1. Naming Ionic Compounds

2. 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

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

4. 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

5. 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

6. 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

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

8. 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

9. 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

10. 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!

11. 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

12. 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

13. 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

14. 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