5.3 Chemical Nomenclature
Naming compounds and writing chemical formulas.
Dr. Fred Omega Garces
Chemistry 100
Miramar College
5.3 Chemical Nomenclature
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Objective
Charge of elemental ions.
Getting to know your polyatomic ions: Top - 12
Expanding your knowledge-base on polyatomic ions.
The oxy ions (…
(…ates)
Behavior of atoms to form compounds.
Criss-Cross trick
Knowing the different type of compounds Ionic vs
Covalent, Type I, Type II, Type III
Naming ionic compounds based on chemical formulas.
Writing chemical formula based on chemical names.
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5.3 Chemical Nomenclature
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Charge of Elemental Ions
The common charge (oxidation state) of many
representative and some transition metals
elements can be determine by the periodic table.
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Polyatomic Ions
Cations : ammonia, NH4+ ; Mercury (I), Hg22+
Anions
-1: hydroxide, OH- ; cyanide, CN- ; nitrate, NO3-2 : carbonate, CO32- ; chromate CrO42-, Dichromate Cr2O72-, sulfate
SO42-
-3 : phosphate, PO43Polyatomic oxy-ions: Chlorate, bromate, iodinate, sulfate,
nitrate, phosphate, chromate
Some form four anions
chlorate: perchlorate chlorate
Some form only two oxy anions
chlorite
hypochlorite
sulfate: sulfate sulfite
Some form only on oxy anion
carbonate: carbonate
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... the `ate
XO4 chg
XO3 chg
2CO
CO332-
3BO
BO333-
NO
NO333PO
PO443-
2SO
SO442-
ClO
ClO33-
3AsO
AsO443-
2SeO
SeO442-
BrO
BrO33-
2TeO
TeO442-
IO
IO33-
-3
-2
-1
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Polyatomic oxyions naming scheme
Oxy-anions
Remember the
-ate ion and start
nomenclature
from there.
Oxy-acids
Add H+
Add H+
Add H+
Not
Not all
all -ate
-ate follow
follow this
this pattern
pattern
22carbonate:
CO
carbonate: CO33
No
No carbonite
carbonite
Add H+
Metals
Metals which
which form
form oxyanions
oxyanions
permanganate,
permanganate, MnO
MnO44-chromate,
chromate, CrO
CrO442-2dichromate,
dichromate, Cr
Cr22O
O772-2...still
...still many
many others
others
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Example of polyatomic ions
Most common polyatomic ions
CationAmmonium
Anion12. Chromate
11. Permanganate
10. Perchlorate
9. Dichromate
8. Acetate
7. Carbonate
6. Phosphate
5. Sulfate
4. Nitrate
3. Cyanide
2. Peroxide
1. Hydroxide.
NH 4+
CrO42MnO4ClO4Cr2O72CH3CO2CO32PO43SO4-2
NO3CNO22OH-
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Behavior of atoms to form Compounds
Two main type of compounds
Ionic
Covalent
electrons are
transferred
electrons are
shared
Sodium
Sodiumand
andchlorine
chlorinecooperate
cooperatesymbiotically
symbioticallyininelectron
electron
transfer
transferininorder
ordertotohave
haveeight
eightelectrons
electronsininitsitsvalence
valenceshell.
shell.
Na
Na+
11 p
12 n
11 p
12 n
Fluorine
Fluorineprefers
preferstotoshare
shareits
itselectrons
electronstotoobtain
obtain88
total
totalininits
itsvalence
valenceshell
shell
F
11 p
12 n
F
9p
10 n
F-
9p
10 n
F
F2
9p
10 n
9p
10 n
9p
10 n
9p
10 n
9p
10 n
NaF
Atoms will transfer or share electrons in order to have
the same number of electrons as its closest noble gas
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Ways Compounds Ionic and Covalent Forms
Ionic Compounds: Type I
Binary Form - Composed from two different elements
bonding
Polyatomic Form - Compounds with some part of
substituents clustered together covalently with some charge.
