1 ACID- BASE EQUILIBRIA ACID- BASE EQUILIBRIA ACID- BASE EQUILIBRIA ACID- BASE EQUILIBRIA.
Lewis acid-base theory
description
Transcript of Lewis acid-base theory
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Lewis acid-base theory
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Lewis acid-base theory
Very different from Brønsted-Lowrey
acid-base.
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Lewis acid-base theory
Very different from Brønsted-Lowrey
acid-base.
Not dependent on protons
or pH.
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Lewis acid-base theory
An acid is a lone-pair acceptor.
Definitions:
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Lewis acid-base theory
An acid is a lone-pair acceptor.
H+ no electrons – by accepting 2 electrons it attains noble gas configuration.
Definitions:
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Lewis acid-base theory
An acid is a lone-pair acceptor.
H+ no electrons – by accepting 2 electrons it attains noble gas configuration.
BF3 electron deficient compound - B needs 2 electrons for noble gas configuration.
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B Group III 3 valence electrons
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B Group III 3 valence electrons
F Group VII 7 valence electrons
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B Group III 3 valence electrons
F Group VII 7 valence electrons
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6 electrons for boron rather than 8
Lewis Acid
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Lewis acid-base theory
Lewis base: lone-pair donorDefinitions:
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Lewis acid-base theory
Lewis base: lone-pair donor
NH3 N has lone pair
Definitions:
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Group V
Group I
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Lewis Base
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Lewis acid-base theory
Lewis base: lone-pair donor
NH3 - N has lone pair
H2O - O has 2 lone pairs
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Lewis acid-base theory
H3N : + BF3 H3N : BF3
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Lewis acid-base theory
H3N : + BF3 H3N : BF3
Lewis base
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Lewis acid-base theory
H3N : + BF3 H3N : BF3
Lewis base Lewis acid
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Lewis acid-base theory
H3N : + BF3 H3N : BF3
Lewis base Lewis acid
Both electrons in thisbond come from nitrogen.
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Lewis acid-base theory
H3N : + BF3 H3N : BF3
Lewis base Lewis acid
Coordinate covalent bond
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(CH3)3N BCl3
(CH3)3N : + BCl3 (CH3)3N : BCl3
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(CH3)3N BCl3
(CH3)3N : + BCl3 (CH3)3N : BCl3
This compound may be referred to as an adduct.
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CH3COOH(aq) + NH3(aq)
NH4+
(aq) + CH3COO-(aq)
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CH3COOH(aq) + NH3(aq)
NH4+
(aq) + CH3COO-(aq)
NH3 Lewis base
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CH3COOH(aq) + NH3(aq)
NH4+
(aq) + CH3COO-(aq)
NH3 Lewis base
CH3COOH is not a Lewis acid.
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H+ + NH3(aq)
NH4+
(aq) + CH3COO-(aq)
NH3 Lewis base
CH3COOH is not a Lewis acid.
CH3COOH(aq) + H2O H3O+ + CH3COO-
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H+ + NH3(aq)
NH4+
(aq) + CH3COO-(aq)
NH3 Lewis base
CH3COOH is not a Lewis acid.
CH3COOH(aq) + H2O H3O+ + CH3COO-
H3O+ H+ + H2O
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CH3COOH(aq) + NH3(aq)
NH4+
(aq) + CH3COO-(aq)
NH3 Lewis base
CH3COOH is not a Lewis acid.
H+ is the Lewis acid.
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Al(OC2H5)3
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Al(OC2H5)3
Tri-ethoxy aluminum
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Al(OC2H5)3
Al is Group III - electron deficient like BF3.
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Al(OC2H5)3
Al is Group III - electron deficient like boron.
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Al(OC2H5)3
Al is Group III - electron deficient like boron.
This molecule is a Lewis acid.
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Al(OC2H5)3
Al is Group III - electron deficient like boron.
This molecule is a Lewis acid.
O has lone pairs, it is a Lewis base
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Al(OC2H5)3
Al is Group III - electron deficient like boron.
This molecule is a Lewis acid.
O has lone pairs, it is a Lewis base
The molecule is both a Lewis acid and base.
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x3
Al ..
.
