Nomenclature:
Naming Chemicals
PO43phosphate ion
HC2H3O2
Acetic Acid
C2H3O2acetate ion
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Before naming….
 Some things you MUST know to be
successful…. You really need to commit
these things to memory
Metals
Conductors
 Lose electrons
 Malleable and ductile

Nonmetals



Brittle or gases
Gain electrons
Covalently bonds to each
other
Semi-metals or Metalloids
•Characteristics of both
metals and nonmetals
•Metallic character
increases as go down PT
Alkali Metals
Alkaline Earth Metals
Transition metals
Inner Transition Metals
Halogens
Noble Gases
Ions
Atoms or groups of atoms with a charge.
 Cations- positive ions - get by losing
electron(s).
 Anions- negative ions - get by gaining
electron(s).
 Ionic bonding- held together by the opposite
charges.
 Ionic solids are called salts.

+1
Common Ions of Elements
+3
+2
Variable, always +
4 -3 -2 -1
+/-
Predicting Charges on Monatomic Ions
KNOW THESE !!!!
+1 +2
-3 -2 -1
Cd+2
0
Polyatomic Ions




Groups of atoms that
have a charge.
Ions that contain
covalently bonded
atoms
* NO3- :nitrate ion
* NO2- :nitrite ion
Yes, you have to
memorize them.
List in your yellow
folder: memorize this
list!!!!
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, hypoprefix, -ite suffix
 hypochlorite = ClO-
Polyatomic Ions
You can make additional polyatomic
ions by adding a H+ to the ion!
CO3 -2 is carbonate
HCO3– is hydrogen carbonate
H2PO4– is dihydrogen phosphate
HSO4– is hydrogen sulfate
Forms of Chemical Bonds
 There are 3 forms bonding atoms:
 Ionic—complete transfer of 1 or more
electrons from one atom to another
(one loses, the other gains)
 metal and non metal or polyatomics
 The resulting cation and anion are
attracted to each other by electrostatic
forces.
Most bonds are
somewhere in
between ionic
and covalent.
 Covalent—some valence electrons
shared between atoms
 we will just learn the rules for 2 nonmetals.
 Metallic – holds atoms of a metal
together
COMPOUNDS
FORMED
FROM IONS
CATION +
ANION --->
COMPOUND
Na+ + Cl- -->
NaCl
A neutral compound
requires
equal number of +
and - charges.
IONIC COMPOUNDS
NH4
+
Cl
ammonium chloride, NH4Cl
Ionic compounds
If the cation is monatomic- Name the metal
(cation) just write the name.
 If the cation is polyatomic- name it.
 If the anion is monatomic- name it but
change the ending to –ide.
 If the anion is poly atomic- just name it
 Practice.

