Chapter 4
Chemical Bonding:
The Ionic Bond Model
Chapter 4
Chapter Outline
4.1
4.2
4.3
4.4
4.5
4.6
4.7
4.8
4.9
4.10
4.11
Chemical bonds
Valence electrons and Lewis symbols
The octet rule
The ionic bond model
The sign and magnitude of ionic charge
Lewis structures for ionic compounds
Chemical formulas for ionic compounds
The structure of ionic compounds
Recognizing and naming binary ionic compounds
Polyatomic ions
Chemical formulas and names for ionic compounds
containing polyatomic ions
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2
Section 4.1
Chemical Bond
•  Attractive force that holds two atoms together in
a more complex unit
•  Formed as a result of interactions between
electrons found in the combining atoms
•  Types
–  Ionic bonds
–  Covalent bonds
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Section 4.1
Chemical Bond
Ionic Bond
•  Formed through the transfer of one or more
electrons from one atom or group of atoms to
another atom or group of atoms
•  Ionic compound: Compounds in which ionic
bonds are present
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4
Section 4.1
Chemical Bond
Covalent Bond
•  Formed through the sharing of one or more pairs
of electrons between two atoms
•  Molecular compound: Compound in which
covalent bonds are present
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Section 4.1
Chemical Bond
Bonding
•  Most bonds are not 100% ionic or 100%
covalent
–  Some degree of both ionic and covalent
characteristics exist
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Section 4.1
Chemical Bond
Fundamental Concepts of Bonding
•  Not all electrons in an atom participate in
bonding
–  Those that do are called valence electrons
•  Certain arrangements of electrons are more
stable than others
–  This is explained by the octet rule
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Section 4.1
Chemical Bond
An ionic bond is formed by the:
a. sharing of one or more electrons between atoms.
b. sharing of two or more electrons between atoms.
c. transfer of one or more electrons from one atom to
another.
d. transfer of two or more electrons from one atom to
another.
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Section 4.1
Chemical Bond
An ionic bond is formed by the:
a. sharing of one or more electrons between atoms.
b. sharing of two or more electrons between atoms.
c. transfer of one or more electrons from one atom to
another.
d. transfer of two or more electrons from one atom to
another.
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Section 4.2
Valence Electrons and Lewis Symbols
Valence Electron
•  Electron in the outermost electron shell of a
representative element or noble-gas element
–  Valence electrons are found in either s or p subshells
in representative elements or noble gases
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Section 4.2
Valence Electrons and Lewis Symbols
Lewis Symbol
•  Chemical symbol of an element surrounded by
dots equal in number to the number of valence
electrons present in atoms of the element
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Section 4.2
Valence Electrons and Lewis Symbols
Figure 4.1 - Lewis Symbols for Selected Representative
and Noble-Gas Elements
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Section 4.2
Valence Electrons and Lewis Symbols
Concept Check
•  Determine the number of valence electrons in
each of the following elements:
Ca
Se
C
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Section 4.2
Valence Electrons and Lewis Symbols
Concept Check
•  Determine the number of valence electrons in
each of the following elements:
Ca
2 valence electrons (4s2)
Se
6 valence electrons (4s24p4)
C
4 valence electrons (2s22p2)
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Section 4.2
Valence Electrons and Lewis Symbols
Important Generalizations About Valence Electrons
1.  Representative elements in the same group
have the same number of valence electrons
2.  The number of valence electrons for
representative elements is the same as the
Roman numeral periodic-table group number
3.  The maximum number of valence electrons for
any element is eight
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Section 4.2
Valence Electrons and Lewis Symbols
Concept Check
•  Write Lewis symbols for the following
elements:
O
P
F
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Section 4.2
Valence Electrons and Lewis Symbols
Concept Check
•  Write Lewis symbols for the following
elements:
O
O
P
P
F
F
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Section 4.2
Valence Electrons and Lewis Symbols
A valence electron is an electron in the outer-most
electron shell of an atom. The shorthand method
developed by scientists to represent the number of
valence electrons in an atom involves the use of:
a. ionic bond model.
b. dot symbols.
c. octet rule.
d. Lewis symbols or electron-dot symbols.
