Naming Ionic Compounds

Type I: Diatomic Writing Names from Formulas Identifying the cation as a Group I metal , Group II metal, Aluminum, Zinc, or Silver Identify the anion as a nonmetal Name the cation (the metal) with its full name Name the anion (the nonmetal) by changing the ending to -ide Example: NaCl cation: sodium anion: chlorine Name: sodium chloride

Sodium Chloride Potassium Bromide Magnesium Iodide Beryllium Oxide Calcium Fluoride Cesium Sulfide Aluminum Chloride Zinc Oxide Silver Phosphide

Writing Formulas from Names Identify charge of cation (1+, 2+, 3+) Identify charge of anion (1-, 2-, 3-) Balance the charges- criss cross! The charge of the cation becomes the subscript of the anion The charge of the anion becomes the subscript of the cation Reduce subscripts if necessary

Write the formula from the name: 𝑨𝒍 𝟐 𝑺 𝟑 𝑩𝒂 𝟐 𝑪 𝑳𝒊 𝟐 𝑺 𝑲 𝟐 𝑶 𝒁𝒏 𝑪𝒍 𝟐 𝑨𝒈𝑭 𝑵𝒂 𝟑 𝑵 𝑲𝑰 CaO

Type I: Polyatomic Writing Names from Formulas Identifying the cation as a Group I metal , Group II metal, Aluminum, Zinc, or Silver Identify the anion as a polyatomic ion Name the cation (the metal) with its full name Name the anion (the polyatomic) with its full name Example: KOH cation: potassium & anion: hydroxide Name: potassium hydroxide

Potassium Cyanide Sodium Hydroxide Calcium Carbonate Lithium Sulfite Cesium Phosphate Ammonium Chloride Francium Chlorite

Writing Formulas from Names (polyatomics) 1. Identify charge of cation (1+, 2+, 3+) --(write it over the element name) 2. Identify charge of polyatomic ion (1-, 2-, 3-) --(write it over the polyatomic) 3. Balance the charges- if equal then just one of each 4. The charge of the cation becomes the subscript of the polyatomic- use brackets around polyatomic if more than 1 5. The charge of the polyatomic becomes the subscript of the cation 6. Reduce subscripts if necessary

Writing Formulas from Names (polyatomics) 𝑨𝒖 𝑵𝑶 𝟑 𝑴𝒈 𝑺𝑶 𝟒 𝑪𝒂( 𝑶𝑯) 𝟐 𝑺𝒓 (𝑪𝒍𝑶 𝟑 ) 𝟐 𝑩𝒂 (𝑪𝑵) 𝟐 𝑨𝒍 𝟐 (𝑪𝒓 𝟐 𝑶 𝟕 ) 𝟑 (𝑵𝑯 𝟒 ) 𝟐 𝑺𝑶 𝟒 𝑲 𝑴𝒏𝑶 𝟒

Transition Metals For transition metals, there is no easy pattern for which cation they form If given a formula unit, we can figure out the charge of the cation using the anion If we are given the name, we will be given a roman numeral- the roman numeral is the charge of the cation!

Identify the cation as a transition metal Identify the anion Type II: Transition Metals Writing Names from Formulas Identify the cation as a transition metal Identify the anion Identify the charge of the cation Name the cation (the transition metal) with its full name and the charge of the ion in roman numerals 5a. Name the anion (the nonmetal) by changing the ending to –ide 5b. Name the anion (the polyatomic) with its full name Example: CoBr2 Cation: cobalt 2+ & anion: 2 bromine Name: cobalt (II) bromide

Cobalt (III) Carbonate 𝑪𝒖 +? 𝑰 −𝟏 Copper (I) Iodide 𝑪𝒖 +? 𝟐 𝒙 𝑰 −𝟏 Copper (II) Iodide 𝑪𝒖 +? 𝑪𝑶 𝟑 −𝟐 Cobalt (II) Carbonate 𝟐 𝒙 𝑪𝒖 +? 𝟑 𝒙 𝑪𝑶 𝟑 −𝟐 Cobalt (III) Carbonate 𝑺𝒏 +? 𝑶 −𝟐 Tin (II) Oxide 𝑺𝒏 +? 𝟐 𝒙 𝑶 −𝟐 Tin (IV) Oxide 𝑯𝒈 +? 𝟐 𝒙 𝑩𝒓 −𝟏 Mercury (II) Bromide 𝟐 𝒙 𝑯𝒈 +? 𝟐 𝒙 𝑩𝒓 −𝟏 Mercury (I) Bromide 𝑺𝒏 +? 𝑺 −𝟐 Tin (II) Sulfide

Writing Formulas from Names (transition metals) 1. Identify charge of cation transition metal (roman numeral) --(write it over the element name) 2. Identify charge of anion or polyatomic ion (1-, 2-, 3-) --(write it over the anion/polyatomic) 3. Balance the charges- if equal then just one of each 4. The charge of the cation becomes the subscript of the anion or (polyatomic- use brackets around polyatomic if more than 1 polyatiomic) 5. The charge of the anion/polyatomic becomes the subscript of the cation 6.Reduce subscripts if necessary

𝑭𝒆 +𝟐 𝑶 −𝟐 𝑭𝒆𝑶 𝑭𝒆 +𝟑 𝑶 −𝟐 𝑭𝒆 𝟐 𝑶 𝟑 𝑪𝒓 +𝟐 𝑷 𝑶 𝟒 −𝟑 𝑪𝒓 𝟑 (𝑷𝑶 𝟒 ) 𝟐 𝑭𝒆 +𝟐 𝑶 −𝟐 𝑭𝒆𝑶 𝑭𝒆 +𝟑 𝑶 −𝟐 𝑭𝒆 𝟐 𝑶 𝟑 𝑪𝒓 +𝟐 𝑷 𝑶 𝟒 −𝟑 𝑪𝒓 𝟑 (𝑷𝑶 𝟒 ) 𝟐 𝑪𝒓 +𝟑 𝑷 𝑶 𝟒 −𝟑 𝑪𝒓𝑷𝑶 𝟒 𝑴𝒏 +𝟐 𝑭 −𝟏 𝑴𝒏𝑭 𝟐 𝑴𝒏 +𝟑 𝑭 −𝟏 𝑴𝒏𝑭 𝟑 𝑭𝒆 +𝟑 𝑶𝑯 −𝟏 𝑭𝒆(𝑶𝑯 ) 𝟑 𝑷𝒃 +𝟒 𝑺 𝑶 𝟑 −𝟐 𝑷𝒃 (𝑺𝑶 𝟑) 𝟐 𝑯𝒈 +𝟏 𝑺 −𝟐 𝑯𝒈 𝟐 𝑺