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 Binary Ionic
Compounds

Examples:
NaCl
sodium chloride
ZnI2
zinc iodide
Al2O3
aluminum oxide
Learning Check
Complete the names of the following binary
compounds:
sodium nitride
Na3N
KBr
potassium bromide
Al2O3
aluminum oxide
MgS
magnesium sulfide
Monatomic Ions
These are from the periodic
table that you saw a few
slides ago!
Transition Metals
Elements that can have more than one possible
charge MUST have a Roman Numeral to
indicate the charge on the individual ion.
1+ or 2+
Cu+, Cu2+
copper(I) ion
copper (II) ion
2+ or 3+
Fe2+, Fe3+
iron(II) ion
iron(III) ion
Names of Variable Ions
These elements REQUIRE Roman Numerals
because they can have more than one possible
charge:
anything except Group 1A, 2A, Ag, Zn, Cd, and Al
(You should already know the charges on these!)
Or another way to say it is: Transition metals and the metals in groups 4A and
5A (except Ag, Zn, Cd, and Al) require a Roman Numeral.
FeCl3
CuCl
SnF4
PbCl2
Fe2S3
(Fe3+)
(Cu+ )
(Sn4+)
(Pb2+)
(Fe3+)
iron (III) chloride
copper (I) chloride
tin (IV) fluoride
lead (II) chloride
iron (III) sulfide
Special names Cations
Some Type II cations have a name using
the “old” system as well as the “new
system”.
The old system, still widely used, adds to
the root or stem of the Latin name of the
metal the suffixes –ous and –ic. These
represent the lower and higher charges
respectively.
Old Names for Type II ions
Ion
Fe2+
Old System
Ferrous
New System
Iron (II)
Fe3+
Ferric
Iron (III)
Cu+
Cuprous
Copper (I)
Cu2+
Cupric
Copper (II)
Sn2+
Stannous
Tin (II)
Sn4+
Stannic
Tin (IV)
Examples of Older Names of Cations
formed from Transition Metals
(you do not have to memorize these)
Learning Check
Complete the names of the following binary
compounds with variable metal ions:
FeBr2
iron (II) bromide
CuCl
copper (I) chloride
SnO2
tin (IV) oxide
Fe2O3
iron (III) oxide
Hg2S
mercury (I) sulfide
Naming Ternary Compounds
 Contains at least 3 elements
 There MUST be at least one polyatomic ion
(it helps to circle the ions)
 Examples:
NaNO3
Sodium nitrate
K2SO4
Potassium sulfate
Al(HCO3)3
Aluminum bicarbonate
or
Aluminum hydrogen carbonate
Learning Check
Match each set with the correct name:
1. Na2CO3
a) magnesium sulfite
MgSO3
b) magnesium sulfate
MgSO4
c) sodium carbonate
2.
Ca(HCO3)2
CaCO3
a) calcium carbonate
b) calcium phosphate
Ca3(PO4)2
c) calcium bicarbonate
 Match each set with the correct name:
 1.


Na2CO3
MgSO3
MgSO4
 2 . Ca(HCO3)2

CaCO3

Ca3(PO4)2
a) sodium carbonate
b) magnesium sulfite
c) magnesium sulfate
a) calcium bicarbonate
b) calcium carbonate
c) calcium phosphate
Mixed Practice!
Name the following:
1. Na2O
2. CaCO3
3. PbS2
4. Sn3N2
5. Cu3PO4
6. HgF2






sodium oxide
calcium carbonate
lead (IV) sulfide
tin (II) nitride
copper (I) phosphate
mercury (II) fluoride
Covalent compounds
Two words, with prefixes.
 Prefixes tell you how many.
 First element whole name with the
appropriate prefix, except mono.
 Second element, -ide ending with
appropriate prefix.
 Practice

Molecular Nomenclature
Prefixes
PREFIX
monoditritetrapentahexaheptaoctanonadeca-
NUMBER
1
2
3
4
5
6
7
8
9
10
Molecular Nomenclature:
Examples
 CCl4
 carbon tetrachloride
 N 2O
 dinitrogen monoxide
 SF6
 sulfur hexafluoride
More Molecular Examples
 arsenic trichloride
 AsCl3
 dinitrogen pentoxide
 N2O5
 tetraphosphorus decoxide
 P4O10
Learning Check
Fill in the blanks to complete the following
names of covalent compounds.
CO
carbon monoxide
CO2
carbon dioxide
PCl3
phosphorus trichloride
CCl4
carbon tetrachloride
N2O
dinitrogen monoxide
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.
Cl2
a) chlorine
b) dichlorine
c) dichloride
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.
Cl2
a) chlorine
b) dichlorine
c) dichloride
Mixed Review
Name the following compounds:
1.
CaO
2.
3.
a) calcium oxide
c) calcium (II) oxide
b) calcium(I) oxide
d) calcium monoxide
SnCl4
a) tin tetrachloride
c) tin(IV) chloride
b) tin(II) chloride
N2O3
a) nitrogen oxide
c) nitrogen trioxide
b) dinitrogen trioxide
Mixed Review
Name the following compounds:
1.
CaO
2.
3.
a) calcium oxide
c) calcium (II) oxide
b) calcium(I) oxide
d) calcium monoxide
SnCl4
a) tin tetrachloride
c) tin(IV) chloride
b) tin(II) chloride
N2O3
a) nitrogen oxide
c) nitrogen trioxide
b) dinitrogen trioxide
Overall strategy for naming
chemical compounds.
A flow chart for naming binary
compounds.
Common Names
 A lot of chemicals have common
names as well as the proper
IUPAC name.
 Chemicals that should always be
named by common name and
never named by the IUPAC
method are:
 H2O water, not dihydrogen
monoxide
 NH3 ammonia, not nitrogen
trihydride
Mixed Practice
1.
2.
3.
4.
5.
6.
7.
8.
9.
BaI2
P4S3
Ca(OH)2
FeCO3
Na2Cr2O7
I2O5
Cu(ClO4)2
CS2
B2Cl4
1.
2.
3.
4.
5.
6.
7.
8.
9.
Barium iodide
Tetraphosphrus trisulfide
Calcium hydroxide
Iron (II) carbonate
Sodium dichromate
Diiodine pentoxide
Copper (II) perchlorate
Carbon disulfide
Diboron tetrachloride
Acid Nomenclature
 Acids
 Compounds that form H+ in water.
 Formulas usually begin with ‘H’.
 In order to be an acid instead of a gas,
binary acids must be aqueous (dissolved in
water)
 Ternary acids are ALL aqueous
 Two types of acids:
Oxyacids
Non-oxyacids
Naming acids






