H2C=CHCH2CH2CH3+•, 1-pentene radical cation

H6
/
H5 - C4
\\
H15C3 - H7
\ /
H14 - C1 - C2
/ | \
H12 - C10H9H8
| \
H13H11
The ion charge is 1. The multiplicity is 2.

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= 0.100
C2 charge=-0.172
C3 charge= 0.108
C4 charge=-0.143
H5 charge= 0.196
H6 charge= 0.218
H7 charge= 0.150
H8 charge= 0.168
H9 charge= 0.193
C10 charge=-0.472
H11 charge= 0.160
H12 charge= 0.174
H13 charge= 0.155
H14 charge= 0.091
H15 charge= 0.068
with a dipole moment of 7.78756 Debye

Bond Lengths:

between C1 and C2: distance=1.519 ang___ between C1 and H8: distance=2.199 ang___
between C1 and C10: distance=1.535 ang___ between C1 and H14: distance=1.114 ang___
between C1 and H15: distance=1.113 ang___ between C2 and C3: distance=1.464 ang___
between C2 and C4: distance=2.548 ang___ between C2 and H5: distance=2.855 ang___
between C2 and H8: distance=1.121 ang___ between C2 and H9: distance=1.143 ang___
between C2 and H14: distance=2.143 ang___ between C3 and C4: distance=1.395 ang___
between C3 and H5: distance=2.182 ang___ between C3 and H7: distance=1.103 ang___
between C3 and H9: distance=2.017 ang___ between C4 and H5: distance=1.099 ang___
between C4 and H6: distance=1.097 ang___ between C10 and H11: distance=1.106 ang___
between C10 and H12: distance=1.102 ang___ between C10 and H13: distance=1.105 ang___

Bond Angles:

for C3-C2-C1: angle=123.1 deg___ for C4-C3-C2: angle=126.0 deg___
for H5-C4-C3: angle=121.6 deg___ for H6-C4-C3: angle=121.0 deg___
for H7-C3-C2: angle=116.1 deg___ for H8-C2-C1: angle=111.9 deg___
for H9-C2-C1: angle=111.6 deg___ for C10-C1-C2: angle=113.9 deg___
for H11-C10-C1: angle=112.1 deg___ for H12-C10-C1: angle=110.2 deg___
for H13-C10-C1: angle=111.7 deg___ for H14-C1-C2: angle=107.9 deg___
for H15-C1-C2: angle=111.2 deg___

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Bond Orders (Mulliken):

between C1 and C2: order=0.648___ between C1 and H8: order=-0.089___
between C1 and C10: order=0.797___ between C1 and H14: order=1.019___
between C1 and H15: order=0.962___ between C2 and C3: order=0.986___
between C2 and C4: order=0.216___ between C2 and H5: order=0.053___
between C2 and H8: order=0.988___ between C2 and H9: order=0.821___
between C2 and H14: order=-0.100___ between C3 and C4: order=1.235___
between C3 and H5: order=-0.070___ between C3 and H7: order=0.893___
between C3 and H9: order=0.077___ between C4 and H5: order=0.943___
between C4 and H6: order=0.935___ between C10 and H11: order=0.972___
between C10 and H12: order=0.980___ between C10 and H13: order=0.968___

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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. The Lewis structure is built for the up and down electrons, separately. Note that the up and down structures can be very different.

Hybridization in the Best Lewis Structure

Down Electrons

1. A bonding orbital for C1-C2 with 0.9951 electrons
__has 46.15% C 1 character in a sp2.73 hybrid
__has 53.85% C 2 character in a sp2.04 hybrid

2. A bonding orbital for C1-C10 with 0.9948 electrons
__has 53.15% C 1 character in a sp2.31 hybrid
__has 46.85% C10 character in a sp2.54 hybrid

3. A bonding orbital for C1-H14 with 0.9900 electrons
__has 60.06% C 1 character in a s0.80 p3 hybrid
__has 39.94% H14 character in a s orbital

4. A bonding orbital for C1-H15 with 0.9916 electrons
__has 59.26% C 1 character in a s0.84 p3 hybrid
__has 40.74% H15 character in a s orbital

5. A bonding orbital for C2-C3 with 0.9958 electrons
__has 48.84% C 2 character in a sp2.57 hybrid
__has 51.16% C 3 character in a sp1.71 hybrid

6. A bonding orbital for C2-H8 with 0.9820 electrons
__has 62.59% C 2 character in a s0.84 p3 hybrid
__has 37.41% H 8 character in a s orbital

7. A bonding orbital for C2-H9 with 0.9711 electrons
__has 61.31% C 2 character in a s0.64 p3 hybrid
__has 38.69% H 9 character in a s orbital

8. A bonding orbital for C3-C4 with 0.9974 electrons
__has 50.34% C 3 character in a sp1.90 hybrid
__has 49.66% C 4 character in a sp1.70 hybrid

