Chemical Nomenclature

Chemical
Nomenclature
I.) Binary Compounds With Fixed Charge Cation
a.) Nomenclature:
naming of chemical formulas
b.) Binary:
means t wo, in this case it means t wo elements
c.) Cation:
(+) positive ion, metal
d.) Anion:
(-) negative ion, non-metal
e.) Given Name, Write The Formula
Example:
Step 1: Write down the symbol and charge of the first word.
Step 2: Write down the symbol and charge of the second word.
Step 3: Use the minimum number of cations and anions need to
make the sum of all charges equal to zero. (criss-cross)
Step 1 Step 2
Step 3
Answer
Sodium Bromide
Na+
Br-
Na+
Br-
Criss Cross
The Charges..in
this case they
cancel out.
NaBr
Teacher Examples
Cesium Chloride
Radium Nitride
Barium Flouride
Student Problems
Problem:
Potassium Iodide
Magnesium Sulfide
Calcium Bromide
Silver Chloride
Sodium Oxide
Lithium Nitride
Step 1
Step 2
Step 3
Answer
Answers To Student Problems
Problem:
Potassium Iodide
Magnesium Sulfide
Calcium Bromide
Silver Chloride
Sodium Oxide
Lithium Nitride
Step 1
K+
I2
+
2
+
Mg
Ca
Step 2
Ag+
Na+
Li+
2
S
Step 3
K+
-
I2
Mg
2
Ca
Cl-
Ag+
O
N
-
3
-
+
Na+
Li+
KI
S
+
Br-
2
Answer
2
-
BrCl-
MgS
CaBr2
AgCl
O
2
-
3
-
N
Na2O
Li3N
Binary Compounds w/ Fixed Charge
Given The Formula, Write The Name
1) MgO
2) LiBr
3) Ca3N2
4) Al2S3
5) KI
6) SrCl2
7) Na2S
8) RaBr2
9) MgS
10) AlN
11) Cs2S
12) KCl
13) Sr3P2
14) BaI2
15) NaF
16) CaBr2
17) BeO
18) SrS
19) BF3
20) AlP
21) Rb2O
22) CaI2
23) Cs2O
24) MgI2
25) LiCl
26) BeBr2
27) Na2O
28) CaF2
29) BP
30) Al2O3
f.) Given Formula, Write The Name
Step 1: Separate formulas into individual ions.
Step 2: Find ions on ION CHARGE SHEET.
Step 3: Look at first element and name it.
Step 4: Look at second element. Use ROOT of its full name.
Step 5: Add “ide” to the root of the second element.
Step 6: Combine the t wo names to get the full name of the compound
Example:
H2S
Step 1
H+
S 2-
Step 4:
Sulfur = “SULF”
Step 2
H+ = hydrogen
S 2- = Sulfur
Step 5:
Sulf + ide
Step 3
H+ = HYDROGEN
Answer
Hydrogen Sulfide
Teacher Examples
Cs2S
Ra3P2
BaCl2
Student Problems
Problem:
CaS
MgI2
K2S
Be3N2
Na2O
Al2S3
Step 1
Step 2
Step 3
Step 4
Step 5
Answer
Answers To Student Problems
Problem Step 1
Step 2
CaS
Ca +S 2-
MgI2
Mg 2+ I -
K2S
+ 2K S
Be3N2
Be
Na2O
Na + O 2-
Al2S3
2
2
2
+
N
+
Ca = Calcium
S 2- = Sulfur
2
+
Mg = Magnesium
I - = Iodine
+
K 2-= Potassium
S = Sulfur
3
Al 3+ S2-
-
Step 3
2+
2
+= Beryllium
Step 4
Ca = Calcium
2
Step 5
Sulfur=SULF
SULF+ide
+
Mg = Magnesium Iodine=IOD IOD+ide
K+ = Potasium
2
+
Be = Beryllium
Nitrogen=NITR
Na+ = Sodium
O 2- =Oxygen
Na+= Sodium
Oxygen=OX
+= Aluminum
Al
S 2- = Sulfur
3
+
Al = Aluminum
Calcium Sulfide
Magnesium
Iodide
Sulfur=SULF SULF+ide Potassium
Sulfide
Be
N3- = Nitrogen
3
Answer
NITR+ide Beryllium
Nitride
OX+ide
Sulfur=SULF SULF+ide
Sodium
Oxide
Aluminum
Sulfide
Binary Compounds w/ Fixed Charge
Given The Name, Write The Formula
1) magnesium sulfide
2) potassium bromide
3) barium nitride
4) aluminum oxide
5) sodium iodide
6) strontium fluoride
7) lithium sulfide
8) radium chloride
9) calcium oxide
10) aluminum phosphide
11) potassium sulfide
12) lithium bromide
13) strontium phosphide
14) barium chloride
15) sodium bromide
16) magnesium fluoride
17) sodium oxide
18) strontium sulfide
19) boron nitride
20) aluminum nitride
21) cesium oxide
22) rubidium iodide
23) magnesium oxide
24) calcium bromide
25) lithium iodide
26) berylium bromide
27) potassium oxide
28) strontium iodide
29) boron fluoride
30) aluminum sulfide
II.) Binary Compounds With Variable Charged Cation
a.) Stock System:
use of roman numerals to show charge
b.) Common System:
use of suffix to show charge
c.) Variable Charged Cation:
d.) Anion:
(+) positive ion, metal
(-) negative ion, non-metal
e.) Given Name, Write The Formula-STOCK SYSTEM
Step 1: First word tells you the symbol of the cation (+ ion).