If the acid doesn’t have oxygen
add the prefix hydrochange the suffix -ide to -ic acid
HCl
Hydrochloric acid
H2S
Hydrosulfic acid
HCN
Hydrocyanic acid
Naming acids
 If the formula has oxygen in it
 write the name of the anion, but change
 ate to -ic acid
 ite to -ous acid
 Watch out for sulfuric and sulfurous
 H2CrO4
 HMnO4
 HNO2
Chromic acid
Manganic acid
Nitrous acid
Acid Nomenclature
Anion
Ending
Binary 
Acid Name
-ide
hydro-(stem)-ic acid
-ate
(stem)-ic acid
-ite
(stem)-ous acid
Ternary
An easy way to remember which goes with which…
“In the cafeteria, you ATE something ICky”
Acid Nomenclature
 HBr (aq)
 2 elements, -ide

hydrobromic acid

carbonic acid

sulfurous acid
 H2CO3
 3 elements, -ate
 H2SO3
 3 elements, -ite
Acid
Name
HNO3
Nitric acid
HNO2
Nitrous acid
H2SO4
Sulfuric acid
H2SO3
Sulfurous acid
H3PO4
Phosphoric acid
HC2H3O2
Acetic Acid
Acid Nomenclature
Flowchart
ACIDS
start with 'H'
2 elements
3 elements
hydro- prefix
-ic ending
no hydro- prefix
-ate ending
becomes
-ic ending
-ite ending
becomes
-ous ending
Acid Nomenclature
 hydrofluoric acid
 2 elements
 H+ F-
 HF (aq)
 sulfuric acid
 3 elements, -ic
 H+ SO42-  H2SO4
 nitrous acid
 3 elements, -ous
 H+ NO2-
 HNO2
Name ‘Em!
 HI (aq)
Hydroiodic acid
 HCl
Hydrochloric acid
 H2SO3
Sulfurous acid
 HNO3
Nitric acid
 HIO4
Periodic acid
Nomenclature Summary Flowchart
Formulas of Ionic
Compounds
Formulas of ionic compounds are determined
from the charges on the ions
atoms
Na
+
F
ions

