Nomenclature
C2H3O2acetate ion
HC2H3O2
Acetic Acid
Forms of Chemical Bonds
Most bonds are
somewhere in
between ionic
and covalent.
• There are 3 forms
bonding atoms:
• Ionic—complete transfer
of 1 or more electrons
from one atom to another
(one loses, the other
gains)
• Covalent—some valence
electrons shared between
atoms
• Metallic– holds atoms of
a metal together
NAMING COMPOUNDS
• Your ability to name
compounds and write
formula’s hinges on your
ability to recognize
whether a compound is
Ionic or Molecular.
COMPOUNDS
FORMED FROM
IONS
CATION +
ANION --->
COMPOUND
Na+ + Cl- --> NaCl
A neutral compound
requires
equal number of +
and - charges.
Naming Monatomic Ions
• Monatomic cations are identified
simply by the element’s name.
• Examples:
K+ is called the potassium cation
Mg2+ is called the magnesium
cation
Naming Monatomic Ions
• For monatomic anions, the ending
of the element’s name is dropped,
and the ending –ide is addend to
the root name. Examples:
F- is called the fluoride anion
N3+ is called the nitride anion
Monatomic Ions
Two Types of Compounds
Smallest
piece
Types of
elements
State
Melting
Point
Ionic
Molecular
Formula Unit
Molecule
Metal and
Nonmetal
Nonmetals
solid
Solid, liquid
or gas
High >300ºC
Low <300ºC
Naming Binary Ionic
Compounds
• Binary ionic compounds involve combining
the manes of the cation and anion that
makes up the compound.
• The name of the cation is given first,
followed by the name of the anion
– Example:
Aluminum Oxide
Al2O3
Name of cation
Aluminum
Name of anion
Oxide
Naming Binary Ionic
Compounds

