C2H4O, ethyleneoxide

H4H5
| /
C3
/ |
C1 - O2
/ |
H6H7
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=-0.200
O2 charge=-0.238
C3 charge=-0.209
H4 charge= 0.163
H5 charge= 0.163
H6 charge= 0.160
H7 charge= 0.161
with a dipole moment of 2.08623 Debye

Bond Lengths:

between C1 and O2: distance=1.449 ang___ between C1 and C3: distance=1.481 ang___
between C1 and H6: distance=1.099 ang___ between C1 and H7: distance=1.099 ang___
between O2 and C3: distance=1.449 ang___ between C3 and H4: distance=1.099 ang___
between C3 and H5: distance=1.099 ang___

Bond Angles:

for C3-O2-C1: angle=61.44 deg___ for H4-C3-O2: angle=115.1 deg___
for H5-C3-O2: angle=115.1 deg___ for H6-C1-O2: angle=115.0 deg___
for H7-C1-O2: angle=115.1 deg___

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Bond Orders (Mulliken):

between C1 and O2: order=0.793___ between C1 and C3: order=1.086___
between C1 and H6: order=0.964___ between C1 and H7: order=0.964___
between O2 and C3: order=0.794___ between C3 and H4: order=0.964___
between C3 and H5: order=0.964___

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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.

Hybridization in the Best Lewis Structure

1. A bonding orbital for C1-O2 with 1.9798 electrons
__has 34.40% C 1 character in a s0.59 p3 hybrid
__has 65.60% O 2 character in a s0.59 p3 hybrid

2. A bonding orbital for C1-C3 with 1.9872 electrons
__has 50.01% C 1 character in a s0.98 p3 hybrid
__has 49.99% C 3 character in a s0.98 p3 hybrid

3. A bonding orbital for C1-H6 with 1.9939 electrons
__has 58.96% C 1 character in a sp2.38 hybrid
__has 41.04% H 6 character in a s orbital

4. A bonding orbital for C1-H7 with 1.9940 electrons
__has 58.96% C 1 character in a sp2.38 hybrid
__has 41.04% H 7 character in a s orbital

5. A bonding orbital for O2-C3 with 1.9798 electrons
__has 65.60% O 2 character in a s0.59 p3 hybrid
__has 34.40% C 3 character in a s0.59 p3 hybrid

6. A bonding orbital for C3-H4 with 1.9939 electrons
__has 58.96% C 3 character in a sp2.38 hybrid
__has 41.04% H 4 character in a s orbital

7. A bonding orbital for C3-H5 with 1.9939 electrons
__has 58.96% C 3 character in a sp2.38 hybrid
__has 41.04% H 5 character in a s orbital

11. A lone pair orbital for O2 with 1.9922 electrons
__made from a sp0.48 hybrid

12. A lone pair orbital for O2 with 1.9464 electrons
__made from a p-pi orbital ( 99.94% p 0.06% d)

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

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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, 1, for C1-O2 with the antibonding acceptor orbital, 94, for O2-C3 is 38.4 kJ/mol.

The interaction of bonding donor orbital, 5, for O2-C3 with the antibonding acceptor orbital, 90, for C1-O2 is 38.4 kJ/mol.

The interaction of the second lone pair donor orbital, 12, for O2 with the antibonding acceptor orbital, 92, for C1-H6 is 28.0 kJ/mol.

The interaction of the second lone pair donor orbital, 12, for O2 with the antibonding acceptor orbital, 93, for C1-H7 is 28.0 kJ/mol.

The interaction of the second lone pair donor orbital, 12, for O2 with the antibonding acceptor orbital, 95, for C3-H4 is 28.1 kJ/mol.

The interaction of the second lone pair donor orbital, 12, for O2 with the antibonding acceptor orbital, 96, for C3-H5 is 28.1 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.

16 ----- 1.993

15 ----- 1.792

14 ----- 0.917

13 ----- 0.744


12 -^-v- -6.240


11 -^-v- -7.813


10 -^-v- -9.301

9 -^-v- -9.799


8 -^-v- -11.84

7 -^-v- -12.55


6 -^-v- -15.51


5 -^-v- -16.52


4 -^-v- -26.64


3 -^-v- -267.8 2 -^-v- -267.8


1 -^-v- -506.9

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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 = -153.8458852583 Hartrees

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