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
Ions: A Refresher
 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- electrostatic attractions.
 Ionic solids are called salts.
 Salts are electrolytes; they conduct
electricity when dissolved in water (aq.)
 Conductors
of heat and electricity
 Make cations (lose e to become + charged)
 Malleable (made into sheets)
 Ductile (made into wire)
-
 Are
a brittle solid or a gas
 Make anions (gain e- to become - charged)
 Covalently bond to each
other
•Characteristics of both
metals and nonmetals
•More metallic as you go
down PT
+1
Common Ions of Elements
+3
+2
Variable, always +
4 -3 -2 -1 0
+/-
Predicting Charges on Monatomic Ions
KNOW THESE !!!!
+1 +2
-3 -2 -1
Cd+2
0
Polyatomic Ions
 Groups of covalently
bonded atoms that
have a charge.
* NO3- :nitrate ion
* NO2- :nitrite ion
 Yes, you have to
memorize them.
 Listed in your
resource handbook:
memorize the
required 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, hypo-
prefix, -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
 PO43- is phosphate:
 HPO4
2-
is hydrogen phosphate
–
 H2PO4 is dihydrogen phosphate
2-
 SO4 is sulfate
–
 HSO4 is hydrogen sulfate
The 3 types of Chemical Bonds:
Metallic, Ionic and Covalent
 Electronegativity and Bond Type
 Bond type can be determined by the difference
in electronegativty between the bonds involved
 Differences of:

2 = ionic
≥
0.5-1.9 = polar covalent
 ≤ 0.4 = nonpolar covalent
.
 Metals bonded to other metals are metallically
bonded, regardless of the difference in
electronegativity

Metallic bonds
 The atoms of metals
are held together when
the atom’s valence
electrons float around
the nuclei of the
metals – the “sea of
electrons”
 Electrostatic forces
keep everything
together
Ionic Bonds
 Complete transfer of 1 or more
electrons from one atom to another
(or a polyatomic ion)
 one loses one or more e-, the other
gains those e-s
 Atoms involved are

a metal and either a non-metal or a
polyatomic ion
 The cation and anion are attracted to
each other by electrostatic attraction
Ionic compounds are neutral
 Ionic compounds are neutral
 That is, they have no overall charge

This is because the number of electrons that
are given up by the metal is the same number
of electrons that are gained by the anion for
the formula.
 Formulas reflect this neutrality- the
charges on the individual ions are not
written in because they cancel out overall
for the compound
COMPOUNDS
FORMED FROM
IONS
CATION +
ANION --->
COMPOUND
Na+
-
+ Cl --> NaCl
A neutral compound
requires
equal number of +
and - charges.
Covalent Bonds
 2, 4, or 6 valence electrons that are shared
between atoms
 We are going to name only simple covalent
compounds that have 2 elements involved
Most bonds are somewhere in between
ionic and covalent (as you already know)
 Because not all atoms share e- equally
 The conventions of naming assume absolute difference
in bond types
 Metals bonded to nonmetals or polyatomic ions are
classified as having ionic bonds*
 Materials made out of all non-metals are classified as
having covalent bonds*
 * semimetals are not a classification in naming; you need
to treat the elements that are on the right of the line as
non-metals, and those on the left as metals.
 For more on this, go back to bonding
Naming things:
 If there is only one element present, name it.
Atomic substances do not require “special”
naming.
 For anything with more than one element,
remember that there is ONE MAIN THING to
look for:
Is there a metal first?
So…some general help for naming:
 Look to see if there is a metal first in the
formula

Again, semimetals are not a classification in naming;
you need to treat the elements that are on the right
of the line as non-metals, and those on the left as
metals.
 If there are only metals, name both metals
 (metallic bonding; nothing else need be done)
 If ONLY the first element is a metal, then the
compound is an ionic compound
 Nonmetals only signify a covalent compound
 There is a flow chart in your handbook to help!
Naming ionic compounds:
 Remember that those are compounds that have
a metal first in the formula*, and then a
nonmetal or a polyatomic ion.
 We can handle these as simple types
 binary (2 elements) compounds
 Ternary(more than 2 element) compounds
 Names are always for the smallest whole
number ratio of the elements, the formula unit
*Two exceptions to this rule:
 Compounds that start with either ammoniums (NH4+) or hydronium (H3O+)
General information for naming
ionic compounds
 If the cation is monatomic- Name
the metal (cation).
 Use Roman Numerals for transition
metals (ONLY) after the metal
 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
Example: CaCl2, or calcium chloride
 Name
the cation first, then the anion root
with an –ide suffix
 For
CaCl2, the monatomic cation is Ca2+ ,
calcium, and the monatomic anion is Cl- ,
named chloride.

