NOMENCLATURE
Chapter 5
Charges on Common Ions
+1
+2
-4 -3 -2 -1
+3
Table 5.1: Common Simple Cations and Anions
Chemical Bonds
- the forces that hold two or more atoms
together to form a compound.
- the two types of chemical bonds are:
metal & nonmetal
1. Ionic bonds.
NaCl KI
2. Covalent bonds. two nonmetals
H2O CH4
Chemical Bonds
(continued)
Ionic Bonding: Force of attraction
between oppositely charged ions.
- Chemical compounds must have a net
charge of zero.
1. Both cations and anions must be present.
2. The number of cations and anions must
be such that the net charge is zero.
Writing Formulas for Ionic
Compounds
Charge must
equal zero for
each compound.
1
1-
Na Cl
2
1
2
1+ & 1- = 0
Ca F
2+ & 2- = 0
3
2
6+ & 6- = 0
23
Al S
COMPOUNDS FORMED
FROM IONS
CATION + ANION --->
COMPOUND
Na+ + Cl- --> NaCl
A neutral compound
requires equal
number of (+)
and (-) charges.
Chemical Bonds
(continued)
Covalent bonding: results from
atoms sharing electrons.
Molecule: a collection of covalentlybonded atoms.
H2O
C12H22O11
Common Names
sugar of lead
blue vitriol
quicklime
Epsom salts
milk of magnesia
gypsum
laughing gas
lead(II) acetate
copper(II) sulfate
calcium oxide
magnesium sulfate
magnesium hydroxide
calcium sulfate
dinitrogen monoxide
Common Names - Exceptions
H2O = water, steam, ice
NH3 = ammonia
CH4 = methane
NaCl = table salt
C12H22O11 = table sugar
Types of Cations
Type I Cations:
 only
one charge
 Group I ions
 Group II ions
 Aluminum
 Cadmium
 Silver
 Zinc
 Memorize Table 5.1,
page 129
Type II Cations:
•more than one charge
•transition elements
•elements under the
stairstep
•Memorize Table 5.2,
page 133
Metal Cations
Type I
 Metals
that can only have one possible charge
 Determine charge by position on the Periodic
Table
Type II
 Metals
that can have more than one possible
charge
 Determine metal cation’s charge from the
charge on anion
Naming Compounds
Binary Ionic
Compounds:
1. Cation first, then anion
2. Monatomic cation = name of the element
Ca2+ = calcium ion
3. Monatomic anion = root + -ide
Cl = chloride
CaCl2 = calcium chloride
Naming Compounds
(continued)
Binary Ionic Compounds (Type II):
-
metal forms more than one cation
use Roman numeral in name
CuCl2 Cu2+ is cation
CuCl2 = Copper (II) chloride
Cupric chloride
Naming Compounds
(continued)
Binary compounds (Type III):
- Compounds between two nonmetals
- First element in the formula is named first.
- Second element is named as if it were an
anion.
- Use prefixes (Table 5.3 on page 137).
- Never use mono- for the first element.
P2O5 = diphosphorus pentoxide
Prefixes
Subscript
1
2
3
4
5
6
7
8
Prefix
mono(not used on first nonmetal)
ditritetrapentahexaheptaocta-
Drop last “a” in the prefix if the name begins with vowel
Figure 5.1: A flow chart for naming binary
compounds.
Common Nomenclature
Mistakes
Compounds:
Polyatomic ions:
SO3 --Sulfur trioxide
NO2 -- Nitrogen
dioxide
NO3 -- Nitrogen
trioxide
NH3 -- Ammonia
SO32- -- Sulfite ion
NO21- -- Nitrite ion
NO31- -- Nitrate ion
NH41+ --Ammonium
ion
MOLECULAR FORMULAS
Formula for glycine is C2H5NO2
In one molecule there are
2
C atoms
5 H atoms
1 N atom
2 O atoms
Molecular Modeling
H H O
H N C C O H
H
Ball & stick
Drawing of glycine
Space-filling
POLYATOMIC IONS
Groups of atoms with a charge.
MEMORIZE the names and formulas
in Table 5.4, page 142.
