CH1120 Nomenclature
of Inorganic Compounds
What type of compound is it ?
Ionic Compound Covalent (Nonionic) Compound
Acid
Cation with fixed charge
Cation with variable charge
Binary Contains polyatomic ion Binary Contains
polyatomic ion
Binary Acid
Oxy Acid
Aluminum, AlChlorine, Cl2 Aluminum chloride, AlCl3Iron (II) chloride, FeCl2Sodium Phosphate, Na3PO4Tin (IV) Chloride SnCl4 Carbon monoxide, COCarbon dioxide, CO2Hydrochloric Acid, HClPerchloric Acid, HClO4
atomic element
ionic compoundmolecular element
molecular compound
ionic compoundionic compound
ionic compound
molecular compoundbinary acidoxy acid
What type of substance is it ?Practice:
Ionic Compounds
Compounds of metals with nonmetals are made of ions. Metal atoms form cations, nonmetal atoms form
anions.
No individual molecule units. A 3-dimensional array of cations and anions made of formula units.
Many contain polyatomic ions-several atoms attached together by covalent bonds into one ion.
Compound must have no total charge, therefore we must balance the numbers of cations and anions in a
compound to get o charge.
name of cation(metal)
base name of anion (nonmetal) “ide”+ +
Ionic Compounds
Naming Metal Cations
Some metals have one possible charge
Groups 1A1+ & 2A2+, Al3+, Ag1+, Zn2+, Sc3+
cation name = metal name
Naming Metal Cations
Metals with Variable Charges metals whose ions can have
more than one possible charge
Determine charge by charge on anion and cation
cation name = metal name (CHARGE)
IVA VA VIA VIIA
H -
hydride
C4-
carbideN3-
nitrideO2-
oxideF -
fluoride
Si4-
silicideP3-
phosphideS2-
sulfideCl -
chloride
As3-
arsenideSe2-
selenideBr -
bromide
Te2-
tellurideI -
iodide
Naming Monatomic Nonmetal AnionsDetermine the charge from position on the Periodic Table.
To name anion, change ending on the element name to –ide.
C22-
carbide
Naming Binary Ionic Compounds for Metals with Invariant Charge
1. Name the metal cation first, name nonmetal anion second
2. Cation name is the metal name
3. Nonmetal anion named by changing the ending on the nonmetal name to -ide
name of cation(metal)
base name of anion (nonmetal) “ide”+ +
1. KCl
2. MgBr2
3. Al2S3
potassium chloride
magnesium bromide
aluminum sulfide
name of cation(metal)
base name of anion (nonmetal) “ide”+ +
Name the following compounds
Naming Binary Ionic Compounds for Metals with Variable Charge
1. Name metal cation first, name nonmetal anion second
2. The metal cation name is the metal name followed by a Roman numeral in parentheses to indicate its charge which is determined by charge on the anion.
3. Nonmetal anion named by changing the ending on the nonmetal name to -ide
name of cation(metal)
base name of anion (nonmetal) “ide”+( )+ +charge of cation (metal)
in roman numerals
Determine a charge from the formula of a specific compound.
The sum of all the charges must be zero.
Example: The charge on iron (Fe) in FeCl3 must be 3+ in order for the compound to be charge neutral with
the three Cl- anions.
name of cation(metal)
base name of anion (nonmetal) “ide”+ +
NaCl Sodium chloride
CaF2 Calcium fluoride
K2O Potassium oxide
Barium nitrideBa3N2
name of cation(metal)
base name of anion (nonmetal) “ide”+( )+ +charge of cation (metal)
in roman numerals
Name the following compounds
1 CuF2 2. TiCl4 3. PbBr2
4. CrO3
5. Fe3N2
6. Fe2S3
Charge on Cation?Cu= 2+
Ti = 4+
Pb = 2+
Cr = 6+Fe = 2+Fe= 3+
copper (II) fluoride
titanium (IV) chloride
lead (II) bromide
chromium (VI) oxideiron (II) nitrideiron (III) sulfide
Na +Na
Cl - NaCl
ClFeCl2
Fe
Fe 2+
Cl
Cl - Cl -
Cl
Fe 3+ FeCl3
Using dot structures can illustrate the formation of binary ionic compounds.
sodium chloride
iron (II) chloride
iron (III) chloride
ClFe
Cl
Cl
Cl -
Cl -Cl -
O
FeOFe
Fe 2+
Na
Na
O 2-Na +Na +
Na2O
Using dot structures can illustrate the formation of binary ionic compounds.
sodium oxide
iron (II) oxide
iron (III) oxide
O O 2-
Fe Fe
O O O
Fe 3+
Fe 3+
O 2-
O 2-O 2- Fe2O3
Compounds Containing Polyatomic Ions
Polyatomic ions are ions that contain more than one atom.
Often identified by parentheses around ion in formula
Name and charge of polyatomic ion do not change
An ionic compound is always named by naming the cation first and then the anion.
