Inorganic Compounds- nomenclature
University of Lincoln
presentation
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INORGANIC COMPOUNDS
• Compounds composed of elements other
than carbon.
• Associated with the nonliving portion of
the world
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NOMENCLATURE OF
INORGANIC COMPOUNDS
•Ionic Compounds
•Molecular Compounds
•Acids
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NAMING IONIC COMPOUNDS
1. CATIONS ( POSITIVE IONS)
A. Cations formed from metal atoms
have the same name as the metal.
Na+
Al3+
sodium ion
Zn2+ zinc ion
aluminum ion
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B. If a metal can form cations of different
charges, the positive charge is given by a
Roman numeral in parenthesis following the
name of the metal.
Fe2+
Fe3+
iron (II) ion
iron (III) ion
Cu+ copper (I) ion
Cu2+ copper (II) ion
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• Ions with different charges exhibit
different properties, such as color.
• Most of the metals that have variable
charges are transition metals.
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• Apply –ous or –ic
• The endings represent the lower and higher
charged ions, respectively.
Fe2+
Fe3+
ferrous ion
ferric ion
Cu+ cuprous ion
Cu2+ cupric ion
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IONIC CHARGES OF
REPRESENTATIVE ELEMENTS
1A
2A
Li+
Be2+
Na+
Mg2+
K+
Ca2+
Rb+
Sr2+
Cs+
Ba2+
3A
Al+3
4A
5A
6A
7A
N3-
O2-
F-
P3-
S2-
Cl-
As3-
Se2-
Br-
0
I-
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FORMULAS AND NAMES OF COMMON METAL IONS WITH MORE THAN ONE
IONIC CHARGE
FORMULA
STOCK NAME
CLASSICAL NAME
Cu+
Copper (I) ion
Cuprous ion
Cu2+
Copper (II) ion
Cupric ion
Fe2+
Iron (II) ion
Ferrous ion
Fe3+
Iron (III) ion
Ferric ion
Hg2+
Mercury (I) ion
Mercurous ion
Hg2+
Mercury (II) ion
Mercuric ion
Pb2+
Lead (II) ion
Plumbous ion
Pb4+
Lead (IV) ion
Plumbic ion
Sn2+
Tin (II) ion
Stannous ion
Sn4+
Tin (IV) ion
Stannic ion
Cr2+
Chromium (II) ion
Chromous ion
Cr3+
Chromium (III) ion
Chromic ion
Mn2+
Manganese (II) ion
Manganous ion
Mn3+
Manganese (III) ion
Manganic ion
Co2+
Co3+
Cobalt (II) ion
Cobalt (III) ion
Cobaltous ion
Cobaltic ion
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C. Cations formed from nonmetals have
names that end in –ium
NH4+
H3 O +
ammonium ion
hydronium ion
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EXERCISES:
• Name each of the following:
1.
2.
3.
4.
5.
6.
Sn2+
Sn4+
K+
Ba2+
Co2+
Co3+
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1.
2.
3.
4.
5.
6.