Step 2: Roman numerals inside () tell you the charge on the cation
Step 3: The anion symbol and charge comes from the second
name given.
Step 4: Make sure charges of symbols equal a net charge of zero.
..............(criss cross charges)
Example:
Step 1 Step 2
Step 3
Step 4
2+
Copper (II) chloride
Cu
(II) = 2+
chloride = Cl
Cu + Cl
Answer
CuCl2
Teacher Examples
Manganese (II) chloride
Iron (III) sulfide
Mercury (I) oxide
Student Problems
Problem:
Iron (III) iodide
Copper (II) sulfide
Mercury (I) bromide
Mercury (II) flouride
Gold (I) phosphide
Lead (IV) oxide
Step 1
Step 2
Step 3
Step 4
Answer
Answers To Student Problems
Problem:
Step 1
Step 2
Step 3
Step 4
++
Answer
-
Iron (III) iodide
Iron = Fe
(III)=3+
iodide = I-
Copper (II) sulfide
Copper = Cu
(II)=2+
sulfide = S2-
Cu 2++ S
Mercury (I) bromide
Mercury = Hg (I)=
bromide =Br-
Hg 2 + Br
Mercury (II) flouride
Mercury = Hg
2
2
(II)=2+
Gold (I) phosphide
+
flouride = F-
Fe
2
(I)=1+
phosphide = P 3-
Lead = Pb
(IV)=4+
oxide = O
2
-
I
2
FeI3
-
+
Hg2+ + F
Gold = Au
Lead (IV) oxide
3
Au
Pb
CuS
-
Hg2Br2
-
++
4
++
HgF2
P
3
-
O
2
Au3P
-
Pb2O4
Binary Compounds w/ Variable Charge: Stock System
Given The Name, Write The Formula
1) FeCl2
2) Cu2S
3) PbI4
4) SnF2
5) Hg2Br2
6) SnO
7) Cr2O3
8) AuI
9) Mn3N2
10) CoP
11) FeCl3
12) CuS
13) PbBr2
14) SnI4
15) HgF2
16) SnO2
17) MnCl3
18) Cr3N2
19) Au2O3
20) Co3P2
21) SnS
22) Hg2S
23) AuBr3
24) MnO
25) CrCl2
26) Pb3N4
27) Co2O3
28) CuI2
29) SnF4
30) Fe3P2
e.) Given Formula, Write The Name-STOCK SYSTEM
Step 1: Separate formulas into individual ions. (un criss-cross)
Step 2: Find ions on ION CHARGE SHEET.
Step 3: Look at first element and its charge...name it using () to show
the charge.
Step 4: Look at second element. Use ROOT of its full name.
Step 5: Add “ide” to the root of the second element.
