Nomenclature Draft

Naming Compounds

Naming and Converting Compounds

• Working Backwards: Naming to Formula

  • It’s possible to determine a formula from a compound's name.

  • Example: Sodium Oxide

    • Write valences: Na^{1}O^{2} → Na_{2}O

  • Example: Copper(II) Oxide

    • Write valences: Cu^{2}O^{2} → CuO

  • For Covalent Compounds:

    • Use prefixes to denote the number of each element.

  • Example: Dinitrogen Trioxide

    • Formula: N_{2}O_{3}

Writing Formulas and Naming Compounds

• Write and name the following covalent compounds:

  • Li{1}S{2}
    ightarrow Li_{2}S

  • N_{2}O
    ightarrow Dinitrogen Monoxide

  • Pb{4}(SO{4}){2} ightarrow Pb{2}(SO{4}){4}
    ightarrow Pb(SO{4}){2}

Name According to IUPAC Rules

1. Name each compound:

   • a) ZnS
     ightarrow Zinc Sulfide

   • b) FeCl_{3}
     ightarrow Iron(III) Chloride

   • c) CaCO_{3}
     ightarrow Calcium Carbonate

   • d) P{2}O{5}
     ightarrow Diphosphorus Pentoxide

   • e) NaCN
     ightarrow Sodium Cyanide

   • f) N{2}F{2}
     ightarrow Dinitrogen Difluoride

   • g) MgHPO_{4}
     ightarrow Magnesium Hydrogen Phosphate

   • h) Cu(BrO{3}){2}
     ightarrow Copper(II) Bromate

   • i) K_{2}O
     ightarrow Potassium Oxide

   • j) BF_{3}
     ightarrow Boron Trifluoride

2. Valence Values:

   • a) Fe in FeO: 2

   • b) Mn in MnO_{2}: 4

3. Write Formulas:

   • a) Sodium Oxide: Na_{2}O

   • b) Potassium Iodide: KI

   • c) Plumbic Sulfide: PbS_{2}

   • d) Mercury(I) Oxide: Hg_{2}O

   • e) Ferrous Oxide: FeO

   • f) Iron(II) Phosphate: Fe{3}(PO{4})_{2}

   • g) Copper(II) Fluoride: CuF_{2}

   • h) Dichlorine Monoxide: Cl_{2}O

   • i) Silver Sulfide: Ag_{2}S

   • j) Magnesium Nitride: Mg{3}N{2}

   • k) Aluminum Hypochlorite: Al(ClO)_{3}

   • l) Iodine Pentafluoride: IF_{5}

   • m) Calcium Chromate: CaCrO_{4}

   • n) Diphosphorus Pentasulfide: P{2}S{5}

Bases and Naming Bases

• Characteristics of Bases:

  • Contain an OH group.

  • Example Compounds:

  • Sodium Hydroxide: NaOH

  • Calcium Hydroxide: Ca(OH)_{2}

  • Naming Rules for Bases:

  • Named like other ionic compounds with the metal (or positive ion) first followed by the polyatomic ion.

  • Example Names:

  • Calcium Hydroxide, Copper(I) Hydroxide, Al(OH){3} (Aluminum Hydroxide), NH{4}OH (Ammonium Hydroxide)

Acid Types and Naming Guidelines

• Characteristics of Acids:

  • All acids begin with H.

  • Two types exist:

  • Binary Acids:

    • Form: H + ext{non-metal}

    • Naming: Depends on state (gaseous or aqueous).

    • Example: HCl(aq)
      ightarrow ext{Hydrochloric Acid}

  • Oxyacids:

    • Form: H + ext{polyatomic ion}

    • Naming Rules:

    1. Name the polyatomic ion.

    2. Replace “ate” with “ic” and “ite” with “ous.”

    3. Change root for pronunciation.

    4. Add “acid” to the name.

    • Example: For H{2}SO{3}, it becomes Sulfurous Acid.

Hydrates

• Definition: Compounds containing H2O in their structure.

  • Different from aqueous (aq) because H2O is part of the molecule.

  • Example: CuSO{4}ullet5H{2}O
    ightarrow ext{Copper(II) Sulfate Pentahydrate}

  • Greek prefixes denote the number of H2O groups:

  • e.g., Sodium Sulfate Decahydrate, Nickel(II) Sulfate Hexahydrate.

• Examples of Hydrates:

  • Sodium Carbonate Monohydrate: Na{2}CO{3}ullet H_{2}O

  • Barium Chloride Dihydrate: BaCl{2}ullet2H{2}O

  • Sodium Sulfate Decahydrate: Na{2}SO{4}ullet10H_{2}O

  • Nickel(II) Sulfate Hexahydrate: NiSO{4}ullet6H{2}O$$