CH3CH2CH(+)OH, 1-dehydropropanol cation

H8H5H7
\ | /
C3 - C4
/ | \
O1 - C2H9H6
/ \
H11H10
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=-0.327
C2 charge= 0.318
C3 charge=-0.015
C4 charge=-0.368
H5 charge= 0.162
H6 charge= 0.137
H7 charge= 0.175
H8 charge= 0.136
H9 charge= 0.142
H10 charge= 0.144
H11 charge= 0.494
with a dipole moment of 7.06433 Debye

Bond Lengths:

between O1 and C2: distance=1.288 ang___ between O1 and C3: distance=2.377 ang___
between O1 and H11: distance=0.991 ang___ between C2 and C3: distance=1.449 ang___
between C2 and H8: distance=2.120 ang___ between C2 and H10: distance=1.107 ang___
between C3 and C4: distance=1.568 ang___ between C3 and H8: distance=1.104 ang___
between C3 and H9: distance=1.121 ang___ between C4 and H5: distance=1.101 ang___
between C4 and H6: distance=1.103 ang___ between C4 and H7: distance=1.101 ang___

Bond Angles:

for C3-C2-O1: angle=120.4 deg___ for C4-C3-C2: angle=111.9 deg___
for H5-C4-C3: angle=110.4 deg___ for H6-C4-C3: angle=112.1 deg___
for H7-C4-C3: angle=107.7 deg___ for H8-C3-C2: angle=111.6 deg___
for H9-C3-C2: angle=104.2 deg___ for H10-C2-O1: angle=118.3 deg___
for H11-O1-C2: angle=114.7 deg___

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Bond Orders (Mulliken):

between O1 and C2: order=1.463___ between O1 and C3: order=-0.081___
between O1 and H11: order=0.791___ between C2 and C3: order=0.966___
between C2 and H8: order=-0.067___ between C2 and H10: order=0.917___
between C3 and C4: order=0.814___ between C3 and H8: order=0.987___
between C3 and H9: order=0.894___ between C4 and H5: order=0.941___
between C4 and H6: order=0.976___ between C4 and H7: order=0.955___

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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 1.9957 electrons
__has 68.16% O 1 character in a sp1.76 hybrid
__has 31.84% C 2 character in a sp2.46 hybrid

2. A bonding orbital for O1-C2 with 1.9958 electrons
__has 84.60% O 1 character in a p3 hybrid
__has 15.40% C 2 character in a p3 hybrid

3. A bonding orbital for O1-H11 with 1.9873 electrons
__has 77.67% O 1 character in a s0.88 p3 hybrid
__has 22.33% H11 character in a s orbital

4. A bonding orbital for C2-C3 with 1.9915 electrons
__has 51.59% C 2 character in a sp1.51 hybrid
__has 48.41% C 3 character in a sp2.94 hybrid

5. A bonding orbital for C2-H10 with 1.9885 electrons
__has 60.43% C 2 character in a sp2.18 hybrid
__has 39.57% H10 character in a s orbital

6. A bonding orbital for C3-C4 with 1.9618 electrons
__has 55.33% C 3 character in a sp2.50 hybrid
__has 44.67% C 4 character in a sp2.93 hybrid

7. A bonding orbital for C3-H8 with 1.9835 electrons
__has 63.08% C 3 character in a sp2.87 hybrid
__has 36.92% H 8 character in a s orbital

8. A bonding orbital for C3-H9 with 1.9309 electrons
__has 62.81% C 3 character in a s0.77 p3 hybrid
__has 37.19% H 9 character in a s orbital

9. A bonding orbital for C4-H5 with 1.9928 electrons
__has 60.70% C 4 character in a s0.99 p3 hybrid
__has 39.30% H 5 character in a s orbital

10. A bonding orbital for C4-H6 with 1.9925 electrons
__has 60.31% C 4 character in a s0.99 p3 hybrid
__has 39.69% H 6 character in a s orbital

11. A bonding orbital for C4-H7 with 1.9877 electrons
__has 61.81% C 4 character in a s0.98 p3 hybrid
__has 38.19% H 7 character in a s orbital

16. A lone pair orbital for O1 with 1.9812 electrons
__made from a sp1.45 hybrid

-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, 3, for O1-H11 with the antibonding acceptor orbital, 131, for C2-C3 is 20.0 kJ/mol.

The interaction of bonding donor orbital, 6, for C3-C4 with the second antibonding acceptor orbital, 129, for O1-C2 is 38.3 kJ/mol.

The interaction of bonding donor orbital, 8, for C3-H9 with the second antibonding acceptor orbital, 129, for O1-C2 is 71.8 kJ/mol.

The interaction of lone pair donor orbital, 16, for O1 with the antibonding acceptor orbital, 132, for C2-H10 is 29.3 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 ----- -3.068

19 ----- -3.570


18 ----- -5.641


17 ----- -9.830


16 -^-v- -13.84

15 -^-v- -14.07

14 -^-v- -14.88

13 -^-v- -15.50

12 -^-v- -16.29


11 -^-v- -17.58

10 -^-v- -18.03


9 -^-v- -20.71

8 -^-v- -21.02


7 -^-v- -23.12


6 -^-v- -25.98


5 -^-v- -34.75


4 -^-v- -271.4


3 -^-v- -272.6


2 -^-v- -276.4


1 -^-v- -515.5

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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 = -193.5206396857 Hartrees

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