Chapter 5
Nomenclature
Polyatomic ions
PolyAtomicIonparticle
polyatomic ion-a charged particle consisting of
atoms which function as a
Name
Formula
Name
Formula
Acetate
CH3COO- or C2H3O2-
Nitrate
NO3-
Ammonium
NH4+
Permanganate
MnO4-
Carbonate
CO32-
Peroxide
O22-
Chromate
CrO42-
Phosphate
PO43-
Cyande
CN-
Sulfate
SO42-
Dichromate
Cr2O72-
Thiosulfate
S2O32-
Hydroxide
OH-
Bisulfate
HSO4-
Chlorate
ClO3-
Iodate
IO3-
Bicarbonate
HCO3-
Bromate
BrO3-
Underlined ions are oxyanions with multiple forms
Adding hydrogen
When adding hydrogen to an ion, the number of hydrogen atoms added is indicated with a
prefix (di, tri) and the charge becomes more positive
CO32- is carbonate
 HCO3- is
carbonate (or
PO43- is phosphate
 HPO42- is
 H2PO4- is
phosphate
phosphate
)
Additional Notes
Oxyanions
Oxyanions—polyatomic ions which have an element bonded to some number of oxygen atoms
Nitrate, Chlorate, Iodate, Sulfate, Phosphate
If you add an oxygen to the base, the prefix
is
added

Chlorate is ClO3
is ClO4If you remove one oxygen from the base the suffix –ate is changed to

is ClO2If you remove another oxygen from the base, the prefix
is added

is ClO-
Additional Notes
Quizlet to help you study: http://quizlet.com/_90p8y
Binary compounds
Binary Compound-a compound containing only 2 elements
  Binary Compounds containing a metal and a nonmetal are
o  Type I ionic compound-a compound   containing a
possible charge and a
o  Type 2 ionic compound-a compound   containing a
possible charge and a
  usually metals not in groups

common exceptions:
and
o  Type 3 binary compound-a compound  containing 2
 Additional Notes
Naming Type 1 binary compounds
1. The
is always named first and the
second
with only
with more than 1
2. A simple cation (obtained from a single atom) takes its name from the name of the
element.
 Na+ is just called a
ion
2+
 Mg is called a
ion
3. A simple anion is named by taking the first part of the element name (the root) and
adding
  Cl- is called a
ion
  O2- is called an
ion
Additional Notes
NaCl
KI
CaS
CsBr
MgO
KCl
ZnS
CaBr2
BaH2
Al2S3
Remember writing formulas with ionic compounds? Try these
rubidium oxide
magnesium telluride
sodium nitride
Type II Ionic Compounds
1. Iron can have 2 different charges,
and
 Is Iron chloride FeCl2 or FeCl3?
2. We need to know the
on the cation from the name
3. We use roman numerals to indicate the
on the cation
2+
  If iron is Fe then the ion would be iron
  If iron is Fe3+ then the ion would be iron
4. The charge is determined by what it is bonded to
  remember:
net charge!
Additional Notes
Determining the charge on the cation

FeCl2 if each chlorine has a 1- charge then there are 2 (1-) charges
o
o Iron has a
charge so the name is

What is the charge and name of a gold ion in Au2O3?
o
o  charge =
o  name =
Additional Notes
Naming type II ionic compounds
1. Write the
first and the
second
2. Include a roman numeral on the cation to indicate the
(not the number of ions!)
3. Write the root of the anion and end with
CoCl3
CuI
SnBr4
HgCl2
PbS
Additional Notes
Writing formulas is the same as type I except you look at the roman numeral to find the charge
on the cation
cobalt (II) chloride
titanium (IV) oxide
lead (II) nitride
Type III Binary Compounds
Type III binary compounds contain only nonmetals
Rules for naming Type III binary compounds
1. The
element in the formula is named  first and the
element name is used
2. the second element is next and ends with
3.
are used to denote the number of  atoms present.
You need to memorize these prefixes!
a. Monob. Dic. Trid. Tetrae. Pentaf. Hexag. Heptah. Octai. Nonaj. Deca 4. The prefix
is never used on the first  element
5. If the name of an
is awkward with the prefix, drop the last letter of the prefix
  monooxide becomes
Name the following:
BF3
NO
N2O5
Additional Notes
Common Names
A couple of compounds don't use their systematic name
H2O
, not dihydrogen monoxide
NH3
, not nitrogen trihydride
You just gotta know these!
Additional Notes
Writing formulas of Type III compounds
o Just do what the prefixes tell you to do!
o carbon monoxide=1 carbon, 1 oxygen=CO
nitrogen dioxide
selenium hexafluoride
dinitrogen monoxide
diiodine heptoxide
Naming compounds with polyatomic ions
Name the same as type I and II including the name of the polyatomic ions with no changes
Na2SO4
KH2PO4
K2SO3
Mn(OH)2
NH4ClO4
Fe(NO3)3
NH4Cl
Mg(IO2)2
CuOH
Al(C2H3O2)3
Writing formulas with polyatomic ions
Write the formula just as you do with type I and II compounds. If there are more than 1
polyatomic ion, it must be in
copper (II) nitrate
lead (II) carbonate
potassium bisulfate
ammonium iodide
sodium cyanide
titanium (IV) hypochlorite
Additional Notes
Naming Acids
Acid-a substance that releases hydrogen ions in solution
1. Binary acid—2 elements: H+?
o Hydro____ic acid
o  HCl=
o  H2S=
2. Oxyacid—H with oxyanion
a.  Ending of ion is
=___ic acid
  H2SO4 = sulfate ion=
  HNO3= nitrate ion=
b.  Ending of ion is
=___ous acid
  HNO2=nitrite ion=
  HClO=hypochlorite ion=
Additional Notes
HBr
HClO4
HIO4
HF
H3PO4
H2SO3
Formulas of Acids
Hydrofluoric acid
Phosphorous acid
Nitric Acid
Bromic Acid
Hydrosulfuric acid
Hydrates
A hydrate is an ionic compound with some number of water molecules
attached to the
ions
The water is trapped during crystallization and is therefore part of the compound and
chemical
It is indicated using a
between the ionic formula and the water(s)
To name hydrates, simply name the ionic compound as a type 1 or 2 compound and then
indicate how many hydrates using the same prefixes we used for type 3
Formulas of Hydrates
To write formulas of hydrates write the ionic formula, add a dot, and write the number of water
molecules attached
Cobalt (II) chloride hexahydrate
Zinc nitrate tetrahydrate