1
SCH 4U Nomenclature Independent Study
An excellent knowledge of Chemical Nomenclature is essential for success in grade 12 Chemistry. For your first
independent study you will review the nomenclature you learned in grade 11 and write a test.
Nomenclature Test Date:___________________________________________
Valence Value
The valence value of an element is defined as the numbers of electrons an atom of that element will
gain/lose/share when forming a compound.
Cross-Over Rule for Writing Formulas
STEPS
1. Write down the symbols of
the elements in the order given
in the name.
2. Write the valences above the
elements symbol.
3. Divide the valences by the
highest common multiple.
4. Cross-over valences
5. Drop all 1’s and unnecessary
brackets
sodium
chloride
magnesium
oxide
calcium
fluoride
lithium
sulphate
aluminum
phosphate
Na Cl
Mg O
Ca F
Li SO4
Al PO4
1 1
Na Cl
1 1
Na Cl
Na1Cl1
NaCl
2 2
Mg O
1 1
Mg O
Mg1O1
MgO
2 1
Ca F
2 1
Ca F
Ca1F2
CaF2
1 2
Li SO4
1 2
Li SO4
Li2(SO4)1
Li2SO4
3 3
Al PO4
1 1
Al PO4
Al1(PO4)1
AlPO4
Notes:
a) You should be able to do all 5 steps in your head when you are finished the unit.
b) When naming compounds, the least electronegative element is usually written first.
c) Groups of elements such as SO42- and PO43- are referred to as radicals or polyatomic ions. These
radicals behave as if they were a single entity and follow the cross over rule in the same manner as
other single elements. Brackets are used in the formula only if there are 2 or more of the radical
indicated in the formula.
Binary Ionic Compounds
A binary compound contains 2 elements only.
Rules for Binary Ionic Compounds:
a) The name of the binary compound always ends in "ide".
b) The first mentioned element may have more than one valence and if it does this must be indicated in the
name.
c) Elements have a valence value determined by their group on the Periodic table unless indicated by the
name.
I
2
3
4
3
2
1
0
2
A) Binary Compounds where the first element has 1 valence only
Use rule “c” and the cross-over rule.
Examples:
sodium oxide Na2O
Exercise:
calcium sulfide CaS
magnesium bromide MgBr2
For all exercises you will give the name if formula provided and the formula if the name is provided.
calcium nitride
________
silver sulphide
________
barium iodide
________
silicon oxide
________
zinc silicide
________
magnesium chloride
________
aluminum carbide
________
sodium fluoride
________
barium carbide
________
aluminum bromide
________
potassium bromide
________
cesium phosphide
________
LiCl
_____________________________
K2S
_____________________________
BaO
_____________________________
Al2O3
_____________________________
B) Binary Compounds with Multivalent Elements
Many transition metals and some other elements have multiple valence values and therefore can form multiple
compounds with the same non-metal. Due to this it is necessary to indicate the valence of the metal in the name of the
compound using either the Stock (IUPAC or Roman Numeral) or Classical (“ous” and “ic”) method. The second element
(non-metal) always has a valence equal to the value as determined from its group in the periodic table.
Method 1: Stock/IUPAC/Roman Numeral Method
This is the currently preferred method as the valence of the first is indicated using the corresponding Roman Numeral in
brackets following the name of the first element.
Examples:
iron(III) chloride
FeCl3
tin(IV) iodide
SnI4
phosphorus (III) oxide
As2O3
mercury(II) oxide
HgO
Exercise:
For all exercises you will give the name if formula provided and the formula if the name is provided.
iron(III) chloride
___________
arsenic(V) iodide
___________
tin(IV) oxide
___________
gold(I) telluride
___________
phosphorus(V) chloride ___________
sulphur(VI) oxide
___________
copper(I) bromide
___________
bismuth(v) phosphide ___________
antimony(V) sulphide
___________
mercury(II) chloride
___________
arsenic(III) oxide
___________
gold(III) chloride
___________
mercury(I) sulphide
___________
copper(II)sulphide
___________
Pb3N2
______________________________
SbF3
__________________________________
NiI2
______________________________
MnO2
Co2Se3
______________________________
BiF5
__________________________________
SnO2
______________________________
ZnO
_________________________________
_________________________________
3
Method 2: Classical/"ous' and "ic" Method
This method can be used when the multivalent element has 2 possible valences. The name of the element ending with
"ous" denotes the lower valence value and the name of the element ending with an "ic" denotes the higher valence
values. In some cases, the Latin name for the element is used.