Roman numeral indicating charge
(if needed)
name of cationic species
name of anionic species
+ +
Compounds Containing Polyatomic Ions
metal or polyatomic
cation
nonmetal or polyatomic
anion
Some Common Polyatomic Ions
+3 +4 +5 +6 +7
BO33-
borateCO32-
carbonateNO3-
nitrate
SiO32-
silicatePO43-
phosphateSO42-
sulfateClO3-
chorate
AsO43-
arsenateSeO42-
selenateBrO3-
bromate
TeO42-
tellurateIO3-
iodate
Periodic Pattern of Polyatomic Ions-“ate” groups
“formal charge” on central atom
Some Common Polyatomic Ions
Name the Following Compounds
1. Na2SO4
2. Fe(NO3)3
3. NH4Cl
4. Ca(C2H3O2)2
5. Cu(NO3)2
sodium sulfate
iron (III) nitrate
ammonium chloridecalcium acetate
copper(II) nitrate
SO42-, sulfate; NO3 -, nitrate;
NH4 +, ammonium; (C2H3O2) -, acetate
Writing formula for ionic compounds containing polyatomic ions
Aluminum sulfate
Iron (III) phosphate
Chromium (II) hydrogen carbonate
Al2(SO4)3
FePO4
Cr(HCO3)2
SO42-, sulfate; PO4 3-, phosphate;
(HCO3) -, hydrogen carbonate
Hydrates
Hydrates are ionic compounds containing a specific number of waters
for each formula unit.
In formula, attached waters indicated
CoCl2·6H2O or CoCl2(H2O)6
In name attached waters indicated by prefix+hydrate
after name of ionic compound:
CoCl2·6H2O cobalt(II) chloride hexahydrate
CaSO4·½H2O calcium sulfate hemihydrate
In name attached waters indicated by prefix+hydrate
after name of ionic compound:
CoCl2·6H2O cobalt(II) chloride hexahydrate
CaSO4·½H2O calcium sulfate hemihydrate
Hydrates
Writing Names of Binary Molecular Compounds of Two Nonmetals
1. Write name of first element in formula a) element furthest left and down on the Periodic Table b) use the full name of the element
2. Writes name the second element in the formula with an -ide suffix, as if it were an anion, however, remember these compounds do not contain ions!
3. Use a prefix in front of each name to indicate the number of atoms (Never use the prefix mono- on the first element)
Subscript <–> Prefixes
1 = mono- 2 = di- 3 = tri- 4 = tetra- 5 = penta-
6 = hexa- 7 = hepta- 8 = octa- 9 = nona-10 = deca-
prefix prefix “ide”name of first element
name of second element+ + + +
BF3
NO2
PCl5
I2F7
Formulas --------------> Names
boron trifluoride
nitrogen dioxide
phosphorous pentachloride
diiodine heptafluoride
prefix prefix “ide”name of first element
name of second element+ + + +
Name -------------> Formula
dinitrogen pentoxide
dinitrogen tetroxide
sulfur hexafluoride
diarsenic trisulfide
N2O5
N2O4
SF6
As2S3
prefix prefix “ide”name of first element
name of second element+ + + +
Acids
Acids are molecular compounds that form H+ when dissolved in water.
(aq) is often written after the formula
Sour taste
Dissolve many metals such as Zn, Fe, Mg; but not Au, Ag, Pt
Formula generally starts with H e.g., HCl, H2SO4
The oxygen is generally associated with a polyatomic anion.
Acids
Binary Acidscontain only two elements
Oxyacidscontain oxygen
Naming Binary Acids
HCl HF HI
hydrochloric acid
base name of nonmetal
“hydro” “ic” acid+ + +
hydrofluoric acidhydroiodic acid
Naming OxyacidsName the polyatomic anion !!!!!
If polyatomic ion name ends in “–ate”,
base name of oxyanion
“ic” acid
If polyatomic ion name ends in “–ite”,
base name of oxyanion
“ous” acid
+ +
+ +
NO2 ⊖ nitrite HNO2 nitrous acid
SO42- sulfate H2SO4 sulfuric acid
ClO2 ⊖ chlorite HClO2 chlorous acid
C2H3O2 ⊖ acetate HC2H3O2 acetic acid
Oxyanion formula
Oxyanion nameAcid
Formula Acid Name
NO2 ⊖ nitrite H+ HNO2 nitrous
NO3 ⊖ nitrate H+ HNO3 nitric
SO3 2⊖ sulfite 2H+ H2SO3 sulfurous
SO4 2⊖ sulfate 2H+ H2SO4 sulfuric
ClO2 ⊖ chlorite H+ HClO2 chlorous
ClO3 ⊖ chlorate H+ HClO3 chloric
C2H3O2 ⊖ acetate H+ HC2H3O2 acetic
CO3 2⊖ carbonate 2H+ H2CO3 carbonic
Names of Common Oxyacids and Their Oxyanions
Formula ----------> Namea. HCl(aq)
b. HBr(aq) c. H2S(aq)
d. H2SO4 e. H2SO3
f. HClO3
g. HNO2
hydrochloric acid
hydrobromic acid
hydrosulfuric acid
sulfuric acid
sulfurous acid
chloric acid
nitrous acid
SO4 2-, sulfate
SO3 2-, sulfite
ClO3-, chlorate
NO2-, nitrite
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