Covalent Compounds: Type II
Combination of nonmetal atoms sharing electrons.
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Principle of Electrical Neutrality
When elements combine to form compounds, the principle
of electrical neutrality allows prediction of formulas of the
ionic compound.
Basic idea:
Sum of the charges must add to zero.
That is the sum of the cation charge and the sum of the anion
charge must cancel each other so that the compound form is neutral.
X
Mn Xm
cation (charges)
10
anion (charges)
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Type I, II and III
Ionic : Type I & II
Type I : Metal - nonmetal
metal has a definite oxidation state.
Ca Ca+2, K K+, Al Al+3, Zn
Zn+2
Type II : Metal(Ox#) - nonmetal
metal has a variable oxidation state.
Cu Cu+2 or Cu+ , Cr Cr+4 or Cr+4
Molecular: Type III
Type III : (prefix1)nonMetal1 - (prefix2)nonMetal2
covalent type of compounds
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Determining Type of Compound
Show me the metal !!
Type I
Type II
Yes
Is the metal
Group I, II or Al,
Zn, Cd and Ag
No
Type I
No
Yes
metal-nonmetal
Type II
metal(Ox. #)-nonmetal
Type III
(Prefix)nonmetal1 (Prefix)nonmetal2
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Type I, II and III
Anion
Elemental
Polyatomic
I (Metal - nonMetal)
Cation - Anion(ide)
Cation; Rep Metal
MgO; Magnesium oxide
Na2S; Sodium sulfide
Cation - Anion
Mg(NO3)2; magnesium nitrate
Type
Cation - Anion
K 2SO4; potassium sulfate
(Transition) metal
Cat (oxidation state) Anion(ide)
FeCl3; Iron(III) chloride
Cat (oxidation state) Anion
Pb(C 2H 3O2)2 ; Lead(II) acetate
Cation (O St #) - Anion
CuS; Copper(II) sulfide
Ag3PO4; Silver(I) phosphate
lower ox. st. -ous
Cation(ous) Anion(ide)
Cation(ic) - Anion(ide)
FeBr3 ; Iron(III) bromide or Ferrric
Cation(ous) Anion
Cation(ic) - Anion
Fe(NO3)2 ; Iron(II) nitrate or
higher ox.st. -ic
bromide
II (Metal - nonMetal)
Cat ; 3rd row and lower
old method
Ferrrous nitrate
(Prefix) nonmetal1 - (Prefix) nonmetal 2 (ide)
III
Molc' compounds -
• Prefixes are indication of the number of atoms:
Compounds which
mono-, di-, tri-, tetra-, penta
• order of naming nonmetal1 & nonmetal2
nonmetal1 is to the left and bottom ofnonmetal2
contains nonmetal
(Prefix ) nonmetal1 (Prefix ) nonmetal 2
it is named first in the nomenclature scheme.
