Transcript chemistry 7.1

Chapter 7
Chemical Formulas and Chemical
Compounds
Table of Contents
Section 1 Chemical Names and Formulas
Section 2 Oxidation Numbers
Section 3 Using Chemical Formulas
Section 4 Determining Chemical Formulas
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Chapter 7
Section 1 Chemical Names and
Formulas
Opener #9 - Thursday, October 18, 2012
• CCl4
MgCl2
• 1. Guess the name of each of the above compounds
based on the formulas written.
• 2. What kind of information can you discern from the
formulas?
• 3. Guess which of the compounds represented is
molecular and which is ionic.
• Chemical formulas form the basis of the language of
chemistry and reveal much information about the
substances they represent.
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Chapter 7
Section 1 Chemical Names and
Formulas
Objectives
• Explain the significance of a chemical formula.
• Determine the formula of an ionic compound formed
between two given ions.
• Name an ionic compound given its formula.
• Using prefixes, name a binary molecular compound
from its formula.
• Write the formula of a binary molecular compound
given its name.
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Chapter 7
Visual Concepts
Reading Chemical Formulas
NOT NEEDED
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7.1
Naming Ions
A rose is rosa in Spanish,
warda in Arabic, and julab in
Hindi. To truly understand
another culture, you must
first learn the language used
in that culture. Similarly, to
understand chemistry, you
must learn its language. For
this you need to know how to
name ions.
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Chapter 7
Section 1 Chemical Names and
Formulas
Significance of a Chemical Formula
• A chemical formula indicates the relative number of
atoms of each kind in a chemical compound.
• For a molecular compound, the chemical formula
reveals the number of atoms of each element
contained in a single molecule of the compound.
• example: octane — C8H18
The subscript after the C
indicates that there are 8
carbon atoms in the molecule.
The subscript after the H
indicates that there are 18
hydrogen atoms in
the molecule.
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Chapter 7
• Hydrocarbons are molecular compounds composed
only of carbon and hydrogen.
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Chapter 7
Section 1 Chemical Names and
Formulas
Significance of a Chemical Formula, continued
• An ionic compound consists of a lattice of positive and
negative ions held together by mutual attraction.
• The chemical formula for an ionic compound
represents one formula unit—the simplest ratio of the
compound’s positive ions (cations) and its negative
ions (anions).
• example: aluminum sulfate — Al2(SO4)3
• Parentheses surround the polyatomic ion
as a unit. The subscript 3 refers to the unit.
to identify it
• Note also that there is no subscript for sulfur: when there is no subscript
next to an atom, the subscript is understood to be 1.
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7.1
Naming Ions
>
Monatomic Ions
Monatomic Ions
How are the charges of Group A metal
and nonmetal ions related to their
positions in the periodic table?
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7.1
Naming Ions
>
Monatomic Ions
Monatomic ions consist of a single atom with a
positive or negative charge resulting from the
loss or gain of one or more valence electrons,
respectively.
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Chapter 7
Section 1 Chemical Names and
Formulas
Monatomic Ions
• Many main-group elements can lose or gain electrons
to form ions.
• Ions formed form a single atom are known as
monatomic ions.
• example: To gain a noble-gas electron
configuration, nitrogen gains three electrons to
form N3– ions.
• Some main-group elements tend to form covalent
bonds instead of forming ions.
• examples: carbon and silicon
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7.1
Naming Ions
>
Monatomic Ions
Cations
When the metals in Groups 1, 2, & 13 (1A, 2A,
and 3A) lose electrons, they form cations with
positive charges equal to their group number.
(13 also known as 3A.)
Group 1 has 1+ charge (loses 1 electron)
Group 2 has 2+ charge (loses 2 electrons)
Aluminum in Group 13 (3A) has 3+ charge
(loses 3 electrons).
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7.1
Naming Ions
>
Monatomic Ions
The names of the cations of the Group 1, 2, and
13 (1A, Group 2A, and Group 3A) metals are the
same as the name of the metal, followed by the
word ion or cation.
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Chapter 7
Section 1 Chemical Names and
Formulas
Monatomic Ions, continued
Naming Monatomic Ions
• Monatomic cations are identified simply by the element’s name.