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Al(OC2H5)3
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Al(OC2H5)3
Covalent bonds
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Al(OC2H5)3
Electron deficient
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Al(OC2H5)3
Empirical formula
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[Al(OC2H5)3]2
Al(OC2H5)3
Empirical formula
Molecular formula
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[Al(OC2H5)3]2
dimer
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[Al(OC2H5)3]2
dimer
Covalent bonds
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[Al(OC2H5)3]2
dimer
Covalent bondsCoordinate covalent bonds
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[Al(OC2H5)3]2
dimer
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AlCl3
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AlCl3
Empirical formula
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AlCl3
Empirical formula
[AlCl3]2
Molecular formula
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[AlCl3]2
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s block
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s blockp block
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s blockp block
Main Group Elements
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Oxides of s and p block elements
are acid and base anhydrides, with
definite trends in respect to the elements’
location in the periodic table.
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Oxides of non-metals tend to be acid anhydridesOxides of metals tend to be base anhydrides
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Structure and bonding in s and p block oxides
From: N. C. Norman Chapter 5
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Norman: Chapter 6 should be read
for acid and base information.
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Structure and bonding in s and p block oxides
From: N. C. Norman
Group numbers are changed in Norman.
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Groups 1 - 18
3 4 5 6 7 8 9 10 11 12
13 14 15 16 17 18
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Structure and bonding in s and p block oxides
Increasing electronegativity
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Binary ionic compounds form
from elements having very
different electronegativities.
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Binary ionic compounds form
from elements having very
different electronegativities.
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Oxygen is high on the electronegativity scale, Rb and Ba have the lowest electronegativities of the metals on the Norman chart.
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K2O : ionic material
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K2O : ionic material
K2O(s) + H2O(l) 2 K+(aq) + O2-(aq)
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K2O : ionic material
K2O(s) + H2O(l) 2 K+(aq) + O2-(aq)
O2-(aq) + H2O(l) 2 OH-(aq)
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K2O : ionic material
K2O(s) + H2O(l) 2 K+(aq) + 2 OH-(aq)
Strong base
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K2O : ionic material
K2O(s) + H2O(l) 2 K+(aq) + 2 OH-(aq)
Strong base
Base anhydride
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Small differences in electronegativities
lead to covalent bonds.
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Small differences in electronegativities
lead to covalent bonds.
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SO3 : covalent molecule
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SO3 : covalent molecule
SO3(g) + H2O(l) H2SO4(aq)
Strong acid
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SO3 : covalent molecule
SO3(g) + H2O(l) H2SO4(aq)
Strong acid
Acid anhydride
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Some of the polymeric oxides will
be amphoteric.
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Some of the polymeric oxides will
be amphoteric.
They will act as acids or bases depending
on how acidic or basic the environment is.
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Some of the polymeric oxides will
be amphoteric.
Al2O3(aq) + 6 H+(aq) 2 Al3+(aq) + 3 H2O(l)
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Some of the polymeric oxides will
be amphoteric.
Al2O3(aq) + 6 H+(aq) 2 Al3+(aq) + 3 H2O(l)
Al2O3 reduces H+ = basic
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Some of the polymeric oxides will
be amphoteric.
Al2O3(aq) + 6 H+(aq) 2 Al3+(aq) + 3 H2O(l)
Al2O3 reduces H+ = basic
Al2O3(aq) + 2 OH-(aq) + 3 H2O(l) 2 [Al(OH)4]-(aq)
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Some of the polymeric oxides will
be amphoteric.
Al2O3(aq) + 2 OH-(aq) + 3 H2O(l) 2 [Al(OH)4]-(aq)
Al2O3 reduces OH- : acidic
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Structures of polymeric oxides
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quartz
SiO4
Empiricalformula
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quartz
SiO4
Empiricalformula
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quartz
SiO4
Empiricalformula
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quartz
Tetrahedra share all cornersEach share = 1/2 O/Si
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quartz
Tetrahedra share all cornersEach share = 1/2 O/Si
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quartz
Tetrahedra share all cornersEach share = 1/2 O/Si
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Binary compounds
with halogens
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chlorides
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chlorides
NaCl : ionic salt
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chlorides
NaCl : ionic salt
CCl4 : dense liquid
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chlorides
NaCl : ionic salt
CCl4 : dense liquid
BCl3 : gascovalent
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chlorides
AlCl3 : dimer
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chlorides
AlCl3 : dimer
GaCl3 : dimer
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chlorides
AlCl3 : dimer
GaCl3 : dimer
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chlorides
BeCl2 : infinite chain