Nomenclature of Ionic Compounds

Overview

• Focus on naming ionic compounds with polyatomic ions and transition metals.
• Importance of knowing names of certain polyatomic ions.

Polyatomic Ions

• SO3 2-: Sulfite
• SO4 2-: Sulfate
• S2-: Sulfide (monoatomic ion ending in -ide)

Examples of Phosphorus and Chlorine Ions

• PO4 3-: Phosphate
• PO3 3-: Phosphite
• P3-: Phosphide
• ClO4-: Perchlorate
• ClO3-: Chlorate
• ClO2-: Chlorite
• Cl-: Chloride (monoatomic ion)

Additional Ions

• OH-: Hydroxide
• CO3 2-: Carbonate
• NO3-: Nitrate
• NO2-: Nitrite
• CH3COO-: Acetate
• CrO4 2-: Chromate
• Cr2O7 2-: Dichromate
• MnO4-: Permanganate
• CN-: Cyanide
• C2O4 2-: Oxalate

Naming Examples

Simple Ionic Compounds

• NaCl: Sodium Chloride
• KClO3: Potassium Chlorate
• Na2CO3: Sodium Carbonate
• MgS: Magnesium Sulfide
• BaSO4: Barium Sulfate
• Al(OH)3: Aluminum Hydroxide

Transition Metals with Multiple Oxidation States

• FeCl2: Iron (II) Chloride
• FeCl3: Iron (III) Chloride
• Use Roman numerals to specify the charge of the transition metal.

Roman Numerals

• I: 1
• II: 2
• III: 3
• V: 5
• IV: 4 (5-1)
• VI: 6 (5+1)
• VII: 7 (5+2)

Oxidation State Examples

• FeS: Iron (II) Sulfide
• Fe2S3: Iron (III) Sulfide
• Use an equation to solve for the oxidation state:
  • Total charge = 0 (neutral compound)
  • Example: 2Fe + 3(-2) = 0
  • Solve for Fe.

Group Charges

• Group 1: +1 (e.g., Sodium, Lithium)
• Group 2: +2 (e.g., Calcium, Magnesium)
• Group 3A: +3 (e.g., Aluminum)
• Group 4A: ±2, ±4 (e.g., Tin, Lead)
• Nitrogen/Phosphorus: -3
• Oxygen/Sulfur/Selenium: -2
• Halogens (e.g., Chlorine): -1

Advanced Examples

• PbO: Lead (II) Oxide
• PbO2: Lead (IV) Oxide

Vanadium and Tin Examples

• V3P5: Vanadium (V) Phosphide
• Sn3(PO4)4: Tin (IV) Phosphate

Conclusion

• Understanding charges and oxidation states is crucial.
• Use Roman numerals for naming transition metal compounds.
• Familiarity with polyatomic ions and their charges is essential.