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Section 4.2
Valence Electrons and Lewis Symbols
A valence electron is an electron in the outer-most
electron shell of an atom. The shorthand method
developed by scientists to represent the number of
valence electrons in an atom involves the use of:
a. ionic bond model.
b. dot symbols.
c. octet rule.
d. Lewis symbols or electron-dot symbols.
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Section 4.3
The Octet Rule
•  Certain arrangements of valence electrons are
more stable than others
•  Valence electron configurations of the noble
gases are considered the most stable of all
valence electron configurations
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Section 4.3
The Octet Rule
Octet Rule
•  In forming compounds, atoms of elements lose,
gain, or share electrons
–  Produce a noble-gas electron configuration for each
of the atoms involved
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Section 4.3
The Octet Rule
The rule that states that atoms lose, gain, or share
electrons to form a noble-gas electron
configuration is known as the:
a. octet rule.
b. electron rule.
c. noble gas rule.
d. bonding rule.
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Section 4.3
The Octet Rule
The rule that states that atoms lose, gain, or share
electrons to form a noble-gas electron
configuration is known as the:
a. octet rule.
b. electron rule.
c. noble gas rule.
d. bonding rule.
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Section 4.4
The Ionic Bond Model
Ion
•  Atom (or group of atoms) that is electrically
charged as a result of the loss or gain of
electrons
•  Negatively charged ion - Atom gains one or
more electrons
•  Positively charged ion - Atom loses one or more
electrons
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Section 4.4
The Ionic Bond Model
Figure 4.3 - Positive and Negative Ions
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Section 4.4
The Ionic Bond Model
Concept Check
•  Give the chemical symbol for each of the
following ions.
a.  The ion formed when a potassium atom loses one
electron.
b.  The ion formed when a sulfur atom gains two
electrons.
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Section 4.4
The Ionic Bond Model
Concept Check
•  Give the chemical symbol for each of the
following ions.
a.  The ion formed when a potassium atom loses one
electron.
K+
b.  The ion formed when a sulfur atom gains two
electrons.
S2–
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Section 4.4
The Ionic Bond Model
Atoms can either lose or gain electrons resulting in
the formation of:
a. ions.
b. cations.
c. anions.
d. all of these.
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Section 4.4
The Ionic Bond Model
Atoms can either lose or gain electrons resulting in
the formation of:
a. ions.
b. cations.
c. anions.
d. all of these.
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Section 4.5
The Sign and Magnitude of Ionic Charge
•  Atoms tend to gain or lose electrons until they
have obtained an electron configuration that is
the same as that of a noble gas
–  Example: Na+ (1s22s22p63s1)
•  Loss of one electron gives it the electron configuration
of neon
–  Ne (1s22s22p6)
•  Gain of seven electrons gives it the electron
configuration of argon
–  Ar (1s22s22p63s23p6)
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Section 4.5
The Sign and Magnitude of Ionic Charge
Guidelines of Electron Loss and Gain by Atoms of
Elements
1.  Metal atoms containing one, two, or three
valence electrons tend to lose electrons to
acquire a noble-gas electron configuration
Group
Charge
IA
1+
IIA
2+
IIIA
3+
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Section 4.5
The Sign and Magnitude of Ionic Charge
Guidelines of Electron Loss and Gain by Atoms of
Elements
2. Nonmetal atoms containing five, six, or seven
valence electrons tend to gain electrons to
acquire a noble-gas electron configuration
Group
Charge
VIIA
1-
VIA
2-
VA
3-
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Section 4.5
The Sign and Magnitude of Ionic Charge
Guidelines of Electron Loss and Gain by Atoms of
Elements
3.  Elements in Group IVA occupy unique positions
relative to the noble gases
–  Could gain or lose four electrons to attain a noblegas structure
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Section 4.5
The Sign and Magnitude of Ionic Charge
Isoelectronic Species
•  An atom and an ion, or two ions, that have the
same number and configuration of electrons
–  Example: The electronic configuration of N3-, O2-, F-,
Na+, Mg2+, and Al3+ is 1s22s22p6
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Section 4.5
The Sign and Magnitude of Ionic Charge
Table 4.1 - Isoelectronic Species Ne and Mg2+
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Section 4.5
The Sign and Magnitude of Ionic Charge
Concept Check
•  Choose an alkali metal, an alkaline earth metal,
a noble gas, and a halogen so that they
constitute an isoelectronic series when the
metals and halogen are written as their most
stable ions.
