Methylpropionate, CH3CH2COOCH3

O3
//
H12O1 - C2H6
\ / \ /
C11 - H14H10 - C4 - C5 - H8
| / \
H13H9H7
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=-0.377
C2 charge= 0.712
O3 charge=-0.535
C4 charge=-0.062
C5 charge=-0.410
H6 charge= 0.127
H7 charge= 0.112
H8 charge= 0.127
H9 charge= 0.065
H10 charge= 0.066
C11 charge=-0.143
H12 charge= 0.155
H13 charge= 0.083
H14 charge= 0.080
with a dipole moment of 4.63252 Debye

Bond Lengths:

between O1 and C2: distance=1.379 ang___ between O1 and O3: distance=2.228 ang___
between O1 and C4: distance=2.491 ang___ between O1 and C11: distance=1.449 ang___
between C2 and O3: distance=1.220 ang___ between C2 and C4: distance=1.526 ang___
between C2 and C11: distance=2.456 ang___ between O3 and C4: distance=2.429 ang___
between O3 and C5: distance=2.823 ang___ between C4 and C5: distance=1.534 ang___
between C4 and H7: distance=2.181 ang___ between C4 and H9: distance=1.108 ang___
between C4 and H10: distance=1.108 ang___ between C5 and H6: distance=1.102 ang___
between C5 and H7: distance=1.103 ang___ between C5 and H8: distance=1.102 ang___
between C5 and H10: distance=2.188 ang___ between C11 and H12: distance=1.100 ang___
between C11 and H13: distance=1.105 ang___ between C11 and H14: distance=1.105 ang___

Bond Angles:

for O3-C2-O1: angle=117.9 deg___ for C4-C2-O1: angle=117.9 deg___
for C5-C4-C2: angle=112.3 deg___ for H6-C5-C4: angle=110.8 deg___
for H7-C5-C4: angle=110.5 deg___ for H8-C5-C4: angle=110.9 deg___
for H9-C4-C2: angle=108.5 deg___ for H10-C4-C2: angle=108.5 deg___
for C11-O1-C2: angle=120.5 deg___ for H12-C11-O1: angle=105.3 deg___
for H13-C11-O1: angle=111.5 deg___ for H14-C11-O1: angle=111.6 deg___

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Bond Orders (Mulliken):

between O1 and C2: order=1.039___ between O1 and O3: order=-0.191___
between O1 and C4: order=-0.151___ between O1 and C11: order=0.696___
between C2 and O3: order=1.974___ between C2 and C4: order=0.770___
between C2 and C11: order=0.060___ between O3 and C4: order=-0.064___
between O3 and C5: order=0.058___ between C4 and C5: order=0.726___
between C4 and H7: order=-0.067___ between C4 and H9: order=1.002___
between C4 and H10: order=1.004___ between C5 and H6: order=0.974___
between C5 and H7: order=1.023___ between C5 and H8: order=0.975___
between C5 and H10: order=-0.050___ between C11 and H12: order=0.983___
between C11 and H13: order=0.981___ between C11 and H14: order=0.981___

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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. 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 1.9924 electrons
__has 68.15% O 1 character in a sp2.31 hybrid
__has 31.85% C 2 character in a sp2.57 hybrid

2. A bonding orbital for O1-C11 with 1.9909 electrons
__has 68.38% O 1 character in a sp2.41 hybrid
__has 31.62% C11 character in a s0.86 p3 hybrid

3. A bonding orbital for C2-O3 with 1.9956 electrons
__has 35.61% C 2 character in a sp1.86 hybrid
__has 64.39% O 3 character in a sp1.53 hybrid

4. A bonding orbital for C2-O3 with 1.9929 electrons
__has 27.34% C 2 character in a p-pi orbital ( 99.35% p 0.65% d)
__has 72.66% O 3 character in a p-pi orbital ( 99.81% p 0.19% d)

5. A bonding orbital for C2-C4 with 1.9894 electrons
__has 48.73% C 2 character in a sp1.66 hybrid
__has 51.27% C 4 character in a s0.96 p3 hybrid

6. A bonding orbital for C4-C5 with 1.9913 electrons
__has 52.52% C 4 character in a sp2.29 hybrid
__has 47.48% C 5 character in a sp2.53 hybrid

