instructor recommends the Active Learning Workbook, do
Questions, Exercises, and Problems 26–40.
Take
the chapter summary test that follows. Check your answers with those at the
end of this assignment.
Chapter 6 Sample Test
Instructions: For each name given, write the formula; for each formula given, write the
name. You may use a “clean” periodic table. Te is the symbol for tellurium, Z = 52.
bromine
H2
nitrogen
O2
chlorine
F2
magnesium oxide
CaI2
sodium fluoride
Ba2+
aluminum nitride
Na2 S
calcium phosphide
Cl–
potassium bromide
Li2 O
barium sulfide
AlCl3
37
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Study Guide for Introductory Chemistry: An Active Learning Approach
lithium fluoride
Mg3 P2
manganese(III) ion
Cu2+
phosphorus tribromide
NaClO
perchloric acid
S2 F2
ammonium phosphate
H2 S
iron(II) nitrate
HIO4
potassium bromite
Na2 TeO3
sodium hydrogen carbonate
Mg(H2 PO4 )2
sulfuric acid
PbCl2
hydrofluoric acid
K2 CO3
potassium iodide
Si2 F6
oxygen difluoride
CuI
magnesium sulfate heptahydrate
BaCl2 • 2 H2 O
___
Answers to Chapter 6 Sample Test
bromine, Br2
H2 , hydrogen
nitrogen, N2
O2 , oxygen
chlorine, Cl2
F2 , fluorine (watch the spelling!)
magnesium oxide, MgO
CaI2 , calcium iodide
sodium fluoride, NaF
Ba2+, barium ion
aluminum nitride, AlN
Na2 S, sodium sulfide
calcium phosphide, Ca3 P2
Cl– , chloride ion
potassium bromide, KBr
Li2 O, lithium oxide
barium sulfide, BaS
AlCl3 , aluminum chloride
lithium fluoride, LiF
Mg3 P2 , magnesium phosphide
manganese(III) ion, Mn3+
Cu2+, copper(II) ion
phosphorus tribromide, PBr3
NaClO, sodium hypochlorite
perchloric acid, HClO4
S2 F2 , disulfur difluoride
ammonium phosphate, (NH4 )3 PO4
H2 S, hydrogen sulfide or hydrosulfuric acid
iron(II) nitrate, Fe(NO3 )2
HIO4 , periodic acid
potassium bromite, KBrO2
Na2 TeO3 , sodium tellurite
sodium hydrogen carbonate, NaHCO3
Mg(H2 PO4 )2 , magnesium dihydrogen phosphate
sulfuric acid, H2 SO4
PbCl2 , lead(II) chloride
hydrofluoric acid, HF
K2 CO3 , potassium carbonate
potassium iodide, KI
Si2 F6 , disilicon hexafluoride
oxygen difluoride, OF2
CuI, copper(I) iodide
magnesium sulfate heptahydrate, MgSO4 • 7 H2 O
BaCl2 • 2 H2 O, barium chloride dihydrate
38
Copyright © 2004 Brooks/Cole, a division of Thomson Learning, Inc.
No part of this work may be reproduced without the written permission of the publisher.