Naming Compounds
Ionic Compounds :
metals and non-metals
Molecular Compounds :
combination of non-metals
Acids Names
Naming Compounds
1.
2.
A binary compound is one made of two
different 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.
Points to remember about naming a compound from its formula
1. The order for names in a binary compound is first the
cation, then the anion.
2. Use the name of cation with a fixed oxidation state
directly from the periodic table.
3. The name of the anion will be made from the root of the
element's name plus the suffix "-ide."
Binary – Ionic Compounds
Example 1: Write the name of the following formula:
MgBr2
Step #1 - Look at first element and name it.
Result of this step = magnesium.
Step #2 - Look at second element. Use root of its
full name ( which is brom-) plus the ending
"-ide." Result of this step = bromide.
Magnesium bromide.
Note the presence of the subscript does not play a role in this name.
Example 2: Write the name of the following formula:
Na2S
1st name: metal name – sodium
2nd name: root of second element – sulf and ends in
“ide” – sulfide.
Sodium sulfide.
Example 3: Write the name of the following formula:
HCl
1st name: name of element – hydrogen
2nd name: root of second element – chlor and ends in
“ide” – chloride.
Hydrogen chloride
Ternary Ionic Compounds
Formulas with 3 or more elements: metals
and polyatomic ions or Polyatomic &
Polyatomic
1st name: name of the element (metal) or
polyatomic ion (NH4).
2nd name: name of the polyatomic ion.
Ex: Na2SO4 : sodium sulfate
NH4NO3: Ammonium Nitrate
Binary Ionic Multi – Charged Ions
There are some elements with more than
one possible charge. Ex: Copper +1, +2
How would you name or recognize which is
used in the formula and name?
One of two systems is used. Stock System
or Traditional.
Stock System of Naming
Compounds
Roman numeral matching the charge is used.
Ex: Cu +1, copper I
Cu +2, copper II
Cu+2 N03-: Cu(N03)2 copper II nitrate
Cu+ NO3- : CuNO3 copper I nitrate
Traditional Naming of Ionic
Compounds
Traditional naming of ionic compounds used the
latin names or some common names and a
suffix corresponding to the charge as follows.
Copper: Cuprum
Cu+1: cuprous Cu+2: cupric
The ous ending was used with the lower charged
ion.
The ic ending was used with the higher charged
ion.
Tradition Names
Ferrous Nitrate : Iron +2, nitrate: Fe(NO3)2
Plumbic Chloride: Lead +4, chlorine: PbCl4
Latin Names:
Ferrum – Iron, Cuprum – Copper,
Stannum – Tin, Hydragryum – Mercury
Common Names: Any element with more
than one possible charge: lead, mercury,
tin, etc.
Molecular Compounds
Combinations of non-metals.
The use of prefixes are used in conjunction with roots and
suffixes.
Number
Prefix
1
mono
2
di
3
tri
4
tetra
5
penta or pent
6
hexa
7
hepta
8
octa
9
nana
10
deca
Naming Molecular Compounds
Molecular Compounds: combination of nonmetals.
Binary Molecular
Use of prefixes to refer to number of atoms
of each element.
Binary Molecular Compounds
1st name: If the 1st element has no
subscript use it’s name. If it does have a
subscript use a prefix which represents
that number plus the name of the 1st
element.
Ex: CO2 : carbon
As2S3: diarsenic
1.
2nd name: use a prefix to match the
subscript of the second element plus the
root of the second element and ends in
“ide”.
Ex: CO2: dioxide
As2O3: trioxide
Complete names: CO2: carbon dioxide
As2O3: diarsenic trioxide
2.
Naming Acids
All acid formulas begin with Hydrogen as
the first element. If the material is an
acid an (aq) will follow the formula.
Meaning aqueous solution of.
There are two systems of acid names
1. Binary – two elements.
2. Ternary – three or more elements.
Binary Acid Names
All binary acid names will follow the
following pattern:
1st name: Begins with the prefix Hydro
+ Root of the second element and ends in
“ic”.
2nd name: Acid
Ex: HF – Hydrofluoric Acid,
HBr – Hydrobromic Acid
Ternary Acid Names
Ternary acid names come from the roots of the
polyatomic ion.
The endings are changed as follows:
ate is changed to ic (higher # of oxygens, greater)
ite is changed to ous (lower # of oxygens)
Ex: H2SO4 – Sulfuric Acid
H2SO3 – Sulfurous Acid
If only one polyatomic ion in group, the name of the
acid is the root of the polyatomic ion and ending
in “ic”.
Ex: HC2H3O2 – Acetic Acid