• examples:
• K+ is called the potassium cation
• Mg2+ is called the magnesium cation
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7.1
Naming Ions
>
Monatomic Ions
These elements have
ionic charges that can be
obtained from their group
numbers.
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7.1
Naming Ions
>
Monatomic Ions
Group 15, 16, & 17
(5A, 6A, 7A)
elements form
anions.
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7.1
Naming Ions
>
Monatomic Ions
Anions
The charge of any ion of a nonmetal
Group is determined by subtracting 8
from the valence electron number.
(example Group 15 would have 5
valence electrons, so 5-8 = -3, so
charge is -3 for Group 15. Similarly
charge for Group 16 is -2 and Group 17
is -1.
Anion names start with the stem of the
element name and end in -ide.
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Chapter 7
Section 1 Chemical Names and
Formulas
Monatomic Ions, continued
Naming Monatomic Ions
• For monatomic anions, the ending of the element’s name is
dropped, and the ending -ide is added to the root name.
• examples:
• F– is called the fluoride anion
• N3– is called the nitride anion
• Group 14 share electrons in covalent bonds.
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7.1
Naming Ions
>
Monatomic Ions
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Chapter 7
Section 1 Chemical Names and
Formulas
Common Monatomic Ions
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Chapter 7
Visual Concepts
Naming Monatomic Ions
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7.1
Naming Ions
>
Monatomic Ions
Ions of Transition Metals
How are the charges of some transition
metal ions determined?
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7.1
Naming Ions
>
Monatomic Ions
The charges of the cations of many
transition metal ions must be determined
from the number of electrons lost.
The d-block (transition metals) form 2 or
more cations with different charges.
Example Copper, Cu may be 1+ or 2+
depending upon if it loses 1 or 2
electrons.
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7.1
Naming Ions
>
Monatomic Ions
These colorful solutions contain the transition
metal ions Co3+, Cr3+, Fe3+, Ni2+, and Mn2+.
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7.1
Naming Ions
>
Monatomic Ions
Many transition metal
compounds are colored and
can be used as pigments.
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7.1
Naming Ions
>
Monatomic Ions
Two methods are used to name the ions of
transition metals.
• The Stock system
• The classical method
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7.1
Naming Ions
>
Monatomic Ions
In the Stock system, a Roman numeral in
parentheses is placed after the name of the
element to indicate the numerical value of the
charge.
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7.1
Naming Ions
>
Monatomic Ions
In an older less, useful method, the classical
name of the element is used to form the root
name for the element.
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7.1
Naming Ions
>
Monatomic Ions
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Chapter 7
Section 1 Chemical Names and
Formulas
Common Monatomic Ions
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1.1
Conceptual Problem 9.1
Conceptual problem 1.1
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1.1
Conceptual Problem 9.1
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1.1
Conceptual Problem 9.1
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Problems
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Problem-Solving 9.1 Solve
Problem 1 with the help of an
interactive guided tutorial.
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7.1
Naming and Writing
Formulas
for Ionic Compounds
A recipe is a formula for
the sauce—a complete list
of ingredients and their
proportions. Chemistry
also uses formulas. Once
you know the rules, you
can write the formula for
any chemical compound.
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Chapter 7
Section 1 Chemical Names and
Formulas
Binary Ionic Compounds
• Compounds composed of two elements are known as
binary compounds.
• In a binary ionic compound, the total numbers
of positive charges and negative charges must be
equal.
• To name any binary ionic compound, place the
cation name first, followed by the anion name.
• The formula for a binary ionic compound can be written
given the identities of the compound’s ions.
• example: magnesium bromide
Ions combined: Mg2+, Br–, Br–
Chemical formula: MgBr2
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Chapter 7
Section 1 Chemical Names and
Formulas
Binary Ionic Compounds, continued
• A general rule to use when determining the formula
for a binary ionic compound is “crossing over” to
balance charges between ions.
• example: aluminum oxide
1) Write the symbols for the ions.
Al3+ O2–
2) Cross over the charges by using the absolute
value of each ion’s charge as the subscript for the
other ion.
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Chapter 7
Section 1 Chemical Names and
Formulas
Binary Ionic Compounds, continued
• example: aluminum oxide, continued
3) Check the combined positive and negative
charges to see if they are equal.
