1. 9.1 Naming Ions, Naming & Writing Formulas for Ionic Copmounds
Chapter 9
Chemical Names and Formulas
9.1 Naming Ions, Naming
& Writing Formulas for
Ionic Copmounds
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2. Do you speak “Chemistry”?
CHEMISTRY & YOU
Do you speak “Chemistry”?
Try looking at the ingredient label on a household product, a bottle of shampoo- sodium laureth sulfate, cocamidoporpyl betaine, distearyl ether, sodium chloride, amodimethacone. Do the names of the ingredients make sense?
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3. Monatomic Ions How can we determine the charges of monatomic ions?
Ionic compounds are made of a + metal
ion and a - nonmetal ion combined in a
proportion so that their charges add up to
a net charge of zero.
The ionic compound NaCl consists of one
sodium ion (Na+) and one chloride ion
(Cl–).
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4. Remember that metals tend to lose valence electrons, and form cations.
Monatomic Ions
It is important to be able to name and write the chemical formulas for all ionic compounds.
Some ions, called monatomic ions, consist of a single atom with a positive or negative charge because of the loss or gain of one or more valence electrons.
Cations
Remember that metals tend to lose valence electrons, and form cations.
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5. All the Group 1A ions have a 1+ charge (Li+, Na+, K+, Rb+, and Cs+).
Monatomic Ions
Cations
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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6. Monatomic Ions
Cations
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.
Anions
Nonmetals tend to gain electrons to form anions, so the charge of a nonmetallic ion is negative.
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7. The elements in Group 7A form anions with a 1– charge (7 – 8 = –1).
Monatomic Ions
Anions
The charge of any ion of a Group A nonmetal is determined by subtracting 8 from the group number.
The elements in Group 7A form anions with a 1– charge (7 – 8 = –1).
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8. Anion names start with the stem of the element name and end in -ide.
Monatomic Ions
Anions
Anion names start with the stem of the element name and end in -ide.
The anions for these flourine and chlorine nonmetals are the fluoride ion (F–) and the chloride ion (Cl–).
Anions of nonmetals in Group 6A have a 2– charge (6 – 8 = –2).
Group 6A elements, oxygen and sulfur, form the oxide anion (O2–) and the sulfide anion (S2–), respectively.
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9. Monatomic Ions
Anions
The first three elements in Group 5A, nitrogen, phosphorus, and arsenic, can form anions with a 3– charge (5 – 8 = –3).
These anions have the symbols N3–, P3–, and As3– and are called, respectively, nitride ion, phosphide ion, and arsenide ion.
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10. 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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11. 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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12. 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.
For example, 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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13. Metals That Form More Than One Ion
Monatomic Ions
Metals That Form More Than One Ion
Two methods are used to name ions that can have more than one common ionic charge.
The preferred method is called the Stock system.
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.
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14. The Fe3+ ion is named iron(III) ion and is read “iron three ion.”
Monatomic Ions
Metals That Form More Than One Ion
For example, the cation Fe2+ is named iron(II) ion and is read “iron two ion.”
The Fe3+ ion is named iron(III) ion and is read “iron three ion.”
A few transition metals have only one ionic charge. Those cations do not have a Roman numeral.
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15. Monatomic Ions
Metals That Form More Than One Ion
These exceptions include silver, with cations that have a 1+ charge (Ag+), and cadmium and zinc, with cations that have a 2+ charge (Cd2+ and Zn2+).
Name the ion formed by each of the following elements:
potassium
lead, 4 electrons lost
sulfur
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16. a. K+ is named potassium ion. b. Pb4+ is named lead(IV).
Sample Problem 9.1
Apply the appropriate rules for naming the ion. Use a Roman numeral if necessary.
a. K+ is named potassium ion.
b. Pb4+ is named lead(IV).
c. S2– is named sulfide ion.
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17. 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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18. 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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19. Polyatomic Ions
Polyatomic Ions
How do polyatomic ions differ from monatomic ions? How are they similar?
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20. Polyatomic Ions
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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21. 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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22. Common Polyatomic Ions
Charge
Formula
Name 1–
HSO4–
NO2–
ClO–
Hydrogen sulfate
Nitrite
Hypochlorite 2–
SO32–
SO42–
CO32–
Sulfite
Sulfate
Carbonate 3–
PO43–
Phosphate 1+
NH4+
Ammonium
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23. 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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24. Ch 9.1 Questions (1) 1. When the metals in Groups 1A, 2A, and 3A lose electrons, they form cations with ________ charges equal to their ______________. 2. List the charge and the name for each of the following ions: a. Li e. N b. K f. O c. Al g. Br d. Ca h. I
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25. Binary Ionic Compounds
How do you determine the formula and name of a binary ionic compound?
Before the science of chemistry developed, compounds were often named to describe some property of the substance or its source.
For example, a common name for potassium carbonate (K2CO3) is potash because the compound was obtained by boiling wood ashes in iron pots.
NaHCO3 is called baking soda because it is used in baking to make baked goods rise.
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26. The French chemist Lavoisier (1743–1794) worked with other chemists to develop a systematic method for naming chemical compounds. Their work is the basis for the system we use today.
A binary compound is composed of two elements. They can be ionic or molecular compounds.
If you know the name of a binary ionic compound, you can write the formula.
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27. To write the formula of a binary ionic
To write the formula of a binary ionic compound, first write the symbol of the cation and then the anion. Then add subscripts as needed to balance the charges.
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28. For example, potassium chloride is composed of potassium cations (K+) and chloride anions (Cl–), so potassium chloride is a binary ionic compound.
The charge of each K+ cation is balanced by the charge of each Cl– anion.
The ions combine in a 1:1 ratio, so the formula for potassium chloride is KCl.
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29. Steel is made using iron ore.
Hematite, a common ore of iron, contains iron(III) oxide. So, what is the formula for this compound?
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30. The balanced formula is Fe2O3.
Iron(III) oxide contains Fe3+ cations combined with oxide anions (O2–).
To balance a 3+ charge and a 2– charge, you must find the least common multiple of the charges, which is 6.
Two Fe3+ cations (a 6+ charge) will balance three O2– anions (a 6– charge).
The balanced formula is Fe2O3.
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31. Another approach is to use the crisscross method.
In this method, the numerical value of the charge of each ion is crossed over and becomes the subscript for the other ion.
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32. Write the formulas for the following binary ionic compounds.
copper(II) sulfide
potassium nitride
Write the symbol and charge for each ion in the compound—the cation first, then the anion.
a. Cu2+ and S2–
b. K+ and N3–
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33. Balance the formula using appropriate subscripts
Balance the formula using appropriate subscripts. Make sure that the formula expresses the lowest whole-number ratio of ions.
a b.
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34. To name any binary ionic. compound, place the cation name
To name any binary ionic compound, place the cation name first, followed by the anion name.
The name of NaBr is: ______________
The name of SrF2 is: _______________
The name of Li2O is: _______________
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35. Naming Compounds With Polyatomic Ions
If the metallic element in a binary ionic compound has more than one common ionic charge, a Roman numeral must be included in the cation name.
Naming Compounds With Polyatomic Ions
The compound NaClO is used as a disinfectant for swimming pools.
The cation in this compound is sodium ion (Na+).
The other ion, ClO–, is a polyatomic ion called hypochlorite ion.
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36. Naming and Writing Formulas-Questions
A binary compound is composed of _____________.
Write the formula for copper oxide.
The name of BaO is: ________________
Write the formula for iron(II) sulfide.
What is the name of the compound Al oxide.
What is the formula for hydrogen sulfide?
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