• 
• 
• 
What is the electron configuration for each species?
Determine the number of electrons for each species.
Determine the number of protons for each species.
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Section 4.5
The Sign and Magnitude of Ionic Charge
What is the electron configuration of the
magnesium ion?
a. 1s22s22p6
b. 1s22s22p63s2
c. 1s22s22p63s1
d. 1s22s2p6
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Section 4.5
The Sign and Magnitude of Ionic Charge
What is the electron configuration of the
magnesium ion?
a. 1s22s22p6
b. 1s22s22p63s2
c. 1s22s22p63s1
d. 1s22s2p6
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Section 4.6
Lewis Structures for Ionic Compounds
Formation of an Ionic Compound
•  Ion formation requires the presence of:
–  A metal that can donate electrons
–  A nonmetal that can accept electrons
•  Electrons lost by the metal are the same ones
gained by the nonmetal
•  Positive and negative ions simultaneously
formed from an electron transfer attract one
another
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Section 4.6
Lewis Structures for Ionic Compounds
Lewis Structure
•  Combination of Lewis symbols that represents
either the transfer or the sharing of electrons in
chemical bonds
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Section 4.6
Lewis Structures for Ionic Compounds
Reaction Between Sodium and Chlorine
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Section 4.6
Lewis Structures for Ionic Compounds
Reaction Between Sodium and Oxygen
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Section 4.6
Lewis Structures for Ionic Compounds
Reaction Between Calcium and Chlorine
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Section 4.6
Lewis Structures for Ionic Compounds
What is the correct definition of a Lewis structure?
a. Lewis structure is a combination of Lewis symbols
representing the transfer of electrons in chemical bonds.
b. Lewis structure is a combination of Lewis symbols
representing the sharing of electrons in chemical bonds.
c. Lewis structure is a combination of Lewis symbols that
represents either the transfer or sharing of electrons in
chemical bonds.
d. Lewis structure is a combination of Lewis symbols
representing an ionic bond.
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Section 4.6
Lewis Structures for Ionic Compounds
What is the correct definition of a Lewis structure?
a. Lewis structure is a combination of Lewis symbols
representing the transfer of electrons in chemical bonds.
b. Lewis structure is a combination of Lewis symbols
representing the sharing of electrons in chemical bonds.
c. Lewis structure is a combination of Lewis symbols that
represents either the transfer or sharing of electrons in
chemical bonds.
d. Lewis structure is a combination of Lewis symbols
representing an ionic bond.
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Section 4.7
Chemical Formulas for Ionic Compounds
•  Ionic compounds are always neutral
–  No net charge is present
•  Ratio in which positive and negative ions
combine is the ratio that achieves charge
neutrality for the resulting compound
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Section 4.7
Chemical Formulas for Ionic Compounds
Writing Chemical Formulas for Ionic Compounds
1.  Symbol for the positive ions is always written
first
2.  Charges on the ions that are present are not
shown in the formula
3.  Subscripts in the formula give the combining
ratio for the ions
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Section 4.7
Chemical Formulas for Ionic Compounds
Example
•  Compound formed between Na+ and P3–
–  Na+ and P3– ions combine in a 3-to-1 ratio
–  Formula - Na3P
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Section 4.7
Chemical Formulas for Ionic Compounds
Concept Check
•  Determine the chemical formula for the
compound that is formed when each of the
following pairs of ions interact.