Step 6: Combine the t wo names to get the full name of the compound
Example:
FeCl2
Step 1
Fe 2+ Cl -
Step 5
CHLOR + ide
Step 2
Fe 2+ = Iron
Cl
= Chlorine
Answer
Iron (II) chloride
Step 3
Fe2+= IRON (II)
Step 4
Chlorine = CHLOR
Teacher Examples
Au2S3
FeO
CrI3
Student Problems
Problem
CuCl2
CuF
Hg2Br2
Fe2S3
FeO
Sn3N2
Step 1
Step 2
Step 3
Step 4
Step 5
Answer
Answers To Student Problems
Problem
CuCl2
CuF
Hg2Br2
Fe2S3
FeO
Sn3N2
Step 1
2
Cu
Cl-
+
Cu+
F2
Hg2
Br-
Step 2
2
Step 3
+
Cu = Copper Copper (II)
Cl- = Chlorine
Cu+ = Copper Copper (I)
F- = Flourine
+
3
+
2
+
Fe2S
2
Step 4
Step 5
Chlorine=CHLOR
CHLOR+ide
Copper (II)
chloride
FLOUR+ide
Copper (I)
flouride
Flourine=FLOUR
+
Hg2 =Mercury Mercury (I) Bromine=BROM
Br- = Bromine
Fe3+
= Iron
2S = Sulfur
2
+
2
+
Fe
2O
Fe2- =Iron
O =Oxygen
Sn2+
N 3-
Sn = Tin
N 3- = Nitrogen
Answer
BROM+ide Mercury (I)
bromide
Iron (III)
Sulfur=SULF
SULF+ide
Iron (III)
sulfide
Iron (II)
Oxygen=OX
OX+ide
Iron (II)
oxide
Tin (II)
Nitrogen=NITR
NITR+ide
Tin (II)
nitride
Binary Compounds w/ Variable Charge: Stock System
Given The Formula, Write The Name
1) copper(II) sulfide
2) lead(IV) bromide
3) lead(II) nitride
4) iron(III) oxide
5) iron(II) iodide
6) tin(IV) phosphide
7) copper(I) sulfide
8) tin(II) chloride
9) mercury(II) oxide
10) mercury(I) fluoride
11) copper(II) chloride
12) copper(I) bromide
13) lead(II) oxide
14) iron(III) sulfide
15) lead(II) chloride
16) tin(II) oxide
17) copper(I) oxide
18) lead(IV) oxide
19) iron(II) oxide
20) tin(IV) oxide
21) mercury(I) oxide
22) mercury(I) iodide
23) gold(III) chloride
24) manganese(II) oxide
25) chromium(III) chloride
26) cobalt(II) oxide
27) manganese(III) oxide
28) cobalt(III) sulfide
29) gold(I) fluoride
30) chromiun(II) bromide
e.) Given Name, Write The Formula-COMMON SYSTEM
Step 1: First word tells you the symbol of the cation (+ ion).
Step 2: The suffix (end of word) tells you the charge of the cation.
ic = the higher of the possible charges
ous = the lower of the possible charges
Step 3: The anion symbol and charge comes from the second
name given.
Step 4: Make sure charges of symbols equal a net charge of zero.
..............(criss cross charges)
Example:
Cupric chloride
Answer
CuCl2
Step 1 Step 2
Cu
(ic) = 2+
Step 3
chloride = Cl
Step 4
Cu2+ + Cl
-
Teacher Examples
Manganic chloride
Ferrous sulfide
Mercurous oxide
Student Problems
Problem:
Ferric iodide
Cuprous sulfide
Mercuric bromide
Mercurous flouride
Aurous phosphide
Plumbic oxide
Step 1
Step 2
Step 3
Step 4
Answer
Answers To Student Problems
Problem:
Step 1 Step 2
Step 3
Step 4
3+
-
Ferric iodide
Fe
(ic) = 3+
Cuprous sulfide
Cu
(ous) = + sulfide = S 2-
Mercuric bromide
Hg
(ic) = 2+
Mercurous flouride Hg2
Aurous phosphide
Plumbic oxide
Au
Pb
iodide = I
Fe + I
Cu + + S
bromide = Br -
(ous) = 2+ flouride = F
(ic) = 4+
2-
oxide = O
-
FeI3
2-
Cu2S
Hg 2++ Br - HgBr2
2+
-
(ous) = + phosphide = P
Answer
Hg2 + F
3-
+
Au + P
4+
-
3-
Pb + O
Hg2F2
Au3P
2-
Pb2O4
Binary Compounds w/ Variable Charge: Common System
Given The Name, Write The Formula
1) Cu3P2
2) Au2S3
3) MnCl2
4) FeBr3
5) Hg2O
6) Au3N
7) SnF2
8) FeI2
9) HgO
10) PbBr2
11) CuF
12) SnS2
13) Fe2S3
14) PbO
15) FeCl3
16) SnO2
17) Cu2S
18) Hg2Cl2
19) CoI3
20) Pb3P4
21) Fe3N2
22) SnBr2
23) PbS
24) CuO
25) CuCl
26) (Hg2)3N2
27) HgS
28) Fe3P2
29) Pb3N4
30) CuCl2
e.) Given Formula, Write The Name-COMMON SYSTEM
Step 1: Separate formulas into individual ions. (un criss-cross)
Step 2: Find ions on ION CHARGE SHEET.
