Acid - Base Theories Acid - Base Theories
• Lavoisier
• Arrhenius
• Bronsted-Lowry
• Lewis
• Lavoisier
• Arrhenius
• Bronsted-Lowry
• Lewis
Acidity is caused by
the presence of
oxygen in the
compound.
Lavoisier - 1777Lavoisier - 1777
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He even created the word
oxygen - from the
Greek oxys, "sour"
and genes, "born"
Lavoisier - 1777Lavoisier - 1777
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Oxygen means
"acid maker".
Lavoisier - 1777Lavoisier - 1777
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Lavoisier's idea about
acids turned out
to be wrong...
Lavoisier - 1777Lavoisier - 1777
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but it is historically important
since it is the first scientific
attempt to chemically
characterize acids
and bases.
Lavoisier - 1777Lavoisier - 1777
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SvanteAugust
Arrhenius QuickTime™ and a
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Arrhenius AcidArrhenius Acid
Any substance
that produces
hydrogen ions,
H+, in water
solution.
Any substance
that produces
hydroxide ions,
OH-, in water
solution.
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Arrhenius BaseArrhenius Base
In a formula, such as HCl,
the positive part of a
Arrhenius acid
will ALWAYS
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In a formula, such as
NaOH, the negative part
of a Arrhenius
base will
ALWAYS
be hydroxide.
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JohannesNicolausBronsted
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Bronsted-Lowry TheoryBronsted-Lowry Theory
ThomasMartinLowry
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Bronsted-Lowry TheoryBronsted-Lowry Theory
Any substance that
acts as a proton donor.
Bronsted-Lowry AcidBronsted-Lowry Acid
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A B-L acid MUST have
hydrogen somewhere
in its
formula.
Bronsted-Lowry AcidBronsted-Lowry Acid
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Bronsted-Lowry BaseBronsted-Lowry Base
Any substance that
acts as a proton
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Bronsted-Lowry BaseBronsted-Lowry Base
Most negative ions can
acts as B-L bases.
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The acid/base definitionsare broadened because nospecific ion must be formed,although hydrogen is the only source of protons.
Bronsted-Lowry TheoryBronsted-Lowry Theory
The hydronium ion is formedby combining a hydrogen ion and a water molecule.
H2O + H+ H3O+
Bronsted-Lowry TheoryBronsted-Lowry Theory
A conjugate base is the
particle that remains
AFTER an acid gives
up a proton.
Bronsted-Lowry TheoryBronsted-Lowry Theory
A conjugate acid is the
particle formed when a
base accepts a proton.
Bronsted-Lowry TheoryBronsted-Lowry Theory
HCl + H2O Cl- + H3O+
Identify the B-L acid in this equation.
What gives up a proton fromthe left side to the right?
Identify the B-L base
in this equation.
What gains a proton from
the left side to the right?
HCl + H2O Cl- + H3O+
HCl + H2O Cl- + H3O+
Identify the conjugate
base in this equation.
What is left when the
acid gives up a proton?
HCl + H2O Cl- + H3O+
Identify the conjugate
acid in this equation.
What is formed when the
base accepts a proton?
GilbertNewtonLewis
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The Lewis TheoryThe Lewis Theory
Lewis AcidLewis Acid
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Any substance thatacts as anelectron-pairacceptor.
Lewis BaseLewis Base
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Any substance thatacts as anelectron-pairdonor.
The Lewis TheoryThe Lewis Theory
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This theory is thebroadest of all.
The Lewis TheoryThe Lewis Theory
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Any reaction thatinvolves the exchangeof electrons WILL have a Lewis acidand Lewis base.
The Lewis TheoryThe Lewis Theory
In an equation, the Lewisacid gets
MORE NEGATIVEfrom the left side to theright side - it gains e-.
The Lewis TheoryThe Lewis Theory
In an equation, the Lewisbase gets
MORE POSITIVEfrom the left side to theright side - it loses e-.
End Acid - Base
Theories
End Acid - Base
Theories
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First:
Determine the stem word.
The stem word comes from
the negative element.
Naming Binary AcidsNaming Binary Acids
First:
Determine the stem word.
Example - HCl
chlorine is the negative
element - CHLOR is the stem.
Naming Binary AcidsNaming Binary Acids
Second:
Add the prefix hydro
to the stem.