Table 5.4: Names of Common Polyatomic Ions
Patterns for Polyatomic Ions
-ate ion
 chlorate
= ClO3-
-ate ion plus 1 O  same charge, per- prefix
 perchlorate
= ClO4-
-ate ion minus 1 O  same charge, -ite suffix
 chlorite
= ClO2-
-ate ion minus 2 O  same charge, hypo- prefix, -ite
suffix
 hypochlorite
= ClO-
Some Common
Polyatomic Ions
NH4+ ammonium ion One of the
few common polyatomic
cations
Some Common
Polyatomic Ions
CO32- carbonate ion
HCO3- bicarbonate ion
- hydrogen carbonate ion
Some Common Polyatomic
Ions
2- sulfate
SO4
ion
SO32- sulfite ion
Some Common
Polyatomic Ions
NO3- nitrate ion
NO2
- nitrite
ion
Figure 5.2: Overall strategy for naming chemical
compounds
NOMENCLATURE OF COMPOUNDS
Binary -- 2 elements
Ternary -- (3 elements) - Ionic
Type I - Ionic
(Type I metal + nonmetal)
Group I, II, Al+3, Ag1+,
Cd2+, & Zn2+
NaCl -- Sodium Chloride
Type II - Ionic
(Type II metal + nonmetal)
All other metals
Fe2S3 -- iron (III) sulfide
-- ferric sulfide
(metal ion + polyatomic ion)
Ca3(PO4)2 -- calcium phosphate
FeSO4 -- iron (II) sulfate
-- ferrous sulfate
Type III - covalent
(2 nonmetals)
CO2 -- carbon dioxide
Binary Acids
• made up of two elements -- hydrogen and a
nonmetal
• named by using:
prefix hydro + root of nonmetal + ic + acid
HCl -- hydrochloric acid
H2Se -- hydroselenic acid
Table 5.5: Names of Acids that Do Not Contain
Oxygen
Ternary Acids (oxyacids)
• contain three elements -- hydrogen,
nonmetal, and oxygen.
• most oxygen per + root of nonmetal + ic +
acid
• less oxygen root of nonmetal + ic + acid
• less oxygen root of nonmetal + ous + acid
• least oxygen hypo + root of nonmetal +
ous + acid
Ternary Acids
(continued)
HBrO4
HBrO3
HBrO2
HBrO
perbromic acid
bromic acid
bromous acid
hypobromous acid
H3PO4 phosphoric acid
H3PO3 phosphorous acid
H3PO2 hypophosphorus acid
Figure 5.3:
A flow chart
for naming
acids
Salt Nomenclature (continued)
Ternary salts ( metal and polyatomic ion)
name of positive ion + root of nonmetal + ate or ite
If the salt comes from an ic acid, change ic to ate.
H2CO3 carbonic acid
Na2CO3 sodium carbonate
H3PO4 phosphoric acid K3PO4 potassium phosphate
If the salt comes from an ous acid, change ous to ite.
H2SO3 sulfurous acid Li2SO3 lithium sulfite
HClO hypochlorous acid NaClO sodium
hypochlorite
Chemical Nomenclature
Name each of the following:
CuCl copper(I) chloride
HgO mercury(II) oxide
Fe2O3 iron(III) oxide
MnO2 manganese(IV) oxide
PbCl2 lead(II) chloride
CrCl3 chromium(III) chloride
cuprous chloride
mercuric oxide
ferric oxide
manganic oxide
plumbous chloride
chromic chloride
Chemical Nomenclature
Name each of the following:
P4O10
tetraphosphorus decoxide
N2O5
dinitrogen pentoxide
Li2O2
lithium peroxide
Ti(NO3)4
titanium(IV) nitrate
SO3
sulfur trioxide
SF6
sulfur hexafluoride
O2F2
dioxygen difluoride
Writing the Formulas from the
Names
For Type III compounds, use the prefixes to
determine the subscripts
For Type I, Type II, polyatomic Compounds
and Acids
Determine
the ions present
Determine the charges on the cation and anion
Balance the charges to get the subscripts
Determining the Charge on a Cation –
Au2S3
Determine the charge on the anion
Au2S3 - the anion is S, since it is in Group 6A, its charge
is -2
Determine the total negative charge
since there are 3 S in the formula, the total negative
charge is -6
Determine the total positive charge
since the total negative charge is -6, the total positive
charge is +6
Divide by the number of cations
since there are 2 Au in the formula & the total positive
charge is +6, each Au has a +3 charge