Chemical Nomenclature

1
Chemical Nomenclature

• 1. Binary Covalent Compounds
• 2. Binary Ionic Compounds - Type I
• 3. Binary Ionic Compounds - Type II
• 4. Ionic Compounds Polyatomic (Complex) Ions
• 5. Hydrated Ionic Compounds

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Type I Binary Ionic Compounds

• The metal cations in these compounds have only
  ONE possible charge.
• Na Zn2 Al3 Ca2
• sodium zinc aluminum calcium
• The charges are memorized or predicted using a
  periodic table!
• The cations are bonded to nonmetal anions
• O2- N3- F- Br -
• oxide nitride
  fluoride bromide
• Notice that simple anions are always named with
  the suffix ide

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• In an ionic compound, the charges of the cations
  and anions must always cancel out.
• Subscripts are used if more than one atom is
  needed to cancel the charges
• sodium chloride Na and Cl-
  NaCl
• lithium oxide Li and O2-
  Li2O
• aluminum bromide Al3 and Br - AlBr3
• zinc nitride Zn2 and N3-
  Zn3N2
• potassium iodide K and I- KI
• silver phosphide Ag and P3- Ag3P

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Examples Type I Binary Ionic Compounds
Write the formula
K
O2-
K2O
Name the compound
Potassium oxide
5
Examples Type I Binary Ionic Compounds
Write the formula
Zn2
Cl-
ZnCl2
Name the compound
zinc chloride
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Examples Type I Binary Ionic Compounds
Write the formula
Ag
S2-
Ag2S
Name the compound
silver sulfide
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Examples Type I Binary Ionic Compounds
Write the formula
Al3
N3-
AlN
Name the compound
aluminum nitride
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Examples Type I Binary Ionic Compounds
Write the formula
Ga3
O2-
Ga2O3
Name the compound
gallium oxide
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Examples Type I Binary Ionic Compounds
Write the formula
Ca2
I-
CaI2
Name the compound
calcium iodide
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Examples Type I Binary Ionic Compounds
Write the name K3N
potassium nitride
Write the ions
K
N3-
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Examples Type I Binary Ionic Compounds
Write the name AgI
silver iodide
Write the ions
Ag
I-
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Examples Type I Binary Ionic Compounds
Write the name ZnBr2
zinc bromide
Write the ions
Zn2
Br -
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Examples Type I Binary Ionic Compounds
Write the names Al2O3
aluminum oxide
Write the ions
Al3
O2-
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Examples Type I Binary Ionic Compounds
Write the names Ba3P2
barium phosphide
Write the ions
Ba2
P3-
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Examples Type I Binary Ionic Compounds
Write the name LiH
lithium hydride
Write the ions
Li
H-
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Type II Binary Ionic Compounds

• These are ionic compounds where the metal cation
  can form TWO different charges.
• Fe2 iron (II) Fe3 iron
  (III)
• Ni2 nickel (II) Ni3 nickel
  (III)
• Co2 cobalt (II) Co3 cobalt
  (III)
• Cu copper (I) Cu2 copper (II)
• Au gold (I) Au3 gold (III)
• Sn2 tin (II) Sn4 tin (IV)
• An older system uses suffixes and Latin names,
  -ous for the lower charge, -ic for the higher
  charge
• Ferrous Ferric, Cuprous Cupric, Stannous
  Stannic

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Examples Type II Binary Ionic Compounds

• Write the formulas
• iron (II) oxide
• copper (II) chloride
• tin (IV) sulfide
• cupric nitride
• nickel (III) oxide
• ferrous iodide
• cobalt (III) selenide

• Write the names
• Fe2O3
• SnS
• NiBr2
• CuS
• Pb3P2
• CuBr
• FeCl3

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Polyatomic (Complex) Ions

• All of the cations and anions so far have been
  simple ions - single atoms that have lost or
  gained electrons.
• A molecule is a particle that forms when two or
  more atoms bond together.
• A complex ion is a charged molecule. Complex
  ions may be cations or anions.
• examples
• nitrate NO3- sulfate SO42- hydroxide OH-

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Writing formulas with Complex Ions

• a) Ammonium chloride NH4Cl
• b) Silver sulfate Ag2SO4
• c) Aluminum hydroxide Al(OH)3
• d) Calcium phosphate Ca3(PO4)2
• e) Iron (III) nitrite Fe(NO2)3
• f) Copper(II) permanganate Cu(MnO4)2
• g) Ammonium dichromate (NH4)2Cr2O7
• h) Zinc acetate Zn(CH3COO)2

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Things to Notice

• Most complex ions are anions. Ammonium, NH4, is
  the most common complex cation.
• Several complex ions form a short series of ions.
  The ions differ only in the number of oxygen
  atoms
• perchorate ClO4- sulfate SO42-
• chlorate ClO3- sulfite SO32-
• chlorite ClO2-
• hypochlorite ClO- nitrate NO3-
• nitrite NO2-

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• If an ion carries a charge like -2 or -3, a
  series of related ions can be formed by adding
  hydrogen cations (H) while still leaving a net
  charge
• examples
• Sulfide S2- hydrogen sulfide HS-
• (bisulfide)
• Sulfate SO42- hydrogen sulfate HSO4-
• (bisulfate)
• Carbonate CO32- hydrogen carbonate HCO3-
• (bicarbonate)
• Phosphate PO43- hydrogen phosphate HPO42-
• dihydrogen phosphate H2PO4-

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More Formulas with Complex Ions

• a) Sodium bicarbonate NaHCO3
• b) Nickel (II) hydrogen sulfide Ni(HS)2
• c) Aluminum perchlorate Al(ClO4)3
• d) Barium dihydrogen phosphate Ba(H2PO4)2
• e) Iron (III) sulfite Fe2(SO2)3
• f) Cuprous bisulfate CuHSO4
• g) Zinc periodate Zn(IO4)2
• h) Lithium selenite Li2SeO3

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Hydrated Ionic Compounds

• A HYDRATE is an salt that has water molecules
  trapped within its crystals.
• Every hydrate has a certain number of water
  molecules associated with each formula unit of
  the ionic compound. The number of water
  molecules is indicated by using prefixes.
• mono hexa
• di hepta
• tri octa
• tetra nona
• penta deca

CuSO4 5 H2O copper (II) sulfate
pentahydrate MgCO3 10 H2O magnesium carbonate
decahydrate
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Examples of hydrates

• Write the formulas
• copper(II) fluoride tetrahydrate CuF2 4
  H2O
• calcium nitrate trihydrate Ca(NO3)2 3 H2O
• Write the names
• MgSO4 7 H2O magnesium sulfate heptahydrate
• FeCl2 H2O iron (II) chloride monohydrate