NamingIonic Compounds

Type I: DiatomicWriting Names from Formulas1. Identifying the cation as a Group I metal , Group

II metal, Aluminum, Zinc, or Silver

2. Identify the anion as a nonmetal

3. Name the cation (the metal) with its full name

4. Name the anion (the nonmetal) by changing the ending to -ide

Example: NaClcation: sodium anion: chlorineName: sodium chloride

Sodium Chloride

Potassium Bromide

Magnesium Iodide

Beryllium Oxide

Calcium Fluoride

Cesium Sulfide

Aluminum Chloride

Zinc Oxide

Silver Phosphide

Writing Formulas from Names

1. Identify charge of cation (1+, 2+, 3+)

2. Identify charge of anion (1-, 2-, 3-)

3. Balance the charges- criss cross!

4. The charge of the cation becomes the subscript of the anion

5. The charge of the anion becomes the subscript of the cation

6. Reduce subscripts if necessary

Write the formula from the name:

𝑨𝒍𝟐𝑺𝟑

𝑩𝒂𝟐𝑪

𝑳𝒊𝟐𝑺

𝑲 𝟐𝑶𝒁𝒏𝑪𝒍𝟐

𝑨𝒈𝑭

𝑵𝒂𝟑𝑵

𝑲𝑰

CaO

Type I: Polyatomic

Writing Names from Formulas

1. Identifying the cation as a Group I metal , Group II metal, Aluminum, Zinc, or Silver

2. Identify the anion as a polyatomic ion

3. Name the cation (the metal) with its full name

4. Name the anion (the polyatomic) with its full name

Example: KOH

cation: potassium & anion: hydroxide

Name: potassium hydroxide

Potassium Cyanide

Calcium Carbonate

Sodium Hydroxide

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)

𝑨𝒖𝑵𝑶𝟑

𝑴𝒈𝑺𝑶𝟒

𝑪𝒂¿

𝑺𝒓 ¿¿

𝑩𝒂(𝑪𝑵 )𝟐

𝑨𝒍𝟐 ¿¿

¿¿𝑲 𝑴𝒏𝑶𝟒

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!

Type II: Transition MetalsWriting Names from Formulas

1. Identify the cation as a transition metal2. Identify the anion3. Identify the charge of the cation4. 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 nameExample: CoBr2

Cation: cobalt 2+ & anion: 2 bromineName: cobalt (II) bromide

𝑪𝒖+? 𝑰−𝟏 Copper (I) Iodide

𝑪𝒖+?𝟐 𝒙 𝑰−𝟏 Copper (II) Iodide

Cobalt (II) Carbonate𝑪𝒖+?𝑪𝑶𝟑−𝟐

𝟐 𝒙 𝑪𝒖+?𝟑 𝒙 𝑪𝑶𝟑−𝟐 Cobalt (III) Carbonate

𝑺𝒏+?𝑶−𝟐 Tin (II) Oxide

𝑺𝒏+?𝟐 𝒙𝑶−𝟐Tin (IV) Oxide

𝑯𝒈+?𝟐 𝒙 𝑩𝒓 −𝟏 Mercury (II) Bromide

𝟐 𝒙𝑯𝒈+?𝟐 𝒙 𝑩𝒓 −𝟏 Mercury (I) Bromide

𝑺𝒏+?𝑺−𝟐Tin (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+𝟐𝑶−𝟐 𝑭𝒆𝑶

𝑭𝒆+𝟑𝑶−𝟐 𝑭𝒆𝟐𝑶𝟑

𝑪𝒓 +𝟐𝑷𝑶𝟒−𝟑 𝑪𝒓𝟑¿¿

𝑪𝒓 +𝟑𝑷𝑶𝟒−𝟑 𝑪𝒓𝑷𝑶𝟒

𝑴𝒏+𝟐𝑭 −𝟏 𝑴𝒏𝑭 𝟐

𝑴𝒏+𝟑𝑭 −𝟏 𝑴𝒏𝑭 𝟑

𝑭𝒆+𝟑𝑶𝑯 −𝟏 𝑭𝒆 ¿

𝑷𝒃+𝟒𝑺𝑶𝟑−𝟐 𝑷𝒃❑¿¿

𝑯𝒈+𝟏𝑺−𝟐 𝑯𝒈𝟐𝑺