9. A bonding orbital for C3-C4 with 0.9947 electrons
__has 38.11% C 3 character in a p3 hybrid
__has 61.89% C 4 character in a p3 hybrid

10. A bonding orbital for C3-H7 with 0.9912 electrons
__has 62.05% C 3 character in a sp2.47 hybrid
__has 37.95% H 7 character in a s orbital

11. A bonding orbital for C4-H5 with 0.9951 electrons
__has 62.54% C 4 character in a sp2.13 hybrid
__has 37.46% H 5 character in a s orbital

12. A bonding orbital for C4-H6 with 0.9948 electrons
__has 62.61% C 4 character in a sp2.18 hybrid
__has 37.39% H 6 character in a s orbital

13. A bonding orbital for C10-H11 with 0.9956 electrons
__has 59.90% C10 character in a s0.94 p3 hybrid
__has 40.10% H11 character in a s orbital

14. A bonding orbital for C10-H12 with 0.9946 electrons
__has 60.78% C10 character in a s0.95 p3 hybrid
__has 39.22% H12 character in a s orbital

15. A bonding orbital for C10-H13 with 0.9958 electrons
__has 59.68% C10 character in a s0.94 p3 hybrid
__has 40.32% H13 character in a s orbital

-With core pairs on: C 1 C 2 C 3 C 4 C10 -

Up Electrons

1. A bonding orbital for C1-C2 with 0.9951 electrons
__has 46.21% C 1 character in a sp2.73 hybrid
__has 53.79% C 2 character in a sp2.05 hybrid

2. A bonding orbital for C1-C10 with 0.9950 electrons
__has 53.09% C 1 character in a sp2.32 hybrid
__has 46.91% C10 character in a sp2.54 hybrid

3. A bonding orbital for C1-H14 with 0.9899 electrons
__has 60.12% C 1 character in a s0.81 p3 hybrid
__has 39.88% H14 character in a s orbital

4. A bonding orbital for C1-H15 with 0.9916 electrons
__has 59.28% C 1 character in a s0.84 p3 hybrid
__has 40.72% H15 character in a s orbital

5. A bonding orbital for C2-C3 with 0.9945 electrons
__has 49.58% C 2 character in a sp2.56 hybrid
__has 50.42% C 3 character in a sp1.74 hybrid

6. A bonding orbital for C2-H8 with 0.9711 electrons
__has 63.53% C 2 character in a s0.79 p3 hybrid
__has 36.47% H 8 character in a s orbital

7. A bonding orbital for C2-H9 with 0.9279 electrons
__has 64.48% C 2 character in a s0.68 p3 hybrid
__has 35.52% H 9 character in a s orbital

8. A bonding orbital for C3-C4 with 0.9974 electrons
__has 51.73% C 3 character in a sp1.85 hybrid
__has 48.27% C 4 character in a sp1.71 hybrid

9. A bonding orbital for C3-H7 with 0.9901 electrons
__has 60.97% C 3 character in a sp2.48 hybrid
__has 39.03% H 7 character in a s orbital

10. A bonding orbital for C4-H5 with 0.9940 electrons
__has 59.50% C 4 character in a sp2.14 hybrid
__has 40.50% H 5 character in a s orbital

11. A bonding orbital for C4-H6 with 0.9937 electrons
__has 59.59% C 4 character in a sp2.17 hybrid
__has 40.41% H 6 character in a s orbital

12. A bonding orbital for C10-H11 with 0.9957 electrons
__has 59.90% C10 character in a s0.94 p3 hybrid
__has 40.10% H11 character in a s orbital

13. A bonding orbital for C10-H12 with 0.9946 electrons
__has 60.78% C10 character in a s0.95 p3 hybrid
__has 39.22% H12 character in a s orbital

14. A bonding orbital for C10-H13 with 0.9957 electrons
__has 59.67% C10 character in a s0.94 p3 hybrid
__has 40.33% H13 character in a s orbital

-With core pairs on: C 1 C 2 C 3 C 4 C10 -

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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, 6, for C2-H8 with the lone pair acceptor orbital, 20, for C3 is 21.3 kJ/mol.

The interaction of bonding donor orbital, 7, for C2-H9 with the lone pair acceptor orbital, 20, for C3 is 94.8 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. Only the spin up electron orbital energies are given.

24 ----- -2.812

23 ----- -3.484

22 ----- -3.620


21 ----- -8.037


20 -^--- -12.57

19 -^-v- -12.94
18 -^-v- -13.01

17 -^-v- -13.65


16 -^-v- -14.65

15 -^-v- -14.93

14 -^-v- -15.44


13 -^-v- -16.75
12 -^-v- -16.84


11 -^-v- -17.88


10 -^-v- -19.20

9 -^-v- -20.16


8 -^-v- -22.50


7 -^-v- -24.28


6 -^-v- -26.38


5 -^-v- -270.3


4 -^-v- -271.5


3 -^-v- -272.6

2 -^-v- -273.6

1 -^-v- -273.8

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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 = -196.2454797674 Hartrees

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