Big Idea: Matter & Atoms
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Naming
Naming
Naming
Naming
Ionic Compounds
Covalent Compounds
Acids
Hydrates
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The cation (positive ion) is written first
◦ Takes the same name as the element if only forms
one charge
◦ Use Roman numerals to distinguish charge if
element forms more than one charge
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The anion (negative ion) is written last
◦ Use the first part of its element name and add –ide
is added as the suffix.
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Examples
Formula
Name
Ions
CuS
Copper (II) Sulfide
Cu2+
S2-
CuBr
Copper (I)
Bromide
Cu+
Br-
Ca2+
Br-
Fe2O3
Lithium Fluoride
MgO
Manganese (II)
Oxide
CoI3
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For polyatomic ions, always use the name
assigned to it
Do not add an additional suffix (such as ide)
◦ Example:
 CO32- --carbonate ion
 CaCO3 – calcium carbonate
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Ammonium, NH4+, is the only polyatomic
cation that you need to know
◦ Example:
 NH4Cl – ammonium chloride
 NO3- -- nitrate ion
 NH4NO3 – ammonium nitrate
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Only three polyatomic ions end in –ide
◦ CN◦ OH◦ O22-
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cyanide
hydroxide
peroxide
Everything else ending in –ide is a monatomic
anion
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A system for oxo-anions
◦
◦
◦
◦
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Hypo_______-ite
_______-ate
Per-
-ite
(
(
less oxygens than
less oxygen than
-ate)
-ate)
-ate
(
more oxygen than
-ate)
All polyatomic ions in such a series carry the
same charge
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Example with chlorate, ClO3◦
◦
◦
◦
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Hypochlorite
Chlorite
Chlorate
Perchlorate
Example with sulfate, SO42◦ Sulfite
◦ Sulfate
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There are no hypo-ite or per-ate for sulfate
Formula
CuCO3
K2CO3
Ca(ClO)2
KClO4
NaClO3
LiNO3
Fe(NO2)3
NaCH3COO
Name
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How do you know that something is an ionic
compound?
Ionic compounds contain either
a metal & nonmetal or
polyatomic ions
If the first word in the
compound is a metal or
ammonium, it is an ionic
compound
Name
Aluminum hydrogen sulfate
Iron (II) oxide
Iron (III) oxide
Strontium chromate
Potassium chloride
Ammonium nitrate
Lithium sulfite
Formula
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Ionic compounds must be neutral
compounds.
◦ All charges of ions must add up to zero
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Charges come from the associated group in
the periodic table or a list
Parenthesis must be used when there is some
multiple of a certain polyatomic ion
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Examples
◦ Calcium chloride
◦ Calcium is always 2+ (Group 2A on the periodic
table)
◦ -ide in Chloride tells you that it is monatomic
◦ Chloride is always 1- (Group 7A from the periodic
table)
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Criss-Cross Method
Ca2+
CaCl2
Cl-
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Iron (III) Sulfate
◦ The iron ion carries a charge of 3+ as the Roman
numeral is (III)
◦ Sulfate is SO42- is a known anion from your memory
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Criss Cross Method
Fe3+
SO42Fe2(SO4)3
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These are made of two non-metals or
metalloids
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Two elements with prefixes where the prefix
explains the number of atoms of element
◦ 1-mono-, 2-di-, 3-tri-, 4-tetra-,5-penta-,
◦ 6-hexa-, 7-hepta-, 8-octa-, 9-nona-, 10-deca-
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The first name is the first element with the
appropriate elemental name and prefix for
number of atoms
◦ Mono- is NOT used when there is only one atom of
the first element
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The second name is the second element with
the correct prefix and the suffix of -ide
Formula
SiO2
CO
CF4
N4O4
XeF6
N2O3
P4O7
Name
Name
Carbon dioxide
Phosphorus trichloride
Sulfur tetrafluoride
Disulfur dichloride
Iodine monochloride
Dinitrogen tetroxide
Nitrogen triodide
Formula
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Formulas for acids usually start with H
◦ Hydrogen is always the cation
◦ For organic acids, the cation is often placed at the
end of the formula instead of in the front
 Acetic acid
 Inorganic
 Organic
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HC2H3O2
CH3COOH
Two types of acids
◦ Acids that contain oxygen (oxyacids)
◦ Acids that do not contain oxygen
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To name all acids, you must look at the anion
Oxygen-containing acids have polyatomic
anions
The name of the polyatomic anion suffix will
change:
◦
◦
◦
◦
◦
-ate to -ic
-ite to –ous
Per—ate to per—ic
Hypo—ite to hypo—ous
And the second name is acid
Formula
Polyatomic Ion Name
Name of Acid
HClO4
Perchlorate
Perchloric acid
H2SO4
Sulfate
Sulfuric acid
CH3COOH
Acetate
Acetic acid
H2SO3
Sulfite
Sulfurous acid
HNO2
Nitrite
Nitrous acid
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If there is no “O” then there is a hydroSo the prefix for these acids is hydro
The suffix changes from the anion which was
–ide to –ic
The second name is acid
Formula
Ion Name
Name of Acid
HCN
Cyanide
Hydrocynanic acid
HCl
Chloride
Hydrochloric acid
HBr
Bromide
Hydrobromic acid
Name
Nitric acid
Phosphoric acid
Hydrofluoric acid
Hydrophosphoric acid
Carbonic acid
Hypochlorous acid
Formula
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Hydrates are ionic compounds that trap water
within their structures.
Both the name and the chemical formula
specify how much water is contained within
the structure.
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Write the formula for the ionic compound
using the ionic compound rules from
previous slides.
Add a dot and the correct number of water
molecules taken from the prefix and the word
hydrate.
Example
◦ Sodium sulfate decahydrate
Na2SO4 · 10H2O
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Barium Chloride Dihydrate
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FeCl3·6H2O