Si - C - As - P - N - H - Se - S - I - Br - Cl - O - F
• S & 3O forms SO3 ; Sulfur trioxide
• 2I & 2Se forms Se2I2; diselinium diiodide
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Example: Type-I
Given the Chem Formula provide the name
Name Type I: Binary Metal - nonmetal(ide)
SrSe
Strontium selenide
Mg3N2
Magnesium nitride
Lithium oxide
Li2O
Chem Formula Type I:
SrSO4
Mg3(PO4 )2
LiClO4
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Polyatomic Metal - polyatomic
Strontium sulfate
Magnesium phosphate
Lithium perchlorate
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Example: Type-I
Given the name provide the chemical formula
Name Type I: Binary
potassium sulfide
Elemental symbol
Charge of ions
Criss-Cross
Metal - nonmetal(ide)
K & S
K (+1) S(-2)
K(2) S(1) g
K2S
Chem Formula Type I: Polyatomic Metal - polyatomic
Cadmium bisulfite
Elemental symbol
Charge of ions
Criss-Cross
Cd & HSO3
Cd (+2) HSO3(-1)
Cd(1) HSO3(2) g
Cd(HSO3)2
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Example: Type-II
Given the Chem Formula provide the name
Name Type II: Binary Metal(Ox.#) - nonmetal(ide)
Mn3N2
Elemental symbol
Mn (3) & N (2
(2)
Reverse Criss-Cross
Ox. State of metal
Name of Chemical
Chem Formula Type II:
Polyatomic Metal(Ox#) - polyatomic
Mn(NO2)2 Elemental symbol
Reverse Criss-Cross
Ox. State of metal
Name of Chemical
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Mn (2
(2) & N (3)
Ox St = 2; Mn(II
Mn(II))
Manganese(II
Manganese(II)) nitride
Mn (1) & NO2 (2
(2)
Mn (2
(2) & NO2 (1)
Ox St= 2; Mn(II
Mn(II))
Manganese(II
Manganese(II)) nitrite
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Example: Type-II
Given the name provide the chemical formula
Name Type II: Binary Metal - nonmetal(ide)
Iron(II) sulfide Elemental symbol Fe & S
Charge of ions
Criss-Cross
Reduce ratio
Fe(+2) S(-2)
Fe(2)
S(2)
FeS
g
Fe2S2
Name Type II: Polyatomic Metal - polyatomic
Tin(IV) sulfite Elemental symbol Sn & SO3
Charge of ions
Criss-Cross
Reduce ratio
Sn(+4) SO3(-2)
Sn(2) SO3(4) g Sn2(SO3)4
Sn(SO3)2
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Example: Type-III
Given the Chem Formula determine the name
Name Type III: (prefix1)nonMetal1 - (prefix2)nonMetal2(ide)
N2O2 Elemental symbol N (2) & O (2)
(2)
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Prefix
Name of Chemical
dinitrogen & dioxide
dinitrogen dioxide
XeF2
Elemental symbol
Prefix
Name of Chemical
Xe (1) & F(2)
F(2)
monoxenon
xenon
& difluoride
mono
xenon difluoride
P4Se10
Elemental symbol
Prefix
Name of Chemical
P (4) & Se(10)
Se(10)
tetraphosphorus & decaselenide
tetraphosphorus decaselenide
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Example: Type-III
Given the name determine the chemical formula
Name Type III: (prefix1)nonMetal1 - (prefix2)nonMetal2(ide)
Diboron trisulfide Elemental symbol B & S
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Prefix for atoms
Chemical formula
B(2) & S(3)
B2S3
Silicon tricarbide
Elemental symbol
Prefix for atoms
Chemical formula
Si & C
Si(1) & C(3)
SiC3
Iodine monochloride
Elemental symbol
Prefix for atoms
Chemical formula
I & Cl
I(1) & Cl(1)
ICl
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Summary
An ionic compound is named with cation first and anion last. For
metals that can form more than one ion, the charge is shown with a
Roman numerical. For example, copper forms the mono-cation Cu+
and the di-cation, Cu2+, these are distinguished from each other in
their chemical name as copper(I) and copper (II). Oxyanions (or
anions with two kinds of element one of which is oxygen) have
suffixes, and some sometimes prefixes, attached to their element root
name to indicate the number of oxygen atoms. For example the oxy
anion containing sulfur and oxygen may form the following anions,
hyposulfite SO22-, sulfite SO32-, sulfate SO42-, and persulfate SO52- .
Binary covalent compounds nomenclature consist of writing the most
electropositive elements first proceeded by a prefix which indicates
the number of atoms , I.e., di-2, tri-3, tetra-4 and so on. The second
more electronegative element is written next which also is proceeded
by the prefix which indicates the number of atoms. For the second
element, a “mono”
mono” prefix must always be written if there is only one
atom in the chemical formula. i.e., carbon monoxide for CO.
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