2.4: Chemical
Nomenclature
1. Molecular Compounds
Naming:
Prefixes
• Put the appropriate prefix IN FRONT of the element1name
– mono
▫ Exception: Do not use mono- on the FIRST element
• Change the ending of the second element to “ide”
• Many also have common names
Formulas:
• Use the prefix to determine the subscript
• DO NOT reduce.
2 – di
3 – tri
4 – tetra
5 – penta
6 – hexa
7 – hepta
8 – octa
9 – nona
10 -- deca
1. MOLECULAR COMPOUNDS
Common Names
Common Name
Ammonia
Methane
Water
Ozone
Formula
1. Molecular Compounds
Common Names
Common Name
Formula
Ammonia
NH3
Methane
Water
Ozone
1. Molecular Compounds
Common Names
Common Name
Formula
Ammonia
NH3
Methane
CH4
Water
Ozone
1. Molecular Compounds
Common Names
Common Name
Formula
Ammonia
NH3
Methane
CH4
Water
H2O
Ozone
1. Molecular Compounds
Common Names
Common Name
Formula
Ammonia
NH3
Methane
CH4
Water
H2O
Ozone
O3
1. Molecular Compounds
Practice
Trinitrogen hexasulfide
Carbon dioxide
Tetrafluorine octachloride
NO
P2Br9
SI3
1. Molecular Compounds
Practice
Trinitrogen hexasulfide
N3S6
Carbon dioxide
Tetrafluorine octachloride
NO
P2Br9
SI3
1. Molecular Compounds
Practice
Trinitrogen hexasulfide
N3S6
Carbon dioxide
CO2
Tetrafluorine octachloride
NO
P2Br9
SI3
1. Molecular Compounds
Practice
Trinitrogen hexasulfide
N3S6
Carbon dioxide
CO2
Tetrafluorine octachloride
F4Cl8
NO
P2Br9
SI3
1. Molecular Compounds
Practice
Trinitrogen hexasulfide
N3S6
Carbon dioxide
CO2
Tetrafluorine octachloride
F4Cl8
Nitrogen monoxide
NO
P2Br9
SI3
1. Molecular Compounds
Practice
Trinitrogen hexasulfide
N3S6
Carbon dioxide
CO2
Tetrafluorine octachloride
F4Cl8
Nitrogen monoxide
NO
Diphosphorus nonabromide
P2Br9
SI3
1. Molecular Compounds
Practice
Trinitrogen hexasulfide
N3S6
Carbon dioxide
CO2
Tetrafluorine octachloride
F4Cl8
Nitrogen monoxide
NO
Diphosphorus nonabromide
P2Br9
Sulfur triiodide
SI3
2.
Ionic
CompoundS
a)
Simple
Binary Compounds
(2 different elements – metal and
non-metal)
Naming:
• Write the metal first, then the non-metal
• Change the ending of the non metal to –ide
Formulas:
• Write the symbol for each element in the correct order (metal first)
• Write the ionic charge above each symbol
▫ Note: Zn2+ and Ag+
• Criss-cross the numbers from the charges to the opposite element
• Simplify (reduce) if necessary
2. IONIC COMPOUNDS
Practice
Beryllium fluoride
Calcium sulfide
Aluminum oxide
CaCl2
MgO
KP3
2. IONIC COMPOUNDS
Practice
Beryllium fluoride
BeF2
Calcium sulfide
Aluminum oxide
CaCl2
MgO
KP3
2. IONIC COMPOUNDS
Practice
Beryllium fluoride
BeF2
Calcium sulfide
CaS
Aluminum oxide
CaCl2
MgO
KP3
2. IONIC COMPOUNDS
Practice
Beryllium fluoride
BeF2
Calcium sulfide
CaS
Aluminum oxide
Al2O3
CaCl2
MgO
KP3
2. IONIC COMPOUNDS
Practice
Beryllium fluoride
BeF2
Calcium sulfide
CaS
Aluminum oxide
Al2O3
Calcium chloride
CaCl2
MgO
K3P
2. IONIC COMPOUNDS
Practice
Beryllium fluoride
BeF2
Calcium sulfide
CaS
Aluminum oxide
Al2O3
Calcium chloride
CaCl2
Magnesium oxide
