## methylethylether, CH3OCH2CH3

 H12 H4 H6 | \ | H10 - C9 C3 - H5 | \ / H11 O1 - C2 | \ H7 H8
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=-0.389
C2 charge= 0.228
C3 charge=-0.316
H4 charge= 0.109
H5 charge= 0.070
H6 charge= 0.092
H7 charge= 0.034
H8 charge= 0.019
C9 charge=-0.136
H10 charge= 0.121
H11 charge= 0.081
H12 charge= 0.085
with a dipole moment of 1.50750 Debye

## Bond Lengths:

between O1 and C2: distance=1.440 ang___ between O1 and C3: distance=2.492 ang___
between O1 and C9: distance=1.432 ang___ between C2 and C3: distance=1.535 ang___
between C2 and H7: distance=1.104 ang___ between C2 and H8: distance=1.113 ang___
between C3 and H4: distance=1.104 ang___ between C3 and H5: distance=1.105 ang___
between C3 and H6: distance=1.104 ang___ between C3 and H8: distance=2.187 ang___
between C9 and H10: distance=1.102 ang___ between C9 and H11: distance=1.112 ang___
between C9 and H12: distance=1.110 ang___

## Bond Angles:

for C3-C2-O1: angle=113.7 deg___ for H4-C3-C2: angle=110.2 deg___
for H5-C3-C2: angle=109.8 deg___ for H6-C3-C2: angle=112.2 deg___
for H7-C2-O1: angle=105.1 deg___ for H8-C2-O1: angle=109.5 deg___
for C9-O1-C2: angle=112.9 deg___ for H10-C9-O1: angle=106.8 deg___
for H11-C9-O1: angle=111.1 deg___ for H12-C9-O1: angle=112.4 deg___

## Bond Orders (Mulliken):

between O1 and C2: order=0.820___ between O1 and C3: order=-0.070___
between O1 and C9: order=0.760___ between C2 and C3: order=0.780___
between C2 and H7: order=1.004___ between C2 and H8: order=1.012___
between C3 and H4: order=0.988___ between C3 and H5: order=0.993___
between C3 and H6: order=0.982___ between C3 and H8: order=-0.051___
between C9 and H10: order=0.990___ between C9 and H11: order=0.983___
between C9 and H12: order=0.983___

## 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 1.9925 electrons
__has 67.04% O 1 character in a sp2.60 hybrid
__has 32.96% C 2 character in a s0.85 p3 hybrid

2. A bonding orbital for O1-C9 with 1.9942 electrons
__has 66.87% O 1 character in a sp2.63 hybrid
__has 33.13% C 9 character in a s0.91 p3 hybrid

3. A bonding orbital for C2-C3 with 1.9964 electrons
__has 49.68% C 2 character in a sp2.30 hybrid
__has 50.32% C 3 character in a sp2.53 hybrid

4. A bonding orbital for C2-H7 with 1.9863 electrons
__has 58.39% C 2 character in a s0.94 p3 hybrid
__has 41.61% H 7 character in a s orbital

5. A bonding orbital for C2-H8 with 1.9897 electrons
__has 57.28% C 2 character in a s0.94 p3 hybrid
__has 42.72% H 8 character in a s orbital

6. A bonding orbital for C3-H4 with 1.9918 electrons
__has 59.62% C 3 character in a s0.95 p3 hybrid
__has 40.38% H 4 character in a s orbital

7. A bonding orbital for C3-H5 with 1.9888 electrons
__has 59.20% C 3 character in a s0.92 p3 hybrid
__has 40.80% H 5 character in a s orbital

8. A bonding orbital for C3-H6 with 1.9921 electrons
__has 59.04% C 3 character in a s0.95 p3 hybrid
__has 40.96% H 6 character in a s orbital

9. A bonding orbital for C9-H10 with 1.9936 electrons
__has 58.66% C 9 character in a sp2.92 hybrid
__has 41.34% H10 character in a s orbital

10. A bonding orbital for C9-H11 with 1.9962 electrons
__has 57.54% C 9 character in a sp2.89 hybrid
__has 42.46% H11 character in a s orbital

11. A bonding orbital for C9-H12 with 1.9965 electrons
__has 57.60% C 9 character in a sp2.86 hybrid
__has 42.40% H12 character in a s orbital

16. A lone pair orbital for O1 with 1.9730 electrons

17. A lone pair orbital for O1 with 1.9413 electrons

-With core pairs on: O 1 C 2 C 3 C 9 -

#### 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, 134, for O1-C2 is 20.1 kJ/mol.

The interaction of the second lone pair donor orbital, 17, for O1 with the antibonding acceptor orbital, 136, for C2-C3 is 37.6 kJ/mol.

The interaction of the second lone pair donor orbital, 17, for O1 with the antibonding acceptor orbital, 138, for C2-H8 is 23.9 kJ/mol.

The interaction of the second lone pair donor orbital, 17, for O1 with the antibonding acceptor orbital, 143, for C9-H11 is 31.7 kJ/mol.

The interaction of the second lone pair donor orbital, 17, for O1 with the antibonding acceptor orbital, 144, for C9-H12 is 37.8 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.

21 ----- 2.024
20 ----- 1.830
19 ----- 1.648

18 ----- 1.157

17 -^-v- -5.790

16 -^-v- -7.309

15 -^-v- -8.420

14 -^-v- -9.070

13 -^-v- -9.555

12 -^-v- -9.885

11 -^-v- -10.91

10 -^-v- -11.72

9 -^-v- -11.89

8 -^-v- -14.55

7 -^-v- -16.72

6 -^-v- -18.54

5 -^-v- -25.32

4 -^-v- -266.0

3 -^-v- -267.2

2 -^-v- -267.4

1 -^-v- -506.4

## 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 = -194.4061678921 Hartrees