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 1.9967 electrons
__has 50.00% C 1 character in a sp1.38 hybrid
__has 50.00% C 2 character in a sp1.38 hybrid
2. A bonding orbital for C1-C2 with 1.9932 electrons
__has 50.00% C 1 character in a p-pi orbital ( 99.86% p 0.14% d)
__has 50.00% C 2 character in a p-pi orbital ( 99.86% p 0.14% d)
3. A bonding orbital for C1-H3 with 1.9791 electrons
__has 61.42% C 1 character in a sp2.11 hybrid
__has 38.58% H 3 character in a s orbital
4. A bonding orbital for C1-Cl4 with 1.9919 electrons
__has 45.79% C 1 character in a sp2.81 hybrid
__has 54.21% Cl 4 character in a s0.62 p3 hybrid
5. A bonding orbital for C2-Cl5 with 1.9919 electrons
__has 45.75% C 2 character in a sp2.82 hybrid
__has 54.25% Cl 5 character in a s0.62 p3 hybrid
6. A bonding orbital for C2-H6 with 1.9792 electrons
__has 61.43% C 2 character in a sp2.11 hybrid
__has 38.57% H 6 character in a s orbital
19. A lone pair orbital for Cl4 with 1.9950 electrons
__made from a sp0.20 hybrid
20. A lone pair orbital for Cl4 with 1.9743 electrons
__made from a p3 hybrid
21. A lone pair orbital for Cl4 with 1.9427 electrons
__made from a p-pi orbital ( 99.97% p)
22. A lone pair orbital for Cl5 with 1.9951 electrons
__made from a sp0.20 hybrid
23. A lone pair orbital for Cl5 with 1.9744 electrons
__made from a p3 hybrid
24. A lone pair orbital for Cl5 with 1.9428 electrons
__made from a p-pi orbital ( 99.97% p)
118. A antibonding orbital for C1-C2 with 0.1101 electrons
__has 50.00% C 1 character in a p-pi orbital ( 99.86% p 0.14% d)
__has 50.00% C 2 character in a p-pi orbital ( 99.86% p 0.14% d)
-With core pairs on: C 1 C 2 Cl 4 Cl 4 Cl 4 Cl 4 Cl 4 Cl 5 Cl 5 Cl 5 Cl 5 Cl 5 -
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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, 3, for C1-H3 with
the antibonding acceptor orbital, 121, for C2-Cl5 is 38.6 kJ/mol.
The interaction of bonding donor orbital, 6, for C2-H6 with
the antibonding acceptor orbital, 120, for C1-Cl4 is 38.4 kJ/mol.
The interaction of the second lone pair donor orbital, 20, for Cl4 with
the antibonding acceptor orbital, 117, for C1-C2 is 28.7 kJ/mol.
The interaction of the second lone pair donor orbital, 20, for Cl4 with
the antibonding acceptor orbital, 119, for C1-H3 is 28.2 kJ/mol.
The interaction of the third lone pair donor orbital, 21, for Cl4 with
the second antibonding acceptor orbital, 118, for C1-C2 is 91.7 kJ/mol.
The interaction of the second lone pair donor orbital, 23, for Cl5 with
the antibonding acceptor orbital, 117, for C1-C2 is 28.7 kJ/mol.
The interaction of the second lone pair donor orbital, 23, for Cl5 with
the antibonding acceptor orbital, 122, for C2-H6 is 28.0 kJ/mol.
The interaction of the third lone pair donor orbital, 24, for Cl5 with
the second antibonding acceptor orbital, 118, for C1-C2 is 91.4 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.
28 ----- 1.809
27 ----- 0.210
26 ----- -1.124
25 ----- -1.750
24 -^-v- -6.448
23 -^-v- -7.735
22 -^-v- -8.001
21 -^-v- -8.553
20 -^-v- -9.829
19 -^-v- -10.27
18 -^-v- -11.81
17 -^-v- -12.76
16 -^-v- -14.38
15 -^-v- -18.41
14 -^-v- -21.50
13 -^-v- -22.54
12 -^-v- -190.6 11 -^-v- -190.6
10 -^-v- -190.7 9 -^-v- -190.7
8 -^-v- -191.0 7 -^-v- -191.1
6 -^-v- -249.1 5 -^-v- -249.1
4 -^-v- -268.4
3 -^-v- -268.4
2 -^-v- -2730. 1 -^-v- -2730.
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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 = -997.8988580470 Hartrees
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