Sn2+ Tin (II) ion
Sn4+
Tin (IV) ion
K+
Potassium ion
Ba2+
Barium ion
Co2+
Cobalt (II) ion
Co3+
Cobalt (III) ion
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2. ANIONS (NEGATIVE IONS)
A. Monoatomic (one-atom) anions have
names formed by replacing the ending of
the name of the element with –ide
H-
O2-
Hydride ion
N3-
OH-
Oxide ion Nitride ion Hydroxide ion
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B. Polyatomic (many-atoms) anions containing oxygen have names ending in
–ate or –ite
• These are called oxyanions
• -ate is used for the most common oxyanion of an element
• -ite is used for an oxyanion that has the same charge but one less O atoms
NO3-
nitrate ion
SO42- sulfate ion
NO2-
nitrite ion
SO32- sulfite ion
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• Prefixes are used when the series of
oxyanions of an element extends to four
members, as with halogens
• The prefix per- indicates one or more O
atom than the oxyanion ending in –ate
• The prefix hypo- indicates one less O atom
than the oxyanion ending in –ite
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ClO4- perchlorate ion (one more O atom
than chlorate)
ClO3- chlorate ion
ClO2- chlorite ion (one less O atom than
chlorate)
ClO- hypochlorite ion (one less O atom
than chlorite)
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C. Anions derived by adding H+ to an
oxyanion are named by adding as a prefix
the word hydrogen or dihydrogen
CO32HCO3PO43H2PO4-
carbonate ion
hydrogen carbonate ion
phosphate ion
dihydrogen phosphate ion
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COMMON POLYATOMIC IONS
1- charge
2- charge
3- charge
H2PO4-
Dihydrogen phosphate
HPO42-
Hydrogen phosphate
Phosphite
C2H3O2-
Acetate
PO33-
C2O42-
Oxalate
Phosphate
HSO3
Hydrogen sulfite
PO43-
SO32-
Sulfite
HSO4-
Hydrogen sulfate
SO42-
Sulfate
HCO3
Hydrogen carbonate
CO32-
Carbonate
NO2-
Nitrite
CrO42-
Chromate
NO3-
Nitrate
Cr2O72-
Dichromate
CN-
Cyanide
SiO32-
Silicate
OH-
Hydroxide
MnO4-
Permanganate
ClO-
Hypochlorite
ClO2-
Chlorite
ClO3-
Chlorate
ClO4-
Perchlorate
-
-
1+ charge
NH4+
Ammonium
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3. IONIC COMPOUNDS
Names of ionic compounds consist of the
cation name followed by the anion name
CaCl2
Al(NO3)3
Cu(ClO4)2
calcium chloride
aluminum nitrate
copper (II)perchlorate
cupric perchlorate
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EXERCISES:
• What is the charge of the ion typically
formed by each element?
1.
2.
3.
4.
5.
6.
Sulfur
Lead, 4 electrons lost
Strontium
Argon
Bromine
Copper, 1 electron lost
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1.
2.
3.
4.
5.
6.
Sulfur
Lead, 4 electrons lost
Strontium
Argon
Bromine
Copper, 1 electron lost
24+
2+
no ion formed
11+
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• Name the following compounds:
1. CuS
2.K3N
3.SnCl2
4.K2S
5.CaI2
6.NaI
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1.
2.
3.
4.
5.
6.
CuS
K3N
SnCl2
K2S
CaI2
NaI
Copper (II) sulfide
Potassium Nitride
Tin (II) chloride
Potassium sulfide
Calcium Iodide
Sodium Iodide
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• Name the following:
1. MgCl2
2. SnCl4
3. HgBr2
4. PbS2
5. FeO
• Write the formula for each of the following:
1. Magnesium bromide
2. Aluminum oxide
3. Ferrous bromide
4. Lead (II) sulfide
5. Stannic oxide
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HOMEWORK:
• Name the following:
1.
2.
3.
4.
5.
6.
CoI2
Cs2O
ZnS
KCI
BaO
CuBr2
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1.
2.
3.
4.
5.
6.
CoI2
Cs2O
ZnS
KCI
BaO
CuBr2
Cobalt Iodide
Cesium Oxide
Zinc sulfide
Potassium chloride
Barium Oxide
Copper bromide
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NAMES OF FORMULAS OF ACIDS
• An acid is a substance whose molecules
yield hydrogen ions (H+) when dissolved in
water.
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1.
Acid based on anions whose names end in –ide. Anions whose
names end in –ide have he asociated acids that have the
hydro- prefix and an –ic ending
ANION
CORRESPONDING ACIDS
Cl- (chloride)
HCl (hydrochloric acid)
S2- (sulfide)
H2S (hydrosulfuric acid)
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2. Anions whose names end in –ate have
associated acids with an –ic ending,
whereas anions whose names end in –ite
have acids with an -ous ending. Prefixes in
the name of the anion are retained in the
name of the acid.
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ANION
CORRESPONDING ACID
ClO4- perchlorate
HClO4 – perchloric acid
ClO3- chlorate
HClO3 – chloric acid
ClO2- chlorite
HClO2 – chlorous acid
ClO- hypochlorite HClO – hypochloric acid
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EXERCISES:
Give the name or formula for the following:
1. H2SO4
2.H2CO3
3.Nitric acid
4.Phosphoric acid
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Acknowledgements
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JISC
HEA
Centre for Educational Research and Development
School of natural and applied sciences
School of Journalism
SirenFM
http://tango.freedesktop.org
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