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.
Please note that your structure can't be well described by a single
Lewis structure, because of extensive delocalization.
Hybridization in the Best Lewis Structure
1. A bonding orbital for S1-O2 with 1.9831 electrons
__has 38.30% S 1 character in a sp1.95 hybrid
__has 61.70% O 2 character in a s0.68 p3 hybrid
2. A bonding orbital for S1-O3 with 1.9989 electrons
__has 20.32% S 1 character in a p-pi orbital ( 94.82% p 5.18% d)
__has 79.68% O 3 character in a p-pi orbital ( 99.84% p 0.16% d)
3. A bonding orbital for S1-O3 with 1.9832 electrons
__has 38.24% S 1 character in a sp1.95 hybrid
__has 61.76% O 3 character in a s0.69 p3 hybrid
4. A bonding orbital for S1-O4 with 1.9831 electrons
__has 38.31% S 1 character in a sp1.95 hybrid
__has 61.69% O 4 character in a s0.68 p3 hybrid
5. A antibonding orbital for O2-O4 with 1.9612 electrons
__has 49.99% O 2 character in a p-pi orbital ( 99.86% p 0.14% d)
__has 50.01% O 4 character in a p-pi orbital ( 99.86% p 0.14% d)
6. A bonding orbital for O2-O4 with 1.4255 electrons
__has 50.01% O 2 character in a p-pi orbital ( 99.86% p 0.14% d)
__has 49.99% O 4 character in a p-pi orbital ( 99.86% p 0.14% d)
15. A lone pair orbital for O2 with 1.9806 electrons
__made from a sp0.22 hybrid
16. A lone pair orbital for O2 with 1.8832 electrons
__made from a p-pi orbital ( 99.87% p 0.13% d)
17. A lone pair orbital for O3 with 1.9806 electrons
__made from a sp0.22 hybrid
18. A lone pair orbital for O3 with 1.8831 electrons
__made from a p-pi orbital ( 99.87% p 0.13% d)
19. A lone pair orbital for O4 with 1.9806 electrons
__made from a sp0.22 hybrid
20. A lone pair orbital for O4 with 1.8834 electrons
__made from a p-pi orbital ( 99.87% p 0.13% d)
100. A antibonding orbital for S1-O2 with 0.1099 electrons
__has 61.70% S 1 character in a sp1.95 hybrid
__has 38.30% O 2 character in a s0.68 p3 hybrid
101. A antibonding orbital for S1-O3 with 0.4923 electrons
__has 79.68% S 1 character in a p-pi orbital ( 94.82% p 5.18% d)
__has 20.32% O 3 character in a p-pi orbital ( 99.84% p 0.16% d)
102. A antibonding orbital for S1-O3 with 0.1098 electrons
__has 61.76% S 1 character in a sp1.95 hybrid
__has 38.24% O 3 character in a s0.69 p3 hybrid
103. A antibonding orbital for S1-O4 with 0.1099 electrons
__has 61.69% S 1 character in a sp1.95 hybrid
__has 38.31% O 4 character in a s0.68 p3 hybrid
-With core pairs on: S 1 S 1 S 1 S 1 S 1 O 2 O 3 O 4 -
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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 S1-O3 with
the bonding acceptor orbital, 6, for O2-O4 is 46.1 kJ/mol.
The interaction of bonding donor orbital, 6, for O2-O4 with
the antibonding acceptor orbital, 101, for S1-O3 is 1015 kJ/mol.
The interaction of the second lone pair donor orbital, 16, for O2 with
the second antibonding acceptor orbital, 102, for S1-O3 is 91.7 kJ/mol.
The interaction of the second lone pair donor orbital, 16, for O2 with
the antibonding acceptor orbital, 103, for S1-O4 is 91.7 kJ/mol.
The interaction of the second lone pair donor orbital, 18, for O3 with
the antibonding acceptor orbital, 100, for S1-O2 is 92.0 kJ/mol.
The interaction of the second lone pair donor orbital, 18, for O3 with
the antibonding acceptor orbital, 103, for S1-O4 is 91.9 kJ/mol.
The interaction of the second lone pair donor orbital, 20, for O4 with
the antibonding acceptor orbital, 100, for S1-O2 is 91.7 kJ/mol.
The interaction of the second lone pair donor orbital, 20, for O4 with
the second antibonding acceptor orbital, 102, for S1-O3 is 91.6 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.
24 ----- 1.942 23 ----- 1.929
22 ----- -4.201
21 ----- -4.464
20 -^-v- -8.554
19 -^-v- -9.993 18 -^-v- -9.995
17 -^-v- -10.45 16 -^-v- -10.45
15 -^-v- -13.40 14 -^-v- -13.40
13 -^-v- -14.04
12 -^-v- -16.13
11 -^-v- -27.10 10 -^-v- -27.11
9 -^-v- -30.44
8 -^-v- -161.7 7 -^-v- -161.8 6 -^-v- -161.9
5 -^-v- -214.6
4 -^-v- -509.0 3 -^-v- -509.0 2 -^-v- -509.0
1 -^-v- -2394.
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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 = -623.9259734732 Hartrees
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