Chapter 2
Chemical Names
and Formulas
Naming Ions
IE
X + energy
Atom
• Cation
• Positive Ion
• Metal
• Loses Electrons
Cation t looks like a +
X+ + eIon
Cation
Naming Ions
EA
X + eAtom
X- + energy
Ion
Anion
• Anion
• Negative Ion
• Nonmetal
• Gains Electrons
Anion
n in middle stands for negative
Monoatomic Ion

Monatomic Ion – Ion that consists of a
single atom
• Cation
• Positive Ion
• Metal
• Loses Electrons
• Anion
• Negative Ion
• Nonmetal
• Gain Electrons
Rules for Ion Names/Symbols: Cation
Metals = use element name
= use symbol with superscript charge
= superscript is written in air
Alkali Metals
Transition Metals
Hydrogen
H+1
Silver
Ag+1
Lithium
Li+1
Gold
Au+1
Sodium
Na+1
Potassium K+1
Rules for Ion Names/Symbols: Cation
Metals = use element name
= use symbol with superscript charge
= superscript is written in air
Alkaline Earth Metals
Transition Metals
Magnesium Mg+2
Cobalt
Co+2
Calcium
Ca+2
Nickel
Ni+2
Strontium
Sr+2
Zinc
Zn+2
Barium
Ba+2
Rules for Ion Names/Symbols: Cation
Some metals have multiple charges.
Stock System uses Roman numerals.
Roman numerals = charge!!
1
I
6
VI
2
II
7
VII
3
III
8
VIII
4
IV
9
IX
5
V
10 X
.
Rules for Ion Names/Symbols: Cation
Copper (I)
Copper (II)
Iron (II)
Iron (III)
Lead (II)
Lead (IV)
Cu+1
Cu+2
Fe+2
Fe+3
Pb+2
Pb+4
Tin (II)
Sn+2
Tin (IV)
Sn+4
Manganese (II) Mn+2
Manganese (IV) Mn+4
Rules for Ion Names/Symbols: Anion
Nonmetals = use element name with ‘ide’
= use symbol with superscript charge
= superscript is written in air
Halogens
Fluorine
Fluoride F-1
Chlorine
Chloride Cl-1
Bromine
Bromide Br-1
Iodine
Iodide
I-1
Rules for Ion Names/Symbols: Anion
Nonmetals = use element name with ‘ide’
= use symbol with superscript charge
= superscript is written in air
Oxygen Family
Nitrogen Family
Oxygen Oxide O-2
Nitrogen Nitride N-3
Sulfur
Sulfide S-2
Phosphorus
Carbon Family
Phosphide P-3
Carbon Carbide C-4
Rules for Ion Names/Symbols:
Cation or Anion ?
Multiples can be cation or anion.
It depends on what other ion is around it.
Cation
Anion
Carbon C+4
Carbide C-4
Nitrogen N+5
Nitride
N-3
Phosphorus P+5
Phosphide P-3
Binary Compounds

Composed of 2 elements
• Can be either ionic or molecular
Binary Ionic Compounds

Consist of Ions
• Metallic Ions bonded to Nonmetal ions
•
or
Cations bonded to Anions
Writing Names for
Binary Ionic Compounds
Steps
1. Use ION names.
2. Write the CATION name.
3. Then write the ANION name.
For example,
NaCl becomes Sodium Chloride
MgBr2 becomes Magnesium Bromide
CuO becomes Copper (II) Oxide
Writing Formulas for
Binary Ionic Compounds
Steps
1. USE the IONS.
2. Write the symbol for the CATION.
3. Then write the symbol for the ANION.
4. Balance the charges to zero. The
subscripts denotes the number of ions
needed to balance the charges to zero.
Example
(Level 1)
Sodium Chloride
Na+1
Cl-1
NaCl
Example
(Level 1)
Magnesium Oxide
Mg+2
O-2
MgO
Example
(Level 1)
Aluminum Nitride
Al+3
N-3
AlN
Practice
1.
2.
3.
4.
5.
6.
7.
Potassium Iodide
Calcium Sulfide
Aluminum Phosphide
Gold Fluoride
Barium Oxide
Sodium Bromide
Strontium Sulfide
Example
(Level 2)
Lithium Oxide
Li+1 Li+1
O-2
Li2O
Example
(Level 2)
Calcium Fluoride
Ca+2
F-1 F-1
CaF2
Example
(Level 2)
Aluminum Iodide
Al+3
I-1 I-1 I-1
AlI3
Practice
1.
2.
3.
4.
5.
6.
7.
Potassium Oxide
Strontium Bromide
Aluminum Chloride
Gold Sulfide
Silver Nitride
Barium Fluoride
Calcium Iodide
Example
(Level 3)
Aluminum Sulfide
Al+3 Al+3
S-2 S-2 S-2
Al2S3
Example
(Level 3)
Tin (IV) Nitride
Sn+4 Sn+4 Sn+4
N-3 N-3 N-3 N-3
Sn3N4
Polyatomic Ions