(2  3+) + (3  2) = 0
The correct formula is Al2O3
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Chapter 7
Section 1 Chemical Names and
Formulas
Writing the Formula of an Ionic Compound
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Chapter 7
Section 1 Chemical Names and
Formulas
Naming Binary Ionic Compounds, continued
Sample Problem A
Write the formulas for the binary ionic compounds
formed between the following elements:
a. zinc and iodine
b. zinc and sulfur
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Chapter 7
Section 1 Chemical Names and
Formulas
Naming Binary Ionic Compounds, continued
Sample Problem A Solution
Write the symbols for the ions side by side. Write the
cation first.
a. Zn2+ I–
b. Zn2+ S2–
Cross over the charges to give subscripts.
a.
b.
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Chapter 7
Section 1 Chemical Names and
Formulas
Naming Binary Ionic Compounds, continued
Sample Problem A Solution, continued
Check the subscripts and divide them by their largest
common factor to give the smallest possible wholenumber ratio of ions.
a. The subscripts give equal total charges of 1  2+ = 2+
and 2  1– = 2–.
The largest common factor of the subscripts is 1.
The smallest possible whole-number ratio of ions in
the compound is 1:2.
The formula is ZnI .
2
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Section 1 Chemical Names and
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Naming Binary Ionic Compounds, continued
Sample Problem A Solution, continued
b. The subscripts give equal total charges of 2  2+ = 4+
and 2  2 = 4.
The largest common factor of the subscripts is 2.
The smallest whole-number ratio of ions in the
compound is 1:1.
The formula is
ZnS.
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Chapter 7
Section 1 Chemical Names and
Formulas
Naming Binary Ionic Compounds
• The nomenclature, or naming system, or binary ionic
compounds involves combining the names of the
compound’s positive and negative ions.
• The name of the cation is given first, followed by the
name of the anion:
• example: Al2O3 — aluminum oxide
• For most simple ionic compounds, the ratio of the ions
is not given in the compound’s name, because it is
understood based on the relative charges of the
compound’s ions.
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Chapter 7
Visual Concepts
Naming Ionic Compounds
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Chapter 7
Section 1 Chemical Names and
Formulas
Naming Binary Ionic Compounds, continued
The Stock System of Nomenclature
• Some elements such as iron, form two or more cations
with different charges.
• To distinguish the ions formed by such elements,
scientists use the Stock system of nomenclature.
• The system uses a Roman numeral to indicate an ion’s
charge.
• examples:
Fe2+
iron(II)
Fe3+
iron(III)
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Chapter 7
Visual Concepts
Naming Compounds Using the Stock System
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Chapter 7
Section 1 Chemical Names and
Formulas
Naming Binary Ionic Compounds, continued
The Stock System of Nomenclature, continued
Sample Problem B
Write the formula and give the name for the compound
formed by the ions Cr3+ and F–.
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Chapter 7
Section 1 Chemical Names and
Formulas
Naming Binary Ionic Compounds, continued
The Stock System of Nomenclature, continued
Sample Problem B Solution
Write the symbols for the ions side by side. Write the
cation first.
Cr3+ F–
Cross over the charges to give subscripts.
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Chapter 7
Section 1 Chemical Names and
Formulas
Naming Binary Ionic Compounds, continued
The Stock System of Nomenclature, continued
Sample Problem B Solution, continued
The subscripts give charges of 1  3+ = 3+ and
3  1 = 3.
The largest common factor of the subscripts is 1, so the
smallest whole number ratio of the ions is 1:3.
The formula is
CrF3.
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Chapter 7
Section 1 Chemical Names and
Formulas
Naming Binary Ionic Compounds, continued
The Stock System of Nomenclature, continued
Sample Problem B Solution, continued
Chromium forms more than one ion, so the name of the
3+ chromium ion must be followed by a Roman
numeral indicating its charge.
The compound’s name is
chromium(III) fluoride.
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Naming and Writing Formulas
for Ionic Compounds
>
Simulation 9.11
CLICK HERE FOR ACTIVITY
ACTIVITY INCLUDES THE FOLLOWING:
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Chapter 7
Practice Problems pg. 223
• Complete the above problems before going to next
page. Ask questions if you do not understand or miss
the problems!!!