Step 3: Look at first element and its charge...name it using its LATIN
name AND “ic” and “ous” to show the charge.
Step 4: Look at second element. Use ROOT of its full name.
Step 5: Add “ide” to the root of the second element.
Step 6: Combine the t wo names to get the full name of the compound
Example:
FeCl2
Step 1
Fe
Step 5
CHLOR + ide
Cl
Step 2
Fe = Iron
Cl = Chlorine
Answer
Ferrous chloride
Step 3
2+
Fe = ferrous
Step 4
Chlorine = CHLOR
Teacher Examples
FeCl3
Hg2Br2
Cu2S
Student Problems
Problem
HgBr2
Cr2S3
Au3P
Sn2O4
PbI2
CuF2
Step 1
Step 2
Step 3
Step 4
Step 5
Answer
Answers To Student Problems
Problem
Step 1
Step 2
Step 3
Step 4
Step 5
2+
HgBr2
Hg Br Hg = Mercury Hg = mercuric bromine = BROM BROM + ide
Br = bromide
Cr2S3
Cr S
Au3P
Sn2O4
PbI2
CuF2
3+
Cr = Chromium Cr = chromic sulfide = SULF
S = sulfide
SULF + ide
Answer
Mercuric Bromide
Chromic sulfide
Au P Au = Gold
Au+= aurous phosphide = PHOSPH PHOSPH + ide Aurous phosphide
P = phosphide
Sn O
Sn = Tin
O = oxide
Sn4+= stannic
Pb I
Pb = Lead
I = Iodide
Pb = plumbous
Cu F
Cu = Copper Cu = 2+
cupric
F =fluoride
2+
oxide = OX
iodide = IOD
flouride = FLOR
OX + ide
Stannic oxide
IOD + ide
Plumbous iodide
FLOR + ide
Cupric fluoride
Binary Compounds w/ Variable Charge: Common System
Given The Formula, Write The Name
1) chromous sulfide
2) plumbic bromide
3) plumbous nitride
4) ferric sulfide
5) ferrous iodide
6) mercurous fluoride
7) cuprous sulfide
8) stannous chloride
9) mercuric oxide
10) stannic phosphide
11) chromic sulfide
12) plumbous chloride
13) stannic nitride
14) ferrous sulfide
15) ferric bromide
16) mercuric fluoride
17) cupric sulfide
18) stannic iodide
19) mercurous oxide
20) plumbic phosphide
21) manganous oxide
22) stannic oxide
23) plumbic oxide
24) ferric oxide
25) cuprous iodide
26) mercurous chloride
27) cupric oxide
28) stannous nitride
29) mercurous peroxide
30) cupric chloride
III.) Covalent Binary Compounds: The Greek System
a.) Covalent:
b.) Greek Prefix System:
Two NEGATIVE IONS combine
Use prefixes (at the beginning of word) to
show the NUMBER OF ATOMS PRESENT of
each element.
c.) Given Name, Write The Formula
Step 1: The first name will tell you the first element in the ....
...
compound.
..............if there is a prefix on the name that will tell
..............you the number of atoms of that element.
..............if there is NO prefix then it is understood to
..............be ONE ATOM.
Step 2: The anion name (second name) will tell you the .element
you are using AND the prefix will tell you .how many
atoms there are of that element.
***”MONO” is never used on the first element. If there is only
one atom there will be no prefix.
