Binary Ionic Compounds (Type I)

•Contain a cation and anion

•The cation is always named first and the anion second

Binary Ionic Compounds (Type I)

•A monatomic cation takes its name from the name of the element

•A monatomic anion is named by taking the first part of the element name and adding -ide

Binary Ionic Compounds (Type I) Practice

• LiI• Lithium Iodide• AgBr• Silver Bromide• KF• Potassium

Fluoride

• Li3N

• Lithium Nitride

• MgO• Magnesium

Oxide

Binary Ionic Compounds (Type II)

•Involves metals that can form more than one cation

•In this case, the charge on the metal ion must be specified with Roman numerals

Binary Ionic Compounds (Type II)

•An older system uses the ending -ic on the cation with the higher charge and -ous on the cation with lower charge

Binary Ionic Compounds (Type II) Practice

•CuCl

•CuCl2

•Fe2O3

•Copper(I) Chloride

•Copper(II) Chloride

•Iron(III) Oxide

Binary Ionic Compounds (Type II) Practice

•HgO

•CoCl2

•MnO2

•Mercury(II)Oxide

•Cobalt(II) Chloride

•Manganese (IV) Oxide

Ionic Compound with Polyatomic Ions

•You must MEMORIZE your polyatomic ions!!!!

•There are a few hints…

•Night-rate NO3-

•Night-right NO2-

Ionic Compound with Polyatomic Ions

•the polyatomic in a series with less oxygen atoms ends in -ite, the other -ate (The ate ate the ite)

Ionic Compounds with Polyatomic Ions

Continued•In summary…•per _ ate 1 more Oxygen• _ate• _ite 1 less Oxygen•hypo_ite 2 less Oxygen

Practice with Polyatomics

• NaOH

• NH4Cl

• NaC2H3O2

• CaCO3

• Sodium Hydroxide

• Ammonium Chloride

• Sodium Acetate• Calcium

Carbonate

Practice with Polyatomics

• KBrO3

• FeSO4

• Mn(OH)2

• Potassium Bromate

• Iron (II) Sulfate

• Manganese (II) Hydroxide

Binary Covalent Compounds

•Formed between two nonmetals

•The first element is the full element name

•The second element is as if it were an anion

Binary Covalent Compounds

•Prefixes are used to denote number of atoms present

•“mono” is never used on cation!

Prefixes Used In Binary Covalent Compounds

• Mono- 1• Di- 2• Tri- 3• Tetra- 4• Penta- 5• Hexa- 6• Hepta- 7• Octa- 8

Practice with Binary Covalent Compounds

• PCl3

• NO2

• CO

• N2O5

• phosphorus trichoride

• nitrogen dioxide• carbon

monoxide• dinitrogen

pentoxide

Naming Acids

•Acid can be viewed as a molecule with one or more H+ ions attached

•Rules depend on whether or not oxygen is present

Naming Acids

•If the anion DOES NOT contain oxygen the acid is named with the prefix hydro- and the suffix -ic

Naming Acids Continued

•If the anion DOES contain oxygen, the acid name is formed from the root name of the anion with a suffix added

Naming Acids Continued

•If the anion ends in -ate, the -ate turns to -ic

•If the anion ends in -ite, the -ite turns to -ous

Practice Naming Acids

• HF

• HCl

• HNO3

• H2SO4

•hydrofluoric acid

•hydrochloric acid

•nitric acid•sulfuric acid

Practice Naming Acids

• HC2H3O2

• HCN

• H2S

• HNO2

•acetic acid•hydrocyanic

acid•hydrosulfuri

c acid•nitrous acid

The Secret To Nomenclature Is…

•Practice!•Practice!!•Practice!!!