Naming Chemical Compounds
Binary Ionic Compounds
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Binary = 2 types of elements
Ionic = made of ions
Compound = atoms bonded
together
Ionic Compounds
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Positive ions are attracted to
Negative ions
FORMULA UNIT
Cation always comes first, then
anion
Elemental anions
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When an element becomes an
anion, it starts to end in –ide
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Fluoride
Chloride
Bromide
Oxide
Sulfide
Nitride
Phosphide
Type I

The cation has a predictable charge
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Alkali Metals +1
Alkaline Earth Metals
Group 3A +3
Silver Ag+
Zinc Zn2+
+2
Type II

The cation has a variable charge

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All Transition metals except for Ag and Zn (for
our purposes)
The name will have a roman numeral to
denote the CHARGE on the cation
Fe2+
Fe3+
Cu+
Cu2+
Iron(II)
Ferrous
Iron(III)
Ferric
Copper(I)
Cuprous
Copper(II)
Cupric
Naming ionic compouds (Type I and II)
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First name cation
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Then name anion
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Just the name of element if Type I
Name of element and roman numeral
with charge on cation if Type II
Elemental anions end in “–ide”
When determining the formula,
remember “swap ‘n’ drop”
Name the following:
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Na3N
MgCl2
Al2O3
CuCl
CuCl2
PbBr4
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Sodium nitride
Magnesium chloride
Aluminum oxide
Copper(I) chloride
Copper(II) chloride
Lead(IV) bromide
Determine the formula of the following
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Aluminum chloride
Magnesium Oxide
Sodium nitride
Calcium chloride
Copper(I) sulfide
Lead (II) bromide
Iron(III) oxide
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AlCl3
MgO
Na3N
CaCl2
Cu2S
PbBr2
Fe2O3
Polyatomic Ions
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Many anions are not just ions of
elements.
Polyatomic Ions = many atomed
particle with an overall charge
Mostly nonmetals bonded to
Oxygens
Polyatomic Ion Naming
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Main polyatomic ion
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Ends in “-ite”
Example: Chlorite
ClO2-
Even fewer oxygens
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
ClO3-
One fewer oxygens
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Ends in “–ate”
Example: Chlorate
Hypo = under
Example: Hypochlorite
ClO-
More oxygens than main ion
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
Hyper = over, shortened to “per”
Example: Perchlorate ClO4-
Common Polyatomic Ions
NO2-
Nitrite
NO3-
Nitrate
SO32-
Sulfite
SO42-
Sulfate
PO43-
Phosphate
PO33-
Phosphite
Common Polyatomic Ions
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
PO43-
HPO4
2-
Hydrogen can attach to the
polyatomic ions as H+
This adds an H and reduces the
overall charge by 1
Phosphate
Hydrogen Phosphate
H2PO41- Dihydrogen
Phosphate
CO32-
Carbonate
HCO31-
Hydrogen carbonate
(bicarbonate)
Name these compounds with PAIs
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AlPO4
Cu(NO3)2
Na2SO4
NaHCO3
Mg3(PO4)2
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Aluminum phosphate
Copper(II) nitrate
Sodium sulfate
Sodium bicarbonate
Magnesium Phosphate
Molecular Compounds
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Molecular compounds are not
bonded by positive and negative
ions
They SHARE electrons
Made of two non-metals
Cannot predict or explain charges
(no charges, because not LOSING
or GAINING electrons – SHARING)
Naming Molecular Compounds
(Type III)
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Because there is no way to
neutralize the compounds (like for
ions) we must determine how many
there are another way:
Use PREFIXES
How to tell if it’s Type III
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Check the FIRST element – is it a
non-metal?
If YES, it’s a Type III
Name the first element as the
element
Name the second element ending in
“-ide”
Prefixes
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1
2
3
4
5
6
7
8
9
10
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Mono
Di
Tri
Tetra
Penta
Hexa
Hepta
Octa
Nona
Deca
Using prefixes
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If there is only one of the first
element, you may omit the “mono”
You may not omit any other prefixes
The more electronegative element
goes last (upper right hand corner)
F, O, N, Cl,
Name the following
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PCl3
CO2
NO
N2O4
N2F5
OF2
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Phosphorus trichloride
Carbon dioxide
Nitrogen monoxide
Dinitrogen tetroxide
Dinitrogen pentafluoride
Oxygen difluoride
Naming Practice! For each of the following
compounds, determine whether it is type I,
II, or III.
1.
2.
3.
4.
5.
6.
7.
8.
FeCl3
NaCl
Cu(OH)2
N2O
BaSO4
PO5
(NH4)CO3
SnBr2
Naming Practice! For each of the following
compounds, determine the CHARGE on
the cation (+1, +2, +3, or +4)
1.
2.
3.
4.
5.
6.
FeCl3
Cu(OH)2
Cr2S3
NiS
Pb(NO3)2
SnCl4
1.
3
2.
2
3.
3
4.
2
5.
2
6.
4
Acids
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All acids have the H+ ion in them as
the cation.
All acids have “acid” in their name
Consider Hydrochloric Acid
HCl
Naming Acids
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If the anion DOES NOT CONTAIN
OXYGEN:
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Prefix hydroRoot name of anion element
Suffix –ic
Examples
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HF
H2S
Hydrofluoric Acid
Hydrosulfuric Acid
Hydrooxygenic acid
Naming Acids
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If the anion CONTAINS OXYGEN (ie:
is a polyatomic ion)
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
Root name of the PAI
If anion ends in -ate,
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acid ends in –ic
If anion ends in –ite,
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acid ends in –ous
Naming Acids Examples
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H2SO4
H2SO3
HNO3
HNO2
HC2H3O2
Phosphoric Acid
Carbonic Acid
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Sulfuric Acid
Sulfurous Acid
Nitric Acid
Nitrous Acid
Acetic Acid
H3PO4
H2CO3
Organic Molecules
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Carbon based
Naming is based on number of
carbons
Functional groups
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Sets of molecules attached to the
carbons
Naming is also based on what
functional groups are where
Alkanes
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The simplest organic molecules are
Alkanes.
Carbons are all single bonded to
each other
When not bonded to another
carbon, bonded to a Hydrogen
All alkanes end in -ane
Prefixes

