1. We will begin Chapter 9 today after a review of shapes and polarity.
Happy Thursday! Ch. 8 Test will be tomorrow! Please study the clicker review on my website.
We will begin Chapter 9 today after a review of shapes and polarity.
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2. Exam Review PowerPoints are on my website – Unit 1 and 2 reviews and Ch. 7,8 and 9 clicker reviews.
Also, highlight and study what we have covered so far on the “Key Chemistry SOL Definitions, Rules and Formulas” packet.
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3. Chapter 9 Chemical Names and Formulas 9.1 Naming Ions
9.2 Naming and Writing Formulas for
Ionic Compounds
9.3 Naming and Writing Formulas for
Molecular Compounds
9.4 Naming and Writing Formulas for
Acids and Bases
9.5 The Laws Governing How
Compounds Form
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4. Monatomic Ions
Ionic compounds consist of a positive metal ion and a negative nonmetal ion combined in a proportion such that their charges add up to a net charge of zero.
For example, the ionic compound sodium chloride (NaCl) consists of one sodium ion (Na+) and one chloride ion (Cl–).
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5. Monatomic Ions
Some ions, called 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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6. Recall that metallic elements tend to lose valence electrons.
Monatomic Ions
Recall that metallic elements tend to lose valence electrons.
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7. Recall that metallic elements tend to lose valence electrons.
Monatomic Ions
Recall that metallic elements tend to lose valence electrons.
All the Group 1A ions have a 1+ charge (Li+, Na+, K+, Rb+, and Cs+).
Group 2A metals, including magnesium and calcium, tend to lose two electrons to form cations with a 2+ charge (Mg2+ and Ca2+).
Aluminum is the only common Group 3A metal, and tends to lose three electrons to form a 3+ cation (Al3+).
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8. Monatomic Ions
Cations
When the metals in Groups 1A, 2A, and 3A lose electrons, they form cations with positive charges equal to their group number.

9. Monatomic Ions
The names of the cations of Group 1A, Group 2A, and Group 3A metals are the same as the name of the metal, followed by the word ion or cation.
Thus, Na+ is the sodium ion (or cation), Ca2+ is the calcium ion (or cation), and Al3+ is the aluminum ion (or cation).
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10. Monatomic Ions
Anions
Nonmetals tend to gain electrons to form anions, so the charge of a nonmetallic ion is negative.
The charge of any ion of a Group A nonmetal is determined by subtracting 8 from the group number.
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11. The elements in Group 7A form anions with a 1– charge (7 – 8 = –1).
Monatomic Ions
The elements in Group 7A form anions with a 1– charge (7 – 8 = –1).
The elements in Group 6A form anions with a 2– charge (6 – 8 = –2).
The elements in Group 5A form anions with a 3– charge (5 – 8 = –3).
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12. Anion names start with the stem of the element name and end in -ide.
Monatomic Ions
Anion names start with the stem of the element name and end in -ide.
For example, two elements in Group 7A are fluorine and chlorine. The anions for these nonmetals are the fluoride ion (F–) and the chloride ion (Cl–).
Group 5A elements for anions that have the symbols N3–, P3–, and As3– and are called, respectively, nitride ion, phosphide ion, and arsenide ion.
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13. Metals That Form More Than One Ion
Monatomic Ions
Metals That Form More Than One Ion
Many of the transition metals (Groups 1B–8B) form more than one cation with different ionic charges. Some are shown at right.
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14. Metals That Form More Than One Ion
Monatomic Ions
Metals That Form More Than One Ion
The charges of the cations of many transition metal ions must be determined from the number of electrons lost.
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15. Monatomic Ions
The charges of the cations of many transition metal ions must be determined from the number of electrons lost.
For example, the transition metal iron forms two common cations, Fe2+ (two electrons lost) and Fe3+ (three electrons lost).
Cations of tin and lead, the two metals in Group 4A, can also have more than one common ionic charge.
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16. Monatomic Ions
In the Stock system, you place a Roman numeral in parentheses after the name of the element to indicate the numerical value of the charge.
For example, the cation Fe2+ is named iron(II) ion and is read “iron two ion.”
No space is left between the element name and the Roman numeral in parentheses.
The Fe3+ ion is named iron(III) ion and is read “iron three ion.”
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17. Symbols and Names of Common Metal Ions With More Than One Ionic Charge
Monatomic Ions
A major disadvantage of using classical names for ions is that they do not tell you the actual charge of the ion.
Symbols and Names of Common Metal Ions With More Than One Ionic Charge
Symbol
Stock Name
Classical Name
Cu1+
Copper(I) ion
Cuprous ion
Cu2+
Copper(II) ion
Cupric ion
Pb2+
Lead(II) ion
Plumbous ion
Pb4+
Lead(IV) ion
Plumbic ion
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18. Metals That Form More Than One Ion
Monatomic Ions
Metals That Form More Than One Ion
A few transition metals have only one ionic charge.
The names of these cations do not have a Roman numeral.
These exceptions include silver, with cations that have a 1+ charge (Ag+), as well as cadmium and zinc, with cations that have a 2+ charge (Cd2+ and Zn2+).
MEMORIZE THESE!!!!!
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19. Naming Cations and Anions
Sample Problem 9.1
Naming Cations and Anions
Name the ion formed by each of the following elements:
potassium
lead, 4 electrons lost
sulfur
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20. Solve Apply concepts to the situation.
