CH3OCN, methyl cyanate

H3
\
C1 - O2
/ | \
H4H5C7
\\
N6
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=-0.128
O2 charge=-0.249
H3 charge= 0.133
H4 charge= 0.123
H5 charge= 0.134
N6 charge=-0.527
C7 charge= 0.515
with a dipole moment of 4.83523 Debye

Bond Lengths:

between C1 and O2: distance=1.482 ang___ between C1 and H3: distance=1.100 ang___
between C1 and H4: distance=1.100 ang___ between C1 and H5: distance=1.100 ang___
between O2 and C7: distance=1.297 ang___ between N6 and C7: distance=1.177 ang___

Bond Angles:

for H3-C1-O2: angle=107.0 deg___ for H4-C1-O2: angle=110.0 deg___
for H5-C1-O2: angle=106.8 deg___ for N6-O2-C1: angle=117.3 deg___
for C7-O2-C1: angle=116.1 deg___

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Bond Orders (Mulliken):

between C1 and O2: order=0.646___ between C1 and H3: order=0.966___
between C1 and H4: order=0.980___ between C1 and H5: order=0.967___
between O2 and C7: order=0.848___ between N6 and C7: order=2.796___

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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 C1-O2 with 1.9753 electrons
__has 29.02% C 1 character in a s0.78 p3 hybrid
__has 70.98% O 2 character in a sp2.69 hybrid

2. A bonding orbital for C1-H3 with 1.9949 electrons
__has 59.37% C 1 character in a sp2.77 hybrid
__has 40.63% H 3 character in a s orbital

3. A bonding orbital for C1-H4 with 1.9953 electrons
__has 59.27% C 1 character in a sp2.75 hybrid
__has 40.73% H 4 character in a s orbital

4. A bonding orbital for C1-H5 with 1.9947 electrons
__has 59.39% C 1 character in a sp2.77 hybrid
__has 40.61% H 5 character in a s orbital

5. A bonding orbital for O2-C7 with 1.9957 electrons
__has 65.35% O 2 character in a sp2.27 hybrid
__has 34.65% C 7 character in a sp1.27 hybrid

6. A bonding orbital for N6-C7 with 1.9975 electrons
__has 55.91% N 6 character in a sp1.84 hybrid
__has 44.09% C 7 character in a sp1.06 hybrid

7. A bonding orbital for N6-C7 with 1.9966 electrons
__has 60.14% N 6 character in a p-pi orbital ( 99.61% p 0.39% d)
__has 39.86% C 7 character in a p-pi orbital ( 99.69% p 0.31% d)

8. A bonding orbital for N6-C7 with 1.9909 electrons
__has 55.80% N 6 character in a s0.19 p3 hybrid
__has 44.20% C 7 character in a s0.24 p3 hybrid

13. A lone pair orbital for O2 with 1.9468 electrons
__made from a sp1.35 hybrid

14. A lone pair orbital for O2 with 1.8826 electrons
__made from a p-pi orbital ( 99.93% p 0.07% d)

15. A lone pair orbital for N6 with 1.9660 electrons
__made from a sp0.69 hybrid

-With core pairs on: C 1 O 2 N 6 C 7 -

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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 third antibonding acceptor orbital, 114, for N6-C7 is 56.2 kJ/mol.

The interaction of lone pair donor orbital, 13, for O2 with the antibonding acceptor orbital, 112, for N6-C7 is 78.7 kJ/mol.

The interaction of the second lone pair donor orbital, 14, for O2 with the second antibonding acceptor orbital, 113, for N6-C7 is 225. kJ/mol.

The interaction of lone pair donor orbital, 15, for N6 with the antibonding acceptor orbital, 111, for O2-C7 is 93.7 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.

19 ----- 1.542

18 ----- 0.478


17 ----- -0.260

16 ----- -1.039


15 -^-v- -7.192

14 -^-v- -8.050

13 -^-v- -8.654


12 -^-v- -10.10

11 -^-v- -10.30


10 -^-v- -12.59

9 -^-v- -12.77


8 -^-v- -14.89


7 -^-v- -19.08


6 -^-v- -22.29


5 -^-v- -28.31


4 -^-v- -268.8
3 -^-v- -268.9


2 -^-v- -377.3


1 -^-v- -509.3

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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 = -208.0158197771 Hartrees

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