2-dehydromethylpropene cation, CH2=C(CH3)CH2+ (see note)

H4H5
\ /
C3
||
H9C1H6
\ / \ /
H11 - C8C2
| |
H10H7
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= 0.289
C2 charge=-0.090
C3 charge=-0.095
H4 charge= 0.222
H5 charge= 0.192
H6 charge= 0.191
H7 charge= 0.221
C8 charge=-0.535
H9 charge= 0.197
H10 charge= 0.208
H11 charge= 0.197
with a dipole moment of 3.61940 Debye

Bond Lengths:

between C1 and C2: distance=1.402 ang___ between C1 and C3: distance=1.402 ang___
between C1 and H5: distance=2.184 ang___ between C1 and H6: distance=2.184 ang___
between C1 and C8: distance=1.507 ang___ between C1 and H9: distance=2.171 ang___
between C1 and H11: distance=2.169 ang___ between C2 and C3: distance=2.356 ang___
between C2 and H6: distance=1.098 ang___ between C2 and H7: distance=1.100 ang___
between C3 and H4: distance=1.100 ang___ between C3 and H5: distance=1.098 ang___
between C8 and H9: distance=1.101 ang___ between C8 and H10: distance=1.106 ang___
between C8 and H11: distance=1.102 ang___

Bond Angles:

for C3-C1-C2: angle=114.2 deg___ for H4-C3-C1: angle=121.5 deg___
for H5-C3-C1: angle=121.2 deg___ for H6-C2-C1: angle=121.2 deg___
for H7-C2-C1: angle=121.5 deg___ for C8-C1-C2: angle=122.8 deg___
for H9-C8-C1: angle=111.6 deg___ for H10-C8-C1: angle=109.6 deg___
for H11-C8-C1: angle=111.5 deg___

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Bond Orders (Mulliken):

between C1 and C2: order=1.150___ between C1 and C3: order=1.152___
between C1 and H5: order=-0.075___ between C1 and H6: order=-0.074___
between C1 and C8: order=0.642___ between C1 and H9: order=-0.092___
between C1 and H11: order=-0.086___ between C2 and C3: order=0.559___
between C2 and H6: order=0.966___ between C2 and H7: order=0.953___
between C3 and H4: order=0.952___ between C3 and H5: order=0.969___
between C8 and H9: order=1.035___ between C8 and H10: order=0.902___
between C8 and H11: order=1.027___

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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 1.9914 electrons
__has 51.99% C 1 character in a sp2.08 hybrid
__has 48.01% C 2 character in a sp1.59 hybrid

2. A bonding orbital for C1-C3 with 1.9915 electrons
__has 52.01% C 1 character in a sp2.07 hybrid
__has 47.99% C 3 character in a sp1.59 hybrid

3. A bonding orbital for C1-C3 with 1.5310 electrons
__has 70.15% C 1 character in a p-pi orbital ( 99.89% p 0.11% d)
__has 29.85% C 3 character in a p3 hybrid

4. A bonding orbital for C1-C8 with 1.9871 electrons
__has 54.11% C 1 character in a sp1.84 hybrid
__has 45.89% C 8 character in a sp2.57 hybrid

5. A bonding orbital for C2-H6 with 1.9887 electrons
__has 60.49% C 2 character in a sp2.23 hybrid
__has 39.51% H 6 character in a s orbital

6. A bonding orbital for C2-H7 with 1.9896 electrons
__has 61.13% C 2 character in a sp2.25 hybrid
__has 38.87% H 7 character in a s orbital

7. A bonding orbital for C3-H4 with 1.9894 electrons
__has 61.13% C 3 character in a sp2.25 hybrid
__has 38.87% H 4 character in a s orbital

8. A bonding orbital for C3-H5 with 1.9887 electrons
__has 60.48% C 3 character in a sp2.24 hybrid
__has 39.52% H 5 character in a s orbital

9. A bonding orbital for C8-H9 with 1.9873 electrons
__has 61.19% C 8 character in a s0.97 p3 hybrid
__has 38.81% H 9 character in a s orbital

10. A bonding orbital for C8-H10 with 1.9796 electrons
__has 61.41% C 8 character in a s0.91 p3 hybrid
__has 38.59% H10 character in a s orbital

11. A bonding orbital for C8-H11 with 1.9867 electrons
__has 61.21% C 8 character in a s0.96 p3 hybrid
__has 38.79% H11 character in a s orbital

16. A lone pair orbital for C2 with 0.4671 electrons
__made from a p-pi orbital ( 99.77% p 0.23% d)

-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 the second bonding donor orbital, 3, for C1-C3 with the lone pair acceptor orbital, 16, for C2 is 913. kJ/mol.

The interaction of the second bonding donor orbital, 3, for C1-C3 with the second antibonding acceptor orbital, 130, for C1-C3 is 26.5 kJ/mol.

The interaction of bonding donor orbital, 5, for C2-H6 with the antibonding acceptor orbital, 131, for C1-C8 is 30.2 kJ/mol.

The interaction of bonding donor orbital, 6, for C2-H7 with the antibonding acceptor orbital, 129, for C1-C3 is 26.8 kJ/mol.

The interaction of bonding donor orbital, 7, for C3-H4 with the antibonding acceptor orbital, 128, for C1-C2 is 26.8 kJ/mol.

The interaction of bonding donor orbital, 8, for C3-H5 with the antibonding acceptor orbital, 131, for C1-C8 is 30.3 kJ/mol.

The interaction of bonding donor orbital, 9, for C8-H9 with the antibonding acceptor orbital, 128, for C1-C2 is 26.2 kJ/mol.

The interaction of bonding donor orbital, 10, for C8-H10 with the second antibonding acceptor orbital, 130, for C1-C3 is 22.2 kJ/mol.

The interaction of bonding donor orbital, 11, for C8-H11 with the antibonding acceptor orbital, 129, for C1-C3 is 25.1 kJ/mol.

The interaction of lone pair donor orbital, 16, for C2 with the second antibonding acceptor orbital, 130, for C1-C3 is 65.2 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.

19 ----- -2.971

18 ----- -3.614


17 ----- -6.817


16 ----- -11.18


15 -^-v- -13.67

14 -^-v- -14.46

13 -^-v- -15.04

12 -^-v- -15.68

11 -^-v- -15.88


10 -^-v- -17.68

9 -^-v- -17.84


8 -^-v- -19.43


7 -^-v- -22.83

6 -^-v- -23.28


5 -^-v- -26.91


4 -^-v- -271.4


3 -^-v- -273.7

2 -^-v- -274.3 1 -^-v- -274.3

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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 = -156.3313251842 Hartrees

Note: 1-dehydro-1-methylcyclopropane, CH2(CH2)C(+)CH3, rearranges to this cation.
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