(CH3)3COH+•, tert-butylalcohol radical cation

H9
\
H3H10 - C6 - H11
\ /
H5 - C1 - C2 - C7 - H13
/ | | \
H4O8H14H12
|
H15
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=-0.609
C2 charge= 0.444
H3 charge= 0.233
H4 charge= 0.247
H5 charge= 0.203
C6 charge=-0.413
C7 charge=-0.575
O8 charge=-0.360
H9 charge= 0.234
H10 charge= 0.212
H11 charge= 0.231
H12 charge= 0.205
H13 charge= 0.232
H14 charge= 0.254
H15 charge= 0.459
with a dipole moment of 6.51992 Debye

Bond Lengths:

between C1 and C2: distance=1.522 ang___ between C1 and H3: distance=1.101 ang___
between C1 and H4: distance=1.109 ang___ between C1 and H5: distance=1.105 ang___
between C2 and C6: distance=1.784 ang___ between C2 and C7: distance=1.523 ang___
between C2 and O8: distance=1.378 ang___ between C6 and O8: distance=2.446 ang___
between C6 and H9: distance=1.100 ang___ between C6 and H10: distance=1.099 ang___
between C6 and H11: distance=1.098 ang___ between C7 and H12: distance=1.100 ang___
between C7 and H13: distance=1.102 ang___ between C7 and H14: distance=1.110 ang___
between O8 and H15: distance=0.989 ang___

Bond Angles:

for H3-C1-C2: angle=111.1 deg___ for H4-C1-C2: angle=107.7 deg___
for H5-C1-C2: angle=113.1 deg___ for C6-C2-C1: angle=105.1 deg___
for C7-C2-C1: angle=118.6 deg___ for O8-C2-C1: angle=115.8 deg___
for H9-C6-C2: angle=101.2 deg___ for H10-C6-C2: angle=105.5 deg___
for H11-C6-C2: angle=105.3 deg___ for H12-C7-C2: angle=111.4 deg___
for H13-C7-C2: angle=112.4 deg___ for H14-C7-C2: angle=106.9 deg___
for H15-O8-C2: angle=112.0 deg___

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Bond Orders (Mulliken):

between C1 and C2: order=0.949___ between C1 and H3: order=0.957___
between C1 and H4: order=0.947___ between C1 and H5: order=0.956___
between C2 and C6: order=0.538___ between C2 and C7: order=0.939___
between C2 and O8: order=1.172___ between C6 and O8: order=0.055___
between C6 and H9: order=0.934___ between C6 and H10: order=0.945___
between C6 and H11: order=0.941___ between C7 and H12: order=0.962___
between C7 and H13: order=0.956___ between C7 and H14: order=0.948___
between O8 and H15: order=0.826___

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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 0.9920 electrons
__has 48.75% C 1 character in a sp2.42 hybrid
__has 51.25% C 2 character in a sp2.12 hybrid

2. A bonding orbital for C1-H3 with 0.9903 electrons
__has 62.68% C 1 character in a s0.96 p3 hybrid
__has 37.32% H 3 character in a s orbital

3. A bonding orbital for C1-H4 with 0.9896 electrons
__has 62.20% C 1 character in a s0.86 p3 hybrid
__has 37.80% H 4 character in a s orbital

4. A bonding orbital for C1-H5 with 0.9923 electrons
__has 61.76% C 1 character in a s0.95 p3 hybrid
__has 38.24% H 5 character in a s orbital

5. A bonding orbital for C2-C6 with 0.9847 electrons
__has 44.68% C 2 character in a s0.56 p3 hybrid
__has 55.32% C 6 character in a s0.81 p3 hybrid

6. A bonding orbital for C2-C7 with 0.9883 electrons
__has 51.89% C 2 character in a sp2.21 hybrid
__has 48.11% C 7 character in a sp2.44 hybrid

7. A bonding orbital for C2-O8 with 0.9959 electrons
__has 28.13% C 2 character in a s0.82 p3 hybrid
__has 71.87% O 8 character in a sp1.65 hybrid

8. A bonding orbital for C6-H9 with 0.9961 electrons
__has 62.38% C 6 character in a sp2.92 hybrid
__has 37.62% H 9 character in a s orbital

9. A bonding orbital for C6-H10 with 0.9966 electrons
__has 62.64% C 6 character in a sp2.79 hybrid
__has 37.36% H10 character in a s orbital

10. A bonding orbital for C6-H11 with 0.9965 electrons
__has 63.45% C 6 character in a sp2.70 hybrid
__has 36.55% H11 character in a s orbital

11. A bonding orbital for C7-H12 with 0.9912 electrons
__has 62.04% C 7 character in a s0.95 p3 hybrid
__has 37.96% H12 character in a s orbital

12. A bonding orbital for C7-H13 with 0.9923 electrons
__has 62.67% C 7 character in a s0.98 p3 hybrid
__has 37.33% H13 character in a s orbital

13. A bonding orbital for C7-H14 with 0.9896 electrons
__has 62.00% C 7 character in a s0.85 p3 hybrid
__has 38.00% H14 character in a s orbital

14. A bonding orbital for O8-H15 with 0.9932 electrons
__has 78.59% O 8 character in a s0.82 p3 hybrid
__has 21.41% H15 character in a s orbital