Polyatomic Ions – Ions composed of
more than one atom
• Most end in ite or ate
Polyatomic Ions
Ammonium NH4+1
Cyanide
CN-1
Hydroxide OH-1
Nitrite
NO2-1
Sulfite
SO3-2
Phosphite PO3-3
Nitrate
Carbonate
Sulfate
Phosphate
NO3-1
CO3-2
SO4-2
PO4-3
Example
(Level 1)
Ammonium Chloride
NH4+1
Cl-
NH4Cl
Example
(level 1)
Barium Sulfate
Ba+2
SO4-2
BaSO4
Polyatomic Ions Only

When writing compounds if you need
more than one polyatomic ion you
must add parenthesis
Example
(Level 2)
Ammonium Sulfate
NH4+1 NH4+1
NH42SO4
SO4-2
(NH4)2SO4
Example
(Level 2)
Barium Hydroxide
Ba+2
BaOH2
OH-1 OH-1
Ba(OH)2
Practice
1.
2.
3.
4.
5.
6.
7.
Ammonium Phosphate
Calcium Hydroxide
Aluminum Nitrate
Magnesium Sulfate
Tin (IV) Carbonate
Strontium Sulfate
Barium Nitrate
Nomenclature
of Ionic Compounds
Steps
1. Use the names of the ions.
2. Write the metal first followed by the
nonmetal
3. The subscripts take care of themselves
Example
NaCl
Na+1
Cl-1
Sodium Chloride
Example
CaCl2
Ca+2
Cl-1 Cl-1
Calcium Chloride
Example
CuSO4
Cu+2
SO4-2
Copper (II) Sulfate
Practice
1.
2.
3.
4.
5.
6.
7.
NaI
(NH4)2SO4
MgBr2
Al2(CO3)3
CuO
Fe2O3
Ca3P2
Formula Writing and Nomenclature
Covalent (Molecular) Compounds
Steps
1. Write the first nonmetal symbol followed
by the second nonmetal symbol.
2. The Greek prefixes denote the
subscripts.
3. Do not need to balance the charges.
Greek Prefixes
for Molecular Compounds
1
2
3
4
5
Mono
Di
Tri
Tetra
Penta
6 Hexa
7 Hepta
8 Octa
9 Nona
10 Deca
Example
Carbon Dioxide
C
2 O
CO2
Example
Dinitrogen Monoxide
2
1
N
N2O
O
Practice
1.
2.
3.
4.
5.
6.
7.
Sulfur Dioxide
Trichlorine Tetraiodide
Pentaphosphorus Hexasulfide
Heptaoxygen Octaselenide
Nonafluorine Decanitride
Dinitrogen Pentoxide
Carbon Tetrachloride
Naming Molecular Compounds
Rules
1. Write the 1st element name.
2. Write the 2nd element name with an
ending of “ide”
3. Add Greek prefixes to both names. The
Greek prefix denotes the subscript.
4. Do not use a mono on the 1st element
name.
Example
SiO2
Silicon
Di
Oxygen
Silicon Dioxide
ide
Example
P4F6
ide
Tetra Phosphorus Hexa Fluorine
Tetraphosphorus Hexafluoride
Practice
1.
2.
3.
4.
5.
6.
7.
CO
Si2F
O3Br7
IS
ON4
F4H3
P7S9
Halogenated Oxyanions
Name:
Prefix
Suffix
Hypo root ite
root ite
root ate
Per root ate
Example:
Chlorine
Hypochlorite ClO-1
Chlorite ClO2-1
Chlorate ClO3-1
Perchlorate ClO4-1
Try Bromine and Iodine.
Polyatomic Oxyacids
Example:
Example:
Chlorine
Chlorine
Hypochlorite ClO-1 Hypochlorous acid
Chlorite ClO2-1
Chlorous acid
Chlorate ClO3-1
Chloric acid
Perchlorate ClO4-1 Perchloric acid
HClO
HClO2
HClO3
HClO4
Binary Acids
Formula: Hydrogen w Halogen
Name: Hydro+Root+ic Acid
HCl Hydrochloric Acid
HBr Hydrobromic Acid
HI
Hydroiodic Acid
HF Hydrofluoric Acid
Alkanes





Methane
Ethane
Propane
Butane
Pentane
Alcohols





Methanol
Ethanol
Propanol
Butanol
Pentanol
Other functional groups?








Alcohols
Ethers
Aldehydes
Ketones
Carboxylic acid
Ester
Amine
Amide
Formula weights/Molar Mass

The sum of atomic
weights for a
compound (in amu)

The number of
grams in one mole
of a substance (in g)
Lewis Dot Structures



For atoms
For ionic
compounds
For molecular
compounds
LDS: Neutral Molecules




Draw the dot structures of each atom
Share one atom for each element (to make
a single bond between each element)
Count electrons around each atom
If octets are incomplete, share more
electrons between atoms
LDS: Negatively Charged
Molecules


Repeat procedure for uncharged molecules
Add one electron for each negative charged
atom
LDS: Positively charged
molecules

Same procedure as negative… except
remove one electron
Web Practice Site

http://www.fernbank.edu/Chemistry/nom
en.html