Forming Chemical Bonds - Mister ChemistryS O Se Te Po Cl F Br I At He Ar Ne Kr Xe Rn 1A 2A 3A 4A 5A...
Transcript of Forming Chemical Bonds - Mister ChemistryS O Se Te Po Cl F Br I At He Ar Ne Kr Xe Rn 1A 2A 3A 4A 5A...
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Forming Chemical Bonds
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Basic Concepts of Chemical
Bonding
© 2012 Pearson Education, Inc.
Chemical Bonds• Three basic types of
bonds•
Covalent• Sharing of
electrons.
Metallic• Metal atoms bonded to
several other atoms.
Ionic• Electrostatic attraction
between ions.
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Types of Chemical Bonds
Why do atoms form chemical bonds ?
so that the system can achieve the lowest possible potential energy
H • H•
Example covalent bonding in H2
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Distance of separation between atoms
0
Pote
ntia
l ene
rgy
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Ionic Bonding
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especially prevalent in compounds formed between group 1A and 2A elements with group 6A and 7A elements.
between Elements with the biggest difference in electronegativity
Ionic compounds
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Ionic compounds are usually formed between metals and nonmetals.
Ionic and Molecular Compounds
Molecular compounds are usually formed between two nonmetals.
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When electrons are removed from or added to a neutral atom or molecule, a
charged particle called an ion is formed.
Ions
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Positively charged ions are calledcations
Negatively charged ions are calledanions
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Atoms vs Ions
Na: 11 protons; 11 electrons
Cl: 17 protons; 17 electrons
Cl–: 17 protons; 18 electrons
–
Na+: 11 protons; 10 electrons
+
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Lewis Dot Symbols
A Lewis dot symbol consists of the symbol of an element and one dot for each valence electron in an atom of the element.
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H
Na
Li
K
Rb
Cs
Fr
Mg
Be
Ca
Sr
Ba
Ra
Al
B
Ga
In
Tl
Si
C
Ge
Sn
Pb
P
N
As
Sb
Bi
S
O
Se
Te
Po
Cl
F
Br
I
At
He
Ar
Ne
Kr
Xe
Rn
1A 2A 3A 4A 5A 6A 7A 8A
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Lewis Dot Symbols
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Formation of LiF
Li(s) + 1/2 F2(g) LiF(s)
1s2 2s1 1s2 2s22p5 1s2 1s2 2s22p6
. .. : . .
.Li F+ Li+ . .: : . .
F-
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the ions are packed together to maximize (+) (-) attractions and minimize (+) (+) and (-) (-) repulsions
Solid structure of LiF
Crystal lattice
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Coulomb’s Law
Energy of electrostatic attraction is directly proportional to product of charge and inversely proportional to distance
therefore, strong lattices are favored when the ions have a high charge to size ratio
k = (2.31 x 10-19 J nm)
Coulombic attraction between
two ions
Q1Q2
r= k
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Coulomb’s Law
Energy of electrostatic attraction is directly proportional to product of charge and inversely proportional to distance
= k Q1Q2
r
therefore, strong lattices are favored when the ions have a high charge to size ratio
small ion size
highly chargedCoulombic
attraction between two ions
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Coulomb’s Law Example:
sodium-chlorides energy of interaction is equal to
Coulombic attraction between
two ions
(Na+)(Cl-)r( )= (2.31 x 10-19 J nm)
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Coulomb’s Law Example:
Coulombic attraction between
two ions
(+1)(-1)r( )= (2.31 x 10-19 J nm)
sodium-chlorides energy of interaction is equal to
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0.276 nm= - 8.37 x 10-19 J
The negative sign indicates an attractive force
i.e. the ion pair has a lower potential energy
Coulomb’s Law Example:
Coulombic attraction between
two ions
(+1)(-1)( )= (2.31 x 10-19 J nm)
sodium-chlorides energy of interaction is equal to
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Lattice Energy of IonicCompounds
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Basic Concepts of Chemical
Bonding
© 2012 Pearson Education, Inc.
Energetics of Ionic Bonding
As we saw in the last chapter, it takes 496 kJ/mol to remove electrons from sodium.
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Basic Concepts of Chemical
Bonding
© 2012 Pearson Education, Inc.
Energetics of Ionic Bonding
We get 349 kJ/mol back by giving electrons to chlorine.
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Basic Concepts of Chemical
Bonding
© 2012 Pearson Education, Inc.
Energetics of Ionic Bonding
Na+496
more energy required to remove the electron than is released
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Basic Concepts of Chemical
Bonding
© 2012 Pearson Education, Inc.
Energetics of Ionic Bonding the numbers don’t explain why the reaction of
sodium metal and chlorine gas to form sodium chloride is so exothermic!
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Basic Concepts of Chemical
Bonding
© 2012 Pearson Education, Inc.
Energetics of Ionic Bonding
• There must be a third piece to the puzzle.
• What is as yet unaccounted for is the electrostatic attraction between the newly formed sodium cation and chloride anion.
Na+ Cl-
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Basic Concepts of Chemical
Bonding
© 2012 Pearson Education, Inc.
Lattice Energy• This third piece of the puzzle is the lattice
energy:
The energy required to completely separate a mole of a solid ionic compound into its gaseous ions.
Eel = κ Q1Q2d
• The energy associated with electrostatic interactions is governed by Coulomb’s law:
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the energy released when an ionic solid forms from its ions
Lattice energy
negative sign (-)
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Basic Concepts of Chemical
Bonding
© 2012 Pearson Education, Inc.
Lattice Energy
• Lattice energy, then, increases with the charge on the ions.
• It also increases with decreasing size of ions.
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Lattice energies of some ionic compounds
compound lattice energy (kJ/mol
lattice energy (kJ/molcompound
-632KI KF
KBr
RbF
NaBr
NaCl
NaI
-671
-774
-681
-732
-769
AgCl
NaF
LiF
SrCl2
MgO
-808
-910
-910
-1030
-2142
-3795
K+ I- Mg2+ O2-
larger ions smaller ionssmaller L.E. = larger L.E. =
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Li(s) + 1/2F2(g) LiF(s)
Li(g)
+155 kJ
Li+(g)
+520 kJ
F(g)
+75 kJ
F–(g)
–333 kJ
–594 kJ
–1012 kJ
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Formation of ionic compounds
requires the lattice energy to be sufficiently large to overcome ionization energy of the element that forms the cation.
balance between energy input (ionization energies) and stability gained from formation of the solid
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Formation of ionic compounds
The main impetus for the formation of an ionic compound rather than a covalent compound results from the strong mutual attraction among the ions
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Example
Ionization energies ( I.E.)
Mg(g) Mg2+(g) ΔH = I.E.1 +I.E.2+ 2e-
= 753 +1435 = +2180 kJ/mol
ΔH = I.E.1 + I.E. 2 + I.E. 3
bonds in AlCl3 are polar covalent
Al (g) Al3+(g) + 3e-
= 580 +1815 + 2740 = +5135 kJ/mol
bonding in MgCl2 is ionic;
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Example
bonds in AlCl3 are polar covalent
Al (g) Al3+(g) + 3e-
energy input (ionization energies) out weighs stability gained from formation of an ionic solid
ΔH = I.E.1 + I.E. 2 + I.E. 3= 580 +1815 + 2740 = +5135 kJ/mol
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Ionic compounds
Any compound when melted that conducts electricity is considered ionic
NaCl( s) is made up of Na+ and Cl- ions
Example : NaCl(s) NaCl( l)