Example:
trinitrogen pentaoxide
Step 1:
trinitrogen
tri = 3
nitrogen = N
Step 2:
pentaoxide
penta = 5
oxide = oxygen = O
Answer:
N3O5
Teacher Examples:
1.) tricarbon tetrafluoride
2.) carbon monoxide
3.) pentanitrogen dioxide
4.) sulfur trioxide
5.) carbon dioxide
Student Examples:
1.) heptacarbon diiodide
2.) carbon tetrafluoride
3.) tetrahydride trioxide
4.) nonasulfur hexabromide
5.) octacarbon decasulfide
Answers To Student Examples:
1.) heptacarbon diiodide
hepta = 7
carbon = C
di = 2
iodide = iodine = I
2.) carbon tetrafluoride
none = 1
carbon = C
tetra = 4
fluoride = fluorine = F
3.) tetrahydride trioxide
tetra = 4
hydride = H
tri = 3
oxide = oxygen = O
C7I 2
CF4
H4O3
4.) nonasulfur hexabromide
nona = 9
sulfur = S
hexa = 6
bromide =bromine = Br
S9Br6
5.) octacarbon decasulfide
octa = 8
carbon = C
deca = 10
sulfide = sulfur = S
C8S10
Binary Compounds Greek Prefix System
Given The Name, Write The Formula
1) ClO
2) OF2
3) BP
4) N2O
5) NF3
6) SCl4
7) XeO3
8) CO2
9) P2O5
10) PCl3
11) SO2
12) BrF5
13) S2Cl2
14) BF3
15) As4O10
16) SiCl4
17) KrF2
18) ClO
19) SiO2
20) BCl3
21) N2S5
22) CO
23) SO3
24) N2O3
25) N2O
26) XeF6
27) SF6
28) PCl5
29) NO
30) BiCl3
d.) Given Formula, Write The Name
Step 1: Find the ions involved in the formula & their charges.
..............if BOTH ions are negative then you are dealing with
..............COVALENT COMPOUNDS & the GREEK PREFIX
..............SYSTEM.
Step 2: The first symbol will tell you the name of the first element
in the compound.
..............the name appears as it would normally.
Step 3: The subscript after the first symbol tells you the number
of atoms of that element.
..............use the GREEK PREFIXES to show this number.
..............*** “MONO” is never used on the first element. If
..............
there is only one atom there will be no prefix.
Step 4: The second symbol will tell you the name of the
second.element in the compound.
..............the rules for binary naming apply (add “ide”)
Step 5: The subscript after the second symbol tells you the
number.of atoms of that element.
..............use the GREEK PREFIXES to show this number.
..............*** “MONO” is used on the second element.
Example:
N2O3
Step 1:
N2
N = nitrogen
2 = di
Step 2:
O3
O = oxygen = oxide
3 = tri
Answer:
dinitrogen trioxide
Teacher Examples:
1.) C2F3
2.) SCl5
3.) H2O
4.) C6Cl3
5.) CO
Student Examples:
1.) N4O
2.) S7O10
3.) N5O6
4.) P9Cl2
5.) CO2
Answers To Student Examples:
1.) N4O
N = nitrogen
4 = tetra
O = oxygen = oxide
none = 1 = mono
tetranitrogen monoxide
2.) S7O10
S = sulfur
7 = hepta
O = oxygen = oxide
10 = deca
heptasulfur decaoxide
3.) N5O6
N = nitrogen
5 = penta
O = oxygen = oxide
6 = hexa
pentanitrogen hexaoxide
4.) P9Cl2
P = phosphorus Cl = chlorine = chloride
9 = nona
2 = di
5.) CO2
C = carbon
none = 1
O = oxygen = oxide
2 = di
nonaphosphorus dichloride
carbon dioxide
Binary Compounds Greek Prefix System
Given The Formula, Write The Name
1) tetrarsenic decoxide
2) bromine trioxide
3) boron nitride
4) dinitrogen trioxide
5) nitrogen triiodide
6) sulfur hexafluoride
7) xenon tetrafluoride
8) phosphorous trichloride
9) carbon monoxide
10) phosphorous pentachloride
11) diphosphorous pentoxide
12) disulfur dichloride
13) iodine dichloride
14) sulfur dioxide
15) tetraphosphorous decoxide
16) uranium hexafluoride
17) oxygen difluoride
18) chlorine dioxide
19) silicon dioxide
20) boron trifluoride
21) dinitrogen pentasulfide
22) carbon dioxide
23) sulfur trioxide
24) xenon hexafluoride
25) krypton difluoride
26) bromine pentachloride
27) sulfur tetrachloride
28) phosphorous trifluoride
29) xenon trioxide
30) osmium tetroxide
IV.) Polyatomic Compounds
a.) Polyatomic:
b.) Use of parentheses ():
More than one element in an ion.
