Nomenclature:
Naming Chemicals
PO43phosphate ion
HC2H3O2
Acetic Acid
C2H3O2acetate ion
Before naming….
• Some things you MUST know
to be successful…. You really
need to commit these things
to memory
Ions:
• Atoms or groups of atoms with a _________.
• Cations- ________ions - get by losing
electron(s).
• Anions- ________ ions - get by gaining
electron(s).
• Ionic bonding- held together by the
______________ (_____________________).
• Ionic solids are called ________.
• Salts are __________________; they conduct
electricity when dissolved in water (aq.)
Metals
•
•
•
•
Conductors of heat and electricity
Make ________ (lose e to become + charged)
Malleable (made into ________)
Ductile (made into ________)
-
Nonmetals
• Are a ________ _______ or a _______
• Make ________(gain e- to become - charged)
• __________ bond to
each other
Semi-metals (AKA ________)
•Characteristics of _____
metals and nonmetals
•More ________ as you
go down PT
Common Ions of Elements
________ _____
Predicting Charges on Monatomic Ions
KNOW THESE !!!!
+1 +2
-3 -2 -1
Variable, always +
Cd+2
0
Polyatomic Ions
• _______ of covalently
bonded atoms that
have a charge.
* NO3- :___________
* NO2- :___________
• Yes, you have to
memorize them.
• Listed in your resource
handbook: memorize
the required list!!!!
Patterns for Polyatomic Ions
• -ate ion
– _________________________________
• -ate ion plus 1 O  same charge, ___- prefix
– _________________________________
• -ate ion minus 1 O  same charge, -___
suffix
– _________________________________
• -ate ion minus 2 O  same charge, ___prefix, -___ suffix
– _________________________________
Polyatomic Ions
You can make additional polyatomic ions by
adding a __ to the ion!
• CO3 -2 is carbonate:
–
– HCO3 is ______________________
• PO43- is phosphate:
2-
– HPO4 is ______________________
–
– H2PO4 is ______________________
2-
• SO4 is sulfate
–
– HSO4 is ______________________
The 3 types of Chemical Bonds:
________, _______ and _________
• Electronegativity and Bond Type
– Bond type can be determined by the difference in
electronegativity (degree of sharing of e-) between the
elements involved
– Differences of:
• ≥ 2 =_________________
• 0.5-1.9 = ______________________
• ≤ 0.4 = ____________________________
• Metals bonded to other metals are
___________________ bonded, regardless of the
difference in electronegativity.
Metallic bonds
– The atoms of metals
are held together when
the atom’s _________
__________________
__________________
__________________
__________________
__________________
__________________
– __________________
keep everything
together
Ionic Bonds
 Complete _______ of 1 or more
electrons from one atom to another
(or a _____________________)
 one _____ one or more e-, the other
____ those e-s
 Atoms involved are

_______________________________________
_______________________________________
 The cation and anion are attracted to each
other by _______________________
Ionic compounds are neutral
• Ionic compounds are ______________
– That is, they have no __________ charge
• This is because the number of electrons _____
_________________________________________
_________________________________________
______________________________________
– Formulas reflect this neutrality- the charges on
the individual ions are not written in because
they _________________
_____________________________________
COMPOUNDS
FORMED FROM
IONS
CATION +
ANION --->
COMPOUND
Na+
-
+ Cl --> NaCl
A neutral compound
requires
Covalent Bonds
– ________________valence electrons that are
______________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
 Because not all atoms __________________________
 The conventions of naming assume _____________
_____________________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*
 * _____________________________________________
______________________________________________
______________________________________________
______________________________________________.
 For more on this, go back to bonding
Naming things:
• If there is only one element present, ________
____. 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
______________________?
So… some general help for naming:
– Look to see if there is a ________ ______in
the formula
– Again, semimetals are not a classification in naming;
_____________________________________________
_____________________________________________
_____________________________________________
• If there are only metals,
__________________________
– (metallic bonding; nothing else need be done)
• If ________the first element is a metal, then the
compound is an ________________ compound
• Nonmetals _________ signify a _______ 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
_______________________________________.
• We can handle these as simple types
– _______________(2 elements) compounds
– ___________(more than 2 element) compounds
• Names are always for the smallest whole number
ratio of the elements, the ___________
*Two exceptions to this rule:
– Compounds that start with either ammoniums (NH4+) or hydronium (H3O+)
General information for naming
ionic compounds:
Specifics for binary ionic compounds:
Example: CaCl2, or calcium chloride
1. Name the cation first, then the anion root with
an –ide suffix
2. For CaCl2, the monatomic cation is Ca2+ , calcium,
and the monatomic anion is Cl- , named chloride.
3. 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…
__________________________are Type II Cations, and are
elements that can have ______________
______________________. They MUST have a
________________________________________________
________________________________________________
__
1+ or 2+
2+ or 3+
Cu+, Cu2+
Fe2+, Fe3+
______________________________________________
________________________________________________
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+) ____________________
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
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
sodium fluoride
Charge balance:
1+ + 1= 0
Neutral, you say?