Sample Problem 9.1
Solve Apply concepts to the situation.
Write the symbol for the element.
a. K
b. Pb
c. S 2
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21. Solve Apply concepts to the situation.
Sample Problem 9.1
Solve Apply concepts to the situation.
Determine the charge of the ion formed by the element.
a. K 1+
b. Pb 4+
c. S 2– 2
A negative charge means electrons gained; a positive charge means electrons lost.
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22. Solve Apply concepts to the situation.
Sample Problem 9.1
Solve Apply concepts to the situation.
Determine whether the ion is a cation or an anion.
a. K 1+ K+ is a cation.
b. Pb 4+ Pb4+ is a cation.
c. S 2– S2– is an anion. 2
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23. Solve Apply concepts to the situation.
Sample Problem 9.1
Solve Apply concepts to the situation.
Apply the appropriate rules for naming the ion. Use a Roman numeral if necessary.
a. Following the rules for naming metallic cations, K+ is named potassium ion.
b. Following the rules for naming metals that can form more than one cation, Pb4+ is named lead(IV) ion.
c. Following the rules for naming nonmetallic anions, S2– is named sulfide ion. 2
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24. Happy???
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25. What type of elements (metals or nonmetals) tends to form cations
What type of elements (metals or nonmetals) tends to form cations? What type of elements tends to form anions?
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26. Metals tend to form cations. Nonmetals tend to form anions.
What type of elements (metals or nonmetals) tends to form cations? What type of elements tends to form anions?
Metals tend to form cations. Nonmetals tend to form anions.
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27. Polyatomic Ions
How do polyatomic ions differ from monatomic ions? How are they similar?
Unlike a monatomic ion, a polyatomic ion is composed of more than one atom. But like a monatomic ion, a polyatomic ion behaves as a unit and carries a charge.
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28. The sulfate anion consists of one sulfur atom and four oxygen atoms.
Polyatomic Ions
The sulfate anion consists of one sulfur atom and four oxygen atoms.
These five atoms together comprise a single anion with an overall 2– charge.
The formula is written SO42–.
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29. Polyatomic Ions
You can see the structure of the sulfate ion along with three other common polyatomic ions below.
Ammonium ion
(NH4+)
Nitrate ion
(NO3–)
Sulfate ion
(SO42–)
Phosphate ion
(PO43–)
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30. Common Polyatomic Ions
Charge
Formula
Name 1–
HSO4–
NO2–
NO3–
ClO–
Hydrogen sulfate
Nitrite
Nitrate
Hypochlorite 2–
SO32–
SO42–
CO32–
Sulfite
Sulfate
Carbonate 3–
PO43–
Phosphate 1+
NH4+
Ammonium
The names and formulas of some common polyatomic ions are shown here.
Note that the names of most polyatomic ions end in -ite or -ate.
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31. SO32−, sulfite SO42–, sulfate NO2–, nitrite NO3–, nitrate
Polyatomic Ions
Note the number of oxygen atoms and the endings on each name. You should be able to discern a pattern in the naming convention.
-ite -ate
SO32−, sulfite SO42–, sulfate
NO2–, nitrite NO3–, nitrate
ClO2–, chlorite ClO3–, chlorate
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32. The -ite ending indicates one less oxygen atom than the -ate ending.
Polyatomic Ions
The charge is the same on each polyatomic ion in a pair for which there is both an -ite and an -ate ion.
The -ite ending indicates one less oxygen atom than the -ate ending.
However, the ending does not tell you the actual number of oxygen atoms in the ion.
For example, the nitrite ion has two oxygen atoms, and the sulfite ion has three oxygen atoms.
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33. For example, HCO3– is a combination of H+ and CO32–.
Polyatomic Ions
When the formula for a polyatomic ion begins with H (hydrogen), you can think of the H as representing a hydrogen ion (H+) combined with another polyatomic ion.
For example, HCO3– is a combination of H+ and CO32–.
Note that the charge on the new ion is the algebraic sum of the ionic charges of the two component ions.
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34. BIG IDEA
An element’s position in the periodic table supplies information on ion formation and bonding tendencies, which is used to write the names and formulas of ions and compounds.
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35. Common Polyatomic Ions
Polyatomic Ions to memorize:
carbonate, sulfate, sulfite, nitrate, nitrite, hydroxide, phosphate, and ammonium
Common Polyatomic Ions
Charge
Formula
Name 1–
NO3–
NO2–
OH–
Nitrate
Nitrite
Hydroxide 2–
SO42–
SO32-
CO32–
Sulfate
Sulfite
Carbonate 3–
PO43–
Phosphate 1+
NH4+
Ammonium
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36. Homework: Due Monday 1-9 pg. 267 and 269 Ch. 8 test tomorrow!
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37. Clicker Review for Ch. 8
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38. Key Concepts
When the metals in Groups 1A, 2A, and 3A lose electrons, they form cations with positive charges equal to their group number.
The charge of any ion of a Group A nonmetal is determined by subtracting 8 from the group number.
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39. Key Concepts
The charges of the cations of many transition metal ions must be determined from the number of electrons lost.
Unlike a monatomic ion, a polyatomic ion is composed of more than one atom. But like a monatomic ion, a polyatomic ion behaves as a unit and carries a charge.
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40. Glossary Terms
monatomic ion: a single atom with a positive or negative charge resulting from the loss or gain of one or more valence electrons
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