MgO
K3P
2. IONIC COMPOUNDS
Practice
Beryllium fluoride
BeF2
Calcium sulfide
CaS
Aluminum oxide
Al2O3
Calcium chloride
CaCl2
Magnesium oxide
MgO
Potassium phosphide
K3P
2. Ionic CompoundS
b) Multivalent Binary Compounds (the metal has more than one ionic charge)
Naming
• Two methods to name these:
a) Stock method – uses roman numerals
 Write the roman number that corresponds with the correct charge AFTER the metal name
(I, II, III, IV, V)
b) Classical method – the “ous-ic” system
 uses latin names of elements
 “ous” = lowest valence
 “ic” = highest valence
Formulas
• Use the criss-cross method and reduce
Multivalent metals
Charges
Copper
Tin
Iron
Nickel
Manganese
Gold
Lead
Mercury
Cu+ Cu2+
Sn2+ Sn4+
Fe2+ Fe3+
Ni2+ Ni3+
Mn2+ Mn4+
Au+ Au3+
Pb2+ Pb4+
Hg+ Hg2+
2. Ionic CompoundS
b) Multivalent Binary Compounds (the metal has more
than one ionic charge)
Latin Name
Cuprum (Cu)
Ferrum (Fe)
Stannum (Sn)
Plumbum (Pb)
Remove
“um” ending
Lower
Valence
Lower Valence
Name (ous)
Higher
Valence
Higher
valence
Name (ic)
2. Ionic CompoundS
b) Multivalent Binary Compounds (the metal has more
than one ionic charge)
Latin Name
Remove
“um” ending
Lower
Valence
Lower Valence
Name (ous)
Higher
Valence
Higher
valence
Name (ic)
Cuprum (Cu)
Cupr
1+
Cuprous
2+
Cupric
Ferrum (Fe)
Stannum (Sn)
Plumbum (Pb)
2. Ionic CompoundS
b) Multivalent Binary Compounds (the metal has more
than one ionic charge)
Latin Name
Remove
“um” ending
Lower
Valence
Lower Valence
Name (ous)
Higher
Valence
Higher
valence
Name (ic)
Cuprum (Cu)
Cupr
1+
Cuprous
2+
Cupric
Ferrum (Fe)
Ferr
2+
Ferrous
3+
Ferric
Stannum (Sn)
Plumbum (Pb)
2. Ionic CompoundS
b) Multivalent Binary Compounds (the metal has more
than one ionic charge)
Latin Name
Remove
“um” ending
Lower
Valence
Lower Valence
Name (ous)
Higher
Valence
Higher
valence
Name (ic)
Cuprum (Cu)
Cupr
1+
Cuprous
2+
Cupric
Ferrum (Fe)
Ferr
2+
Ferrous
3+
Ferric
Stannum (Sn)
Stann
2+
Stannous
4+
Stannic
Plumbum (Pb) plumb
2+
plumbous
4+
Plumbic
2. IONIC COMPOUNDS
Practice
Copper (II) fluoride
Tin (IV) sulfide
Mercury (I) oxide
Stannous phosphide
Ferrous oxide
SnCl2
Fe2S3
PbS2
2. IONIC COMPOUNDS
Practice
Copper (II) fluoride
Cupric fluoride
CuF2
Tin (IV) sulfide
Mercury (I) oxide
Stannous phosphide
Ferrous oxide
SnCl2
Fe2S3
PbS2
2. IONIC COMPOUNDS
Practice
Copper (II) fluoride
Cupric fluoride
CuF2
Tin (IV) sulfide
Stannic sulfide
SnS2
Mercury (I) oxide
Stannous phosphide
Ferrous oxide
SnCl2
Fe2S3
PbS2
2. IONIC COMPOUNDS
Practice
Copper (II) fluoride
Cupric fluoride
CuF2
Tin (IV) sulfide
Stannic sulfide
SnS2
Mercury (I) oxide
Mercurous oxide
Hg2O
Tin (II) phosphide
Stannous phosphide
Sn3P2
Iron (II) oxide
Ferrous oxide
FeO
Tin (II) chloride
Stannous chloride
SnCl2
Iron (III) sulfide
Ferric sulfide
Fe2S3
Lead (IV) sulfide
Plumbic sulfide
PbS2
2. Ionic CompoundS
c) Polyatomic Compounds
• Polyatomic ions: ions that contain more than one type of atom
▫ Can be + or – charged