iron:
gold:
copper:
tin:
lead:
cobalt
nickel
mercury
platinum
ferrous
aurous
cuprous
stannous
plumbous
cobaltous
nickelous
mercurous
platinous
(valence = 2)
(valence = 1)
(valence = 1)
(valence = 2)
(valence = 2)
(valence = 2)
(valence = 2)
(valence = 1)
(valence = 2)
and
and
and
and
and
and
and
and
and
ferric
auric
cupric
stannic
plumbic
cobaltic
nickelic
mercuric
platinic
(valence = 3)
(valence = 3)
(valence = 2)
(valence = 4)
(valence = 4)
(valence = 3)
(valence = 3)
(valence = 2)
(valence = 4)
*Some elements having more than two valence values or oxidation states use specific values for the "ous" and the "ic".
nitrogen
manganese
arsenic
ous = 1 ic = 2
ous = 2 ic = 3
ous = 3 ic = 5
chromium
phosphorus
bismuth
ous = 2 ic = 3
ous = 3 ic = 5
ous = 3 ic = 5
Examples:
stannous chloride
arsenic phosphide
SnCl2
As3P5
phosphorous oxide
nitric oxide
P2O3
NO
Exercise:
For all exercises you will give the name if formula provided and the formula if the name is provided.
ferric oxide
_______________
auric iodide
_______________
phosphoric sulfide
_______________
nitrous phoshpide
_______________
cuprous fluoride
_______________
stannic oxide
_______________
stannic fluoride
_______________
arsenious nitride
_______________
antimonous sulfide
_______________
mercuric fluoride
_______________
arsenious bromide
_______________
cuprous nitride
_______________
nickelic iodide
_______________
auric chloride
_______________
chromous oxide
_______________
cupric sulfide
_______________
NiI2
__________________________
Sb2S5
_________________________
HgBr
__________________________
As4C5
_________________________
CoCl3
__________________________
Au2S
_________________________
As3N5
__________________________
PAs
_________________________
Fe2C
__________________________
NiP
_________________________
PbS
__________________________
CoF3
_________________________
CuO
__________________________
Au2Se3
_________________________
4
Formula of Elements
Most elements are written as single entities.
Example:
iron Fe(S)
copper Cu(S)
The exceptions to this rule are:
a) the diatomic gases: H O F B I N Cl
hydrogen H2(g)
oxygen O2(g)
nitrogen N2(g)
chlorine Cl2(g)
b) two other non-metals:
helium He(g)
fluorine F2(g)
bromine Br2(l)
sulphur S8(s)
iodine
I2(s)
phosphorus P4(s)
** The exceptions must be memorized! **
Common Radicals or Polyatomic Ions
Radicals or polyatomic ions are groups of atoms that are treated as a single entity when writing formulas and names.
The following list of common radicals (polyatomic ions) must be memorized along with their valences. Positive
polyatomic ions replace metals in an ionic compound and a negatively charged polyatomic ion goes in place of the nonmetal. If more than 1 of the radical is required in the chemical formula, brackets are placed around the radical’s
formula with the subscript outside the bracket.