Example - hydro + chlor
Naming Binary AcidsNaming Binary Acids
Third:
Change the ending
of the stem to ic.
Example - hydro + chlor + ic
Naming Binary AcidsNaming Binary Acids
• HCl hydro chlor ic acid
• HF hydro fluor ic acid
• HBr
• HI
Naming Binary AcidsNaming Binary Acids
• HCl hydro chlor ic acid
• HF hydro fluor ic acid
• HBr hydro brom ic acid
• HI
Naming Binary AcidsNaming Binary Acids
• HCl hydro chlor ic acid
• HF hydro fluor ic acid
• HBr hydro brom ic acid
• HI hydro iod ic acid
Naming Binary AcidsNaming Binary Acids
Ternary acids composed of
three elements:
hydrogen, oxygen,
and a nonmetal
Naming Ternary AcidsNaming Ternary Acids
First:
Determine the stempart of the name of
the third element
Naming Ternary AcidsNaming Ternary Acids
First:
Determine the stemExample - H2SO4
sulfur is the third element,
SULFUR is the stem.
Naming Ternary AcidsNaming Ternary Acids
Second:
The most common form of the acid is given the suffix ic.
Naming Ternary AcidsNaming Ternary Acids
Second:
The most common form of the acid is given the suffix ic.
Example - sulfur + ic acid
Naming Ternary AcidsNaming Ternary Acids
Third:
If the acid is NOT in its
most common form,
do the following:
Naming Ternary AcidsNaming Ternary Acids
Naming Ternary AcidsNaming Ternary Acids
Add the prefix per if the acid
has one more oxygen than
the most common form.
Add the prefix per if the acid
has one more oxygen than
the most common form.
Example - H2SO5
per + sulfuric acid
Naming Ternary AcidsNaming Ternary Acids
Naming Ternary AcidsNaming Ternary AcidsAdd the suffix ous if the acid
has one less oxygen than
the most common form.
Add the suffix ous if the acid
has one less oxygen than
the most common form.
Example - H2SO3
sulfur + ous acid
Naming Ternary AcidsNaming Ternary Acids
Naming Ternary AcidsNaming Ternary Acids
Add the prefix hypo if the acid
has two less oxygen atoms
than the most common form.
Add the prefix hypo if the acid
has two less oxygen atoms
than the most common form.
Example - H2SO2
hypo + sulfur + ous acid
Naming Ternary AcidsNaming Ternary Acids
HClO4 Perchloric Acid
HClO3 Chloric Acid
HClO2 Chlorous Acid
Naming Ternary AcidsNaming Ternary Acids
HClO4 Perchloric Acid
HClO3 Chloric Acid
HClO2 Chlorous Acid
HClO
Naming Ternary AcidsNaming Ternary Acids
HClO4 Perchloric Acid
HClO3 Chloric Acid
HClO2 Chlorous Acid
HClO Hypochlorous Acid
Naming Ternary AcidsNaming Ternary Acids
Strong or WeakStrong or Weak
In Strong ternary acids,
the number of oxygen
atoms exceeds the
number of...
Strong or WeakStrong or Weak
hydrogen atoms by
two or more.H2SO4 and HNO3 are strong.
H3PO4 is weak.
AmphotericAmphoteric
A substance that acts
as either an acid or
base, depending on
what it reacts with.
Anhydrous - Without H2OAnhydrous - Without H2O
Write the anhydrous form of:
1. H2SO3
2. H2C2O4
3. H3PO4
4. H4C2O2
Anhydrous - Without H2OAnhydrous - Without H2O
Write the anhydrous form of:
1. H2SO3 SO2
2. H2C2O4
3. H3PO4
4. H4C2O2
Anhydrous - Without H2OAnhydrous - Without H2O
Write the anhydrous form of:
1. H2SO3 SO2
2. H2C2O4 C2O3
3. H3PO4
4. H4C2O2
Anhydrous - Without H2OAnhydrous - Without H2O
Write the anhydrous form of:
1. H2SO3 SO2
2. H2C2O4 C2O3
3. H3PO4 HPO3
4. H4C2O2
Anhydrous - Without H2OAnhydrous - Without H2O
Write the anhydrous form of:
1. H2SO3 SO2
2. H2C2O4 C2O3
3. H3PO4 HPO3
4. H4C2O2 C2