1. 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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2. Monatomic Ions
Do Now:
1. Determine the charge of the cations in the following ionic compounds.
a) FeO
b) Fe2O3
c) Cu2O
d) CuO
2. Give a name to each compound above.
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3. Do Now: a) FeO Fe2+ b) Fe2O3 Fe3+ c) Cu2O Cu+ d) CuO Cu2+
Monatomic Ions
Do Now:
a) FeO Fe2+
b) Fe2O3 Fe3+
c) Cu2O Cu+
d) CuO Cu2+
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4. Do Now: a) FeO Fe2+ Iron (II) Oxide b) Fe2O3 Fe3+ Iron (III) Oxide
Monatomic Ions
Do Now:
a) FeO Fe2+ Iron (II) Oxide
b) Fe2O3 Fe3+ Iron (III) Oxide
c) Cu2O Cu Copper (I) Oxide
d) CuO Cu Copper (II) Oxide
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5. Do Now: a) FeO Fe2+ Iron (II) Oxide Ferrous Oxide
Monatomic Ions
Do Now:
a) FeO Fe2+ Iron (II) Oxide Ferrous Oxide
b) Fe2O3 Fe3+ Iron (III) Oxide Ferric Oxide
c) Cu2O Cu Copper (I) Oxide Cuprous Oxide
d) CuO Cu Copper (II) Oxide Cupric Oxide
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6. Naming Metals That Form More Than One Ion
Monatomic Ions
Naming Metals That Form More Than One Ion
Many transition metals and Group 4A metals can form more than one type of cation
Roman numeral in parentheses indicates charge.
Examples:
Copper (I) is Cu+
Copper (II) is Cu+2
Iron (II) is Fe+2
Iron(III) is Fe+3
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7. Cadmium – only forms Cd2+ Zinc – only forms Zn2+
Monatomic Ions
Exceptions
Transition metals that only form one ion do not have a Roman numeral in their name.
Silver – only forms Ag+
Gold – only forms Au+
Cadmium – only forms Cd2+
Zinc – only forms Zn2+
Group 4A elements that form multiple ions
Tin – forms Sn2+ and Sn4+
Lead – forms Pb2+ and Pb4+
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8. Binary Ionic Compounds
Write names for the following
a) Co3N2
b) Co2O3
c) Ti2S
d) CrF2
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9. Binary Ionic Compounds
Write names for the following
a) Co3N2 Cobalt (II) Nitride
b) Co2O3 Cobalt (III) Oxide
c) Ti2S Titanium (I) Sulfide
d) CrF2 Chromium(II) Fluoride
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10. Monatomic Ions
With your groups, formulate the steps involved in naming binary ionic compounds on your white boards.
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11. Binary Ionic Compounds
Write formulas for the following
a) Lead (II) Sulfide
b) Manganese (II) Fluoride
c) Cobalt (III) Chloride
d) Tin (IV) Bromide
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12. Binary Ionic Compounds
Writing Formulas for Binary Ionic Compounds
a) Lead (II) Sulfide PbS
b) Manganese (II) Fluoride MnF2
c) Cobalt (III) Chloride CoCl3
d) Tin (IV) Bromide SnBr4
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13. Binary Ionic Compounds
Writing Formulas for Binary Ionic Compounds
Write symbols of elements.
Determine ionic charge for each symbol.
If the sum of the charges is zero, you are done.
If the sum of the charges does not equal zero, use the criss-cross method to add subscripts to balance the charges.
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14. Monatomic Ions
Monatomic ions: single atom with a positive or negative charge resulting from the loss or gain of one or more valence electrons.
Ca F N3-
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15. Polyatomic Ions
Polyatomic Ions - Composed of more than one atom, behaves as a unit, and carries a charge
Ammonium ion
(NH4+)
Nitrate ion
(NO3–)
Sulfate ion
(SO42–)
Phosphate ion
(PO43–)
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16. Common Polyatomic Ions
Charge
Formula
Name 1–
HSO4–
NO2–
ClO–
OH-
Hydrogen sulfate
Nitrite
Hypochlorite
Hydroxide 2–
SO32–
SO42–
CO32–
Sulfite
Sulfate
Carbonate 3–
PO43–
Phosphate 1+
NH4+
Ammonium
Note that the names of most polyatomic ions end in -ite or -ate.
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17. SO32−, sulfite SO42–, sulfate NO2–, nitrite NO3–, nitrate
Polyatomic Ions
Note the number of oxygen atoms and the endings on each name. There is a pattern in the naming convention.
-ite -ate
SO32−, sulfite SO42–, sulfate
NO2–, nitrite NO3–, nitrate
ClO2–, chlorite ClO3–, chlorate
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18. -ite indicates one less oxygen atom than –ate
Polyatomic Ions
-ite indicates one less oxygen atom than –ate
SO32−, sulfite NO2–, nitrite ClO2–, chlorite
SO42–, sulfate NO3–, nitrate ClO3–, chlorate
The charge on both ions in each pair are the same.
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19. Polyatomic Ions
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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20. Compounds With Polyatomic Ions
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21. Compounds With Polyatomic Ions
Write the formula for Calcium nitrate.
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22. Compounds With Polyatomic Ions
Writing Formulas for Compounds With Polyatomic Ions
Example - Calcium nitrate
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23. Writing Formulas for Compounds With Polyatomic Ions
Sample Problem 9.4
Writing Formulas for Compounds With Polyatomic Ions
What are the formulas for these ionic compounds?
Lithium nitrate
Copper(I) Sulfate
Aluminum Hydroxide
Ammonium Phosphate
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24. Writing Formulas for Compounds With Polyatomic Ions
Sample Problem 9.4
Writing Formulas for Compounds With Polyatomic Ions
What are the formulas for these ionic compounds?
Lithium Nitrate – LiNO3
Copper(I) Sulfate - Cu2SO4
Aluminum Hydroxide – Al(OH)3
Ammonium Phosphate – (NH4)3PO4
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25. Compounds With Polyatomic Ions
Writing Formulas for Compounds With Polyatomic Ions
Write the symbol (or formula) for the cation followed by the symbol (or formula) for the anion.
If the charges cancel, you are done.
If the charges do not cancel, add subscripts as needed to balance the charges.
NOTE – Put the polyatomic ion in parentheses and place the subscript outside. Ex – Ca(OH)2
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26. Compounds With Polyatomic Ions
Naming Compounds With Polyatomic Ions
Identify and name the cation and polyatomic ion
If the cation only has one possible charge, write the formula.
If the cation has more than one possible charge, identify the charge of the cation.
If subscripts present, reverse criss-cross
If no subscripts, determine the charge of the polyatomic ion and the cation is the opposite
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27. Compounds With Polyatomic Ions
Naming Compounds With Polyatomic Ions
NaClO is used as a disinfectant for swimming pools and as a bleach.
Na ClO–
Sodium ion Hypochlorite ion
The name for NaClO is sodium hypochlorite.
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28. Naming Compounds With Polyatomic Ions
Sample Problem 9.5
Naming Compounds With Polyatomic Ions
Name the following ionic compounds.
BaSO4
Al(NO2)3
(NH4)2S
CaSO3
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29. Naming Compounds With Polyatomic Ions
Sample Problem 9.5
Naming Compounds With Polyatomic Ions
Name the following ionic compounds.
BaSO4 – Barium Sulfate
Al(NO2)3 – Aluminum Nitrite
(NH4)2S – Ammonium Sulfide
CaSO3 – Calcium Sulfite
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