We use chloride because the root for
chlorine is chlor, and we use = root + -ide
for the second element in binary
compounds
 CaCl2 = calcium chloride
Learning Check
Complete the names of the following binary
compounds:
Na3N
KBr
Al2O3
MgS
If the Metal is a Transition Metal…
Transition metals are Type II Cations, and are
elements that can have more than one possible
charge. They MUST have a Roman Numeral to
indicate the charge on the individual ion.
1+ or 2+
Cu+, Cu2+
2+ or 3+
Fe2+, Fe3+
copper(I) ion iron(II) ion
copper (II) ion iron(III) ion
Type II Cations
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
You will appreciate this more when we go from names to formulas!
Type II 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.
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
CuCl
SnBr4
Fe2O3
Hg2S
General naming rules for
covalent (molecular) compounds
 Names are two words, with prefixes.
 Prefixes tell you how many.
 Use the first element’s whole name with
the appropriate prefix
 *********except mono.
 NEVER use mono for the first element
 For the second element, use the root of
the name and the -ide ending with
appropriate prefix for that many.
Covalent Naming Prefixes:
PREFIX
monoditritetrapentahexaheptaoctanonadeca-
NUMBER
1
2
3
4
5
6
7
8
9
10
Example: CO2 is carbon dioxide
 Name
the first element, using a prefix if
there is more than one atom of the element
present
 Name
the second element, using the
appropriate prefix in all cases

CO2 is carbon dioxide because there is one
carbon (no prefix when there is only one
atom of the element,) and two oxygens (diprefix)
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
Give the names of following covalent
compounds:
CO
CO2
PCl3
CCl4
N2O
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
Hydrates: Ionic Compounds·Water
 Some salts trap water crystals when they
form crystals.
 Ex: CuSO4·H2O
 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.
 CuSO4·H2O is copper (II) sulfate pentahydrate
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
Acid Nomenclature
 Acids
 Compounds that form H+ in water.
 Formulas usually begin with ‘H’.
 In order to be an acid instead of a gaseous covalent
compound, it must be aqueous

Meaning dissolved in water; symbolized by (aq)
 Ternary acids are ALL aqueous
 Two types:

