Best Lewis Structure
The Lewis structure that is closest to your structure is determined.
The hybridization of the atoms in this idealized Lewis structure
is given in the table below.
The Lewis structure is built for the up and down electrons,
separately. Note that the up and down structures can be very
different.
Hybridization in the Best Lewis Structure
Down Electrons
1. A bonding orbital for C1-C2 with 0.9992 electrons
__has 46.47% C 1 character in a sp2.63 hybrid
__has 53.53% C 2 character in a sp1.68 hybrid
2. A bonding orbital for C1-H3 with 0.9928 electrons
__has 62.60% C 1 character in a s0.89 p3 hybrid
__has 37.40% H 3 character in a s orbital
3. A bonding orbital for C1-H4 with 0.9928 electrons
__has 62.91% C 1 character in a s0.92 p3 hybrid
__has 37.09% H 4 character in a s orbital
4. A bonding orbital for C1-H5 with 0.9911 electrons
__has 63.14% C 1 character in a sp2.79 hybrid
__has 36.86% H 5 character in a s orbital
5. A bonding orbital for C2-H6 with 0.9948 electrons
__has 60.48% C 2 character in a s0.75 p3 hybrid
__has 39.52% H 6 character in a s orbital
6. A bonding orbital for C2-F7 with 0.9986 electrons
__has 28.79% C 2 character in a s0.89 p3 hybrid
__has 71.21% F 7 character in a sp2.74 hybrid
7. A bonding orbital for C2-H8 with 0.9948 electrons
__has 60.47% C 2 character in a s0.75 p3 hybrid
__has 39.53% H 8 character in a s orbital
11. A lone pair orbital for F7 with 0.9965 electrons
__made from a sp0.36 hybrid
12. A lone pair orbital for F7 with 0.9879 electrons
__made from a p3 hybrid
13. A lone pair orbital for F7 with 0.9865 electrons
__made from a p-pi orbital ( 99.97% p)
-With core pairs on: C 1 C 2 F 7 -
Up Electrons
1. A bonding orbital for C1-C2 with 0.9992 electrons
__has 47.91% C 1 character in a sp2.57 hybrid
__has 52.09% C 2 character in a sp1.67 hybrid
2. A bonding orbital for C1-H3 with 0.9209 electrons
__has 67.03% C 1 character in a s0.88 p3 hybrid
__has 32.97% H 3 character in a s orbital
3. A bonding orbital for C1-H4 with 0.9328 electrons
__has 66.61% C 1 character in a s0.89 p3 hybrid
__has 33.39% H 4 character in a s orbital
4. A bonding orbital for C1-H5 with 0.9909 electrons
__has 63.10% C 1 character in a sp2.76 hybrid
__has 36.90% H 5 character in a s orbital
5. A bonding orbital for C2-F7 with 0.9989 electrons
__has 28.92% C 2 character in a s0.90 p3 hybrid
__has 71.08% F 7 character in a sp2.59 hybrid
6. A bonding orbital for C2-H8 with 0.8412 electrons
__has 79.90% C 2 character in a sp1.51 hybrid
__has 20.10% H 8 character in a s orbital
10. A lone pair orbital for C2 with 0.2353 electrons
__made from a p3 hybrid
11. A lone pair orbital for H6 with 0.1818 electrons
__made from a s orbital
12. A lone pair orbital for F7 with 0.9963 electrons
__made from a sp0.39 hybrid
13. A lone pair orbital for F7 with 0.9887 electrons
__made from a p3 hybrid
14. A lone pair orbital for F7 with 0.8650 electrons
__made from a p-pi orbital ( 99.95% p)
-With core pairs on: C 1 C 2 F 7 -
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Donor Acceptor Interactions in the Best Lewis Structure
The localized orbitals in your best Lewis structure
can interact strongly. A filled bonding or lone pair orbital can
act as a donor and an empty or filled bonding, antibonding, or
lone pair orbital can act as an acceptor. These
interactions can strengthen and weaken bonds. For example, a
lone pair donor->antibonding acceptor orbital interaction
will weaken the bond
associated with the antibonding orbital. Conversly, an interaction
with a bonding pair as the acceptor will strengthen the bond.
Strong electron delocalization in your best Lewis structure will
also show up as donor-acceptor interactions.
Interactions greater than 20 kJ/mol for bonding and lone pair
orbitals are listed below.
The interaction of bonding donor orbital, 2, for C1-H3 with
the lone pair acceptor orbital, 10, for C2 is 59.3 kJ/mol.
The interaction of bonding donor orbital, 3, for C1-H4 with
the lone pair acceptor orbital, 10, for C2 is 44.8 kJ/mol.
The interaction of lone pair donor orbital, 10, for C2 with
the antibonding acceptor orbital, 102, for C2-H8 is 59.5 kJ/mol.
The interaction of the third lone pair donor orbital, 14, for F7 with
the lone pair acceptor orbital, 10, for C2 is 219. kJ/mol.
The interaction of bonding donor orbital, 1, for C1-C2 with
the lone pair acceptor orbital, 11, for H6 is 13.8 kJ/mol.
The interaction of bonding donor orbital, 5, for C2-F7 with
the lone pair acceptor orbital, 11, for H6 is 3.93 kJ/mol.
The interaction of bonding donor orbital, 6, for C2-H8 with
the lone pair acceptor orbital, 11, for H6 is 535. kJ/mol.
The interaction of lone pair donor orbital, 10, for C2 with
the lone pair acceptor orbital, 11, for H6 is 487. kJ/mol.
The interaction of lone pair donor orbital, 11, for H6 with
the antibonding acceptor orbital, 102, for C2-H8 is 27.6 kJ/mol.
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Molecular Orbital Energies
The orbital energies are given in eV, where 1 eV=96.49 kJ/mol.
Orbitals with very low energy are core 1s orbitals.
More antibonding orbitals than you might expect are sometimes
listed, because d orbitals are always included for heavy
atoms and p orbitals are included for H atoms.
Up spins are shown with a ^ and down spins are shown as v.
Only the spin up electron orbital energies are given.
17 ----- -3.876
16 ----- -4.786 15 ----- -4.796
14 ----- -5.558
13 -^--- -15.12
12 -^-v- -16.15
11 -^-v- -16.89
10 -^-v- -16.93
9 -^-v- -19.04
8 -^-v- -19.97
7 -^-v- -20.68
6 -^-v- -23.34
5 -^-v- -26.72
4 -^-v- -38.10
3 -^-v- -273.6
2 -^-v- -276.8
1 -^-v- -663.8
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Total Electronic Energy
The total electronic energy is a very large number, so by convention
the units are given in atomic units, that is Hartrees (H). One
Hartree is 2625.5 kJ/mol. The energy reference is for totally
dissociated atoms. In other words, the reference state is a gas
consisting of nuclei and electrons all at infinite distance from
each other. The electronic energy includes all electric
interactions and the kinetic energy of the electrons. This energy
does not include translation, rotation, or vibration of the
the molecule.
Total electronic energy = -178.7140768876 Hartrees
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