Ba2+ and Cl–
Fe3+ and O2–
Pb4+ and O2–
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Section 4.7
Chemical Formulas for Ionic Compounds
Concept Check
•  Determine the chemical formula for the
compound that is formed when each of the
following pairs of ions interact.
Ba2+ and Cl–
BaCl2
Fe3+ and O2–
Fe2O3
Pb4+ and O2–
PbO2
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Section 4.7
Chemical Formulas for Ionic Compounds
What is the correct formula for the combination of
Al3+ and Cl-?
a. Al3Cl
b. Al2Cl3
c. AlCl3
d. Al3Cl1
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Section 4.7
Chemical Formulas for Ionic Compounds
What is the correct formula for the combination of
Al3+ and Cl-?
a. Al3Cl
b. Al2Cl3
c. AlCl3
d. Al3Cl1
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Section 4.8
The Structure of Ionic Compounds
Solid Ionic Compounds
•  Consist of positive and negative ions arranged in
such a way that each ion is surrounded by
nearest neighbors of the opposite charge
•  Any given ion is bonded by electrostatic
attractions to all the other ions of opposite
charge immediately surrounding it
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Section 4.8
The Structure of Ionic Compounds
Figure 4.4 - Two-Dimensional Cross-Section and ThreeDimensional View of Sodium Chloride (NaCl)
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Section 4.8
The Structure of Ionic Compounds
Formula Unit
•  Smallest whole-number repeating ratio of ions
present in an ionic compound that results in
charge neutrality
•  Chemical formulas for ionic compounds
represent the simplest ratio of ions present
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Section 4.8
The Structure of Ionic Compounds
Figure 4.5 - Cross-Section of the Structure of the Ionic
Solid NaCl
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Section 4.8
The Structure of Ionic Compounds
What term is used to refer to the smallest wholenumber repeating ratio of ions present in an ionic
compound?
a. Molecule unit
b. Ion unit
c. Ion molecule unit
d. Formula unit
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Section 4.8
The Structure of Ionic Compounds
What term is used to refer to the smallest wholenumber repeating ratio of ions present in an ionic
compound?
a. Molecule unit
b. Ion unit
c. Ion molecule unit
d. Formula unit
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Section 4.9
Recognizing and Naming Binary Ionic Compounds
•  Binary compounds: Compounds composed of
two elements
•  Binary ionic compounds: Compound in which
one element present is a metal and the other is
a nonmetal
–  Metal is present as the positive ion and the nonmetal
is present as the negative ion
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Section 4.9
Recognizing and Naming Binary Ionic Compounds
Naming Binary Ionic Compounds
•  Full name of the metallic element is given first
–  This is followed by a separate word containing
the stem of the nonmetallic element name and
the suffix –ide
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Section 4.9
Recognizing and Naming Binary Ionic Compounds
Table 4.2 - Names of Selected Common Nonmetallic
Ions
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Section 4.9
Recognizing and Naming Binary Ionic Compounds
Examples
KCl
Potassium chloride
MgBr2
Magnesium bromide
CaO
Calcium oxide
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Section 4.9
Recognizing and Naming Binary Ionic Compounds
Naming Ionic Compounds for Metals with Variable Charges
•  Transition and inner transition metals form more
than one type of positive charge
•  Charge on the metal ion must be incorporated
into the name
–  Accomplished by using roman numerals
–  Charge on the nonmetal ion present can be used to
calculate the charge on the metal ion if the latter is
unknown
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Section 4.9
Recognizing and Naming Binary Ionic Compounds
Examples
CuBr
Copper(I) bromide
FeS
Iron(II) sulfide
PbO2
Lead(IV) oxide
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Section 4.9
Recognizing and Naming Binary Ionic Compounds
Figure 4.8 - Metallic Elements That Exhibit a Fixed Ionic
Charge
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Section 4.9
Recognizing and Naming Binary Ionic Compounds
Exercise
•  Name each of the following compounds:
K2S
Fe2O3
CoCl2
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Section 4.9
Recognizing and Naming Binary Ionic Compounds
Exercise
•  Name each of the following compounds:
K2S
potassium sulfide
Fe2O3
iron(III) oxide
CoCl2
cobalt(II) chloride
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Section 4.9
Recognizing and Naming Binary Ionic Compounds
What is a binary ionic compound?