Radical name
Formula
Valence
Radical name
Formula
Valence
1
hydroxide
OH
1
ammonium
NH4+
cyanide
1
manganate
MnO3-
1
chromate
CNCrO22-
2
dichromate
Cr2O72-
2
cyanate
CNO-
1
thiocyanate
SCN-
1
carbonate
CO32-
2
nitrate
NO3-
1
phosphate
PO43-
3
sulfate
SO42-
2
fluorate
FO3-
chlorate
ClO3-
1
-
Examples:
sodium hydroxide
lithium cyanide
sodium dichromate
NaOH
LiCN
Na2Cr2O7
1
potassium chromate
ammonium hydroxide
magnesium permanganate
K2CrO4
NH4OH
Mg(MnO4)2
Exercise:
For all exercises you will give the name if formula provided and the formula if the name is provided.
potassium hydroxide
__________________
cobalt(II) cyanate
__________________
iron(III) cyanate
__________________
zinc hydroxide
__________________
barium hydroxide
__________________
gallium dichromate
__________________
ammonium chloride
__________________
potassium chromate
__________________
copper(II) chromate
__________________
Sn(CN)4 _______________________________
ammonium dichromate __________________
Al(OH)3 _______________________________
ammonium bromate
__________________
KMnO4 _______________________________
ferrous hydroxide
__________________
CsCN
________________________________
nickel(III) cyanide
__________________
XeF6
________________________________
auric bromide
__________________
Ca(SCN)2 ______________________________
5
Acids
There are three groups of acids:
- binary acids
- oxy acids
- derived oxy acids
1. Binary Acids
This is a very small but common group of acids. The following rules apply to all of the members.
1. All have the prefix “hydro” and end with “ic”.
2. All must contain hydrogen as the first element.
3. Use the normal cross-over-rule to determine the formula.
4. All are dissociated in water and must be so indicated by using (aq) behind the formula.
5. Have no oxygen in their formula
Examples:
hydrochloric acid
HCl(aq)
hydrosulfuric acid
H2S(aq)
hydrocyanic acid
HCN(aq)
Exercise:
For all exercises you will give the name if formula provided and the formula if the name is provided.
hydrobromic acid
________
hydrotelluric acid
________
hydrofluoric acid
________
hydroiodic acid
________
hydroselenic acid
________
hydrosulfuric acid
________
hydrochloric acid
________
hydrophosphoric acid
________
2. Oxy Acids
This is a larger group of acids. They are alike in that they all contain H, O and at least one other non-metal element. All
members of this group of acids follow the rules below.
1. The name of the acid ends in “ic”.
2. The name of the associated radical ends in “ate”.
3. The valence value of the associated radical is equal to the number of acidic hydrogens in the acid.
The following 6 oxy acids and their associated radicals along with their valences must be memorized.
Name of the Acid
Formula of the Acid
Name of the
Formula of the
valence value for the
associated radical
associated radical
associated radical
chromate
C2H3O2-
1
1
acetic acid
HC2H3O2
nitric acid
HNO3
nitrate
NO3-
fluoric acid
HFO3
fluorate
FO3-
1
carbonic acid
H2CO3
carbonate
CO32-
2
2
3
sulfuric acid
H2SO4
sulfate
SO42-
phosphoric acid
H3PO4
phosphate
PO43-
NOTE:
Using the periodic table it is possible to write the names and formulas for a number of other oxy acids using the fact
that members of the same chemical family have similar chemical properties. Elements of the same chemical family
(group) follow the pattern of the oxy acid immediately above the oxy acid that has been memorized.
Example:
memorized acid: fluoric acid = HFO3
therefore: chloric acid = HClO3
iodic acid = HIO3
bromic acid = HBrO3
If hydrogens are joined with the radicals learned earlier a few more acids can be formed.
chromate = CrO42chromic acid = H2CrO4
cyanate = CNOcyanic acid = HCNO
6
Exercise:
On a separate piece of paper complete the following chart for the acids listed.
Name of the acid
bromic acid
manganic acid
Formula of the acid
telluric acid
selenic acid
Name of the
Formula of the
Valence value of the
associated radical
associated radical
associated radical
iodic acid
cyanic acid
silicic acid
arsenic acid
dichromic acid
chromic acid
3. Derived Oxy Acids
Theses acids are all derived from the parent oxy acids which you are to memorize. The table below shows the rule to
determine the derived oxy acids from the parent acid. When adding or removing oxygen atoms from the parent acid,
the number of hydrogens on the acid and the valence of the associated radical remains the same as the parent.
