## tert-butanol, (CH3)3OH, 2-methyl-2-propanol

 H4 \ H15 H6 - C3 - H5 | / O1 - C2 H8 | \ | H13 \ - C11 C7 - H10 / / H14 H9
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=-0.709
C2 charge= 0.796
C3 charge=-0.664
H4 charge= 0.148
H5 charge= 0.170
H6 charge= 0.162
C7 charge=-0.668
H8 charge= 0.149
H9 charge= 0.163
H10 charge= 0.170
C11 charge=-0.572
H12 charge= 0.161
H13 charge= 0.128
H14 charge= 0.162
H15 charge= 0.402
with a dipole moment of 1.73513 Debye

## Bond Lengths:

between O1 and C2: distance=1.461 ang___ between O1 and C11: distance=2.372 ang___
between O1 and H15: distance=0.977 ang___ between C2 and C3: distance=1.542 ang___
between C2 and H5: distance=2.200 ang___ between C2 and C7: distance=1.542 ang___
between C2 and H10: distance=2.199 ang___ between C2 and C11: distance=1.537 ang___
between C2 and H13: distance=2.190 ang___ between C3 and H4: distance=1.107 ang___
between C3 and H5: distance=1.105 ang___ between C3 and H6: distance=1.104 ang___
between C3 and C7: distance=2.540 ang___ between C3 and C11: distance=2.539 ang___
between C7 and H8: distance=1.107 ang___ between C7 and H9: distance=1.104 ang___
between C7 and H10: distance=1.105 ang___ between C7 and C11: distance=2.540 ang___
between C11 and H12: distance=1.104 ang___ between C11 and H13: distance=1.104 ang___
between C11 and H14: distance=1.104 ang___

## Bond Angles:

for C3-C2-O1: angle=109.4 deg___ for H4-C3-C2: angle=110.7 deg___
for H5-C3-C2: angle=111.3 deg___ for H6-C3-C2: angle=110.1 deg___
for C7-C2-O1: angle=109.4 deg___ for H8-C7-C2: angle=110.7 deg___
for H9-C7-C2: angle=110.1 deg___ for H10-C7-C2: angle=111.3 deg___
for C11-C2-O1: angle=104.5 deg___ for H12-C11-C2: angle=110.0 deg___
for H13-C11-C2: angle=111.0 deg___ for H14-C11-C2: angle=110.1 deg___
for H15-O1-C2: angle=107.5 deg___

## Bond Orders (Mulliken):

between O1 and C2: order=0.702___ between O1 and C11: order=-0.080___
between O1 and H15: order=0.850___ between C2 and C3: order=1.021___
between C2 and H5: order=-0.071___ between C2 and C7: order=1.022___
between C2 and H10: order=-0.072___ between C2 and C11: order=0.973___
between C2 and H13: order=-0.084___ between C3 and H4: order=0.951___
between C3 and H5: order=1.000___ between C3 and H6: order=0.968___
between C3 and C7: order=-0.089___ between C3 and C11: order=-0.129___
between C7 and H8: order=0.951___ between C7 and H9: order=0.968___
between C7 and H10: order=1.000___ between C7 and C11: order=-0.131___
between C11 and H12: order=0.962___ between C11 and H13: order=1.008___
between C11 and H14: order=0.962___

## 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.

### Hybridization in the Best Lewis Structure

1. A bonding orbital for O1-C2 with 1.9928 electrons
__has 66.59% O 1 character in a sp2.49 hybrid
__has 33.41% C 2 character in a s0.75 p3 hybrid

2. A bonding orbital for O1-H15 with 1.9903 electrons
__has 72.89% O 1 character in a s0.78 p3 hybrid
__has 27.11% H15 character in a s orbital

3. A bonding orbital for C2-C3 with 1.9900 electrons
__has 50.66% C 2 character in a sp2.75 hybrid
__has 49.34% C 3 character in a sp2.56 hybrid

4. A bonding orbital for C2-C7 with 1.9901 electrons
__has 50.66% C 2 character in a sp2.74 hybrid
__has 49.34% C 7 character in a sp2.56 hybrid

5. A bonding orbital for C2-C11 with 1.9864 electrons
__has 51.45% C 2 character in a sp2.74 hybrid
__has 48.55% C11 character in a sp2.60 hybrid

6. A bonding orbital for C3-H4 with 1.9920 electrons
__has 58.85% C 3 character in a s0.93 p3 hybrid
__has 41.15% H 4 character in a s orbital

7. A bonding orbital for C3-H5 with 1.9896 electrons
__has 59.24% C 3 character in a s0.94 p3 hybrid
__has 40.76% H 5 character in a s orbital

8. A bonding orbital for C3-H6 with 1.9922 electrons
__has 59.77% C 3 character in a s0.96 p3 hybrid
__has 40.23% H 6 character in a s orbital

9. A bonding orbital for C7-H8 with 1.9920 electrons
__has 58.86% C 7 character in a s0.93 p3 hybrid
__has 41.14% H 8 character in a s orbital

10. A bonding orbital for C7-H9 with 1.9921 electrons
__has 59.77% C 7 character in a s0.96 p3 hybrid
__has 40.23% H 9 character in a s orbital

11. A bonding orbital for C7-H10 with 1.9896 electrons
__has 59.23% C 7 character in a s0.94 p3 hybrid
__has 40.77% H10 character in a s orbital

12. A bonding orbital for C11-H12 with 1.9917 electrons
__has 59.70% C11 character in a s0.96 p3 hybrid
__has 40.30% H12 character in a s orbital

13. A bonding orbital for C11-H13 with 1.9899 electrons
__has 58.90% C11 character in a s0.94 p3 hybrid
__has 41.10% H13 character in a s orbital

14. A bonding orbital for C11-H14 with 1.9917 electrons
__has 59.70% C11 character in a s0.96 p3 hybrid
__has 40.30% H14 character in a s orbital

20. A lone pair orbital for O1 with 1.9860 electrons

21. A lone pair orbital for O1 with 1.9719 electrons
__made from a p-pi orbital ( 99.96% p)

-With core pairs on: O 1 C 2 C 3 C 7 C11 -

#### 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, 7, for C3-H5 with the antibonding acceptor orbital, 167, for O1-C2 is 21.5 kJ/mol.

The interaction of bonding donor orbital, 11, for C7-H10 with the antibonding acceptor orbital, 167, for O1-C2 is 21.5 kJ/mol.

The interaction of the second lone pair donor orbital, 21, for O1 with the antibonding acceptor orbital, 169, for C2-C3 is 27.6 kJ/mol.

The interaction of the second lone pair donor orbital, 21, for O1 with the antibonding acceptor orbital, 170, for C2-C7 is 28.4 kJ/mol.

## 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.

25 ----- 2.125
24 ----- 2.065

23 ----- 1.840

22 ----- 0.636

21 -^-v- -6.216

20 -^-v- -7.667

19 -^-v- -8.329

18 -^-v- -8.497

17 -^-v- -8.748

16 -^-v- -9.148

15 -^-v- -9.593

14 -^-v- -9.969

13 -^-v- -10.95
12 -^-v- -11.03

11 -^-v- -11.98

10 -^-v- -13.92

9 -^-v- -16.85
8 -^-v- -16.87

7 -^-v- -19.36

6 -^-v- -25.01

5 -^-v- -265.8

4 -^-v- -266.0 3 -^-v- -266.0

2 -^-v- -267.9

1 -^-v- -506.2

## 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 = -233.7528237634 Hartrees