2-dehydro-butane cation, CH3CH2CH(+)CH3

H5
\
H12H13C3 - H4
\ | / \
C1 - C2H7
/ \
H10 - C8H6
| \
H11H9
The ion charge is 1.

Tell me about the atomic charges, dipole moment, bond lengths, angles, bond orders,
molecular orbital energies, or total energy.
Tell me about the best Lewis structure.

Atomic Charges and Dipole Moment

C1 charge=-0.021
C2 charge= 0.290
C3 charge=-0.558
H4 charge= 0.248
H5 charge= 0.222
H6 charge= 0.136
H7 charge= 0.270
C8 charge=-0.443
H9 charge= 0.155
H10 charge= 0.183
H11 charge= 0.186
H12 charge= 0.134
H13 charge= 0.193
with a dipole moment of 5.34604 Debye

Bond Lengths:

between C1 and C2: distance=1.433 ang___ between C1 and C3: distance=2.565 ang___
between C1 and C8: distance=1.533 ang___ between C1 and H12: distance=1.108 ang___
between C1 and H13: distance=1.155 ang___ between C2 and C3: distance=1.449 ang___
between C2 and H5: distance=2.167 ang___ between C2 and H6: distance=1.106 ang___
between C2 and C8: distance=2.585 ang___ between C2 and H12: distance=2.137 ang___
between C2 and H13: distance=1.841 ang___ between C3 and H4: distance=1.109 ang___
between C3 and H5: distance=1.101 ang___ between C3 and H7: distance=1.124 ang___
between C8 and H9: distance=1.103 ang___ between C8 and H10: distance=1.100 ang___
between C8 and H11: distance=1.103 ang___

Bond Angles:

for C3-C2-C1: angle=125.6 deg___ for H4-C3-C2: angle=112.4 deg___
for H5-C3-C2: angle=115.6 deg___ for H6-C2-C1: angle=116.9 deg___
for H7-C2-C1: angle=132.3 deg___ for C8-C1-C2: angle=121.1 deg___
for H9-C8-C1: angle=112.6 deg___ for H10-C8-C1: angle=110.0 deg___
for H11-C8-C1: angle=109.1 deg___ for H12-C1-C2: angle=113.9 deg___
for H13-C1-C2: angle=90.00 deg___

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Bond Orders (Mulliken):

between C1 and C2: order=0.898___ between C1 and C3: order=0.139___
between C1 and C8: order=0.894___ between C1 and H12: order=0.996___
between C1 and H13: order=0.796___ between C2 and C3: order=0.864___
between C2 and H5: order=-0.066___ between C2 and H6: order=0.854___
between C2 and C8: order=-0.057___ between C2 and H12: order=-0.088___
between C2 and H13: order=0.122___ between C3 and H4: order=0.934___
between C3 and H5: order=0.982___ between C3 and H7: order=0.875___
between C8 and H9: order=0.949___ between C8 and H10: order=0.967___
between C8 and H11: order=0.959___

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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 C1-C2 with 1.9915 electrons
__has 50.71% C 1 character in a sp2.47 hybrid
__has 49.29% C 2 character in a sp1.77 hybrid

2. A bonding orbital for C1-C8 with 1.9833 electrons
__has 55.13% C 1 character in a sp2.15 hybrid
__has 44.87% C 8 character in a sp2.73 hybrid

3. A bonding orbital for C1-H12 with 1.9748 electrons
__has 62.95% C 1 character in a s0.97 p3 hybrid
__has 37.05% H12 character in a s orbital

4. A bonding orbital for C1-H13 with 1.8230 electrons
__has 62.21% C 1 character in a s0.53 p3 hybrid
__has 37.79% H13 character in a s orbital

5. A bonding orbital for C2-C3 with 1.9926 electrons
__has 50.44% C 2 character in a sp1.78 hybrid
__has 49.56% C 3 character in a sp2.38 hybrid

6. A bonding orbital for C2-H6 with 1.9796 electrons
__has 61.04% C 2 character in a sp2.55 hybrid
__has 38.96% H 6 character in a s orbital

7. A bonding orbital for C3-H4 with 1.9624 electrons
__has 63.40% C 3 character in a s0.93 p3 hybrid
__has 36.60% H 4 character in a s orbital

8. A bonding orbital for C3-H5 with 1.9887 electrons
__has 62.67% C 3 character in a sp2.77 hybrid
__has 37.33% H 5 character in a s orbital

9. A bonding orbital for C3-H7 with 1.9170 electrons
__has 63.56% C 3 character in a s0.77 p3 hybrid
__has 36.44% H 7 character in a s orbital

10. A bonding orbital for C8-H9 with 1.9911 electrons
__has 60.47% C 8 character in a s0.98 p3 hybrid
__has 39.53% H 9 character in a s orbital

11. A bonding orbital for C8-H10 with 1.9891 electrons
__has 61.56% C 8 character in a s0.98 p3 hybrid
__has 38.44% H10 character in a s orbital

12. A bonding orbital for C8-H11 with 1.9875 electrons
__has 60.89% C 8 character in a s0.94 p3 hybrid
__has 39.11% H11 character in a s orbital

17. A lone pair orbital for C2 with 0.3014 electrons
__made from a p3 hybrid

-With core pairs on: C 1 C 2 C 3 C 8 -

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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, 4, for C1-H13 with the lone pair acceptor orbital, 17, for C2 is 313. kJ/mol.

The interaction of bonding donor orbital, 7, for C3-H4 with the lone pair acceptor orbital, 17, for C2 is 33.7 kJ/mol.

The interaction of bonding donor orbital, 9, for C3-H7 with the lone pair acceptor orbital, 17, for C2 is 127. kJ/mol.

The interaction of bonding donor orbital, 11, for C8-H10 with the antibonding acceptor orbital, 139, for C1-C2 is 22.0 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.

20 ----- -3.198

19 ----- -3.495

18 ----- -4.012


17 ----- -9.860


16 -^-v- -13.70

15 -^-v- -13.94

14 -^-v- -14.61

13 -^-v- -15.03

12 -^-v- -15.73


11 -^-v- -16.85

10 -^-v- -16.97

9 -^-v- -17.49


8 -^-v- -20.00


7 -^-v- -21.59


6 -^-v- -24.15


5 -^-v- -26.71


4 -^-v- -271.1


3 -^-v- -272.3

2 -^-v- -272.9


1 -^-v- -274.8

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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 = -157.5693686306 Hartrees

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