Parent Oxy Acid + 1 O
Parent Oxy Acid
Parent Oxy Acid - 1 O
Parent Oxy Acid - 2 O
Type of Acid
per______ic
ic
ous
hypo_____ous
Associated Radical
per______ate
ate
ite
hypo_____ite
Example
perchloric acid HClO4
perchlorate ion ClO4chloric acid HClO3
chlorate ion ClO3chlorous acid HClO2
chlorite ion ClO2hypochlorous acid HClO
hypochlorite ion ClO-
Exercise:
On a separate piece of paper complete the following chart for the acids listed.
Name of the acid
Formula of the acid
phosphoric acid
phosphorous acid
hypophosphorous acid
sulfuric acid
sulfurous acid
nitric acid
nitrous acid
Name of the
Formula of the
Valence value of the
associated radical
associated radical
associated radical
perbromic acid
bromic acid
bromous acid
hypobromous acid
iodic acid
iodous acid
hypoiodous acid
selenic acid
selenous acid
telluric acid
tellurous acid
manganic acid
permanganic acid
Salts
The word, salt, is the general term given to a class of compounds which can be formed when an acid and a base
neutralize each other. According to this definition then, most of the compounds we dealt with in the section on binary
compounds could be considered to be salts formed from a base and a binary acid. In the same manner, we can get salts
formed from a base and an oxy acid or derived oxy acid.
Examples:
sodium sulphate
aluminum carbonate
cupric nitrite
Na2SO4
Al2(CO3)3
Cu(NO2)2
calcium phosphate
zinc perchlorate
stannous hypoiodite
Ca3(PO4)2
Zn(ClO4)2
Sn(IO)2
7
Salts from oxy acids
potassium chlorate____________________
sodium carbonate
__________________
sodium nitrate
ferric sulfate
__________________
iron(III) acetate ____________________
gold(I) phosphate
__________________
aluminum silicate ____________________
magnesium chlorate
_________________________
magnesium phosphate __________________
ammonium nitrate
_________________________
aurous sulfate
K2CO3
_______________________________
ammonium chlorate ____________________
Na3PO4
_______________________________
zinc nitrate
Fe(ClO3)2
_______________________________
potassium acetate _____________________
Al(C2H3O2)3
_______________________________
lithium chromate ______________________
Zn3(PO4)2
_______________________________
____________________
____________________
________________________
Salts from Derived Oxy Acids
aluminum sulfite
__________________
copper(I) permanganate ____________________
cobalt(III) chlorite
__________________
ammonium hypophosphite __________________
tin(IV) hypochlorite
__________________
mercuric perchlorate
_____________________
sodium phosphite
__________________
magnesium sulfite
_____________________
aluminum nitrite
__________________
cuprous chlorite
_____________________
cobalt(II) hypophosphite__________________
ammonium hypoiodite _____________________
stannic perchlorate
__________________
gold(III) chromate
sodium sulphite
__________________
Ga(BrO4)3
___________________________
aluminum chlorite
__________________
Pt(ClO)4
___________________________
nickel(III) hypochlorite __________________
Ag2O
___________________________
tin(IV) phosphite
NH4CNO
___________________________
__________________
_____________________
Acid Radicals and Acid Salts
1. Acid Radicals
In certain circumstances the oxy acids with multiple acidic hydrogens are able to lose the hydrogens one at a time. This
results in radicals with acidic hydrogens still attached which are referred to as acid radicals.
Step 1: H3PO4  H+ + H2PO4Step 2: H2PO4-  H+ + HPO42- Step 3: HPO42-  H+ + PO43Radical
PO43HPO42H2PO4-
Name
phosphate
monohydrogenphosphate
dihydrogenphosphate
Valence
3
2
1
Notes:
a) Valence = # of hydrogen removed from the acid OR valence of non-acid radical-# of H’s still attached
b) Mono may be left off a monohydrogen acid radical
c) For oxy acids with 2 acidic hydrogens (diprotic acids), the prefix “bi” may be used in place of monohydrogen (eg.