a. An ionic compound composed of a metal and a nonmetal.
b. An ionic compound composed of two metals.
c. An ionic compound composed of two nonmetals.
d. An ionic compound composed of two metals and two
nonmetals.
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Section 4.9
Recognizing and Naming Binary Ionic Compounds
What is a binary ionic compound?
a. An ionic compound composed of a metal and a nonmetal.
b. An ionic compound composed of two metals.
c. An ionic compound composed of two nonmetals.
d. An ionic compound composed of two metals and two
nonmetals.
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Section 4.10
Polyatomic Ions
•  Ions formed from a group of atoms through loss
or gain of electrons
•  Stable and maintain their identities during
chemical reactions
•  Examples of compounds containing polyatomic
ions
–  NaOH
–  Mg(NO3)2
–  (NH4)2SO4
Sodium hydroxide
Magnesium nitrate
Ammonium sulfate
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Section 4.10
Polyatomic Ions
Generalizations
1. Most polyatomic ions have a negative charge
–  Exceptions: H3O+ (hydronium) and NH4+ (ammonium)
2. Most of the ions contain oxygen atoms
–  Exceptions: CN− (cyanide) and NH4+ (ammonium)
3. Two of the negatively charged polyatomic ions,
OH– and CN–, have names ending in –ide and
the rest of them have names ending in –ate
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Section 4.10
Polyatomic Ions
Generalizations
3.  Two positive ions have names that end in –ium
–  Hydronium (H3O+) and ammonium (NH4+)
4.  A number of pairs of ions exist wherein one
member of the pair differs from the other by
having a hydrogen atom present
–  In such pairs, the charge on the ion that contains
hydrogen is always 1 less than that on the other ion
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Section 4.10
Polyatomic Ions
What is a polyatomic ion?
a. An ion formed by a group of positive and negative ions.
b. An ion formed from a group of atoms held together by
covalent bonds and is positively or negatively charged.
c. An ion formed by a group of positive and negative ions
held together by covalent bonds.
d. All of these.
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Section 4.10
Polyatomic Ions
What is a polyatomic ion?
a. An ion formed by a group of positive and negative ions.
b. An ion formed from a group of atoms held together by
covalent bonds and is positively or negatively charged.
c. An ion formed by a group of positive and negative ions
held together by covalent bonds.
d. All of these.
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Section 4.11
Chemical Formulas and Names for Ionic Compounds Containing Polyatomic Ions
•  Determined in the same way as those for ionic
compounds that contain monatomic ions
•  Positive and negative charges present must add
to zero
–  Na+ and OH– form NaOH
–  Mg2+ and NO3– form Mg(NO3)2
–  NH4+ and SO42– form (NH4)2SO4
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Section 4.11
Chemical Formulas and Names for Ionic Compounds Containing Polyatomic Ions
Exercise
•  Which of the following compounds is named
incorrectly?
a. 
b. 
c. 
d. 
e. 
KNO3
TiO2
Sn(OH)4
(NH4)2SO3
CaCrO4
potassium nitrate
titanium(II) oxide
tin(IV) hydroxide
ammonium sulfite
calcium chromate
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Section 4.11
Chemical Formulas and Names for Ionic Compounds Containing Polyatomic Ions
Exercise
•  Which of the following compounds is named
incorrectly?
a. 
b. 
c. 
d. 
e. 