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Chapter 7
ANSWERS to pg. 223
• Ask me if you do not understand.
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Chapter 7
Practice Problems pg. 225
• Complete all problems above before going to the next
page. ASK QUESTIONS if you do not understand!
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Chapter 7
ANSWERS pg. 225
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7.1
Naming Ions
>
Polyatomic Ions
Polyatomic Ions
What are the two endings of the names
of most polyatomic ions?
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7.1
Naming Ions
>
Polyatomic Ions
Some ions, called polyatomic ions, are
composed of more than one atom.
The names of most polyatomic anions
end in -ite or -ate.
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Chapter 7
Section 1 Chemical Names and
Formulas
Naming Binary Ionic Compounds, continued
Compounds Containing Polyatomic Ions
• Many common polyatomic ions are oxyanions—
polyatomic ions that contain oxygen.
• Some elements can combine with oxygen to form
more than one type of oxyanion.
• example: nitrogen can form
or
.
• The name of the ion with the greater number of oxygen
atoms ends in -ate. The name of the ion with the smaller
number of oxygen atoms ends in -ite.
nitrate
nitrite
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Chapter 7
Section 1 Chemical Names and
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Naming Binary Ionic Compounds, continued
Compounds Containing Polyatomic Ions, continued
• Some elements can form more than two types of
oxyanions.
• example: chlorine can form
,
,
or
• In this case, an anion that has one fewer oxygen atom
than the -ite anion has is given the prefix hypo-.
• An anion that has one more oxygen atom than the -ate
anion has is given the prefix per-.
hypochlorite
chlorite
chlorate
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7.1
Naming Ions
>
Polyatomic Ions
These models show the structures of four
common polyatomic ions.
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7.1
Naming Ions
>
Polyatomic Ions
Sodium hydrogen carbonate can relieve an
upset stomach.
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7.1
Naming Ions
>
Polyatomic Ions
HCO3–, HPO42–, and H2PO4– ions in your blood
are critical for your health.
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7.1
Naming Ions
>
Polyatomic Ions
Fertilizers contain HPO42– and H2PO4– ions.
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7.1
Naming Ions
>
Polyatomic Ions
Names and Formulas of
Some Common Polyatomic
Ions
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Chapter 7
Section 1 Chemical Names and
Formulas
Polyatomic Ions
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Chapter 7
Section 1 Chemical Names and
Formulas
Naming Compounds with Polyatomic Ions
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7.1
Naming and Writing Formulas
for Ionic Compounds
>
Compounds With Polyatomic
Ions
Naming Compounds with Polyatomic Ions
To name a compound containing a
polyatomic ion, state the cation first
and then the anion, just as you did in
naming binary ionic compounds.
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7.1
Naming and Writing Formulas
for Ionic Compounds
>
Compounds With Polyatomic
Ions
Sodium hypochlorite
(NaClO) is used as a
disinfectant for
swimming pools. The
metallic cation in this
compound is sodium
(Na+) so the polyatomic
ion must be ClO–.
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Naming and Writing Formulas
for Ionic Compounds
>
Simulation 9
CLICK HERE FOR ACTIVITY
ACTIVITY INCLUDES THE FOLLOWING:
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Chapter 7
Section 1 Chemical Names and
Formulas
Understanding Formulas for Polyatomic
Ionic Compounds
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Chapter 7
Visual Concepts
Naming Compounds Containing Polyatomic
Ions
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7.1
Naming and Writing Formulas
for Ionic Compounds
>
Compounds With Polyatomic
Ions
Compounds with Polyatomic Ions
How do you write the formulas and
names of compounds containing
polyatomic ions?
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7.1
Naming and Writing Formulas
for Ionic Compounds
>
Compounds With Polyatomic
Ions
Write the symbol for the cation followed
by the formula for the polyatomic ion
and balance the charges.
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7.1
Naming and Writing Formulas
for Ionic Compounds
>
Compounds With Polyatomic
Ions
For example, calcium nitrate is composed of a
calcium cation (Ca2+) and a polyatomic nitrate
anion (NO3–).