▫ Will combine with an oppositely charged ion to make a compound
▫ See chart for polyatomic ions
Naming
• Do not change endings of polyatomic ions. Otherwise, same ionic naming rules apply
Formulas
• Use criss-cross method
▫ DO NOT alter the subscripts of the polyatomic ion
▫ Put the polyatomic in brackets, criss-cross the number to the OUTSIDE of these brackets
▫ Simplify if necessary
2. IONIC COMPOUNDS
Practice
Copper (II) chlorate
Zinc sulfate
Magnesium hydroxide
NaCN
Fe(NO3)3
NH4OH
2. IONIC COMPOUNDS
Practice
Copper (II) chlorate
Cu(ClO3)2
Zinc sulfate
Magnesium hydroxide
NaCN
Fe(NO3)3
NH4OH
2. IONIC COMPOUNDS
Practice
Copper (II) chlorate
Cu(ClO3)2
Zinc sulfate
ZnSO4
Magnesium hydroxide
NaCN
Fe(NO3)3
NH4OH
2. IONIC COMPOUNDS
Practice
Copper (II) chlorate
Cu(ClO3)2
Zinc sulfate
ZnSO4
Magnesium hydroxide
Mg(OH)2
NaCN
Fe(NO3)3
NH4OH
2. IONIC COMPOUNDS
Practice
Copper (II) chlorate
Cu(ClO3)2
Zinc sulfate
ZnSO4
Magnesium hydroxide
Mg(OH)2
Sodium cyanide
NaCN
Fe(NO3)3
NH4OH
2. IONIC COMPOUNDS
Practice
Copper (II) chlorate
Cu(ClO3)2
Zinc sulfate
ZnSO4
Magnesium hydroxide
Mg(OH)2
Sodium cyanide
NaCN
Iron (III) nitrate
Fe(NO3)3
NH4OH
2. IONIC COMPOUNDS
Practice
Copper (II) chlorate
Cu(ClO3)2
Zinc sulfate
ZnSO4
Magnesium hydroxide
Mg(OH)2
Sodium cyanide
NaCN
Iron (III) nitrate
Fe(NO3)3
Ammonium hydroxide
NH4OH
2. Ionic CompoundS
d) Derivatives of Polyatomic Ions
• Other polyatomic ions may have different amounts of oxygen atoms
Naming
• Name the original ion
• Add prefix “per-” if there is 1 MORE oxygen
• Change suffix to “-ite” if there is 1 LESS oxygen
• Add prefix “hypo-” and change suffix to “-ite” if there are 2 LESS oxygen
Formulas
• Add or subtract the appropriate number of oxygen from the original ion
• Overall charge of ion does NOT change
2. IONIC COMPOUNDS
Example
Chlorate
ClO3-
2. IONIC COMPOUNDS
Example
perchlorate
ClO4-
Chlorate
ClO3-
2. IONIC COMPOUNDS
Example
perchlorate
ClO4-
Chlorate
ClO3-
chlorite
ClO2-
2. IONIC COMPOUNDS
Example
perchlorate
ClO4-
Chlorate
ClO3-
chlorite
ClO2-
hypochlorite
ClO-
2. IONIC COMPOUNDS
Practice (ions only)
Iodite
Hypophosphite
persulfate
BrO2-
Practice (compounds)
Iron (II) hyposulfite
Lithium chlorite
NaIO
K3PO5
2. IONIC COMPOUNDS
Practice (ions only)
Iodite
IO2-
Hypophosphite
persulfite
BrO2-
Practice (compounds)
Iron (II) hyposulfite
Lithium chlorite
NaIO
K3PO5
2. IONIC COMPOUNDS
Practice (ions only)
Iodite
IO2-
Hypophosphite
PO23-
persulfate
BrO2-
Practice (compounds)
Iron (II) hyposulfite
Lithium chlorite
NaIO
K3PO5
2. IONIC COMPOUNDS
Practice (ions only)
Iodite
IO2-
Hypophosphite
PO23-
persulfate
SO52BrO2-
Practice (compounds)
Iron (II) hyposulfite
Lithium chlorite
NaIO
K3PO5
2. IONIC COMPOUNDS
Practice (ions only)
Iodite
IO2-
Hypophosphite
PO23-
persulfate
SO52-
Bromite
BrO2-
Practice (compounds)
Iron (II) hyposulfite
Lithium chlorite
NaIO
K3PO5
2. IONIC COMPOUNDS
Practice (ions only)
Iodite
IO2-
Hypophosphite
PO23-
persulfate
SO52-
Bromite
BrO2-
