Nomenclature
Chapter 4
Ionic Compounds
Ca2+ Cl ­
Metal Nonmetal
Calcium Chloride
CaCl2
Molecular Compounds
2 Non­metals
2 Carbon atoms 1 oxygen atom
CO2
PREFIXES
Transition Metals
Cu2+ Cl ­
Copper II Chloride
CuCl2
Title: Sep 24­3:59 PM (1 of 16)
Polyatomic Ions
Ca2+ NO 3­
Calcium Nitrate
CaNo3
1­Mono
7­Hepta
2­Di
8­Octa
3­Tri
9­Nona
4­Tetra 10­Deca
5­Penta
6­Hexa
Acids
H+
Cl ­
Hydrochloric Acid
HCl
4.1 Naming compounds that contain aMetal and a Nonmetal
*Ionic Compounds or Binary Type I Compounds
Naming Ions
Naming Cations (metals) : Simply use the name of the ________________
Example: Na+1 _______________________
Naming Anions: Drop the ending and add _________
Example: Cl ­1_________________________
Name the following ions
1. H1+_________________________
2. Li 1+________________________
3. Br 1­________________________
4. S 2­ ________________________
5. K 1+________________________
6. O 2­ ________________________
Title: Sep 24­4:23 PM (2 of 16)
Title: Sep 24­4:59 PM (3 of 16)
Naming Ionic Compounds
Naming ionic compounds is similar to naming ions. Just like when writing formulas, the
_________________ is written first, followed by the _______________. The cation is named the same
as the element, but the anion is named by dropping the end of the name and adding ­ide.
Example: NaCl __________________
Step #1 ­ Look at first element and name it. Result of this step = sodium.
Step #2 ­ Look at second element. Use root of its full name ( which is chlor­) plus the ending "­ide." Result of this step = chloride.
Name the following Compounds
1. CaCl2
5. BeO
2. CsF
6. Al2O3
3. AlCl3
7. K2S
4. MgI2
8. BaBr2
Naming Metallic (Transition Metals) Ions (Type II Binary Compounds)
So far all of the ions we have looked at have one specific charge. But some metals can have more than
one charge. Because these metals can have more than one charge, you must know what charge the particular
ion you are working with has.
When the names of these ions are written, a __________ ____________ is used to denote the charge that
the ion has. So, Iron II is an ion of iron with a charge of +2. All metallic ions are positive.
*The anions are still named by dropping the end of the atom name and adding ­ide.
Title: Sep 24­4:50 PM (4 of 16)
Title: Sep 24­5:31 PM (5 of 16)
Write the ion symbol and name for the common ions of these metals
For example
Iron
Fe 2+ Iron II
Fe 3+
Iron III
_________________________________________________________________
Lead
_________________________________________________________________
Tin
_________________________________________________________________
Mercury
Copper
__________________________________________________________________
Cobalt
_________________________________
Name the following compounds
1. CuCl
4. CoF2
2. CuCl2
5. PbCl4
3. Fe2O3
6. SnO
Title: Sep 24­5:24 PM (6 of 16)
Title: Sep 24­6:35 PM (7 of 16)
Quiz Time!!!
1. Take apart the following compounds and break them into ions!
CaCl2
NaO
FeO
2. Name the following Ionic Compounds
a. NaCl ___________________________
b. BaF2 ___________________________
d. PbO2 ___________________________
c. CuO ___________________________
3. Write the formula for the following Ionic Compounds (Be sure to show ions and the
criss­cross method)
a. Calcium fluoride
b. Aluminum oxide
c. Tin(IV) oxide
Title: Sep 25­7:52 PM (8 of 16)
Section 4.2 Naming Binary Compounds that Contain ONLY NONMETALS (Type III)
Type II binary compounds contain only ______________________ elements
Rules for Naming Type III Binary Compounds (p. 95)
1.
2.
3.
4.
The first element in the formula is named first, and the full element name is used.
The second element is named as though it were an anion.
Prefixes are used to denote the numbers of atoms present. These prefixes are given in Table 4.3
The prefix mono­ is never used for maning the first element.
Using the numerical prefixes, name these compounds:
PREFIXES
1. CO ____________________ 6. NO2_____________________
2. CO2____________________ 7. N2O_____________________
3. N2O4___________________ 8. CCl4_____________________
4. P2O5___________________ 9. As2O5____________________
5. SO2____________________ 10. N2O3_____________________
Title: Sep 25­7:19 PM (9 of 16)
1­Mono
7­Hepta
2­Di
8­Octa
3­Tri
9­Nona
4­Tetra 10­Deca
5­Penta
6­Hexa
*Tutorial
Section 4.4 Naming Compounds that Contain POLYATOMIC IONS
Polyatomic ions are groups of ___________________ bonded atoms that have a charge
These groups bond with other ions the same way that all ions bond, by giving up electrons.
Formulas are made using the criss­cross method, as with the other ions. The biggest difference
is in the way the formulas are written. When you add the subscript to a polyatomic ion, you need to
put parenthesies around the (Polyatomic Ion)
For example, if you combine the ions Al 3+and CO32­, you end up with a 2 subscript on
the aluminum, and a 3 subscript on the carbonate. Instead of writing Al
2CO33,you need to
write _______________
Naming ionic compounds that contain a polyatomic ion is very similar to naming binary
ionic compounds. For example, the compound NaOH is called ______________________
because it contains the ______ (sodium) cations and the ______ (hydroxide) anion. To name
these compounds, you must learn to recognize the common polyatomic ions.
Memorize Them !!!
Title: Sep 25­7:34 PM (10 of 16)
Name the following compounds that contain Polyatomic Ions
Ca(CN)2
Calcium Cyanide
(NH4)2O
Ammonium Oxide
ZnSO4
AgNO3
NH4ClO4
Ca(NO2)2
Sn(CrO4)2
Ba(OH)2
Cr(CN)3
CoC2O4
Title: Sep 25­7:44 PM (11 of 16)
Title: Sep 25­7:49 PM (12 of 16)
4.5 Naming Acids
When dissolved in water, certain molecules produce _____ ions. These substances are called
_________________.
*Rules for Naming Acids
Does it contain Oxygen or not?
1. If the anion does not contain oxygen...
Use prefix Hydro
Use suffix ­ic
Example:
HCl
H2S
2. If the anion contains oxygen...
No prefix
*Use the suffix ­ic (if the anion name ends in ­ate)
*Use the suffix ­ous (if the anion name ends in ­ite)
Example:
HsSO4
H2SO3
H3PO4
HNO2
Title: Sep 26­5:29 PM (13 of 16)
Name the following Acids
1. HBr
4. HNO2
2. H2S
5. H3PO4
3. HNO3
6. HC2H3O2
Title: Sep 26­6:18 PM (14 of 16)
4.6 Writing Formulas from Names
Write the formula for the following compounds
1. Cobalt II hydroxide
7. Sodium fluoride
2. Potassium chlorate
8. Lithium nitrite
3. Hydrochloric acid
9. Sulfuric acid
4. Ammonium sulfate
10. Sodium phosphate
5. Dinitrogen trioxide
11. Phosphoric acid
6. Sulfur hexafluoride
12. Zinc Nitrate
Title: Sep 26­6:21 PM (15 of 16)
H3PO4 FeO2
CO2
Magnesium Hydroxide
NH4NO3
Acid
Covalent
Ionic
NaCl
N2O3
Nitrogen Dioxide
Title: Sep 27­10:44 AM (16 of 16)
Tin IV Oxide
H2SO4
CCl4
Carbon Monoxide
Attachments
Nomenclature Tutorial