Non-oxyacids

Oxyacids
Naming acids: Non-Oxy acids
If the acid doesn’t have oxygen
 add the prefix “hydro-”
 change the suffix “–ide” to “-ic acid”
HCl
H2S
HCN
Hydrochloric acid
Hydrosulfic acid
Hydrocyanic acid
Naming acids: Oxy 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 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
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)
 H2CO3 (aq)
 H2SO3 (aq)
Acid
HNO3
HNO2
H2SO4
H2SO3
H3PO4
HC2H3O2
Name
Name ‘Em!
 HI (aq)
 HCl (aq)
 H2SO3 (aq)
 HNO3 (aq)
 HIO4 (aq)
Writing Formulas for Ionic Compounds from
Names
Formulas of ionic compounds are determined
from the charges on the ions
Na
+ F 
Na+ + F-  NaF
Sodium atom + fluoride ion
Charge balance:
1+ +
sodium fluoride
1= 0
Remember that all ionic compounds have no net charge, and
that the charges are not written in! Ever. Nope.
Neutral, you say?
 Formulas are written to make the compound
have a neutral charge overall.
 You do NOT write the charges in the formula
because they MUST cross out to accurately
represent the compound.
 Ex: NaF2 is INCORRECT for sodium chloride
because Na has an oxidation state of +1, and
F of -1. There is a one to one ratio of Na+ to
F- to make a neutral ionic compound.
Writing the formula…
Write the formula for the barium chloride, the
compound that will form between Ba2+ and Cl-.
Solution:
1. Write the cation, and then the anion
2. Balance charge with the number of + and – ions
ClThink:
ClWhy is Cl- written twice?
3. Write the number of ions needed as
Ba++
subscripts:
BaCl2
So what if the oxidation numbers
aren’t even?
 If the oxidation numbers or charges do not
balance, you can write the number of ions of each
until you get the same number of each charge in
total.
Is there an easier way?
 Yes. The “Criss Cross” method. You take the
charge number from the cation, and you make
it the number of anions (subscript)and take the
charge on the anion, and you make that many
cations (subscript).
Criss-Crossing in action:
Example: Lead (II) nitrate
Pb2+ N3-
*the charges do not balance
Pb2+ N3-
Pb3N2
 The 2 and the 3 are brought down to the
opposite element, so that there are now 3 Pb2+
ions and 2 N3- ions
 This means there were 6e- transferred from the
lead atoms to the nitrogen atoms; the compound
is neutral
Learning Check
Write the correct formula for the
compounds containing the following
ions:
1. Na+ and S2a) NaS
b) Na2S
c) NaS2
2. Al3+ and Cla) AlCl3
b) AlCl
c) Al3Cl
3. Mg2+ and N3a) MgN
b) Mg2N3c) Mg3N2
Ternary Ionic Compounds:
 Contain at least 3 elements
 There MUST be at least one polyatomic ion
(it helps to circle the ions)
Examples:
NaNO3
Sodium nitrate
K2SO4
Al(HCO3)3
Potassium sulfate
Aluminum bicarbonate
(Aluminum hydrogen carbonate)
Specifics for ternary ionic compounds
Examples: NaNO3, and Co(NO3)2
 Name the cation first, then polyatomic ion
 For NaNO3, the monatomic cation is Na+ ,
sodium, and the polyatomic anion is NO3- ,
named nitrate.
 NaNO3 is sodium nitrate
 For Co(NO3)2, the monatomic cation is Co+2,
cobalt (II) and the polyatomic anion is NO3- ,
named nitrate.
 Co(NO3)2 is cobalt (II) nitrate
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
Writing Formulas for Ternary Ionic Compounds
 Write the cation first, then the anion.
 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 (transition metals)
 Remember that the final formula should not have
charges written in.
Writing Formulas, cont’d
Example:
Cr2+ PO43Cr2+ PO43-
the charges do not balance
*
Cr3(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!
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)
Ternary Ionic Nomenclature:
You Criss-cross these, too.
Sodium Sulfate
Iron (III) hydroxide
Ammonium carbonate
Write the Formula:
Copper (II) chlorate
Calcium nitride
Aluminum carbonate
Potassium bromide
Barium fluoride
Cesium hydroxide
never
NEVER
You
criss-cross charges
with covalent
compounds.
Since you are sharing electrons, rather than giving
them away/ picking them up, the charges are not
relevant.
More Covalent Examples
 arsenic trichloride
 dinitrogen pentoxide
 tetraphosphorus decoxide
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’s to
balance the charges.
Acid Nomenclature
 hydrofluoric acid
 sulfuric acid
 nitrous acid
Formulas for acids
hydrofluoric acid
dichromic acid
carbonic acid
hydrophosphoric acid
hypofluorous acid
perchloric acid
phosphorous acid
Write the Formula!
 Hydrobromic acid
 Nitrous acid
 Carbonic acid
 Phosphoric acid
 Hydrotelluric acid
Mixed Practice
Dinitrogen monoxide
Potassium sulfide
Copper (II) nitrate
Dichlorine heptoxide
Chromium (III)
sulfate
6. Iron (III) sulfite
7. Calcium oxide
8. Barium carbonate
9. Iodine monochloride
1.
2.
3.
4.
5.
 Match each set with the correct name:
Na2CO3
MgSO3
MgSO4
a) sodium carbonate
b) magnesium sulfite
c) magnesium sulfate
Ca(HCO3)2
CaCO3
Ca3(PO4)2
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
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 b) dinitrogen trioxide
c) nitrogen trioxide
Mixed Practice
1.
2.
3.
4.
5.
6.
7.
8.
9.
BaI2
P 4S3
Ca(OH)2
FeCO3
Na2Cr2O7
I2O5
Cu(ClO4)2
CS2
B2Cl4
DONE!
Now it is time to study!
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)