Practice (compounds)
Iron (II) hyposulfite
FeSO2
Lithium chlorite
NaIO
K3PO5
2. IONIC COMPOUNDS
Practice (ions only)
Iodite
IO2-
Hypophosphite
PO23-
persulfate
SO52-
Bromite
BrO2-
Practice (compounds)
Iron (II) hyposulfite
FeSO2
Lithium chlorite
LiClO2
NaIO
K3PO5
2. IONIC COMPOUNDS
Practice (ions only)
Iodite
IO2-
Hypophosphite
PO23-
persulfate
SO52-
Bromite
BrO2-
Practice (compounds)
Iron (II) hyposulfite
FeSO2
Lithium chlorite
LiClO2
Sodium hypoiodite
NaIO
K3PO5
2. IONIC COMPOUNDS
Practice (ions only)
Iodite
IO2-
Hypophosphite
PO23-
persulfate
SO52-
Bromite
BrO2-
Practice (compounds)
Iron (II) hyposulfite
FeSO2
Lithium chlorite
LiClO2
Sodium hypoiodite
NaIO
Potassium perphosphate
K3PO5
3. Acids
a) Binary Acids
• An acid which is made by dissolving certain gases in water
• Acids always start with a hydrogen that acts like a metal
• A binary acid is formed from a binary compound
• The subscript (aq) is used to denote the acid
▫ (aq) = aqueous = dissolved in water
Naming
• Has the same formula as the gas, but a different name
(hydro_______ic acid)
Formulas
• Use “criss-cross” – H+ is the cation (H acts like a metal)
3. Acids
a) Binary Acids
Name of Gas
Formula
Name of Acid
Formula
Hydrogen chloride
HCl (g)
Hydrochloric acid
HCl (aq)
HBr (g)
Hydroiodic acid
Hydrogen fluoride
H2S (aq)
3. Acids
a) Binary Acids
Name of Gas
Formula
Name of Acid
Formula
Hydrogen chloride
HCl (g)
Hydrochloric acid
HCl (aq)
Hydrogen bromide
HBr (g)
Hydrobromic acid
HBr (aq)
Hydroiodic acid
Hydrogen fluoride
H2S (aq)
3. Acids
a) Binary Acids
Name of Gas
Formula
Name of Acid
Formula
Hydrogen chloride
HCl (g)
Hydrochloric acid
HCl (aq)
Hydrogen bromide
HBr (g)
Hydrobromic acid
HBr (aq)
Hydrogen iodide
HI (g)
Hydroiodic acid
HI (aq)
Hydrogen fluoride
HF (g)
Hydrofluoric acid
HF (aq)
Hydrogen sulfide
H2S (g)
Hydrosulfuric acid
H2S (aq)
3. Acids
b) Oxyacids
• Contain oxygen, hydrogen, plus another element
Naming
• Remove “-ate” and add “-ic acid”
Formulas
• Combine hydrogen with the corresponding polyatomic ion
3. Acids
b) Oxyacids
Original Polyatomic Ion
Acid Name
Nitrate
Nitric Acid
Chlorate
Chloric Acid
Sulfate
Sulfuric Acid
Carbonate
Carbonic Acid
Phosphate
Phosphoric Acid
Acetate
Acetic acid
Chromate
Chromic Acid
Dichromate
Dichromic Acid
Acid Formula
3. Acids
b) Oxyacids
Original Polyatomic Ion
Acid Name
Acid Formula
Nitrate
Nitric Acid
HNO3 (aq)
Chlorate
Chloric Acid
Sulfate
Sulfuric Acid
Carbonate
Carbonic Acid
Phosphate
Phosphoric Acid
Acetate
Acetic acid
Chromate
Chromic Acid
Dichromate
Dichromic Acid
3. Acids
b) Oxyacids
Original Polyatomic Ion
Acid Name
Acid Formula
Nitrate
Nitric Acid
HNO3 (aq)
Chlorate
Chloric Acid
HClO3 (aq)
Sulfate
Sulfuric Acid
Carbonate
Carbonic Acid
Phosphate
Phosphoric Acid
Acetate
Acetic acid
Chromate
Chromic Acid
Dichromate
Dichromic Acid
3. Acids
b) Oxyacids
Original Polyatomic Ion
Acid Name
Acid Formula
Nitrate
Nitric Acid
HNO3 (aq)
Chlorate
Chloric Acid
HClO3 (aq)
Sulfate
Sulfuric Acid