In calcium nitrate, two nitrate anions, each with a
1– charge, are needed to balance the 2+ charge
of each calcium cation. The formula for calcium
nitrate is Ca(NO3)2.
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Practice Problems For Conceptual Problem 9.3
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Problem-Solving 9.12 Solve
Problem 12 with the help of an
interactive guided tutorial.
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Naming and Writing Formulas
for Ionic Compounds
>
Simulation 9
Simulation 9 Simulate combining ions and
deriving the chemical formulas for several
ionic compounds.
CLICK BELOW TO SEE SIMULATION
ACTIVITY.
ACTIVITY - CLICK HERE
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Chapter 7
Section 1 Chemical Names and
Formulas
Naming Binary Ionic Compounds, continued
Compounds Containing Polyatomic Ions, continued
Sample Problem C
Write the formula for tin(IV) sulfate.
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Chapter 7
Section 1 Chemical Names and
Formulas
Naming Binary Ionic Compounds, continued
Compounds Containing Polyatomic Ions, continued
Sample Problem C Solution
Write the symbols for the ions side by side. Write the
cation first.
Cross over the charges to give subscripts. Add
parentheses around the polyatomic ion if necessary.
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Chapter 7
Section 1 Chemical Names and
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Naming Binary Ionic Compounds, continued
Compounds Containing Polyatomic Ions, continued
Sample Problem C Solution, continued
The total positive charge is 2  4+ = 8+.
The total negative charge is 4  2 = 8.
The largest common factor of the subscripts is 2, so the
smallest whole-number ratio of ions in the compound is
1:2.
The correct formula is therefore Sn(SO4)2.
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9.2
Conceptual Problem 9.2
TRY THESE
WITHOUT
WRITING
DOWN
Note if ratio
can be
simplified to
lower terms,
it will be reduced.
Example - a ratio
of 2:2 will reduce to
1:1.
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Sample Problems For Conceptual Problem 9.2
SEE IF YOU CAN GET THESE CORRECT BEFORE DOING THE
ADDITIONAL PRACTICE PROBLEMS - NOTE THE CLICK BELOW.
CLICK HERE FOR ACTIVITY
Problem Solving 9.11 Solve
Problem 11 with the help of an
interactive guided tutorial.
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Chapter 7
Practice Problems pg. 227
Complete all of these before going to next slide!
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Chapter 7
ANSWERS pg. 227
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7.1
Naming and Writing
Formulas for Molecular
Compounds
>
Naming Binary Molecular
Compounds
Naming Binary Molecular Compounds
What does a prefix in the name of a
binary molecular compound tell you
about the compound’s composition?
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Chapter 7
Section 1 Chemical Names and
Formulas
Naming Binary Molecular Compounds
• Unlike ionic compounds, molecular compounds are
composed of individual covalently bonded units, or
molecules.
• As with ionic compounds, there is also a Stock
system for naming molecular compounds.
• The old system of naming molecular compounds is
based on the use of prefixes.
• examples: CCl4 — carbon tetrachloride (tetra- = 4)
CO — carbon monoxide (mon- = 1)
CO2 — carbon dioxide (di- = 2)
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7.1
Naming and Writing
Formulas for Molecular
Compounds
>
Naming Binary Molecular
Compounds
A prefix in the name of a binary molecular
compound tells how many atoms of an
element are present in each molecule of
the compound.
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Chapter 7
Section 1 Chemical Names and
Formulas
Prefixes for Naming Covalent Compounds
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Chapter 7
Visual Concepts
Naming Covalently-Bonded Compounds
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Chapter 7
Visual Concepts
Naming Compounds Using Numerical Prefixes
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Chapter 7
Prefix Method for COVALENT
• Prefix method:
1)The element that has the smaller group number is usually
given first. If both are in same group, then the element
whose period number is greater goes first. The element is
given a prefix only if greater than one. Do not use monoon the first element.
2)The 2nd element is named by combining a prefix and the
root name of the element
ending in –ide.
3)The o or a at the end of a prefix is usually dropped when
the word following the prefix begins with another vowel.
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Chapter 7
Section 1 Chemical Names and
Formulas
Naming Binary Molecular Compounds,
continued
Sample Problem D
a. Give the name for As2O5.
b. Write the formula for oxygen difluoride.
