chemical nomenclature 1. binary ionic compounds - type i 2. binary ionic compounds - type ii 3....
TRANSCRIPT
Chemical Nomenclature
1. Binary Ionic Compounds - Type I
2. Binary Ionic Compounds - Type II
3. Ionic Compounds & Polyatomic
(Complex) Ions
4. Oxy-Acids
5. Hydrated Ionic Compounds
6. Binary Acids
7. Binary Covalent 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 formulas:
•potassium oxide
• zinc chloride
• silver sulfide
• aluminum nitride
• gallium oxide
•calcium iodide
Write the names:
• K3N
• AgI
• ZnBr2
• Al2O3
• Ba3P2
• LiH
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
Examples: Type II Binary Ionic CompoundsWrite the formulas:
• iron (II) oxide FeO
• copper (II) chloride CuCl2
• tin (IV) sulfide SnS2
• cupric nitride Cu3N2
• nickel (III) oxide Ni2O3
• ferrous iodide FeI2
•cobalt (III) selenide Co2Se3
Write the names: Fe2O3 Iron (III) oxide Ferric oxide SnS Tin(II)sulphide stannous sulfide NiBr2 Nickle (II) bromide CuS Copper (II) Sulfide Cupric
sulphide Pb3P2 L CuBr FeCl
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
b) Silver sulfate
c) Aluminum hydroxide
d) Calcium phosphate
e) Iron (III) nitrate
f) Copper(II) permanganate
g) Ammonium dichromate
h) Zinc acetate
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) nitrate Fe(NO3)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:
perchlorate ClO4- sulfate SO4
2-
chlorate ClO3- sulfite SO3
2-
chlorite ClO2-
hypochlorite ClO- nitrate NO3-
nitrite NO2-
More Formulas with Complex Ionsa) Sodium carbonate
b) Nickel (II) sulfite
c) Aluminum chlorate
d) Barium phosphite
e) Iron (III) sulfite
f) Cupric sulfate
g) Zinc periodate
More Formulas with Complex Ionsa) Sodium carbonate Na2CO3
b) Nickel (II) sulfite NiSO3
c) Aluminum chlorate Al(ClO3)3
d) Barium phosphite Ba3(PO3)2
e) Iron (III) sulfite Fe2(SO3)3
f) Cupric sulfate CuSO4 copper (II) Sulphate
Cuprous sulphate Cu2SO4 copper (I)Sulphate
g) Zinc periodate Zn(IO4)2
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
calcium nitrate trihydrate
Write the names:
MgSO4 · 7 H2O
FeCl2 · H2O
CuF2 ·4 H2O
Ca(NO3)2 ·3 H2O
magnesium sulfate heptahydrate
iron (II) chloride monohydrate
Examples of hydrates: Write the formulas:
copper(II) fluoride tetrahydrate
calcium nitrate trihydrate
Write the names:
MgSO4 · 7 H2O
FeCl2 · H2O
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- SO4
2- CO32- PO4
3-
nitric acid: HNO3
sulfuric acid: H2SO4
carbonic acid: H2CO3
phosphoric acid: H3PO4
Chloric acid HClO3
Can you propose a rule for naming oxy-acids
with complex ions ending in “ate”?
More Oxy-Acids Complex ions ending in “ite”:
NO2- SO3
2- ClO- ClO2-
nitrous acid: HNO2
sulfurous acid: H2SO3
hypochlorous acid: HClO
( from hypochlorite ion)
chlorous acid HClO2
Can you propose a rule for naming oxy-acids
with complex ions ending in “ite”?
Acids Nitric Acid Nitrous acid Hyposulphurous acid Perchloric acid
Acids Nitric Acid HNO3
Nitrous acid HNO2
Hyposulphurous acid H2SO2
Perchloric acid HClO4
Acid SaltsAcid Salt ions can be formed if an oxy 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 remainder net charge:
examples:
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 hydrogen carbonate
b) Nickel (II) hydrogen sulfate
c) Aluminum perchlorate
d) Barium dihydrogen phosphate
e) Iron (III) sulfite
f) Cuprous Hydrogen hyposulphite
g) Zinc periodate
More Formulas with Complex Ionsa) Sodium bicarbonate NaHCO3
b) Nickel (II) hydrogen sulfate Ni(HSO4)2
c) Aluminum perchlorate Al(ClO4)3
d) Barium dihydrogen phosphate Ba(H2PO4)2
e) Iron (III) sulfite Fe2(SO3)3
f) Cuprous hydrogen hyposulphite CuHSO2
g) Zinc periodate Zn(IO4)2
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
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. Brandon is awesome.
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!
Examples of Covalent Naming Write the names:
SO2
P4O10
Write the formulas:
phosphorus pentachloride
dinitrogen trioxide
Examples of Covalent Naming Write the names:
SO2 sulfur dioxide
P4O10 tetraphosphorus decoxide
Write the formulas:
phosphorus pentachloride PCl5
dinitrogen trioxide N2O3