H2SO4 (aq)
Carbonate
Carbonic Acid
H2CO3 (aq)
Phosphate
Phosphoric Acid
H3PO4 (aq)
Acetate
Acetic acid
CH3COOH (aq)
Chromate
Chromic Acid
H2CrO4 (aq)
Dichromate
Dichromic Acid
H2Cr2O7 (aq)
3. Acids
c) Derivatives of Oxyacids
• Many of the oxyacids have various forms, or derivatives
Naming
• Similar to derivatives of polyatomic ions and “ous/ic” system
▫
▫
▫
▫
Start with original acid ( - ic acid)
Add prefix “per-” if there is 1 MORE oxygen
Change suffix “-ic” to “-ous” if there is 1 LESS oxygen
Add prefix “hypo-” and change suffix “ic” to “-ous” if there are 2 LESS oxygen
Formulas
• Use prefixes and suffixes to determine the correct number of oxygen atoms
3. ACIDS
Practice
Chloric Acid
HClO3 (aq)
Nitrous Acid
Percarbonic Acid
H3PO2
H2CO
3. ACIDS
Practice
Perchloric acid
HClO4 (aq)
Chloric Acid
HClO3 (aq)
Nitrous Acid
Percarbonic Acid
H3PO2
H2CO
3. ACIDS
Practice
Perchloric acid
HClO4 (aq)
Chloric Acid
HClO3 (aq)
Chlorous acid
HClO2 (aq)
Nitrous Acid
Percarbonic Acid
H3PO2
H2CO
3. ACIDS
Practice
Perchloric acid
HClO4 (aq)
Chloric Acid
HClO3 (aq)
Chlorous acid
HClO2 (aq)
Hypochlorous acid
HClO (aq)
Nitrous Acid
Percarbonic Acid
H3PO2
H2CO
3. ACIDS
Practice
Perchloric acid
HClO4 (aq)
Chloric Acid
HClO3 (aq)
Chlorous acid
HClO2 (aq)
Hypochlorous acid
HClO (aq)
Nitrous Acid
HNO2(aq)
Percarbonic Acid
H3PO2 (aq)
H2CO (aq)
3. ACIDS
Practice
Perchloric acid
HClO4 (aq)
Chloric Acid
HClO3 (aq)
Chlorous acid
HClO2 (aq)
Hypochlorous acid
HClO (aq)
Nitrous Acid
HNO2 (aq)
Percarbonic Acid
H2CO4 (aq)
H3PO2 (aq)
H2CO (aq)
3. ACIDS
Practice
Perchloric acid
HClO4 (aq)
Chloric Acid
HClO3 (aq)
Chlorous acid
HClO2 (aq)
Hypochlorous acid
HClO (aq)
Nitrous Acid
HNO2 (aq)
Percarbonic Acid
H2CO4 (aq)
Hypophosphorous acid
H3PO2 (aq)
H2CO (aq)
3. ACIDS
Practice
Perchloric acid
HClO4(aq)
Chloric Acid
HClO3(aq)
Chlorous acid
HClO2 (aq)
Hypochlorous acid
HClO (aq)
Nitrous Acid
HNO2 (aq)
Percarbonic Acid
H2CO4 (aq)
Hypophosphorous acid
H3PO2 (aq)
Hypocarbonous acid
H2CO (aq)
3. Acids
d) Acid Salts
• Formed when only some of the hydrogen atoms in an acid are
replaced by a metal
Naming
• If 1 hydrogen replaced – use hydrogen or bi
• If more than 1 hydrogen replaced – use a prefix to indicate the
number of hydrogen atoms that are present
Formulas
• Will see hydrogen in the middle of the name – this is a part of a
polyatomic ion (see chart)
• Use criss-cross
3. ACIDS
Practice
Sodium hydrogen carbonate
(OR sodium bicarbonate)
Calcium dihydrogen phosphate
Potassium biphosphate
LiHSO3
Ba(HSO4)2
3. ACIDS
Practice
Sodium hydrogen carbonate
(OR sodium bicarbonate)
NaHCO3
Calcium dihydrogen phosphate
Potassium biphosphate
LiHSO3
Ba(HSO4)2
3. ACIDS
Practice
Sodium hydrogen carbonate
(OR sodium bicarbonate)
NaHCO3
Calcium dihydrogen phosphate
Ca(H2PO4)2
Potassium biphosphate
LiHSO3
Ba(HSO4)2
3. ACIDS
Practice
Sodium hydrogen carbonate
(OR sodium bicarbonate)
NaHCO3
Calcium dihydrogen phosphate
Ca(H2PO4)2
Potassium biphosphate
