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Ionic Nomenclature
Cation
Defn: A positively charged particle.
Name of metal+ the word “ion”.
Ex. Potassium
Potassium Ion
Anion
Defn: a negatively charged particle.
Name of non-metal w/ ending changed
to “ide”
Ex. Chlorine
Chloride
Binary Ionic Compounds
Contains only 2 different elements in the
compound
Naming the Compounds
Name of metal + Name of non-metal with “ide”
ending.
Ex NaCl
Sodium Chloride
More Examples
MgO
Magnesium Oxide
MgCl2
Magnesium Chloride
LiBr
Lithium Bromide
Ca3P2
Calcium Phosphide
Transition Metals
Transition metals can give up different
numbers of electrons
Therefore they can have multiple charges
(This applies to lead and tin, too.)
Ex. If Titanium loses 3e- Ti3+
Roman Numerals
Tells the charge of the ion preceding it. When an ion
can have more than one charge, you need to use a
roman numeral to specify the charge.
Ex Lead
Pb2+
Lead (II) ion
Pb4+
Lead (IV) ion
Exceptions
If the transition metal only has one charge,
then DO NOT use a roman numeral!
Ex. Zinc
Zn2+ Zinc ion
What are other examples of a transition metal
with only one charge?
Ag+, Cd2+, Sc3+
Reminder
Roman numerals tell the charge of an
ion, NOT HOW MANY!
Ex. Gold (III) chloride
What is the charge of the gold ion in gold
(III) chloride?
3+
Example:
Tin (II) bromide
What is the charge of the tin ion in tin
(II) bromide?
2+
Writing Formulas
The positive and negative charges must equal ZERO in
the compound.
1. Write the symbol and charge for each individual ion
2. Use the least common denominator (LCD) to determine
how many of each ion is needed in order to make a zero
net charge.
3. Write the formula, using a subscript(s) to indicate the
number of each ion in the compound
Example
Zinc sulfide
Zn2+ S2-
ZnS
Example
Sodium Oxide
Na+ O2-
Na2O
Example
Scandium bromide
Sc3+ Br –
ScBr3
Naming ionic compounds with polyatomic ions
(tertiary ionic compounds):
1. Name of cation first
2. Name of anion second
3. Remember roman numerals, if necessary
4. Enclose polyatomic ions in parenthesis when
it requires a subscript
Example
Zn2+ SO42-
Balanced Formula?
ZnSO4
Name?
Zinc sulfate
Calcium Phosphate
Ca2+ PO43-
Balanced Formula?
Ca3(PO4)2
Name?
Calcium Phosphate
Manganese (IV) Nitrite
Mn4+ NO2-
Balanced Formula?
Mn(NO2)4
Name?
Manganese(IV) Nitrite
MgCl2
CuSO4
Example: Copper (I) Chlorate
Cu+ ClO3-
Balanced Formula?
CuClO3
Name?
Copper (I) Chlorate
Chromium (III) Hydroxide
Cr3+ OH-
Balanced Formula?
Cr(OH)3
Name?
Chromium(III) hydroxide
NaNO3
Al(OH)3
Cu3PO4
Covalent Nomenclature
aka Molecular Compounds
To Name Covalent Compounds:
1. Translate the subscript of the first element into
a prefix + the name of the element
2. Translate the subscript of the 2nd element into a
prefix + root name of element with the “ide”
ending1 Mono 4 Tetra 7 Hepta
2 Di 5 Penta 8 Octa
3 Tri 6 Hexa 9 Nona
10 Deca
NOTE
If there is only 1 of the 1st
element, do not use a prefix
Ex. CO
carbon monoxide
Name the Following Compounds
N2O
Dinitrogen monoxide
PCl3
Phosphorus trichloride
SF6
Sulfur hexafluoride
Name the Following Compounds
CO2
Carbon dioxide
NO
nitrogen monoxide
CCl4
carbon tetrachloride
To Write Formulas for Covalent Compounds:
1. Correlate the prefix of the 1st element to its
numerical value…write it as the subscript
2. Correlate the prefix of the 2nd element to its
numerical value…write it as the subscript
3. Prefix should match the subscript written for
each element
*Remember, if there is not a prefix, then it’s just 1.
Write the formula for each
Tetraiodine nonoxide
I4O9
Sulfur trioxide
Phosphorus pentafluoride
Write the formula for each
Nitrogen dioxide
NO2
Dichlorine heptoxide
Cl2O7
Carbon disulfide
CS2
Acid Nomenclature
Naming Acids
Acids always have hydrogen.
Binary Acids
Hydrogen + 1 other element
Oxy Acids
Hydrogen + oxygen (from a polyatomic
ion)
Binary Acids
1. Use “hydro” for hydrogen
2. Root of 2nd element + ic (take off the
ending)
3. add “acid” to the end
Ex : HCl
Hydrochloric acid
Name the Binary Acids
H2S
Hydrosulfuric acid
(notice here that it is sulfuric, not sulfic)
HF
Hydrofluoric acid
HBr
Hydrobromic acid
Oxy Acids “ite”
The name of the acid comes from the name of the
polyatomic ion.
If the polyatomic ion ended in “–ite”, then the ending for the
acid is “–ous”
Take off the “ite” ending of the polyatomic ion and add
–”ous”
Add the word “acid”
Ex. HNO2
Nitrous Acid
Name the oxy acids
H2SO3
Sulfite Ion
Sulfurous acid
H3PO3
Phosphite Ion
Phosphorous acid
Oxy Acids “ate”
If the polyatomic ion ended in “–ate”, then the ending
for the acid is “–ic”
Take off the “ate” ending of the polyatomic ion and add
–”ic”
Add acid
Ex. HNO3
nitrate ion
Nitric acid
Name the oxy acids
H2SO4
Sulfate ion
Sulfuric Acid
H3PO4
Phosphate ion
Phosphoric Acid
Writing formulas for binary acids
Determine what kind of acid it is; binary or
oxy
Does it have hydro at the front?
If yes, then it is binary
Determine the charges for the individual ions
Write the formula so that the overall charge
equals zero
Example
Hydroiodic acid
H+ I-
HI
Hydroselenic acid
H+ Se2-
H2Se
Writing formulas for oxy acids
Determine what kind of acid it is; binary or
oxy
Does it have -ous or –ic at the end?
If yes, then it is an oxy acid
Determine the charges for the individual ions
Write the formula so that the overall charge
equals zero
Example
Chlorous acid
from chlorite ion
ClO2- HClO2
Boric acid
From borate ion
BO33-
H3BO3
Chloric acid
from chlorate ion
ClO3- HClO3
Examples
Sulfurous acid
from sulfite ion,
SO32- H2SO3
Carbonic acid
from carbonate ion,
CO32- H2CO3