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Molecules
Acids
Ionic
Chemical
Nomenclature
1. Binary Ionic Compounds - Type I
2. Binary Ionic Compounds - Type II
3. Ionic Compounds & Polyatomic (Complex) Ions
4. Hydrated Ionic Compounds
5. Binary Covalent Compounds
6. Binary Acids
7. Oxy-Acids
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Definitions
An IONIC COMPOUND consists of a metal
cation bonded to a nonmetal anion.
Electrostatic attraction holds them together.
A COVALENT COMPOUND consists of two
nonmetal atoms sharing valence electrons.
A BINARY compound is one that is made of
just two elements. There can be one of each
element such as in NaCl or KF. There can
also be several of each element such as
Na2O or AlBr3.
Type I Binary Ionic Compounds
The metal cations in these compounds have
only ONE possible charge.
Na+
sodium
Zn2+
zinc
Al3+
aluminum
Ca2+
calcium
The charges are memorized or predicted using a periodic table!
The cations are bonded to nonmetal anions:
O2oxide
N3nitride
Ffluoride
Br bromide
Notice that simple anions are always named with the
suffix “ide”
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Predicting Charges on Monatomic Ions
KNOW THESE !!!!
+1 +2
-3 -2 -1
0
Cd+2
Compounds
formed from
ions
CATION +
ANION --->
--->
COMPOUND
Na+ + Cl- -->
--> NaCl
A neutral compound
requires
equal number of +
and - charges.
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Naming Compounds
Binary Ionic Compounds:
1. Cation first, then anion
2. Monatomic cation = name of the element
2+ = calcium ion
Ca
3. Monatomic anion = root + -ide
− = chloride ion
Cl
CaCl2 = calcium chloride
Naming Binary Ionic Compounds
Examples:
NaCl
KI
Al2O3
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Learning Check
Complete the names of the following binary
compounds:
1. Na3N
sodium
________________
2. KBr
potassium ________________
3. Al2O3
aluminum
4. MgS
_________________________
________________
Formulas for Binary
Ionic Compounds
A binary compound is one made of two
different elements. There can be one of
each element such as in sodium bromide or
potassium iodide. There can also be several
of each element such as lithium oxide or
aluminum bromide.
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Formulas of Ionic Compounds
Formulas of ionic compounds are
determined from the charges on the ions
atoms
ions
••
Na • +
•
F : →
••
Na+
••
sodium + fluorine
–
: F : → NaF
••
sodium fluoride
Charge balance:
1+
formula
1-
= 0
Writing Formulas
Formula Unit – lowest whole number ratio of
ions in an ionic compound
1.
2.
3.
4.
5.
Points to remember about writing the formula from
the name
The order in a formula is first the cation, then the anion.
You must know the charges associated with each
cation and anion.
The sum of the positive charge and the sum of the
negative charges MUST add up to zero.
You MAY NOT adjust the charges of the cations or
anions to get a total charge of zero.
You MAY adjust the subscripts to get a total charge of
zero.
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Example #1
Suppose you must write the formula for sodium chloride.
Write down the Na+ and Cl- right next to each other, as in this image:
Move the positive charge (dropping the sign) to the subscript position of
the anion:
Move the negative charge (dropping the sign) to the subscript position of
the cation:
The result of all this moving is:
Since subscripts of one are not written, but understood to be present,
the final answer is:
Example #2
Write the formula for aluminum oxide.
Write down the Al3+ and O2 right next to each other :
-
Move the positive charge (dropping the sign) to the subscript
position of the anion:
Move the negative charge (dropping the sign) to the subscript
position of the cation:
The result of all this moving is:
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Learning Check
Write the correct formula for the
compounds containing the following
ions:
1. Sodium sulfide
a) NaS
b) Na2S
c) NaS2
2. Aluminum chloride
a) AlCl3
b) AlCl
c) Al3Cl
3. Magnesium nitride
a) MgN
b) Mg2N3
c) Mg3N2
Solutions
1. Na+ S2b) Na2S
2. Al3+ Cla) AlCl3
3. Mg2+ N3c) Mg3N2
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Examples: Type I Binary Ionic Compounds
Write the formulas:
Write the names:
•potassium oxide
• K3N
• zinc chloride
• AgI
• silver sulfide
• ZnBr2
• aluminum nitride
• Al2O3
• gallium oxide
• Ba3P2
•calcium iodide
• LiH
Type II Binary Compounds Contain
Transition Metals
Elements that can have more than one
possible charge MUST have a Roman
Numeral to indicate the charge on the
individual ion.
1+ or 2+
2+ or 3+
Cu+, Cu2+
Fe2+, Fe3+
copper(I) ion
copper (II) ion
iron(II) ion
iron(III) ion
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Names of Variable Ions
These elements REQUIRE Roman Numerals because
they can have more than one possible charge:
anything except Group 1A, 2A, Ag, Zn, Cd, and Al
Or another way to say it is: Transition metals and the metals in
groups 4A and
5A (except Ag, Zn, Cd, and Al) require a Roman Numeral.
FeCl3
CuCl
SnF4
PbCl2
Fe2S3
(Fe3+) iron (III) chloride
(Cu+ ) copper (I) chloride
(Sn4+) tin (IV) fluoride
(Pb2+) lead (II) chloride
(Fe3+) iron (III) sulfide
Learning Check
Complete the names of the following binary
compounds with variable metal ions:
FeBr2
iron (_____) bromide
CuCl
copper (_____) chloride
SnO2
___(_____ ) ______________
Fe2O3
________________________
Hg2S
________________________
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Examples: Type II Binary Ionic Compounds
Write the formulas:
Write the names:
• iron (II) oxide
• Fe2O3
• copper (II) chloride
• SnS
• tin (IV) sulfide
• NiBr2
• cupric nitride
•CuS
• nickel (III) oxide
• Pb3P2
• ferrous iodide
• CuBr
•cobalt (III) selenide
• FeCl3
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