Chemical Nomenclature
1. Binary Covalent Compounds 2. Binary Ionic Compounds - Type I3. Binary Ionic Compounds - Type II4. Ionic Compounds & Polyatomic (Complex) Ions5. Hydrated Ionic Compounds
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”
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
Examples: Type I Binary Ionic Compounds
Write the formula: K+ O2-
K2OName the compound:
Potassium oxide
Examples: Type I Binary Ionic Compounds
Write the formula: Zn2+ Cl-
ZnCl2
Name the compound:zinc chloride
Examples: Type I Binary Ionic Compounds
Write the formula: Ag+ S2-
Ag2SName the compound:
silver sulfide
Examples: Type I Binary Ionic Compounds
Write the formula: Al3+ N3-
AlN
aluminum nitrideName the compound:
Examples: Type I Binary Ionic Compounds
Write the formula: Ga3+ O2-
Ga2O3
Name the compound:gallium oxide
Examples: Type I Binary Ionic Compounds
Write the formula: Ca2+ I-
CaI2
calcium iodideName the compound:
Examples: Type I Binary Ionic Compounds
Write the name:
K3Npotassium nitride
Write the ions:K+ N3-
Examples: Type I Binary Ionic Compounds
Write the name:
AgIsilver iodideWrite the ions:
Ag+ I-
Examples: Type I Binary Ionic Compounds
Write the name:
ZnBr2zinc bromide
Write the ions:
Zn2+ Br -
Examples: Type I Binary Ionic Compounds
Write the names:
Al2O3
aluminum oxideWrite the ions:
Al3+ O2-
Examples: Type I Binary Ionic Compounds
Write the names:
Ba3P2
barium phosphideWrite the ions:Ba2+ P3-
Examples: Type I Binary Ionic Compounds
Write the name:
LiHlithium hydride
Write the ions:Li+ H-
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
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
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: SO4
2- hydroxide: OH-
Writing formulas with Complex Ionsa) 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
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 SO4
2-
chlorate ClO3- sulfite SO3
2-
chlorite ClO2-
hypochlorite ClO- nitrate NO3-
nitrite NO2-
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: HPO4
2-
dihydrogen phosphate: H2PO4-
More Formulas with Complex Ionsa) 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
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 hexadi heptatri octatetra nonapenta deca
CuSO4 · 5 H2O
copper (II) sulfate pentahydrate
MgCO3 ·10 H2O
magnesium carbonate decahydrate
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
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