K2HPO4
LiHSO3
Ba(HSO4)2
3. ACIDS
Practice
Sodium hydrogen carbonate
(OR sodium bicarbonate)
NaHCO3
Calcium dihydrogen phosphate
Ca(H2PO4)2
Potassium biphosphate
K2HPO4
Lithium hydrogen sulfite (OR lithium bisulfite)
LiHSO3
Ba(HSO4)2
3. ACIDS
Practice
Sodium hydrogen carbonate
(OR sodium bicarbonate)
NaHCO3
Calcium dihydrogen phosphate
Ca(H2PO4)2
Potassium biphosphate
K2HPO4
Lithium hydrogen sulfite (OR lithium bisulfite)
LiHSO3
Barium hydrogen sulfate (OR barium bisulfate)
Ba(HSO4)2
4. Hydrates
• Not all substances are “dry” – many have traces of water in them
• Even if we try to evaporate certain substances, some of the water
remains
Naming
• Name the compound normally, followed by _______hydrate (use the
appropriate prefix for the number of water molecules)
Formulas
• Write the formula for the compound first, followed by a dot and the
number of water molecules present
4. HYDRATES
Practice
Copper (II) sulfate pentahydrate
Barium hydroxide octahydrate
CoCl2  6 H2O
Na3PO3 2 H2O
4. HYDRATES
Practice
Copper (II) sulfate pentahydrate
CuSO4  5 H2O
Barium hydroxide octahydrate
CoCl2  6 H2O
Na3PO3 2 H2O
4. HYDRATES
Practice
Copper (II) sulfate pentahydrate
CuSO4  5 H2O
Barium hydroxide octahydrate
Ba(OH)2  8 H2O
CoCl2  6 H2O
Na3PO3 2 H2O
4. HYDRATES
Practice
Copper (II) sulfate pentahydrate
CuSO4  5 H2O
Barium hydroxide octahydrate
Ba(OH)2  8 H2O
Cobalt (II) chloride hexahydrate
CoCl2  6 H2O
Na3PO3 2 H2O
4. HYDRATES
Practice
Copper (II) sulfate pentahydrate
CuSO4  5 H2O
Barium hydroxide octahydrate
Ba(OH)2  8 H2O
Cobalt (II) chloride hexahydrate
CoCl2  6 H2O
Sodium phosphite dihydrate
Na3PO3 2 H2O
5. PEROXIDES
Peroxides:
• These are binary oxides, which contain an extra oxygen atom.
Rule:
• Write the formula as if the regular oxide
CaO
• Add on one extra oxygen atom
H2O2
CaO2
Na2O
Na2O2
Do not at this stage cancel any of the subscripts.
H2O
5. PEROXIDES
Practice
• zinc peroxide
• calcium peroxide
• cesium peroxide
• copper(II) peroxide
• magnesium peroxide
• potassium peroxide
• strontium peroxide
• hydrogen peroxide
• barium peroxide
• aluminum peroxide
____________________
____________________
____________________
____________________
____________________
____________________
____________________
____________________
____________________
____________________
6. THIO COMPOUNDS
Thio Compounds
• The prefix thio in the name indicates that an oxygen atom has been
replaced by a sulphur atom.
Examples:
• potassium sulphate
• sodium carbonate
• potassium cyanate
K2SO4
Na2CO3
KCNO
potassium thiosulphate
sodium thiocarbonate
potassium thiocyanate
K2S2O3
Na2SCO2
KSCN
6. THIO COMPOUNDS
Practice
• ammonium thiocyanate ___________________
• potassium thiosulfate ___________________
• sodium monohydrogenthiosulphate ___________
• aluminum thiocarbonate __________________
• CaS2O2
• AlSPO3
_________________________
_________________________
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