20. A lone pair orbital for O8 with 0.9903 electrons
__made from a sp1.43 hybrid

21. A lone pair orbital for O8 with 0.9799 electrons
__made from a p3 hybrid

-With core pairs on: C 1 C 2 C 6 C 7 O 8 -

Up Electrons

1. A bonding orbital for C1-C2 with 0.9799 electrons
__has 47.57% C 1 character in a sp2.51 hybrid
__has 52.43% C 2 character in a sp1.67 hybrid

2. A bonding orbital for C1-H3 with 0.9909 electrons
__has 62.47% C 1 character in a s0.95 p3 hybrid
__has 37.53% H 3 character in a s orbital

3. A bonding orbital for C1-H4 with 0.9698 electrons
__has 63.87% C 1 character in a s0.94 p3 hybrid
__has 36.13% H 4 character in a s orbital

4. A bonding orbital for C1-H5 with 0.9910 electrons
__has 61.81% C 1 character in a s0.92 p3 hybrid
__has 38.19% H 5 character in a s orbital

5. A bonding orbital for C2-C7 with 0.9716 electrons
__has 53.59% C 2 character in a sp1.66 hybrid
__has 46.41% C 7 character in a sp2.55 hybrid

6. A bonding orbital for C2-O8 with 0.9934 electrons
__has 28.54% C 2 character in a s0.78 p3 hybrid
__has 71.46% O 8 character in a sp1.60 hybrid

7. A bonding orbital for C2-O8 with 0.9251 electrons
__has 24.97% C 2 character in a s0.14 p3 hybrid
__has 75.03% O 8 character in a p3 hybrid

8. A bonding orbital for C6-H9 with 0.9824 electrons
__has 62.17% C 6 character in a sp2.07 hybrid
__has 37.83% H 9 character in a s orbital

9. A bonding orbital for C6-H10 with 0.9907 electrons
__has 61.32% C 6 character in a sp2.15 hybrid
__has 38.68% H10 character in a s orbital

10. A bonding orbital for C6-H11 with 0.9918 electrons
__has 61.91% C 6 character in a sp2.13 hybrid
__has 38.09% H11 character in a s orbital

11. A bonding orbital for C7-H12 with 0.9918 electrons
__has 61.76% C 7 character in a s0.94 p3 hybrid
__has 38.24% H12 character in a s orbital

12. A bonding orbital for C7-H13 with 0.9912 electrons
__has 62.65% C 7 character in a s0.95 p3 hybrid
__has 37.35% H13 character in a s orbital

13. A bonding orbital for C7-H14 with 0.9663 electrons
__has 63.81% C 7 character in a s0.94 p3 hybrid
__has 36.19% H14 character in a s orbital

14. A bonding orbital for O8-H15 with 0.9932 electrons
__has 77.13% O 8 character in a s0.83 p3 hybrid
__has 22.87% H15 character in a s orbital

21. A lone pair orbital for O8 with 0.9897 electrons
__made from a sp1.53 hybrid

-With core pairs on: C 1 C 2 C 6 C 7 O 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, 3, for C1-H4 with the second antibonding acceptor orbital, 118, for C2-O8 is 44.7 kJ/mol.

The interaction of bonding donor orbital, 13, for C7-H14 with the second antibonding acceptor orbital, 118, for C2-O8 is 49.7 kJ/mol.

The interaction of bonding donor orbital, 1, for C1-C2 with the lone pair acceptor orbital, 20, for C6 is 49.7 kJ/mol.

The interaction of bonding donor orbital, 5, for C2-C7 with the lone pair acceptor orbital, 20, for C6 is 61.8 kJ/mol.

The interaction of bonding donor orbital, 6, for C2-O8 with the lone pair acceptor orbital, 20, for C6 is 6.94 kJ/mol.

The interaction of the second bonding donor orbital, 7, for C2-O8 with the lone pair acceptor orbital, 20, for C6 is 156. kJ/mol.

The interaction of bonding donor orbital, 8, for C6-H9 with the antibonding acceptor orbital, 117, for C2-O8 is 8.95 kJ/mol.

The interaction of bonding donor orbital, 8, for C6-H9 with the second antibonding acceptor orbital, 118, for C2-O8 is 46.4 kJ/mol.

The interaction of bonding donor orbital, 9, for C6-H10 with the second antibonding acceptor orbital, 118, for C2-O8 is 37.0 kJ/mol.

The interaction of bonding donor orbital, 10, for C6-H11 with the antibonding acceptor orbital, 112, for C1-C2 is 2.38 kJ/mol.

The interaction of bonding donor orbital, 10, for C6-H11 with the second antibonding acceptor orbital, 118, for C2-O8 is 32.7 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.

25 ----- -2.847

24 ----- -3.386


23 ----- -4.591

22 ----- -5.277


21 -^--- -12.73


20 -^-v- -14.28

19 -^-v- -14.48

18 -^-v- -14.58
17 -^-v- -14.67

16 -^-v- -15.18

15 -^-v- -15.84

14 -^-v- -16.03


13 -^-v- -17.23
12 -^-v- -17.28

11 -^-v- -18.17


10 -^-v- -21.00


9 -^-v- -22.78

8 -^-v- -22.93


7 -^-v- -25.51


6 -^-v- -33.10


5 -^-v- -271.6

4 -^-v- -271.8


3 -^-v- -273.0


2 -^-v- -275.2


1 -^-v- -514.3

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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 = -233.4061215744 Hartrees

*The Lewis Structure (NBO) analysis was done at the DZVP level without diffuse functions to decrease the size of the calculation

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