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Chapter 7
Section 1 Chemical Names and
Formulas
Naming Binary Molecular Compounds,
continued
Sample Problem D Solution
a. A molecule of the compound contains two arsenic
atoms, so the first word in the name is diarsenic.
The five oxygen atoms are indicated by adding the
prefix pent- to the word oxide.
The complete name is diarsenic pentoxide.
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Chapter 7
Section 1 Chemical Names and
Formulas
Naming Binary Molecular Compounds,
continued
Sample Problem D Solution, continued
b. Oxygen is first in the name because it is less
electronegative than fluorine.
Because there is no prefix, there must be only one
oxygen atom.
The prefix di- in difluoride shows that there are two
fluorine atoms in the molecule.
The formula is OF2.
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Chapter 7
›
• DO NOT GO TO THE NEXT PAGE UNTIL YOU ARE
DONE WITH THE PROBLEMS. ASK FOR HELP IF
NEEDED.
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Chapter 7
ANSWERS pg. 229
ANSWERS pg. 229
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Chapter 7
Section 1 Chemical Names and
Formulas
Covalent-Network Compounds
• Some covalent compounds do not consist of
individual molecules.
• Instead, each atom is joined to all its neighbors in a
covalently bonded, three-dimensional network.
• Subscripts in a formula for covalent-network
compound indicate smallest whole-number ratios of
the atoms in the compound.
• examples: SiC, silicon carbide
SiO2, silicon dioxide
Si3N4, trisilicon tetranitride.
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Chapter 7
7.1 QUESTION - use points later as needed
to incorporate into other ppt
• not using the next slides right now - may incorporate
some of them at later date for 7.1
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7.1 Section Quiz.
Assess students’ understanding of the
concepts in Section 7.1.
Continue to:
-or-
Launch:
Section Quiz
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7.1 Section Quiz.
1. Which of the following compounds is named
INCORRECTLY?
a. CS2, carbon disulfide
b. BCl3, boron trichloride
c. IF7, iodine heptafluoride
d. PCl5, phosphorus hexachloride
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7.1 Section Quiz.
2. Which of the following molecular compounds
is named INCORRECTLY?
a. SbCl3, antimony trichloride
b. C2O5, dicarbon pentoxide
c. CF4, carbon tetrafluoride
d. H3As, hydrogen arsenide
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7.1 Section Quiz.
3. The correct formula for tetraphosphorus
trisulfide is
a. P3S4
b. S3P4
c. P4S3
d. S4P3
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7.1 Section Quiz
4. Which of the following are positively charged
polyatomic ions?
a. (I) ammonium ion
b. (II) perchlorate ion
c. (III) ferric ion
a. I only
b. II only
c. III only
d. I and III
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7.1 Section Quiz
5. If the name of an ion ends in -ite or -ate, the
ion is a
a. polyatomic cation.
b. polyatomic anion.
c. transition metal cation.
d. monatomic anion.
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7.1 Section Quiz
6. The correct name for CrCl3 is
a. chromium chlorine.
b. chromium(III) chloride.
c. monochromium trichloride.
d. chromium(III) trichloride.
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7.1 Section Quiz
7. What is the correct formula for strontium
nitride?
a. Sr3N2
b. SrN2
c. Sr2N3
d. Sr3N
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7.1 Section Quiz
8. Which one of the following compounds is
named correctly?
a. sodium chlorite, NaClO
b. potassium nitrate, KNO2
c. sodium acetate, NaC2H3O2
d. lithium sulfate, Li2SO3
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7.1
Naming and Writing
Formulas for Acids and
Bases
Some ants can give painful
stings when threatened or
disturbed. Certain ant species
called formicines have poison
glands that produce venom
containing formic acid. You
will learn the names and
formulas of some important
acids such as formic acid.
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7.1
Naming and Writing
Formulas for Acids
and Bases
>
Naming Acids
An acid is a compound that contains one or
more hydrogen atoms and produces hydrogen
ions (H+) when dissolved in water. Acids have
various uses.
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Chapter 7
Section 1 Chemical Names and
Formulas
Acids and Salts
• Most acids used in the laboratory are either binary
acids or oxyacids.
