Chemical Nomenclature

1
Chemical Nomenclature

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

2
Definitions

• An IONIC COMPOUND consists of a metal cation
  bonded to a nonmetal anion. Electrostatic
  attraction holds them together.
• A COVALENT COMPOUND consists of two nonmetal
  atoms sharing valence electrons.
• A BINARY compound is one that is made of just two
  elements.

3
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

4

• 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

5
Examples Type I Binary Ionic Compounds

• Write the formulas
• potassium oxide
• zinc chloride
• silver sulfide
• aluminum nitride
• gallium oxide
• calcium iodide

• Write the names
• K3N
• AgI
• ZnBr2
• Al2O3
• Ba3P2
• LiH

6
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

7
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

8
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-

9
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

10
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-

11

• 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-

12
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

13
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
14
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

15
Binary Covalent Compounds

• Covalent compounds are made of two NONMETAL
  elements sharing valence electrons.
• There are no ions involved!!
• Because there are no charges to help us write the
  formulas of covalent compounds, prefixes are used
  to indicate the number of each atom present in
  the formula.
• CO2 is named carbon dioxide
• CO is named carbon monoxide
• N2O is named dinitrogen monoxide
• SO3 is named sulfur trioxide

The prefix, mono is never used for the first
element in the formula!
16
Examples of Covalent Naming

• Write the names
• SO2 sulfur dioxide
• P4O10 tetraphosphorus decoxide
• Write the formulas
• phosphorus pentachloride PCl5
• dinitrogen trioxide N2O3

17
Binary Acids

• A simple definition of an acid is a substance
  which produces H ions in water.
• Most acids have hydrogen ions in their formulas.
• A binary acid composed of a hydrogen cation
  bonded to one other element
• HCl HBr H2S
• hydrochloric acid hydrobromic acid hydrosulfuric
  acid
• Binary acids are always named hydro____ic acid

18
Oxy-Acids

• An acid can also be made of a hydrogen ion bonded
  to a complex ion.
• Complex ions whose names end in ate
• NO3- SO42- CO32- PO43-
• nitric acid HNO3
• sulfuric acid H2SO4
• carbonic acid H2CO3
• phosphoric acid H3PO4

Can you propose a rule for naming oxy-acids with
complex ions ending in ate?
19
More Oxy-Acids

• Complex ions ending in ite
• NO2- SO32- ClO- ClO2-
• nitrous acid HNO2
• sulfurous acid H2SO3
• hypochlorous acid HClO
• chlorous acid HClO2

Can you propose a rule for naming oxy-acids with
complex ions ending in ite?