HCO3- = bicarbonate or monohydrogen carbonate)
8
For the following give the formula and valence value of the radicals listed:
phosphite
___________
_____
monohydrogensulphate
___________
_____
monohydrogenphosphite
___________
_____
suphite
___________
_____
dihydrogenphosphite
___________
_____
monohydrogensulphite
___________
_____
hypophosphite
___________
_____
carbonate
___________
_____
monohydrogenhypophosphite ___________
_____
monohydrogencarbonate
___________
_____
dihydrogenhypophosphite
___________
_____
chromate
___________
_____
sulphate
___________
_____
monohydrogechromate
___________
_____
2. Acid Salts
The acid radicals are treated just like any other radical.
Examples:
calcium dihydrogenhypophosphite
Ca(H2PO2)2
potassium monohydrogen carbonate KHCO3
aluminum bisulphite
sodium hydrogensulfate
Al(HSO3)3
NaHSO4
Exercise:
For all exercises you will give the name if formula provided and the formula if the name is provided.
sodium monohydrogenphosphate _____________
ferric monohydrogensulphate _______________
magnesium dihydrogenphosphate _____________
ammonium hydrogencarbonate ______________
aluminum dihydrogenphosphite _____________
chromium(III) hydrogensulphite ______________
chromium(III) hydrogenphosphite _____________
nickel(II) monohydrogensilicate ______________
cupric monohydrogenarsenate ______________
cadmium monohydrogenselenate ___________
stannic dihydrogenhypophosphite ____________
potassium monohydrogenselenite ___________
K2HPO3 ___________________________
Bi2(HPO3)5
__________________________
Ba(HSO3)2
Pb(H 2PO2)2
__________________________
___________________________
Hydrates
Hydrates are crystals containing a given number of water molecules within their structure. When naming a hydrate
Greek prefixes in front of the word hydrate are used to indicate the number of water molecules into the crystal. In the
chemical formula the number of water molecules is separated from the formula of the compound by a dot “∙”
Examples:
copper(II) sulfate pentahydrate
CuSO4 ∙ 5H2O
chlorine octahydrate
Cl2 ∙ 8H2O
Exercise:
For all exercises you will give the name if formula provided and the formula if the name is provided.
calcium sulfate dihydrate
__________
chromium(III) nitrate nonahydrate
__________
magnesium sulfite heptahydrate
__________
cobalt(II) perchlorate pentahydrate
__________
sodium carbonate decahydrate
__________
barium chloride dihydrate
__________
aluminum oxide monohydrate
__________
aluminum nitrate monohydrate
__________
ferric chloride hexahydrate
__________
bromine decahydrate
__________
calcium nitrate trihydrate
__________
odine tetrahydrate
__________
cadmium bromide tetrahydrate
__________
copper(II) bromate hexahydrate
__________
9
Peroxides
These are binary oxides, which contain an extra oxygen atom.
Rules:
1. Write the formula of the regular oxide.
2. Add on one extra oxygen atom.
3. Do not at this stage cancel any of the subscripts.
Na2O
Na2O2
H2O
H2O2
CaO
CaO2
Exercise:
For all exercises you will give the name if formula provided and the formula if the name is provided.
zinc peroxide
____________________
potassium peroxide
____________________
calcium peroxide
____________________
strontium peroxide
____________________
cesium peroxide
____________________
hydrogen peroxide
____________________
copper(II) peroxide
____________________
barium peroxide
____________________
magnesium peroxide
____________________
aluminum peroxide
____________________
Thio Compounds
The prefix “thio” in the name indicates that an oxygen atom has been replaced by a sulphur atom.
Examples:
potassium sulphate
K2SO4
potassium thiosulphate
K2S2O3
sodium carbonate
Na2CO3
sodium thiocarbonate
Na2SCO2
potassium cyanate
KCNO
potassium thiocyanate
KSCN
Exercise:
For all exercises you will give the name if formula provided and the formula if the name is provided.
ammonium thiocyanate _____________________
potassium thiosulfate ______________________
sodium monohydrogenthiosulphate ___________
aluminum thiocarbonate _____________________
CaS2O2
AlSPO3
______________________________
_____________________________
Molecular Compounds
These compounds contain 2 non-metals and are named using Greek prefixes. This method does not use the valence
values. The Greek prefix is placed in front of the element name to indicate how many atoms of the element to place in
the formula. If there is only 1 atom of the first element, mono is not used on the name of the first element.