Note that the prefixes pertain to all
types of carbon based molecules
with any types of functional groups
or chains
•Meth
•Eth
•Prop
•But
•Pent
•Hex
•Hept
•Oct
Alkenes and Alkynes
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A functional group can be a set of
atoms, or the way they are bonded.
Alkenes
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Carbons have double bonds between
them
Alkynes
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Carbons have triple bonds between
them
Alkenes and Alkynes
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To Name
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All alkenes end with –ene.
All alkynes end with –yne
Number the carbons in the longest
chain.
Carbon 1 is at the end of the chain
closest to the first functional group
Put the number that the bond is on,
then the chain length
(some name by putting the number
BEFORE the functional group ending)
Isomer = molecule with SAME
formula but DIFFERENT structure
Alcohols
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Have an –OH group attached
Name the carbon chain (prefix and
bond)
End in –ol
Indicate which carbon the –OH is on
2-propanol
1-Butanol
3-Octenol
What are the formulas for these
alcohols?
Alcohols
Some
alcohols
have
common
names
like
glycerol
Branched Hydrocarbons
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The longest continuous chain of carbon
atoms gives the root name/prefix.
Substituent is named by the number of
carbons.
Specify location of substituent by
numbering carbon atoms in longest
chain.
Substituent often referred to as R or R’
(for second substituent)
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
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Substituent often referred to as R or
R’ (for second substituent)
If more than one alkyl group, use
prefix di, tri, etc. to alkyl name
Substituents listed in alphabetical
order (disregarding prefix)
Branched Hydrocarbon Substituent
Alkyl groups
What is the name of the compound?
Hints
•Number Carbon chain from on side closest to first alkyl group
•Single carbon branch called methyl, triple carbon group called
propyl
•More than one branch, use prefixes di-, tri-, etc.
2,4 dimethyl hexane
4 ethyl,5 methyl heptane
Tricky ones!!!
Each END of a line is a
Carbon atom. No H’s
are indicated, but they
are assumed
See if you can name
these.
Halohydrocarbons
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
Functional group is a halogen (X =
F, Cl, Br, I)
General Formula


R–X
Naming
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
Select longest chain containing halogen
Number so that C with halogen gets
lowest number
Ethers

Functional group


General Formula
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
-O–
R – O – R’
Naming
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
Name the R group as an alkyl
Name the R’ group as an alkyl
End in ether
Aldehydes

Functional group

-C–H
||
O

General Formula

R–C–H
||
O

Naming
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
Name the R group
Change the ending to -al