Use () to show that the subscript stays with
the ions included inside the ().
c.) Given Name, Write The Formula
Step 1: The first name will tell you the first element in
the compound.
..............if there are roman numerals included that is
..............the charge on the cation.
..............if there are suffixes of “ic” or “ous” that is the
..............charge on the cation.
Step 2: The polyatomic name comes from the formula
of the ion AND the charge on that polyatomic ion.
Step 3: Remember that the entire formula must have a
net charge of ZERO.
..............criss cross the charges.
..............super scripts become subscripts
Example:
Copper (II) chlorate
Step 1:
Copper (II)
(II) = 2+
copper = Cu
Step 2:
Chlorate
chlorate = ClO3 -
Answer:
2+
Cu + ClO3
-
------->
Cu(ClO3)2
Teacher Examples:
1.) Cupric bromate
2.) Sodium carbonate
3.) Ferrous nitrite
4.) Magnesium peroxide
5.) Mercury (I) phosphate
Student Examples:
1.) Calcium phosphate
2.) Magnesium hydroxide
3.) Ferric sulfate
4.) Stannous perchlorate
5.) Ammonium oxalate
Answers To Student Examples:
1.) Calcium phosphate
2+
2+
calcium = Ca 3phosphate = PO4
3-
Ca + PO4
------->
Ca3(PO4)2
Mg 2+ + OH
------->
Mg(OH)2
2.) Magnesium hydroxide
Magnesium = Ca2+
hydroxide = OH 3.) Ferric sulfate
3+
3+
Ferric = Fe 2sulfate = SO4
Fe + SO
24 ------->
Fe2(SO4)3
4.) Stannous perchlorate
2+
Stannous = Sn perchlorate = ClO4
2+
-
Sn + ClO4
------->
Sn(ClO4)2
------->
(NH4)2C2O4
5.) Ammonium oxalate
+
Ammonium = NH4
2oxalate = C2O4
+
2-
NH4 + C2O4
Polyatomics
Given The Name, Write The Formula
1) Ag2CO3
2) K2HPO4
3) Al(OH)3
4) NaHCO3
5) Ca(C2H3O2)2
6) KMnO4
7) Ca(ClO4)2
8) Li2CO3
9) Mg(HSO3)2
10) NaClO
11) Sn(ClO2)4
12) Hg3(PO4)2
13) SnCO3
14) Hg2(C2H3O2)2
15) PbCrO4
16) Cu2SO3
17) SnCr2O7
18) Fe(NO3)3
19) Fe2(SO4)3
20) Fe(OH)2
21) KClO4
22) Pb(HPO4)2
23) Al2(SO4)3
24) Fe(HCO3)2
25) Ba(IO3)2
26) Sn(HS)2
27) Mg(H2PO4)2
28) Pb(CN)2
29) Ag3PO4
30) Co(NO2)3
31) (NH4)2SO4
32) NH4NO3
d.) Given Formula, Write The Name
Step 1: Uncriss-cross the formula and find the ions
involved.
..............if a VARIABLE CATION is used you will need to use the
..............common system (”ic” or “ous”) or the stock system
..............(roman numerals)
..............make sure to find the charge on the NEGATIVE ANION
..............first...this will help you greatly in finding the charge
..............on the cation
Step 2: The first symbol will tell you the name of the first element
in the compound.
..............the name appears as it would normally.
Step 3: The second symbol will tell you the name of the polyatomic
ion in the compound.
..............remember that () tell you that everything inside
..............stays together
Step 4: Combine the t wo names to form the overall name of
the compound.
............
Example:
Fe(NO3)2
Step 1:
Fe
+
NO3
NO3 is always (-)
The () around the NO3 tell you that the 3 stays with the NO...AND that the
2 outside the () is from the Fe.
So...
