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Chapter 4 Nomenclature 4.1 Naming Compounds that contain a Metal and a Nonmetal Binary Ionic Compound Type I Compounds Cation is always named 1 st , and the anion second A simple cation takes its name from the element. - PowerPoint PPT Presentation
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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
Table 4.1
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)
Examples:
CuCl HgO Fe2O3
MnO2 PbCl4
Table 4.2
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:CCl4 NO2 IF5
BF3 NO N2O5
Figure 4.1: A flow chart for naming binary compounds.
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
Table 4.4
Figure 4.2: Overall strategy for naming chemical compounds.
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
4.6 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