• Binary acids are acids that consist of two
elements, usually hydrogen and a halogen.
• Oxyacids are acids that contain hydrogen, oxygen,
and a third element (usually a nonmetal).
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7.1
Naming and Writing Formulas for
Acids and Bases
>
Naming Acids
Naming Acids
What are the three rules for naming
acids?
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7.1
Naming and Writing
Formulas for Acids
and Bases
>
Naming Acids
Three rules can help you name an acid with the
general formula HnX.
When the name of the anion (X) ends in
-ide, the acid name begins with the
prefix hydro-. The stem of the anion
has the suffix -ic and is followed by the
word acid.
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7.1
Naming and Writing
Formulas for Acids
and Bases
>
Naming Acids
When the anion name ends in -ite, the
acid name is the stem of the anion with
the suffix -ous, followed by the word
acid.
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7.1
Naming and Writing
Formulas for Acids
and Bases
>
Naming Acids
When the anion name ends in -ate, the
acid name is the stem of the anion with
the suffix -ic followed by the word acid.
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7.1
Naming and Writing
Formulas for Acids
and Bases
>
Naming Acids
A Summary of the Three Rules for Naming
Acids.
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Chapter 7
Visual Concepts
Prefixes and Suffixes for Oxyanions and
Related Acids
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Visual Concept
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9.3
Naming and Writing
Formulas for Molecular
Compounds
One milligram of gold is worth
only about one cent, but one
kilogram of gold is worth
approximately $12,500. The
correct prefix ( milli- or kilo-)
makes quite a difference!
Prefixes are important in
chemistry, too. The prefixes
in the name of a binary
molecular compound tell you
its composition.
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9.3
Naming and Writing
Formulas for Molecular
Compounds
>
Naming Binary Molecular
Compounds
Carbon and oxygen combine to form carbon
monoxide (CO) and carbon dioxide (CO2), but
these two invisible gases are very different.
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9.3
Naming and Writing
Formulas for Molecular
Compounds
>
Naming Binary Molecular
Compounds
Sitting in a room with small amounts of CO2 in
the air would not present any problems. If the
same amount of CO were in the room, you could
die of asphyxiation. A naming system that
distinguishes between these two compounds is
needed.
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of 15
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9.3
Naming and Writing
Formulas for Molecular
Compounds
>
Naming Binary Molecular
Compounds
A prefix in the name of a binary molecular
compound tells how many atoms of an
element are present in each molecule of
the compound.
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of 15
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9.3
Naming and Writing
Formulas for Molecular
Compounds
>
Naming Binary Molecular
Compounds
Some guidelines for naming binary
molecular compounds:
• Name the elements in the order listed
in the formula.
• Use prefixes to indicate the number of
each kind of atom.
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9.3
Naming and Writing
Formulas for Molecular
Compounds
>
Naming Binary Molecular
Compounds
• Omit the prefix mono- when the
formula contains only one atom of the
first element in the name.
• The suffix of the name of the second
element is -ide.
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9.3
Naming and Writing
Formulas for Molecular
Compounds
>
Writing Formulas for Binary
Molecular Compounds
Writing Formulas for Binary Molecular
Compounds
How do you write the formula for a
binary molecular compound?
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9.3
Naming and Writing
Formulas for Molecular
Compounds
>
Writing Formulas for Binary
Molecular Compounds
Use the prefixes in the name to tell you the
subscript of each element in the formula.
Then write the correct symbols for the two
elements with the appropriate subscripts.
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9.3
Naming and Writing
Formulas for Molecular
Compounds
>
Writing Formulas for Binary
Molecular Compounds
Silicon carbide is a hard material like diamond.
The name silicon carbide has no prefixes, so the
subscripts of silicon and carbon must be one.
Thus, the formula for silicon carbide is SiC.
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9.1 Section Quiz.
Assess students’ understanding of
the concepts in Section
9.1.
Continue to:
-or-
Launch:
Section Quiz
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9.1 Section Quiz.
1. When metals from groups 1A, 2A, and 3A
form cations, the charge on the ion is equal to
a. 8 minus the group number.
b. the group number minus 8.
c. the period number.
d. the group number.
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9.2 section Quiz.
