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Naming Bases
• Bases contain an (OH-) group
• If an OH group is present it will be clearly
indicated: e.g. NaOH, Ca(OH)2
• Also notice that bases have a metal (or positive
ion such as NH4+ at their beginning)
• Bases are named like other ionic compounds:
• + ion is named first, followed by the polyatomic
ion
- calcium hydroxide
Ca(OH)2
- copper(I) hydroxide
CuOH
- Al(OH)3
aluminum hydroxide
- NH4OH
ammonium hydroxide
Acids
• Compounds that give off hydrogen ions
(H1+) when dissolved in water (the Arrhenius
definition)
• In the laboratory, the term acid usually
refers to a solution in water (aqueous
solution) of an acid compound rather
than the acid itself.
• Hydrogen is always the first element in
the formula and it is next to an anion.
• The anion determines the name.
Types of Acids
BINARY ACIDS
– acids that consist of two elements, usually
hydrogen and a halogen.
H + non-metal
E.g. HCl
OXYACIDS
– acids that contain hydrogen and a
polyatomic ion (oxygen and a nonmetal)
(H + polyatomic ion E.g. H2SO4
• Each type of acid has different naming rules.
Naming Acids: Binary acids
• All acids start with H
• Binary acids: naming depends on state of acid
• If it’s not aqueous: hydrogen + non-metal
HCl(g) = hydrogen chloride
• If it is aqueous: hydro + non-metal + ic acid
HCl(aq) = hydrochloric acid (aqueous hydrogen
chloride)
HBr(s) hydrogen bromide HI(aq) hydroiodic acid
H2S(aq)hydrosulfuric acid H2S(g) hydrogen sulfide
Binary Acids
Acid Name
Chemical Formula
Hydrofluoric acid
HF(aq)
Hydrochloric acid
HCl(aq)
Hydrobromic acid
HBr(aq)
Hydroiodic acid
HI(aq)
Hydrosulfuric acid
H2S(aq)
Hydrocyanic acid
HCN(aq)
- Recall: Binary acids do not contain oxygen
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Rules for Naming Oxyacids
ACIDS
(anion contains the element oxygen)
• In the laboratory, the term acid usually refers
to a solution in water of an acid compound
rather than the acid itself.
• Many polyatomic ions are produced by the
loss of hydrogen ions from oxyacids.
H2SO4
sulfate
SO2
4
nitric acid
HNO3
nitrate
NO3
phosphoric acid
H3PO4
phosphate
PO3
4
sulfuric acid
• Since all acids have the same cation,
H+, we don't need to name the cation.
• Acid name comes from the “root” name
of the polyatomic ion name or the
central element of the polyatomic ion.
• Suffixes are used based on the ending
of the original name of the oxyanion.
• Naming does not depend on the state
(aq).
Naming Oxyacids
Naming Oxyacids
Parent Oxyanion
(polyatomic ion)
Acid Name
Chemical Formula
nitrate, NO3 -
nitric acid
HNO3(aq)
chloric acid
HClO3(aq)
chlorate, ClO3 carbonate, CO3
2-
sulfate, SO4 2phosphate, PO4
3-
carbonic acid
H2CO3(aq)
sulfuric acid
H2SO4(aq)
phosphoric acid
H3PO4(aq)
Polyatomic
Name
Acid
Name
ClO4-
perchlorate
HClO4
perchloric Acid
ClO3-
chlorate
HClO3
chloric acid
ClO2-
chlorite
HClO2
chlorous acid
ClO-
hypochlorite
HClO
hypochlorous
acid
Simplified Chart for Naming Oxyacids
Oxygen
Content
Oxyacid
Oxyanion
per……..ic acid
per……..ate
……..ic acid
……..ate
1 less than
“normal”
……..ous acid
……..ite
2 less than
“normal”
hypo……..ous acid
1 more than
“normal”
“Normal
Oxyacid”
hypo……..ite
Insert the non-metal “root” name:
“chlor”, “iod”, “nitr”, “carbon”, “sulfur”
Example with chloric acid, HClO3
Oxygen Content
Oxyacid
Formula
1 more than
“normal”
Per…..ate
ClO4-
perchloric acid
HClO4
“Normal
Oxyacid”
ate
ClO3-
chloric acid
HClO3
1 less than
“normal”
ite
ClO2-
chlorous acid
HClO2
2 less than
“normal”
hypo …ite
ClO-
hypochlorous acid HClO
Root name is “chlor”
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Naming Acids: Oxyacids
E.g. H2SO3
Naming Acids: Oxyacids
E.g. H2SO3
1) sulfite,
2) sulfous,
3) sulfurous,
4) sulfurous acid
HNO2
hypochlorous acid
H3PO4(aq)
carbonic acid
HYDRATES
And rehydrated
by adding water
hydrate
2) sulfous,
3) sulfurous,
4)
HNO2
- nitrous acid
H3PO4(aq)
- phosphoric acid
hypochlorous acid
- HClO
carbonic acid
- H2CO3
Naming Hydrates
• Hydrates are substances that
include water in their formula.
• Ex: CuSO4 . 5H2O
• This formula means that for
every one CuSO4 in the
formula unit, there are also
five water molecules
incorporated in the crystal
lattice.
• Ionic solids that contain
water molecules as part
of their crystalline
structure. The water in
the hydrate is known as
the water of hydration
or the water of
crystallization.
A hydrate can be
“dehydrated” by
heating it and
turning it into its
anhydrous
(without water)
form…..
1) sulfite,
anhydrous
• The substance is not wet, it appears
dry. The dot . is not a multiplication sign,
it just shows that the water is part of the
compound.
• The name for CuSO4 . 5H2O is:
• copper (II) sulfate pentahydrate
• Notice “penta” meaning 5, and “hydrate”
meaning water.
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Recall:Prefixes
1 = mono2 = di3 = tri4 = tetra5 = penta6 = hexa7 = hepta8 = octa9 = nona10 = deca-
Naming Hydrates
Compound name +
.
+ prefixhydrate
CuSO4 . 5H2O
copper (II) sulfate pentahydrate
Ex: name this substance:
MgSO4 . 9H2O
Ex: Write the formula for:
barium chloride dihydrate
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