2-dehydro-propanol linear cation, CH3CH(+)CH2OH (*see note)

H6H7
\ /
H5 - C4
\
C3 - H8
/
O1 - C2
| | \
H11H10H9
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

O1 charge=-0.566
C2 charge= 0.085
C3 charge= 0.318
C4 charge=-0.485
H5 charge= 0.258
H6 charge= 0.258
H7 charge= 0.223
H8 charge= 0.116
H9 charge= 0.149
H10 charge= 0.149
H11 charge= 0.492
with a dipole moment of 7.94049 Debye

Bond Lengths:

between O1 and C2: distance=1.392 ang___ between O1 and C3: distance=2.382 ang___
between O1 and H11: distance=0.979 ang___ between C2 and C3: distance=1.446 ang___
between C2 and C4: distance=2.527 ang___ between C2 and H9: distance=1.129 ang___
between C2 and H10: distance=1.129 ang___ between C3 and C4: distance=1.436 ang___
between C3 and H8: distance=1.102 ang___ between C4 and H5: distance=1.122 ang___
between C4 and H6: distance=1.122 ang___ between C4 and H7: distance=1.097 ang___

Bond Angles:

for C3-C2-O1: angle=114.1 deg___ for C4-C3-C2: angle=122.5 deg___
for H5-C4-C3: angle=108.1 deg___ for H6-C4-C3: angle=108.0 deg___
for H7-C4-C3: angle=116.3 deg___ for H8-C3-C2: angle=115.9 deg___
for H9-C2-O1: angle=114.6 deg___ for H10-C2-O1: angle=114.7 deg___
for H11-O1-C2: angle=111.5 deg___

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Bond Orders (Mulliken):

between O1 and C2: order=0.989___ between O1 and C3: order=-0.108___
between O1 and H11: order=0.801___ between C2 and C3: order=0.991___
between C2 and C4: order=0.060___ between C2 and H9: order=0.905___
between C2 and H10: order=0.904___ between C3 and C4: order=0.883___
between C3 and H8: order=0.893___ between C4 and H5: order=0.888___
between C4 and H6: order=0.887___ between C4 and H7: order=0.956___

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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 O1-C2 with 1.9972 electrons
__has 63.50% O 1 character in a sp2.39 hybrid
__has 36.50% C 2 character in a sp2.81 hybrid

2. A bonding orbital for O1-H11 with 1.9875 electrons
__has 75.75% O 1 character in a s0.88 p3 hybrid
__has 24.25% H11 character in a s orbital

3. A bonding orbital for C2-C3 with 1.9910 electrons
__has 50.89% C 2 character in a sp2.34 hybrid
__has 49.11% C 3 character in a sp1.94 hybrid

4. A bonding orbital for C2-H9 with 1.9292 electrons
__has 62.03% C 2 character in a s0.85 p3 hybrid
__has 37.97% H 9 character in a s orbital

5. A bonding orbital for C2-H10 with 1.9289 electrons
__has 62.03% C 2 character in a s0.85 p3 hybrid
__has 37.97% H10 character in a s orbital

6. A bonding orbital for C3-C4 with 1.9939 electrons
__has 50.50% C 3 character in a sp1.72 hybrid
__has 49.50% C 4 character in a sp2.42 hybrid

7. A bonding orbital for C3-H8 with 1.9820 electrons
__has 61.41% C 3 character in a sp2.38 hybrid
__has 38.59% H 8 character in a s orbital

8. A bonding orbital for C4-H5 with 1.9256 electrons
__has 64.84% C 4 character in a s0.84 p3 hybrid
__has 35.16% H 5 character in a s orbital

9. A bonding orbital for C4-H6 with 1.9251 electrons
__has 64.84% C 4 character in a s0.84 p3 hybrid
__has 35.16% H 6 character in a s orbital

10. A bonding orbital for C4-H7 with 1.9903 electrons
__has 63.11% C 4 character in a sp2.66 hybrid
__has 36.89% H 7 character in a s orbital

15. A lone pair orbital for O1 with 1.9823 electrons
__made from a sp1.08 hybrid

16. A lone pair orbital for O1 with 1.9552 electrons
__made from a p-pi orbital ( 99.95% p)

17. A lone pair orbital for C3 with 0.2723 electrons
__made from a p-pi orbital ( 99.92% p 0.08% d)

-With core pairs on: O 1 C 2 C 3 C 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 O1-H11 with the antibonding acceptor orbital, 131, for C2-C3 is 22.3 kJ/mol.

The interaction of bonding donor orbital, 4, for C2-H9 with the lone pair acceptor orbital, 17, for C3 is 86.6 kJ/mol.

The interaction of bonding donor orbital, 5, for C2-H10 with the lone pair acceptor orbital, 17, for C3 is 87.1 kJ/mol.

The interaction of bonding donor orbital, 7, for C3-H8 with the antibonding acceptor orbital, 129, for O1-C2 is 23.5 kJ/mol.

The interaction of bonding donor orbital, 8, for C4-H5 with the lone pair acceptor orbital, 17, for C3 is 89.8 kJ/mol.

The interaction of bonding donor orbital, 9, for C4-H6 with the lone pair acceptor orbital, 17, for C3 is 90.8 kJ/mol.

The interaction of the second lone pair donor orbital, 16, for O1 with the antibonding acceptor orbital, 132, for C2-H9 is 43.4 kJ/mol.

The interaction of the second lone pair donor orbital, 16, for O1 with the antibonding acceptor orbital, 133, for C2-H10 is 42.8 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 ----- -3.170

19 ----- -3.841

18 ----- -4.669


17 ----- -10.13


16 -^-v- -12.66


15 -^-v- -14.23

14 -^-v- -15.09

13 -^-v- -15.68

12 -^-v- -16.43


11 -^-v- -17.68
10 -^-v- -17.72


9 -^-v- -19.29


8 -^-v- -20.44


7 -^-v- -23.56


6 -^-v- -26.36


5 -^-v- -31.70


4 -^-v- -272.3


3 -^-v- -274.3

2 -^-v- -274.8


1 -^-v- -512.6

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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 = -193.4888079451 Hartrees

** In calculations this cation shows a tendency to rearrange to the 1-dehydro-propanol cation or the 3-dehydro-propanol cation. This linear cation is higher in energy than the cyclic 2-dehydropropanol cation.

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