Assess students’ understanding of the
concepts in Section 9.2.
Continue to:
-or-
Launch:
Section Quiz
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Chapter 7
Section 1 Chemical Names and
Formulas
Acids and Salts, continued
• In the laboratory, the term acid usually refers to a solution in
water of an acid compound rather than the acid itself.
• example: hydrochloric acid refers to a water solution of the
molecular compound hydrogen chloride, HCl
• Many polyatomic ions are produced by the loss of hydrogen ions
from oxyacids.
• examples:
sulfuric acid
H2SO4
sulfate
nitric acid
HNO3
nitrate
phosphoric acid H3PO4
phosphate
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Chapter 7
Visual Concepts
Naming Binary Acids
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Chapter 7
Visual Concepts
Naming Oxyacids
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Chapter 7
OTHER EXAMPLES - add roots
•
•
•
•
•
•
H2SO3 - sulfurous acid (coming from sulfite)
HClO3 - chloric acid
HClO2 - chlorous acid
HClO - hypochlorous acid
H2S - hydrosulfuric acid
HClO4 - perchloric acid
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7.1
Naming and Writing Formulas for
Acids and Bases
>
Writing Formulas for Acids
Writing Formulas for Acids
How are the formulas of acids
determined?
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7.1
Naming and Writing
Formulas for Acids
and Bases
>
Writing Formulas for Acids
Use the rules for writing the names of
acids in reverse to write the formulas for
acids.
What is the formula for hydrobromic acid?
Following Rule 1, hydrobromic acid (hydroprefix and -ic suffix) must be a combination
of hydrogen ion (H+) and bromide ion (Br–).
The formula of hydrobromic acid is HBr.
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7.1
Naming and Writing
Formulas for Acids
and Bases
>
Writing Formulas for Acids
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Chapter 7
Section 1 Chemical Names and
Formulas
Acids and Salts, continued
• An ionic compound composed of a cation and the
anion from an acid is often referred to as
a salt.
• examples:
• Table salt, NaCl, contains the anion from
hydrochloric acid, HCl.
• Calcium sulfate, CaSO4, is a salt containing
the anion from sulfuric acid, H2SO4.
• The bicarbonate ion,
carbonic acid, H2CO3.
, comes from
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Chapter 7
Visual Concepts
Salt
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Chapter 7
Section Review pg. 231
• Answer questions #2, 3, and 4 in your notes before going
to next page..
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Chapter 7
Answers pg. 231
• Be sure you answered these on
your own first.
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7.1
Naming and Writing Formulas for
Acids and Bases
>
Names and Formulas for
Bases
Names and Formulas for Bases
How are bases named?
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7.1
Naming and Writing
Formulas for Acids
and Bases
>
Names and Formulas for Bases
Bases are named in the same way as
other ionic compounds—the name of the
cation is followed by the name of the
anion.
For example, aluminum hydroxide consists
of the aluminum cation (Al3+) and the
hydroxide anion (OH–). The formula for
aluminum hydroxide is Al(OH)3.
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Section Assessment
Test yourself on the concepts in Section
7.1. Continue to:
Launch:
-or-
Section Quiz
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7.1 Section Quiz
1. The name for H2S(aq) is
a) sulfuric acid.
b) hydrosulfuric acid.
c) sulfurous acid.
d) hydrosulfurous acid.
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7.1 Section Quiz
2. The chemical formula for chlorous acid is
a) HClO2.
b) HClO3.
c) HClO4.
d) HCl.
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7.1 Section Quiz
3. The correct chemical name for NH4OH is
a) nitrogen tetrahydrogen hydroxide.
b) nitrogen pentahydrogen oxide.
c) ammonium oxyhydride.
d) ammonium hydroxide.
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Online Self-Check Quiz
Complete the online Quiz and record answers.
Ask if you have any questions about your
answers.
click here for online Quiz 7.1
(10 questions)
You must be in the “Play mode” for the
slideshow for hyperlink to work.
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VIDEOS FOR ADDITIONAL INSTRUCTION
Additional Videos for
Section 7.1: Chemical Names and
Formulas
Elements and Compounds
Acid and Base Properties
Salts
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7.1
End of 7.1 Notes and Practice Problems
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