• Formulas are written to make the compound
have a _____________________________.
• 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_______________________________
______________________________________
______________________________________
______________________________________
Writing the formula…
Write the formula for the barium chloride, the
compound that will form between Ba2+ and Cl-.
Solution:
1. Write the ___________, and then the ___________.
2. Balance charge with the number of + and – ions
3. Write the number of ions needed ____________
__________________________:
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 “___________ ____________” _________.
You take the ______ __________from the
_________, and you make it the number of
_________ (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-
Pb2+ N3-
*the charges do not balance
Pb3N2
• The 2 and the 3 are brought down to the opposite
element, so that there are now ___________ ions
and ___________ions
• This means there were _____ 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) Mg2N3
c) Mg3N2
Ternary Ionic Compounds:
• Contain at least 3 elements
• There MUST be at least one polyatomic ion
(it helps to ______________)
Examples:
NaNO3 ____________________________
K2SO4
_____________________________
Al(HCO3)3
______________________________
Specifics for ternary ionic compounds
Examples: NaNO3, and Co(NO3)2
1. Name the cation first, then polyatomic ion
2. For NaNO3, the monatomic cation is Na+ , sodium,
and the polyatomic anion is NO3- , named nitrate.
– NaNO3 is sodium nitrate
3. 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
Ca3(PO4)2
a) calcium carbonate
b) calcium phosphate
c) calcium bicarbonate
Writing Formulas for Ternary Ionic Compounds
• Write the _______ first, then the _____________.
• Overall charge must equal ____________.
– If charges cancel, just write symbols.
– If not, use ________________ to balance charges.
• Use parentheses to
____________________________
_________________________________________
_____.
• Use ______________________ to indicate the
ion’s charge when needed (transition metals)
• Remember that the final formula should ________
__________________________written in.
Writing Formulas, cont’d
Example:
Cr2+ PO43- *the charges do not balance
Cr2+ PO43-
______________
The polyatomic ions is in parentheses
_____________________
________________________________.
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
General naming rules for
covalent (molecular) compounds
• Names are _______________,
__________________.
– Prefixes tell you________________________.
• First element whole name with the
appropriate prefix
– ***NEVER use ______ for the first element!
• For the second element, use the
_________ _____________ and the -ide
ending with appropriate prefix for that
many.
NEVER
never
You
.
Since you are sharing electrons, rather than giving them away/
picking them up, the charges _______________
________________.
Covalent Naming Prefixes:
PREFIX
NUMBER
1
2
3
4
5
6
7
8
9
10
Specifics for binary covalent compounds
Example: CO2 is carbon dioxide
1. Name the first element, using a prefix if there is
more than one atom of the element present
2. Name the second element, using the appropriate
prefix in all cases
3. CO2 is carbon dioxide because there is one
carbon (no prefix when there is only one atom of
the element,) and two oxygens (di- prefix)
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
More Covalent Examples
 arsenic trichloride
 dinitrogen pentoxide
 tetraphosphorus decoxide
Hydrates: Ionic Compounds·Water
• Some salts trap water crystals when they
form crystals.
– Ex: CuSO4· ___H2O
• These are ______________.
• Both the name and the formula needs to
indicate _____________________________.
• In the name we add the word hydrate with a
prefix that tells us how many water
molecules.
• ____________________________________
Hydrates
• In the formula ________________________
____________________________________.
• _____________________________________
• _____________________________________
Acid Nomenclature
• Acids
– Compounds that
_________________________________
– Formulas
usually_________________________________
– In order to be an acid instead of a gaseous covalent
compound, it
___________________________________
• Meaning dissolved in water; symbolized by _______
– Ternary acids are ALL aqueous
– Two types:
• ____________________
• ____________________
Naming acids: Non-oxy acids
If the acid ________________________
• add the prefix ____________• change the suffix -________________
HCl
H2S
HCN
_______________________
_______________________
_______________________
Naming acids: Oxyacids
If the formula has oxygen in it
• write the name of the ___________, but change:
• _____________________________
• _____________________________
• Watch out for sulfuric and sulfurous!
H2CrO4
HMnO4
HNO2
____________________
____________________
___________________
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
Specifics: 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)
 H2CO3 (aq)
 H2CO2 (aq)
Acid
HNO3
HNO2
H2SO4
H2SO3
H3PO4
HC2H3O2
Name
Name ‘Em!
• HI (aq)
• HCl (aq)
• H2SO3 (aq)
• HMnO4 (aq)
• HIO4 (aq)
Formulas of Acids
• Backwards from names.
• If it has hydro- in the name:
– _____________________________
– Anion ends in ____________
• No hydro, anion ends in ____________
– Write anion and add ________________
______________________
Write the Formula!
• Hydrobromic acid
• Hydrosulfic acid
• Carbonic acid
• Phosphoric acid
• Hydrotelluric acid
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 _________________________
_______________________________
___
– NH3
_____________________________
_______________________________
___