Prefixes
1 = mono 2 = di
3 = tri
4 = tetra
5 = penta 6 = hexa
7 = hepta 8 = octa
9 = nona
10 = deca
Examples:
diphosphorus pentoxide
P2O5
arsenic trichloride
AsCl3
carbon monoxide
CO
xenon tetrafluoride
XeF4
Exercise:
For all exercises you will give the name if formula provided and the formula if the name is provided.
xenon hexafluoride
_________________
silicon dioxide
_________________
sulfur dioxide
_________________
carbon tetrachloride
_________________
sulphur trioxide
_________________
lead dioxide
_________________
carbon dioxide
_________________
manganese dioxide
_________________
carbon disulphide
_________________
nitrogen dioxide
_________________
nitrogen tetroxide
_________________
diphosphorus trisulfide _________________
10
carbon tetrachloride
_________________
ICl
_______________________________
lead dioxide
_________________
SeCl2
_______________________________
dichlorine monoxide
_________________
ICl7
_______________________________
___________
NF3
_______________________________
_______________________________
P2S5
_______________________________
diphosphorus pentasulphide
KrF2
PRACTICE, PRACTICE, PRACTICE
sulphur
___________________
lead (IV) nitride
___________________
plumbous peroxide
___________________
cupric chloride
___________________
calcium iodite
___________________
stannous iodide
___________________
sulfur dioxide
___________________
aluminum nitride
___________________
boron hypoarsenite
___________________
antimonous bromide
___________________
neon
___________________
tin (IV) sulfide
___________________
platinum (IV) thiocarbonite
___________________
silver oxide
___________________
calcium cyanide heptahydrate ___________________
calcium phosphide
___________________
cuprous permanganate
___________________
iron (II) sulfide
___________________
chromous acid
___________________
arsenic phosphide
___________________
cyanic acid
___________________
mercury (II) nitride
___________________
iodine monochloride
___________________
tin (IV) fluoride
___________________
stannic dihydrogen hypophosphite ________________
sodium hydride
___________________
auric peroxide
___________________
sodium monohydrogen phosphate _________________
ammonium selenide
___________________
barium hydroxide
___________________
titanium
___________________
sodium bicarbonate
___________________
ferrous thiosilicate
___________________
perchloric acid
___________________
cadmium bisulphate
___________________
nitrous acid
___________________
lithium phosphide
___________________
calcium peroxide
___________________
bromine
___________________
plumbous oxide
___________________
potassium oxide
___________________
potassium chloride
___________________
barium sulfide
___________________
hydrogen iodide
___________________
magnesium fluoride
___________________
antimonous phosphide
___________________
mercurous bromide
___________________
silver sulfide
___________________
zinc hydride
___________________
mercuric oxide
___________________
ferric sulfide
___________________
phosphorus (III) chloride
___________________
arsenic (V) oxide
___________________
ferrous oxide
___________________
11
magnesium peroxide
___________________
silver hypoarsenite
___________________
zinc chromate dehydrate
___________________
copper (II) sulphate pentahydrate _________________
phosphoric acid
___________________
cyanic acid
___________________
chromic cyanide
___________________
sulfur dioxide
___________________
sodium thiosulfate hexahydrate ___________________
potassium permanganate
___________________
iron (III) carbonate
___________________
zinc chloride
___________________
magnesium phosphide
___________________
diarsenic pentasulfide
___________________
fluorine
___________________
hypophosphorous acid
___________________
chlorous acid
___________________
potassium hydroxide
___________________
dicarbon tetrahydride
___________________
iron (III) cyanate
___________________
hydrosulfuric acid
___________________
barium chromate
___________________
stannous tungstenate
___________________
ammonium thiocyanate
___________________
magnesium peroxide
___________________
potassium dichromate
___________________
ammonium hydrogenhypophosphite _______________
mercuric tellurite
___________________
tetracarbon decahydride
___________________
platinum (IV) silicate
___________________
nickelic perbromate
___________________
cobaltous thioselenite
___________________
chlorine dihydrate
___________________
tricarbon octahydride
___________________
copper (II) hypoarsenite
___________________
thiocyanic acid
___________________
dichromic acid
___________________
silver hypophosphite
___________________
aurous hydroxide
