## methylacetate, CH3COOCH3

 H10 / H9 - C8 - H11 O3 \ // O1 - C2 \ H7 - C4 - H6 / H5
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=-0.376
C2 charge= 0.863
O3 charge=-0.558
C4 charge=-0.757
H5 charge= 0.208
H6 charge= 0.211
H7 charge= 0.207
C8 charge=-0.178
H9 charge= 0.136
H10 charge= 0.121
H11 charge= 0.120
with a dipole moment of 1.90637 Debye

## Bond Lengths:

between O1 and C2: distance=1.371 ang___ between O1 and O3: distance=2.284 ang___
between O1 and C4: distance=2.382 ang___ between O1 and C8: distance=1.458 ang___
between C2 and O3: distance=1.224 ang___ between C2 and C4: distance=1.514 ang___
between C2 and H6: distance=2.143 ang___ between C4 and H5: distance=1.103 ang___
between C4 and H6: distance=1.099 ang___ between C4 and H7: distance=1.103 ang___
between C8 and H9: distance=1.099 ang___ between C8 and H10: distance=1.103 ang___
between C8 and H11: distance=1.103 ang___

## Bond Angles:

for O3-C2-O1: angle=123.2 deg___ for C4-C2-O1: angle=111.2 deg___
for H5-C4-C2: angle=110.1 deg___ for H6-C4-C2: angle=109.1 deg___
for H7-C4-C2: angle=110.0 deg___ for C8-O1-C2: angle=115.1 deg___
for H9-C8-O1: angle=105.2 deg___ for H10-C8-O1: angle=110.5 deg___
for H11-C8-O1: angle=110.3 deg___

## Bond Orders (Mulliken):

between O1 and C2: order=1.101___ between O1 and O3: order=-0.192___
between O1 and C4: order=-0.107___ between O1 and C8: order=0.688___
between C2 and O3: order=1.935___ between C2 and C4: order=0.677___
between C2 and H6: order=-0.061___ between C4 and H5: order=0.985___
between C4 and H6: order=0.999___ between C4 and H7: order=0.982___
between C8 and H9: order=0.992___ between C8 and H10: order=0.978___
between C8 and H11: order=0.978___

## 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 1.9936 electrons
__has 68.11% O 1 character in a sp2.33 hybrid
__has 31.89% C 2 character in a sp2.56 hybrid

2. A bonding orbital for O1-C8 with 1.9914 electrons
__has 69.28% O 1 character in a sp2.49 hybrid
__has 30.72% C 8 character in a s0.82 p3 hybrid

3. A bonding orbital for C2-O3 with 1.9980 electrons
__has 35.47% C 2 character in a sp1.86 hybrid
__has 64.53% O 3 character in a sp1.54 hybrid

4. A bonding orbital for C2-O3 with 1.9930 electrons
__has 26.32% C 2 character in a p-pi orbital ( 99.31% p 0.69% d)
__has 73.68% O 3 character in a p-pi orbital ( 99.82% p 0.18% d)

5. A bonding orbital for C2-C4 with 1.9877 electrons
__has 49.52% C 2 character in a sp1.67 hybrid
__has 50.48% C 4 character in a sp2.87 hybrid

6. A bonding orbital for C4-H5 with 1.9817 electrons
__has 60.68% C 4 character in a s0.97 p3 hybrid
__has 39.32% H 5 character in a s orbital

7. A bonding orbital for C4-H6 with 1.9911 electrons
__has 60.72% C 4 character in a sp2.96 hybrid
__has 39.28% H 6 character in a s orbital

8. A bonding orbital for C4-H7 with 1.9814 electrons
__has 60.69% C 4 character in a s0.97 p3 hybrid
__has 39.31% H 7 character in a s orbital

9. A bonding orbital for C8-H9 with 1.9933 electrons
__has 58.72% C 8 character in a sp2.85 hybrid
__has 41.28% H 9 character in a s orbital

10. A bonding orbital for C8-H10 with 1.9961 electrons
__has 58.93% C 8 character in a sp2.78 hybrid
__has 41.07% H10 character in a s orbital

11. A bonding orbital for C8-H11 with 1.9960 electrons
__has 58.90% C 8 character in a sp2.78 hybrid
__has 41.10% H11 character in a s orbital

17. A lone pair orbital for O1 with 1.9704 electrons

18. A lone pair orbital for O1 with 1.8577 electrons
__made from a p-pi orbital ( 99.95% p)

19. A lone pair orbital for O3 with 1.9766 electrons

20. A lone pair orbital for O3 with 1.8863 electrons
__made from a p-pi orbital ( 99.90% p 0.10% d)

149. A antibonding orbital for C2-O3 with 0.1475 electrons
__has 73.68% C 2 character in a p-pi orbital ( 99.31% p 0.69% d)
__has 26.32% O 3 character in a p-pi orbital ( 99.82% p 0.18% d)

-With core pairs on: O 1 C 2 O 3 C 4 C 8 -

#### 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 C4-H5 with the second antibonding acceptor orbital, 149, for C2-O3 is 24.7 kJ/mol.

The interaction of bonding donor orbital, 7, for C4-H6 with the antibonding acceptor orbital, 146, for O1-C2 is 20.7 kJ/mol.

The interaction of bonding donor orbital, 8, for C4-H7 with the second antibonding acceptor orbital, 149, for C2-O3 is 25.3 kJ/mol.

The interaction of lone pair donor orbital, 17, for O1 with the antibonding acceptor orbital, 148, for C2-O3 is 44.3 kJ/mol.

The interaction of the second lone pair donor orbital, 18, for O1 with the second antibonding acceptor orbital, 149, for C2-O3 is 245. kJ/mol.

The interaction of the second lone pair donor orbital, 18, for O1 with the antibonding acceptor orbital, 155, for C8-H10 is 25.1 kJ/mol.

The interaction of the second lone pair donor orbital, 18, for O1 with the antibonding acceptor orbital, 156, for C8-H11 is 25.4 kJ/mol.

The interaction of the second lone pair donor orbital, 20, for O3 with the antibonding acceptor orbital, 146, for O1-C2 is 176. kJ/mol.

The interaction of the second lone pair donor orbital, 20, for O3 with the antibonding acceptor orbital, 150, for C2-C4 is 97.7 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.

24 ----- 1.984

23 ----- 1.624

22 ----- 0.781

21 ----- -1.221

20 -^-v- -6.493

19 -^-v- -7.401

18 -^-v- -8.682

17 -^-v- -9.058

16 -^-v- -9.826

15 -^-v- -10.24

14 -^-v- -10.57

13 -^-v- -11.61

12 -^-v- -12.00

11 -^-v- -12.22

10 -^-v- -13.98

9 -^-v- -17.27

8 -^-v- -19.00

7 -^-v- -25.15

6 -^-v- -27.37

5 -^-v- -266.6

4 -^-v- -267.7

3 -^-v- -269.8

2 -^-v- -506.2

1 -^-v- -507.8

## 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 = -268.4880850339 Hartrees