Chemical Bonding Lewis Structures, Polarity and Bond Classification.
Bond Polarity
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Transcript of Bond Polarity
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Tro, Chemistry: A Molecular Approach 1
Bond Polarity• covalent bonding between unlike atoms results in
unequal sharing of the electronsone atom pulls the electrons in the bond closer to its sideone end of the bond has larger electron density than the
other• the result is a polar covalent bond
bond polaritythe end with the larger electron density gets a partial
negative chargethe end that is electron deficient gets a partial positive
charge
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Tro, Chemistry: A Molecular Approach 2
HF
H F••
FH
EN 2.1 EN 4.0
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Tro, Chemistry: A Molecular Approach 3
Electronegativity• measure of the pull an atom has on bonding
electrons• increases across period (left to right) and• decreases down group (top to bottom)
fluorine is the most electronegative elementfrancium is the least electronegative element
• the larger the difference in electronegativity, the more polar the bondnegative end toward more electronegative atom
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Tro, Chemistry: A Molecular Approach 4
Electronegativity Scale
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Electronegativity and Bond Polarity• If difference in electronegativity between bonded atoms is 0, the
bond is pure covalentequal sharing
• If difference in electronegativity between bonded atoms is 0.1 to 0.4, the bond is nonpolar covalent
• If difference in electronegativity between bonded atoms 0.5 to 1.9, the bond is polar covalent
• If difference in electronegativity between bonded atoms larger than or equal to 2.0, the bond is ionic
“100%”
0 0.4 2.0 4.0
4% 51%Percent Ionic Character
Electronegativity Difference
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Tro, Chemistry: A Molecular Approach 6
Bond Polarity
ENCl = 3.03.0 - 3.0 = 0
Pure Covalent
ENCl = 3.0ENH = 2.1
3.0 – 2.1 = 0.9Polar Covalent
ENCl = 3.0ENNa = 1.0
3.0 – 0.9 = 2.1Ionic
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Tro, Chemistry: A Molecular Approach 7
Water – a Polar Molecule
stream of water attracted to a charged glass rod
stream of hexane not attracted to a charged glass rod
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Tro, Chemistry: A Molecular Approach 8
Example 9.3(c) - Determine whether an N-O bond is ionic, covalent, or polar covalent.
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Tro, Chemistry: A Molecular Approach 9
Lewis Structures of Molecules
• shows pattern of valence electron distribution in the molecule
• useful for understanding the bonding in many compounds
• allows us to predict shapes of molecules• allows us to predict properties of molecules and
how they will interact together
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Tro, Chemistry: A Molecular Approach 10
Lewis Structures• use common bonding patterns
C = 4 bonds & 0 lone pairs, N = 3 bonds & 1 lone pair, O= 2 bonds & 2 lone pairs, H and halogen = 1 bond, Be = 2 bonds & 0 lone pairs, B = 3 bonds & 0 lone pairs
often Lewis structures with line bonds have the lone pairs left off their presence is assumed from common bonding patterns
• structures which result in bonding patterns different from common have formal charges
B C N O F
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Tro, Chemistry: A Molecular Approach 11
Writing Lewis Structures of Molecules HNO3
1) Write skeletal structure H always terminal
in oxyacid, H outside attached to O’s make least electronegative atom central
N is central
2) Count valence electrons sum the valence electrons for each
atom add 1 electron for each − charge subtract 1 electron for each + charge
ONOH
O
N = 5H = 1O3 = 3∙6 = 18Total = 24 e-
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Tro, Chemistry: A Molecular Approach 12
Writing Lewis Structures of Molecules HNO3
3) Attach central atom to the surrounding atoms with pairs of electrons and subtract from the total
ONOH
O
———
ElectronsStart 24Used 8Left 16
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Tro, Chemistry: A Molecular Approach 13
Writing Lewis Structures of Molecules HNO3
4) Complete octets, outside-in H is already complete with 2
1 bond
and re-count electrons
:
::
——— ONOH
O
N = 5H = 1O3 = 3∙6 = 18Total = 24 e-
ElectronsStart 24Used 8Left 16
ElectronsStart 16Used 16Left 0
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Tro, Chemistry: A Molecular Approach 14
Writing Lewis Structures of Molecules HNO35) If all octets complete, give extra electrons to central
atom. elements with d orbitals can have more than 8 electrons
Period 3 and below
6) If central atom does not have octet, bring in electrons from outside atoms to share
follow common bonding patterns if possible
:::
—— ONOH|
O
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Tro, Chemistry: A Molecular Approach 15
Practice - Lewis Structures
• CO2
• SeOF2
• NO2-1
• H3PO4
• SO3-2
• P2H4
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Tro, Chemistry: A Molecular Approach 16
Formal Charge• during bonding, atoms may wind up with more
or less electrons in order to fulfill octets - this results in atoms having a formal charge
FC = valence e- - nonbonding e- - ½ bonding e-
left O FC = 6 - 4 - ½ (4) = 0S FC = 6 - 2 - ½ (6) = +1right O FC = 6 - 6 - ½ (2) = -1• sum of all the formal charges in a molecule = 0
in an ion, total equals the charge
•• •• ••••••••
••O S O••••
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Tro, Chemistry: A Molecular Approach 17
Writing Lewis Formulas of Molecules (cont’d)
7) Assign formal charges to the atoms a) formal charge = valence e- - lone pair e- - ½ bonding e-
b) follow the common bonding patterns
OSO
H|
HOCCH|||OH
0 +1 -1
all 0
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Tro, Chemistry: A Molecular Approach 18
Common Bonding Patterns
B C N O
C+
N+
O+
C-
N-
O-
B-
F
F +
-F
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Tro, Chemistry: A Molecular Approach 19
Practice - Assign Formal Charges
• CO2
• SeOF2
• NO2-1
• H3PO4
• SO3-2
• P2H4
O P
O
O
O
HH
H
••••
•• ••
••
••
••
••
••
F Se
O
F
•••••• ••••
••
••
••
••
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O S
O
O
•••••• ••••
••
••
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O N O ••••••
••
••••H P P H
HH
•• ••
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Tro, Chemistry: A Molecular Approach 20
Resonance• when there is more than one Lewis structure for a
molecule that differ only in the position of the electrons, they are called resonance structures
• the actual molecule is a combination of the resonance forms – a resonance hybridit does not resonate between the two forms,
though we often draw it that way• look for multiple bonds or lone pairs
•••• •• ••••••••
•• ••O S O O S O•••••• ••••
••••
••••
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Tro, Chemistry: A Molecular Approach 21
Resonance
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Tro, Chemistry: A Molecular Approach 22
Ozone Layer
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Tro, Chemistry: A Molecular Approach 23
Exceptions to the Octet Rule• expanded octets
elements with empty d orbitals can have more than 8 electrons
• odd number electron species e.g., NOwill have 1 unpaired electronfree-radicalvery reactive
• incomplete octetsB, Al