___________________
bromine
___________________
barium bithiocarbonate
___________________
silicon tetrahydride
___________________
hydrogen chloride
___________________
cesium arsenite dehydrate
___________________
sulfuric acid
___________________
manganic hydroxide
___________________
chromous cyanate
___________________
arsenious oxide
___________________
magnesium thiophosphate
___________________
silver chlorate
___________________
ferrous iodide
___________________
calcium perbromate
___________________
barium dichromate
___________________
barium phosphide
___________________
phosphorus
___________________
nickel (II) cyanide
___________________
periodic acid
___________________
beryllium phosphate
___________________
tetraphosphorus decaoxide
___________________
cadmium sulfite
___________________
hydrotelluric acid
___________________
boron tribromide
___________________
ammonium bitungstenate
___________________
silicon carbide
___________________
iron (III) peroxide
___________________
mercuric hydroxide
___________________
neon
___________________
cupric perchlorate
___________________
12
gold (III) selenate
___________________
cupric acetate
___________________
stannic phosphide
___________________
acetic acid
___________________
arsenic (V) oxide
___________________
ammonium phosphate dehydrate _________________
sulfur trioxide
___________________
aurous chromate
___________________
hydrogen cyanide
___________________
ferrous hydroxide
___________________
lithium hypoiodite
___________________
stannic bromide
___________________
magnesium thiosilicate
___________________
plumbous thiocyanate
___________________
zinc phosphide
___________________
oxygen
___________________
aluminum peroxide
___________________
arsenic trihydride
___________________
lithium sulfate
___________________
ammonium dihydrogenphosphate _________________
magnesium hypochlorite
___________________
phosphorus pentachloride
___________________
manganese dioxide
___________________
silver nitrate
___________________
strontium nitrate
___________________
calcium chlorite
___________________
lead (IV) iodite
___________________
manganese (III) dichromate
___________________
zirconium chloride
___________________
potassium permanganate
___________________
cobalt (III) hypobromite
___________________
silicon dioxide
___________________
chromium (III) oxide
___________________
palladium (IV) nitrite
___________________
iodine monofluoride
___________________
diboron hexahydride
___________________
ammonium perbromate
___________________
sulfur
___________________
carbon disulphide
___________________
helium
___________________
aluminum hydroxide
___________________
uranium hexafluoride
___________________
beryllium sulfite
___________________
antimonic sulfate
___________________
lead (II) dihydrogenphosphite
___________________
phosphorus pentachloride
___________________
chromic hydrogenhypophosphite __________________
sulfur hexafluoride
___________________
iron (III) dihydrogenhypophosphite ________________
tin (II) cyanide
___________________
potassium hydrogenarsenite
___________________
phosphorus
___________________
mercury (II) bisulfate
___________________
chlorine
___________________
zinc monohydrogentellurite
___________________
cesium manganite
___________________
sodium bicarbonate
___________________
ammonium chromite
___________________
cobalt (III) bromite
___________________
calcium tungstenate
___________________
aluminum hydride
___________________
silver acetate hexahydrate
___________________
vanadium (V) oxide
___________________
potassium peroxide
___________________
carbon tetraiodide
___________________
sodium thiocarbonate
___________________
mercurous peroxide
___________________
lithium dithiosulfite
___________________
13
PbS2O2
________________________________
HIO4 (aq)
________________________________
MgO2
________________________________
Ag2S
________________________________
Al2(SO2)3
________________________________
Fe(OH)2
________________________________
Au(MnO3)3
________________________________
N2O4
________________________________
BrCl5
________________________________
K2S2O
________________________________
Ba(FO)2
________________________________
HMnO4 (aq)
________________________________
ZnHAsO5
________________________________
H2SiO3 (aq)
________________________________
Co(NO3)3
________________________________
CaS2O2
________________________________
HgSCO
________________________________
N2O4
________________________________
H2S (aq)
________________________________
Au(IO4)3
________________________________
SrCl2∙8 H2O
________________________________
PbO3
________________________________
MnP