sodium + fluorine
Charge balance:
Na+ +
F-  NaF
sodium fluoride formula
1+
1-
= 0
Writing Ionic Formulas
Formulas are written to make the
compound have a neutral charge overall.
If the oxidation numbers or charges do
not balance, you “Criss-Cross”.
Writing a Formula
Write the formula for the ionic compound that
will form between Ba2+ and Cl-.
Solution:
1. Balance charge with + and – ions
2. Write the positive ion of metal first, and the
negative ion
Ba2+
ClCl3. Write the number of ions needed as
subscripts
BaCl2
Criss-Crossing
Examples:
Pb2+ N3- (the charges do not balance)
Pb2+ N3-
Pb3N2
The 2 and the 3 are brought down to the
opposite element
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
Solution
1. Na+, S2b) Na2S
2. Al3+, Cla) AlCl3
3. Mg2+, N3c) Mg3N2
Ternary Ionic Nomenclature
Writing Formulas
 Write each ion, cation first. Don’t show
charges in the final formula.
 Overall charge must equal zero.
 If charges cancel, just write symbols.
 If not, use subscripts to balance charges.
 Use parentheses to show more than one
of a particular polyatomic ion.
 Use Roman numerals indicate the ion’s
charge when needed (stock system)
Ternary Ionic Nomenclature:
You Criss-cross these, too.
Sodium Sulfate
Na+ and SO4 -2
Na2SO4
Iron (III) hydroxide
Fe+3 and OHFe(OH)3
Ammonium carbonate
NH4+ and CO3 –2
(NH4)2CO3
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)
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)
Writing Formulas with
Polyatomic Ions
Example:
Pb2+ PO43-
(the charges do not balance)
Pb2+ PO43-
Pb3(PO4)2
The polyatomic ions is in
parentheses whenever a
subscript is added.
This is so that we know to count a
number of those groups!
Mixed Up… The Other
Way
Write the formula:
1. Copper (II) chlorate
2. Calcium nitride
3. Aluminum carbonate
4. Potassium bromide
5. Barium fluoride
6. Cesium hydroxide
Cu(ClO3)2
Ca3N2
Al2(CO3)3
KBr
BaF2
CsOH
never
You NEVER crisscross charges with
covalent
compounds.
Mixed Practice
1.
2.
3.
4.
5.
6.
7.
8.
9.
Dinitrogen monoxide
Potassium sulfide
Copper (II) nitrate
Dichlorine heptoxide
Chromium (III) sulfate
Iron (III) sulfite
Calcium oxide
Barium carbonate
Iodine monochloride
1.
2.
3.
4.
5.
6.
7.
8.
9.
N2O
K2S
Cu(NO3)2
Cl2O7
Cr2(SO4)3
Fe2(SO3)3
CaO
BaCO3
ICl
Hydrates
 A hydrate is an ionic compound that is
surrounded by loosely bonded water
molecules that can easily be evaporated.
 Typically have brilliant colors.
 To name them, name the ionic compound
first, then use prefixes to indicate the
number of water molecules present.
Hydrates
MgSO4·7H2O
Ba(OH)2·8H2O
CaCl2·2H2O
CuSO4·5H2O
Sodium Sulfate decahydrate
Iron (II) sulfate heptahydrate
Hydrogen sulfate monohydrate
Formulas for acids
 Backwards from names.
 If it has hydro- in the name it has no
oxygen
 Anion ends in -ide
 No hydro, anion ends in -ate or -ite
 Write anion and add enough H to balance
the charges.
Formulas for acids







hydrofluoric acid
HF
dichromic acid
H2Cr2O7
carbonic acid
H2CO3
hydrophosphoric acid H3P
hypofluorous acid
HClO4
perchloric acid
phosphorous acid
H3PO3
Write the Formula!
 Hydrobromic
acid
 Nitrous acid
 Carbonic acid
 Phosphoric acid
 Hydrotelluric acid
Hydrates
 Some salts trap water crystals when they
form crystals.
 These are hydrates.
 Both the name and the formula needs to
indicate how many water molecules are
trapped.
 In the name we add the word hydrate
with a prefix that tells us how many water
molecules.
Hydrates
 In the formula you put a dot and then
write the number of molecules.
 Calcium chloride dihydrate =
CaCl22O
 Chromium (III) nitrate hexahydrate =
Cr(NO3)3 6H2O
Now it’s Study Time
DONE
Rainbow Matrix Game
 Link on Chemistry Geek.com on
Chemistry I page
 http://chemistrygeek.com/rainbow
Use [ ] to represent subscripts since you
can’t enter subscripts into the computer
So H2O would be H[2]O
And Al2(SO4)3 would be Al[2](SO[4])[3]
Additional Polyatomic Ions (you do not have
to memorize these, but they are in the
game!)
Borate = BO3 -3 ; Silicate = SiO4 -4 ;
Manganate = MnO4 -2 (permanganate is -1)