1. 4.1 Naming Compounds that contain a Metal and a Nonmetal
Chapter 4 Nomenclature
4.1 Naming Compounds that contain a Metal and a Nonmetal
Binary Ionic Compound
Type I Compounds
Cation is always named 1st, and the anion second
A simple cation takes its name from the element.
A simple anion is named with the root of the element name and adding the suffix –ide.
Examples:
CsF AlCl3 MgI2
Rb2O SrI2 K2S
Chapter 4 Nomenclature
4.1 Naming Compounds that contain a Metal and a Nonmetal
Binary Ionic Compound
Type I Compounds
Cation is always named 1st, and the anion second
A simple cation takes its name from the element.
A simple anion is named with the root of the element name and adding the suffix –ide.
Examples:

2. Table 4.1

3. Older nomenclature: the cation with the higher charge ends in –ic
Type II Compounds
Older nomenclature: the cation with the higher charge ends in –ic
the cation with the lower charge ends in –ous.
Examples:
CuCl CuCl2
Stock system- naming system using Roman numerals in parentheses for the charges; no other suffixes are needed (This is the most commonly used system)
CuCl HgO Fe2O3
MnO2 PbCl4
Type II Compounds
Older nomenclature: the cation with the higher charge ends in –ic
the cation with the lower charge ends in –ous.
Examples:
Stock system- naming system using Roman numerals in parentheses for the charges; no other suffixes are needed (This is the most commonly used system)
Examples

4. Table 4.2

5. 4.2 Naming Binary Compounds that contain only Nonmetals (Type III)
Prefixes:
Mono- hexa-
Di- hepta-
Tri- octa-
Tetra- nona-
Penta- deca-
(Sometimes it is appropriate to eliminate an extra vowel sound: decaoxide to decoxide)
Do not use prefix for mono- on 1st element if it is only one.
Continue to use suffix –ide on second element name
4.2 Naming Binary Compounds that contain only Nonmetals (Type III)
Prefixes:
Mono- hexa-
Di- hepta-
Tri- octa-
Tetra- nona-
Penta- deca-
(Sometimes it is appropriate to eliminate an extra vowel sound: decaoxide to decoxide)
Do not use prefix for mono- on 1st element if it is only one.
Continue to use suffix –ide on second element name
Examples:

6. Examples:
CCl4 NO2 IF5
BF3 NO N2O5
Examples

7. Figure 4.1: A flow chart for naming binary compounds.

8. 4.4 Naming Compounds that contain Polyatomic Ions
YOU MUST MEMORIZE THESE!!
Oxyanions: hypochlorite
chlorite
chlorate
perchlorate
Examples:
Na2SO4 KH2PO4 Fe(NO3)3
Mn(OH)2 Na2SO3 Ca(OH)2
Na3PO4 KMnO4 (NH4)2Cr2O7
Co(ClO4)2 KClO3 Ca(NO2)2
4.4 Naming Compounds that contain Polyatomic Ions
YOU MUST MEMORIZE THESE!!
Oxyanions
hypochlorite
chlorite
chlorate
perchlorate

9. Table 4.4

10. Figure 4.2: Overall strategy for naming chemical compounds.

11. Binary Acid (no oxygen). Use prefix hydro-, and suffix –ic Examples:
4.5 Naming Acids
Binary Acid (no oxygen). Use prefix hydro-, and suffix –ic
Examples:
HCl HBr HI
H2S H2Se HF
Tertiary acids (oxygen present)
If anion ends in –ite, acid ends in –ous.
If anion ends in –ate, acid ends in –ic.
Examples:HNO3 HNO2
HC2H3O2 H2SO4 H2SO3
H3PO4 H3PO3 HClO
HClO2 HClO3 HClO4
4.5 Naming Acids
Binary Acid (no oxygen)
Use prefix hydro-, and suffix –ic
Examples:
Tertiary acids (oxygen present)
If anion ends in –ite, acid ends in –ous.
If anion ends in –ate, acid ends in –ic.
Examples

12. 4.6 Writing Formulas from Names
Criss-cross method (always check that a neutral compound is made)
(You cannot reduce subscripts that would change a polyatomic ion)
(BUT you should reduce subscripts in other cases)
Magnesium oxide tin(II)oxide tin(IV)oxide
Examples: potassium hydroxide sodium carbonate
Cobalt (III) nitrate calcium chloride lead (IV) oxide
Dinitrogen pentoxide ammonium perchlorate
Ammonium sulfate vanadium (V) fluoride
Disulfur dichloride rubidium peroxide
Aluminum oxide
4.6 Writing Formulas from Names
Criss-cross method (always check that a neutral compound is made)
(You cannot reduce subscripts that would change a polyatomic ion)
(BUT you should reduce subscripts in other cases)