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.
Hybridization in the Best Lewis Structure
1. A bonding orbital for C1-C2 with 1.9838 electrons
__has 49.34% C 1 character in a sp2.64 hybrid
__has 50.66% C 2 character in a sp2.64 hybrid
2. A bonding orbital for C1-C10 with 1.9927 electrons
__has 50.50% C 1 character in a sp2.52 hybrid
__has 49.50% C10 character in a sp2.41 hybrid
3. A bonding orbital for C1-H14 with 1.9843 electrons
__has 58.57% C 1 character in a s0.85 p3 hybrid
__has 41.43% H14 character in a s orbital
4. A bonding orbital for C1-H15 with 1.9846 electrons
__has 58.90% C 1 character in a s0.86 p3 hybrid
__has 41.10% H15 character in a s orbital
5. A bonding orbital for C2-C3 with 1.9866 electrons
__has 50.98% C 2 character in a sp2.43 hybrid
__has 49.02% C 3 character in a sp2.01 hybrid
6. A bonding orbital for C2-H8 with 1.9844 electrons
__has 59.05% C 2 character in a s0.86 p3 hybrid
__has 40.95% H 8 character in a s orbital
7. A bonding orbital for C2-H9 with 1.9773 electrons
__has 59.09% C 2 character in a s0.81 p3 hybrid
__has 40.91% H 9 character in a s orbital
8. A bonding orbital for C3-C4 with 1.9928 electrons
__has 50.86% C 3 character in a sp1.52 hybrid
__has 49.14% C 4 character in a sp1.47 hybrid
9. A bonding orbital for C3-C4 with 1.9832 electrons
__has 47.98% C 3 character in a p-pi orbital ( 99.85% p 0.15% d)
__has 52.02% C 4 character in a p-pi orbital ( 99.85% p 0.14% d)
10. A bonding orbital for C3-H7 with 1.9783 electrons
__has 59.03% C 3 character in a sp2.65 hybrid
__has 40.97% H 7 character in a s orbital
11. A bonding orbital for C4-H5 with 1.9870 electrons
__has 58.91% C 4 character in a sp2.36 hybrid
__has 41.09% H 5 character in a s orbital
12. A bonding orbital for C4-H6 with 1.9869 electrons
__has 59.26% C 4 character in a sp2.33 hybrid
__has 40.74% H 6 character in a s orbital
13. A bonding orbital for C10-H11 with 1.9923 electrons
__has 58.95% C10 character in a s0.92 p3 hybrid
__has 41.05% H11 character in a s orbital
14. A bonding orbital for C10-H12 with 1.9920 electrons
__has 59.22% C10 character in a s0.93 p3 hybrid
__has 40.78% H12 character in a s orbital
15. A bonding orbital for C10-H13 with 1.9924 electrons
__has 58.93% C10 character in a s0.92 p3 hybrid
__has 41.07% H13 character in a s orbital
-With core pairs on: C 1 C 2 C 3 C 4 C10 -
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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, 7, for C2-H9 with
the second antibonding acceptor orbital, 174, for C3-C4 is 20.2 kJ/mol.
The interaction of bonding donor orbital, 10, for C3-H7 with
the antibonding acceptor orbital, 176, for C4-H5 is 24.7 kJ/mol.
The interaction of bonding donor orbital, 11, for C4-H5 with
the antibonding acceptor orbital, 175, for C3-H7 is 26.8 kJ/mol.
The interaction of bonding donor orbital, 12, for C4-H6 with
the antibonding acceptor orbital, 170, for C2-C3 is 29.9 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.
24 ----- 2.019
23 ----- 1.767
22 ----- 1.365
21 ----- -0.944
20 -^-v- -6.324
19 -^-v- -7.772
18 -^-v- -7.980
17 -^-v- -8.267
16 -^-v- -8.694
15 -^-v- -9.318
14 -^-v- -9.986
13 -^-v- -10.36
12 -^-v- -10.96
11 -^-v- -11.63
10 -^-v- -13.43
9 -^-v- -14.38
8 -^-v- -16.49
7 -^-v- -18.41
6 -^-v- -19.78
5 -^-v- -265.9
4 -^-v- -266.0
3 -^-v- -266.2
2 -^-v- -266.3
1 -^-v- -266.4
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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 = -196.5874291813 Hartrees
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