________________________________
Mg(MnO3)2
________________________________
Cr(H2PO3)3
________________________________
H2S (aq)
________________________________
K2O2
________________________________
Fe(H2PO3)3
________________________________
Al(ClO4)3
________________________________
PCl5
________________________________
Ga2(SiO3)3
________________________________
Rb2SSiO2
________________________________
P2S3
________________________________
Ra3P2 · 7 H2O
________________________________
HNO3 (aq)
________________________________
NH4OH
________________________________
FeCr2O7
________________________________
HCN (aq)
________________________________
CuSO4∙5H2O
________________________________
Ni3SPO2
________________________________
H2SeO3 (aq)
________________________________
HTeO2 (aq)
________________________________
CaCr2O7
________________________________
Cu2Se
________________________________
P2O5
________________________________
Ga(OH)3
________________________________
Cr(BrO)3
________________________________
B2H6
________________________________
MnO2
________________________________
BaF2
________________________________
Al2O4
________________________________
H2CrO3 (aq)
________________________________
HI (aq)
________________________________
Pb(ClO)2
________________________________
Au2(HAsO2)3 · 9 H2O _____________________________
H2Se(aq)
________________________________
SO3
________________________________
CaMoO4
________________________________
Li2SCO2
________________________________
C4H8
________________________________
Sr3N2 · 3 H2O
________________________________
ZnSeO2
________________________________
(NH4)2SiO2
________________________________
BaF2
________________________________
H2Te (aq)
________________________________
H2Te(aq)
________________________________
Cr(CNO)3
________________________________
Co2(HPO2)3∙4 H2O ______________________________
14
NaBr
________________________________
SnCl4
__________________________________________________
Ca(C2H3O2)2
________________________________
Cu2O
__________________________________________________
P2O5
________________________________
CuSO4
________________________________
Ti(SO4)2
________________________________
Ag2S
________________________________
FePO4
________________________________
CsI
________________________________
K3N
________________________________
Al2S3
________________________________
SO2
________________________________
Ni(NO3)2
________________________________
CuOH
________________________________
CoPO4
________________________________
Zn(NO2)2
________________________________
MnSO3
________________________________
V2S3
________________________________
Fe(ClO4)3
________________________________
NaOH
________________________________
GaCl3
________________________________
H2SO3
________________________________
Cr2O3
________________________________
H2S
________________________________
KNO2
________________________________
H3PO4
________________________________
Rb2CrO4
________________________________
NH3
________________________________
(NH4)2HPO4
________________________________
HCN
________________________________
Cs2CO3
________________________________
Ca(OH)2
________________________________
Li2HPO4
________________________________
Fe(OH)3
________________________________
Mg(HCO3)2
________________________________
H3P
________________________________
Ca(ClO3)2
________________________________
Na2CO3
________________________________
Sr(MnO4)2
________________________________
P2O5
________________________________
SCI3
________________________________
NH3
________________________________
Fe(C2H3O2)3
________________________________
FeSO4
________________________________
Ag2SO3
________________________________
SiO2
________________________________
Hg2Cl2
________________________________
GaCl3
________________________________
TiO2
________________________________
CoBr2
________________________________
(NH4)HSO4
________________________________
B2H4
________________________________
P2O5
________________________________
CO
________________________________
NO2
________________________________
P4
__________________________________________________
SO3
________________________________
NH4Cl
__________________________________________________
CCl4
________________________________
Al2O3
__________________________________________________
Ag2Cr2O7
________________________________
KBr
__________________________________________________
CuSiO2
________________________________
K2S
__________________________________________________
AsBr5
________________________________
SnI2
__________________________________________________
Sb3N5
________________________________