KNO3
potassium nitrate
TiO2
titanium(II) oxide
Sn(OH)4
tin(IV) hydroxide
(NH4)2SO3 ammonium sulfite
CaCrO4
calcium chromate
titanium(IV) oxide
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Section 4.11
Chemical Formulas and Names for Ionic Compounds Containing Polyatomic Ions
What is the correct chemical formula for the
combination of ammonium(NH4+) and carbonate
(CO32-) ions?
a. 2(NH4)CO3
b. 2NH4CO3
c. (NH4)2CO3
d. NH4CO3
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Section 4.11
Chemical Formulas and Names for Ionic Compounds Containing Polyatomic Ions
What is the correct chemical formula for the
combination of ammonium(NH4+) and carbonate
(CO32-) ions?
a. 2(NH4)CO3
b. 2NH4CO3
c. (NH4)2CO3
d. NH4CO3
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Chapter 4
Concept Question 1
After placing a soft, lustrous, and malleable material in a container of
yellowish gas, a violent reaction occurs leaving a white crystalline
material. You decide to break the rule “Never taste chemicals in a
laboratory” and find that it tastes very salty. Which of the following is
correct?
a. Not enough information is provided to determine what the two materials and
product are.
b. The two materials are likely to be the elements sodium and chlorine reacting
to share electrons to produce the molecular compound sodium chloride.
c. The two materials are likely to be the elements sodium and chlorine, both
reacting by a transfer of electrons to produce the ionic compound sodium
chloride.
d. The two materials are homogenous compounds reacting to produce an
unidentifiable salt.
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Chapter 4
Concept Question 1
After placing a soft, lustrous, and malleable material in a container of
yellowish gas, a violent reaction occurs leaving a white crystalline
material. You decide to break the rule “Never taste chemicals in a
laboratory” and find that it tastes very salty. Which of the following is
correct?
a. Not enough information is provided to determine what the two materials and
product are.
b. The two materials are likely to be the elements sodium and chlorine reacting
to share electrons to produce the molecular compound sodium chloride.
c. The two materials are likely to be the elements sodium and chlorine, both
reacting by a transfer of electrons to produce the ionic compound sodium
chloride.
d. The two materials are homogenous compounds reacting to produce an
unidentifiable salt.
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81
Chapter 4
Concept Question 2
Fill in the following table with the correct information.
a. 1. Sodium carbonate; 2. Magnesium carbonate; 3. Na3PO4; 4.
MgPO4
b. 1. Sodium hydrogen carbonate; 2. Magnesium bicarbonate; 3.
Na3PO4; 4. Mg3(PO4)2
c. 1. Sodium hydrogen carbonate; 2. Magnesium bicarbonate; 3.
Na(PO4)3; 4. Mg3PO4
d. 1. Sodium hydrogen carbonate; 2. Magnesium bicarbonate; 3.
NaPO4; 4. Mg3(PO4)2
Copyright ©2016 Cengage Learning. All Rights Reserved.
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82
Chapter 4
Concept Question 2
Fill in the following table with the correct information.
a. 1. Sodium carbonate; 2. Magnesium carbonate; 3. Na3PO4; 4.
MgPO4
b. 1. Sodium hydrogen carbonate; 2. Magnesium bicarbonate; 3.
Na3PO4; 4. Mg3(PO4)2
c. 1. Sodium hydrogen carbonate; 2. Magnesium bicarbonate; 3.
Na(PO4)3; 4. Mg3PO4
d. 1. Sodium hydrogen carbonate; 2. Magnesium bicarbonate; 3.
NaPO4; 4. Mg3(PO4)2
Copyright ©2016 Cengage Learning. All Rights Reserved.
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83