Fe 2+
NO3 -
Step 2:
Fe2+ = Ferrous or Iron (II)
NO3 -= Nitrate
Answer:
Ferrous nitrate
or
Iron (II) nitrate
Teacher Examples:
1.) Fe2(SO3)3
2.) Hg2O2
3.) NH4(NO2)
4.) Cu3(PO4)2
5.) Ca(OH)2
Student Examples:
1.) Cr2(O2)3
2.) HgSO4
3.) Ag2CO3
4.) AuPO4
5.) Mn2(CrO4)3
Answers To Student Examples:
1.) Cr2(O2)3
Cr + O2
Cr3+ = Chromium (III)
O22- = peroxide
2.) HgSO4
Hg + SO4
Hg 2+ = Mercury (II)
SO42- = sulfate
3.) Ag2CO3
Ag + CO3
Ag +
= Silver
CO32- = carbonate
4.) AuPO4
Au + PO4
Au 3+ = Gold (III)
PO43- = phosphate
5.) Mn2(CrO4)3
Mn + CrO4
Mn 3+
= Manganese (III)
2CrO4
= chromate
Chromium (III) peroxide
Mercury (II) sulfate
Silver carbonate
Gold (III) phosphate
Manganese (III) chromate
Polyatomics
16) lead(IV) hydroxide [plumbic hydroxide]
17) copper(I) dichromate [cuprous dichromate]
18) copper(II) chlorate [cupric chlorate]
1) aluminum phosphate
19) iron(II) sulfate [ferrous sulfate]
2) potassium nitrite
20) mercury(I) perchlorate [mercurous perchlorate]
3) sodium hydrogen carbonate
21) potassium chlorate
[sodium bicarbonate]
22) tin(II) sulfate [stannous sulfate]
4) calcium carbonate
23) aluminum permanganate
5) magnesium hydroxide
24) lead(II) nitrate [plumbous nitrate]
6) sodium cromate
25) magnesium phosphate
7) barium cyanide
26) copper(I) dihydrogen phosphate
8) potassium sulfate
[cuprous dihydrogen phosphate]
9) sodium dihydrogen phosphate
27) calcium hydrogen phosphate
10) ammonium nitrate
28) iron(III) hydrogen carbonate
11) tin(II) nitrate [stannous nitrate]
[ferric hydrogen carbonate, iron(III) bicarbonate, ferric
12) iron(III) phosphate [ferric phosphate]
bicarbonate] Yep! Gotta know all four!
13) copper(I) sulfate [cuprous sulfate]
14) nickel(II) acetate [nickelous acetate] 29) sodium carbonate
30) manganese(II) sulfate [manganous sulfate]
15) mercury(II) carbonate
[mercuric carbonate]
Given The Formula, Write The Name
V.) Naming Acids
a.) Binary Acid:
b.) Polyatomic Acid:
c.) Assumption:
Two Elements TOTAL in the acid..
More than t wo total elements in the acid.
99.9% of all acids or compounds that are
acids start with H.
d.) Given Formula, Write The Name
Step 1: Determine if it is binary or polyatomic.
a.) Binary acids have TWO total elements.
b.) Polyatomic acids have MORE THAN t wo total
elements.
Step 2: The first element will always be Hydrogen (H +)
Step 3:
If the acid is BINARY
Hydro + root of second element + ic Acid
HCl
Hydro + CHLOR + ic Acid
Step 4:
If it is POLYATOMIC
H + Polyatomic Ion
H2CO3 -------> H + +
Step 5:
CO3 2-
Determine the name of the POLYATOMIC Acid Ion
“ate” on end of the ion = Polyatomic Root + “ic”
“ite” on end of the ion = Polyatomic Root + “ous”
H2CO3 -------> H
+
+
CO3
2-
CO3 = carbonATE = carbon + ic
Carbonic Acid
Teacher Examples:
1.) H2SO3
2.) HCl
3.) HNO2
4.) HBr
5.) H2SO4
Acids
1) phosphoric acid
2) carbonic acid
3) sulfuric acid
4) iodic acid
5) hydrofluoric acid
6) nitrous acid
Acids
7) HBr
8) HCN [even though CN¯ is polyatomic, it is named according to the binary rule]
9) HNO3
10) H2SO3
11) H3PO3
12) CH3COOH or HC2H3O2
Hydrates
1) trihydrate = . 3 H2O
2) octahydrate = . 8 H2O
Now, I know you may have just said three and eight to yourself. That's OK. Just remember the business with the dot AND putting
H2O.
One really silly mistake I've seen is where the kid multiplies everything out. For example, with trihydrate, the person writes H6O3.
So, what they did was take the three which should be out front and distributed it over the H2O.
Nah! No! Nein! Non!
You get the point.
Right?
3) Name this substance:
MgSO4 . 9 H2O
4) Write the formula for: barium chloride dihydrate
Answers:
3) Magnesium sulfate nonahydrate
4) BaCl2 . 2 H2O

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