7. A bonding orbital for C4-H9 with 1.9748 electrons
__has 60.07% C 4 character in a s0.88 p3 hybrid
__has 39.93% H 9 character in a s orbital

8. A bonding orbital for C4-H10 with 1.9749 electrons
__has 60.05% C 4 character in a s0.88 p3 hybrid
__has 39.95% H10 character in a s orbital

9. A bonding orbital for C5-H6 with 1.9916 electrons
__has 59.98% C 5 character in a s0.94 p3 hybrid
__has 40.02% H 6 character in a s orbital

10. A bonding orbital for C5-H7 with 1.9906 electrons
__has 59.13% C 5 character in a s0.94 p3 hybrid
__has 40.87% H 7 character in a s orbital

11. A bonding orbital for C5-H8 with 1.9916 electrons
__has 60.00% C 5 character in a s0.94 p3 hybrid
__has 40.00% H 8 character in a s orbital

12. A bonding orbital for C11-H12 with 1.9929 electrons
__has 59.42% C11 character in a sp2.86 hybrid
__has 40.58% H12 character in a s orbital

13. A bonding orbital for C11-H13 with 1.9953 electrons
__has 58.18% C11 character in a sp2.83 hybrid
__has 41.82% H13 character in a s orbital

14. A bonding orbital for C11-H14 with 1.9952 electrons
__has 58.16% C11 character in a sp2.83 hybrid
__has 41.84% H14 character in a s orbital

21. A lone pair orbital for O1 with 1.9689 electrons
__made from a sp1.46 hybrid

22. A lone pair orbital for O1 with 1.8648 electrons
__made from a p-pi orbital ( 99.95% p)

23. A lone pair orbital for O3 with 1.9786 electrons
__made from a sp0.64 hybrid

24. A lone pair orbital for O3 with 1.8835 electrons
__made from a p3 hybrid

182. A antibonding orbital for C2-O3 with 0.1372 electrons
__has 72.66% C 2 character in a p-pi orbital ( 99.35% p 0.65% d)
__has 27.34% O 3 character in a p-pi orbital ( 99.81% p 0.19% d)

-With core pairs on: O 1 C 2 O 3 C 4 C 5 C11 -

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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, 7, for C4-H9 with the second antibonding acceptor orbital, 182, for C2-O3 is 24.8 kJ/mol.

The interaction of bonding donor orbital, 8, for C4-H10 with the second antibonding acceptor orbital, 182, for C2-O3 is 24.7 kJ/mol.

The interaction of lone pair donor orbital, 21, for O1 with the antibonding acceptor orbital, 183, for C2-C4 is 32.9 kJ/mol.

The interaction of the second lone pair donor orbital, 22, for O1 with the second antibonding acceptor orbital, 182, for C2-O3 is 224. kJ/mol.

The interaction of the second lone pair donor orbital, 22, for O1 with the antibonding acceptor orbital, 191, for C11-H13 is 29.6 kJ/mol.

The interaction of the second lone pair donor orbital, 22, for O1 with the antibonding acceptor orbital, 192, for C11-H14 is 28.5 kJ/mol.

The interaction of the second lone pair donor orbital, 24, for O3 with the antibonding acceptor orbital, 179, for O1-C2 is 170. kJ/mol.

The interaction of the second lone pair donor orbital, 24, for O3 with the antibonding acceptor orbital, 183, for C2-C4 is 104. 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.

28 ----- 1.269

27 ----- 0.831

26 ----- 0.577


25 ----- -1.196


24 -^-v- -6.378

23 -^-v- -7.206


22 -^-v- -8.260

21 -^-v- -8.614

20 -^-v- -9.189

19 -^-v- -9.724
18 -^-v- -9.783

17 -^-v- -10.28

16 -^-v- -11.12

15 -^-v- -11.61

14 -^-v- -12.30

13 -^-v- -12.64


12 -^-v- -13.91


11 -^-v- -16.18


10 -^-v- -18.09


9 -^-v- -19.45


8 -^-v- -25.19


7 -^-v- -27.22


6 -^-v- -266.2

5 -^-v- -267.1


4 -^-v- -268.1


3 -^-v- -269.7


2 -^-v- -506.0


1 -^-v- -507.8

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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 = -307.8008465868 Hartrees

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