Examples:
NaCl sodium chloride
ZnI2
zinc iodide
Al2O3 aluminum oxide
Learning Check
Complete the names of the following binary compounds:
Na3N
nitride
sodium __________________
KBr
bromide
potassium________________
Al2O3
oxide
aluminum ________________
MgS
Magnesium sulfide
_________________________
Writing the formulas of
Binary Ionic Compounds
1. Find the charge for each atom.
(Remember: if you don’t
see a number, then it is
Mg2+
Cl-
implied to be a 1)
2. Switch the numbers on
the elements.(you want to
balance the positive charges
and the negative charges.)
Mg2+
Cl-
Writing the formulas of
Binary Ionic Compounds
3. Write your formula.
(Remember + and - signs
Go away.)
MgCl2
There is one catch! If the charges have the same
magnitude, then the ions will form a compound
with a 1:1 ratio.
+2
Mg
2O
MgO
Learning Check
Write the correct formula for the compounds
containing the following ions:
1. Na+, S2a) NaS
b) Na2S
c) NaS2
2. Al3+, Cla) AlCl3
b) AlCl
c) Al3Cl
3. Mg2+, N3a) MgN
b) Mg2N3
c) Mg3N2
Stock system of Nomenclature
• Transition metals (the d-block elements) can
form two or more cations with different
charges.
• These elements REQUIRE Roman Numerals
because they can have more than one possible
charge:
anything except Group 1A, 2A, Ag, Zn, Cd, and Al
– Examples:
Fe2+
Fe3+
Iron (II)
Iron (III)
Learning Check
Complete the names of the following binary
compounds with variable metal ions:
FeBr2
II bromide
iron (_____)
CuCl
I
copper (_____)
chloride
SnO2
Fe2O3
oxide
Tin
IV ) ______________
___(_____
Iron
(III)
oxide
________________________
Hg2S
Mercury (I) sulfide
________________________
Polyatomic Ions
NO3nitrate ion
NO2nitrite ion
Naming Oxyanions
• Oxyanion: polyatomic ions that contains oxygen.
• Some elements can combine with oxygen to form
more than one type of oxyanion.
Example: nitrogen can form NO3- or NO2-.
The name of the ion with the greater number of oxygen
atoms ends in –ate. The name of the ion with the
smaller number of oxygen atoms ends in –ite.
NO3
Nitrate
NO2
Nitrite
Naming Oxyanions
• In this example, an anion that has one
fewer oxygen atom than the –ite anion
has is given the prefix hypo-. An anion
that has one more oxygen atom that the
–ate anion has is given the prefix per-.
ClOhypochlorite
ClO2chlorite
ClO3chlorate
ClO4perchlorate
Ternary Ionic Nomenclature
(Polyatomic Ions)
• Ionic compounds involving polyatomic ions
are named in the same way as binary
compounds.
• The name of the cation is given first
followed by the name of the anion
• Example
Al2(SO4)3 Aluminum sulfate
NH4Cl
Ammonium chloride
Learning Check
Na2CO3
MgSO3
MgSO4
Ca(HCO3)2
CaCO3
Ca3(PO4)2
sodium carbonate
magnesium sulfite
magnesium sulfate
calcium bicarbonate
calcium carbonate
calcium phosphate
Ternary Ionic Nomenclature
Writing Formulas
1
. Find the charge for each atom.
(Remember: if you don’t
see a number, then it is
+
K
2SO4
implied to be a 1. It helps to circle the ions)
2. Switch the numbers on
K+
SO42the elements.(you want to
balance the positive charges
and the negative charges.)
Ternary Ionic Nomenclature
Writing Formulas
3. Write your formula.
(Remember + and - signs
Go away.)
K2SO4
There is one catch! If you need more than one of the
polyatomic ions to make the charge neutral, you must
enclose it in parenthesis.
Ca+2 CH3COOCa(CH3OO)2
Ternary Ionic Nomenclature
Sodium Sulfate
Na+ and SO4 -2
Na2SO4
Iron (III) hydroxide
Fe+3 and OHFe(OH)3
Ammonium carbonate
NH4+ and CO3 –2
(NH4)2CO3
Learning Check
1. aluminum nitrate
a) AlNO3
b) Al(NO)3
c) Al(NO3)3
2. copper(II) nitrate
a) CuNO3
b) Cu(NO3)2
c) Cu2(NO3)
3. Iron (III) hydroxide
a) FeOH
b) Fe3OH
c) Fe(OH)3
4. Tin(IV) hydroxide
a) Sn(OH)4 b) Sn(OH)2
c) Sn4(OH)
Mixed Practice!
Name the following:
Sodium oxide
1. Na2O
Calcium carbonate
2. CaCO3
Lead (IV) sulfide
3. PbS2
Tin (II) nitride
4. Sn3N2
Copper (I) phosphate
5. Cu3PO4
6. HgF2
Mercury (II) fluoride
Naming Molecular Compounds
CO2 Carbon dioxide
CH4 methane
BCl3
boron trichloride
All are formed
from two or
more
nonmetals.
Molecular (Covalent) Nomenclature
1. Less electronegative
atom comes first. It is
given a prefix only it is
contributes more than
one atom to the
molecule.
In general, the order of nonmetals in molecular
names and formulas (which one comes first):
C, P, N, H, S, I, Br, Cl, O, F
Molecular (Covalent)Nomenclature
2. The second element is named by
combining:
 a prefix indicating the number
of atoms contributed by the
element .
 The root word of the second
element.
 The ending changes to –ide.
Molecular (Covalent)Nomenclature
3. The o or a at the end of a prefix is
dropped if the main word starts
with a vowel.
P4O10
tetraphosphorus decoxide
Molecular Nomenclature Prefixes
PREFIX
monoditritetrapentahexaheptaoctanonadeca-
NUMBER
1
2
3
4
5
6
7
8
9
10
Learning Check
CO
mon
carbon ______oxide
CO2
dioxide
carbon _______________
PCl3
phosphorus_______chloride
tri
CCl4
tetra
carbon ________chloride
N2O
di
mon
_____nitrogen
_____oxide
Learning Check
1.
P2O5
a) phosphorus oxide
b) phosphorus pentoxide
c) diphosphorus pentoxide
2.
Cl2O7
a) dichlorine heptoxide
b) dichlorine oxide
c) chlorine heptoxide
3.
NF3
a) nitrogen trifluoride
b) mononitrogen fluoride
c) nitrogen difluoride
Acid Nomenclature
• Acid: usually refers to a solution in water of an
acid compound rather that the acid itself.
– Formulas usually begin with ‘H’.
– In binary acids, there are only two elements that make
up the molecule. Example HF, hydrofluoric acid
– In ternary acids are ALL aqueous and are made up of
at least one polyatomic ion.
Example :H2SO4 – sulfuric acid
Acid Nomenclature
Anion
Ending
No Oxygen
w/Oxygen
Acid Name
-ide
hydro-(stem)-ic acid
-ate
(stem)-ic acid
-ite
(stem)-ous acid
An easy way to remember which goes with which for those
that contain oxygen…
“In the cafeteria, you ATE something ICky”
Learning Check
• HBr
(aq)
• No oxygen, -ide

hydrobromic acid

carbonic acid

sulfurous acid
• H2CO3
• Has oxygen, -ate
• H2SO3
• Has oxygen, -ite
Learning Check
• hydrofluoric acid
• 2 elements
 H+ F-
 HF (aq)
 H+ SO42-
 H2SO4
 H+ NO2-
 HNO2
• sulfuric acid
• 3 elements, -ic
• nitrous acid
• 3 elements, -ous
The End