Transcript Chapter

Chapter 4
NOMENCLATURE
Binary Ionic Compounds
compounds formed from a
combination of metal and
nonmetal
 Compounds contain a positive
ion and a negative ion

Oxidation Number

Is the number of electrons that
is apparently lost or gained by
an atom in a molecule formation
He
H
Li
Be
B
C
N
O
F
Ne
Na
Mg
Al
Si
P
S
Cl
Ar
K
Ca
Ga
Ge
As
Se
Br
Kr
Rb
Sr
In
Sn
I
Xe
Cs
Ba
Ti
Pb
At
Rn
Fr
Ra
Bi
Po
Oxidation Numbers of
Common Elements
1
2
3
4
5
6
7
(+1)
(+2)
( +3)
(-3)
(-2)
(-1)
Li
Na
K
Rb
Cs
Be
Mg
Ca
Sr
Ba
B
Al
(+4)
(-4 )
C
Si
N
P
O
S
Se
F
Cl
Br
I
Naming Cation and Anion





Cation
Named by its
parent atom
Na+ = Sodium
Mg2+=Magnesium
Al3+ = Aluminum

Anion

Named by taking the
root name of the atom
and add a suffix ide

F- Flourine
Flour + ide = Flouride
Cl- Chlorine
Chlor + ide = Chloride
O2– Oxygen
Ox + ide = Oxide
S2+ -Sulfur
Sulf + ide = Sulfide



Types of Binary Ionic
Compounds
Type 1 Binary Ionic Compound
The metal present formed only
one type of cation
Ex: Na+, Cs+, Ca2+, Al3+
Type II Binary Ionic
Compound
Metals present can form two or more
cations that have different charges
 Composed of transition metals
 Ex: Copper  Cu+, Cu2+
Iron
 Fe2+, Fe3+
Lead  Pb2+, Pb4+
Tin
 Sn2+, Sn 4+
Co
 Co2+ , Co 3+
Sn
 Sn2+ , Sn4+

Naming Binary
Ionic Compounds
Naming Type I



The Cation is named first then the
anion
Cation is named by its parent name
The anion is named by taking the
root plus ide
Ex: Na+
+ Cl- = NaCl -> Sodium Chloride
K+ + I- = KI -> Potassium Iodide
Ca2+ + S2- = CaS -> Calcium Sulfide
Cs+ + Br- = CsBr -> Cesium Bromide
Formula Writing for type I


The sum of the total positive charges
must be equal to the sum of the
negative charges
Ex: K+ and Cl-  KCl
(+) + (-) = 0
Ca2+ and Br- -> CaBr2
(+2) + 2 (-1) = 0
Formula Writing for type I
Criss-cross method
-> simply write the charge of the ion
and cross over the numbers but not
The + or – sign
Ca 2+ Br-  CaBr2
Ex: Write the formula for Magnesium Nitride
Mg2+ N 3 Mg3N2
Write the formula for Magnesium Oxide
Mg2+
O2-  MgO
Classwork

a)
b)

a)
b)
c)
Name each binary Compound
KCl
c) BaH2
ZnS
d) Al2S3
Write the formula for the following
compound
Strontium Flouride
Calcium Sulfide
Calcium Phosphide
Answer
KCl – Potassium Chloride
 ZnS – Zinc Sulfide
 BaH3 – Barium Hydride
 Al2S3 – Aluminum Sulfide
Write the formula for the following compound
 Strontium Flouride
Sr 2+
F-  SrF2
Calcium Sulfide
 Ca2+ and S2-  CaS
Calcium Phosphide
 Ca2+ and P3-  Ca3P2

Naming Type II Ionic
Compound
Determine the charge of the cation
Ex: CuCl  Cu+
Cl
Fe2O3  Fe3+ O2 Use a Roman Numeral to specify the
charge on the cation(Stock System) or use
(Classical System) – ous for lower oxidation
and ic for higher oxidation
Systematic
Classical
Ex: CuCl Copper(I)Chloride Cuprous oxide
Fe2O3 Iron ( III)Oxide
Ferric Oxide

Symbols Derived in their Latin
Name

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
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





Sodium
Potassium
Iron
Copper
Tin
Silver
Antimony
Gold
Mercury
Lead
Na
K
Fe
Cu
Sn
Ag
Sb
Au
Hg
Pb
Natrium
Kallium
Ferrum
Cuprum
Stannum
Argentum
Stibium
Aurum
Hydrargyrum
Plumbum
Common Type IICations (page
90) Table 4.2

Ion
Fe3+
Fe2+
Cu2+
Co3+
Co2+
Sn4+
Sn2+
Pb 4+
Pb 2+
Systematic Name
Iron (III)
Iron (II)
Copper(II)
Cobalt (III)
Cobalt(II)
Tin (IV)
Tin (II)
Lead(IV)
Lead (II)
Older/ Classical Name
Ferric
Ferrous
Cupric
Cobaltic
Cobaltous
Stannic
Stannous
Plumbic
Plumbous
Examples( page 91)
Name the following compound
CuCl Cu+
Cl-
Copper(I)
Chloride
b) HgO  Hg 2+
O2-
Mercury(II)
Chloride
a)
c) Fe2O3  Fe3+
Iron(III)
O2
Oxide
d)
MnO2  contains 2 O2- anions
Mn +
O
?
+ 2( -2) = 0
Mn4+ ---> Manganese(IV)
O2Oxide
Practice Problems

a)
b)
c)
d)
e)
f)
g)
h)
Give the systematic Name of the
following compounds
PbBr2
PbBr4
CuO
PbI2
CoCl3
FeS
SnF4
CrF2