CH3O radical

H3
\
H5 - C1 - O2
/
H4
The multiplicity is 2.

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= 0.249
O2 charge=-0.355
H3 charge= 0.082
H4 charge= 0.009
H5 charge= 0.013
with a dipole moment of 2.52739 Debye

Bond Lengths:

between C1 and O2: distance=1.363 ang___ between C1 and H3: distance=1.129 ang___
between C1 and H4: distance=1.115 ang___ between C1 and H5: distance=1.116 ang___

Bond Angles:

for H3-C1-O2: angle=105.4 deg___ for H4-C1-O2: angle=114.6 deg___
for H5-C1-O2: angle=114.1 deg___

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Bond Orders (Mulliken):

between C1 and O2: order=0.866___ between C1 and H3: order=0.952___
between C1 and H4: order=0.968___ between C1 and H5: order=0.968___

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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. The Lewis structure is built for the up and down electrons, separately. Note that the up and down structures can be very different.

Hybridization in the Best Lewis Structure

Down Electrons

1. A bonding orbital for C1-O2 with 0.9995 electrons
__has 34.04% C 1 character in a sp2.87 hybrid
__has 65.96% O 2 character in a sp2.45 hybrid

2. A bonding orbital for C1-H3 with 0.9986 electrons
__has 55.81% C 1 character in a s0.84 p3 hybrid
__has 44.19% H 3 character in a s orbital

3. A bonding orbital for C1-H4 with 0.9987 electrons
__has 57.72% C 1 character in a sp2.75 hybrid
__has 42.28% H 4 character in a s orbital

4. A bonding orbital for C1-H5 with 0.9987 electrons
__has 57.64% C 1 character in a sp2.79 hybrid
__has 42.36% H 5 character in a s orbital

7. A lone pair orbital for O2 with 0.9969 electrons
__made from a sp0.40 hybrid

8. A lone pair orbital for O2 with 0.9843 electrons
__made from a p3 hybrid

9. A lone pair orbital for O2 with 0.9773 electrons
__made from a p-pi orbital ( 99.96% p)

-With core pairs on: C 1 O 2 -

Up Electrons

1. A bonding orbital for C1-O2 with 0.9995 electrons
__has 38.55% C 1 character in a sp2.80 hybrid
__has 61.45% O 2 character in a sp2.20 hybrid

2. A bonding orbital for C1-H3 with 0.9682 electrons
__has 62.31% C 1 character in a s0.83 p3 hybrid
__has 37.69% H 3 character in a s orbital

3. A bonding orbital for C1-H4 with 0.9936 electrons
__has 59.09% C 1 character in a sp2.79 hybrid
__has 40.91% H 4 character in a s orbital

4. A bonding orbital for C1-H5 with 0.9928 electrons
__has 59.20% C 1 character in a sp2.82 hybrid
__has 40.80% H 5 character in a s orbital

7. A lone pair orbital for O2 with 0.9965 electrons
__made from a sp0.44 hybrid

8. A lone pair orbital for O2 with 0.9730 electrons
__made from a p-pi orbital ( 99.96% p)

-With core pairs on: C 1 O 2 -

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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, 2, for C1-H3 with the third lone pair acceptor orbital, 9, for O2 is 57.2 kJ/mol.

The interaction of the second lone pair donor orbital, 8, for O2 with the antibonding acceptor orbital, 65, for C1-H4 is 32.2 kJ/mol.

The interaction of the second lone pair donor orbital, 8, for O2 with the antibonding acceptor orbital, 66, for C1-H5 is 30.9 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. Only the spin up electron orbital energies are given.

13 ----- 3.280
12 ----- 3.119

11 ----- 1.951

10 ----- 1.450


9 -^--- -6.498

8 -^-v- -7.470


7 -^-v- -10.69

6 -^-v- -11.40

5 -^-v- -11.76


4 -^-v- -16.56


3 -^-v- -25.32


2 -^-v- -268.0


1 -^-v- -507.4

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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 = -115.0940388286 Hartrees

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