CH3NH=N

H3H7
\ /
H5 - C1 - N2
/ \\
H4N6
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=-0.318
N2 charge= 0.513
H3 charge= 0.100
H4 charge= 0.102
H5 charge= 0.131
N6 charge=-0.574
H7 charge= 0.043
with a dipole moment of 3.80176 Debye

Bond Lengths:

between C1 and N2: distance=1.523 ang___ between C1 and H3: distance=1.104 ang___
between C1 and H4: distance=1.104 ang___ between C1 and H5: distance=1.099 ang___
between C1 and N6: distance=2.451 ang___ between N2 and H5: distance=2.126 ang___
between N2 and N6: distance=1.216 ang___ between N2 and H7: distance=1.069 ang___
between N6 and H7: distance=2.014 ang___

Bond Angles:

for H3-C1-N2: angle=108.6 deg___ for H4-C1-N2: angle=108.5 deg___
for H5-C1-N2: angle=107.2 deg___ for N6-N2-C1: angle=126.5 deg___
for H7-N2-C1: angle=109.9 deg___

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Bond Orders (Mulliken):

between C1 and N2: order=0.678___ between C1 and H3: order=0.973___
between C1 and H4: order=0.973___ between C1 and H5: order=0.978___
between C1 and N6: order=0.068___ between N2 and H5: order=-0.057___
between N2 and N6: order=1.549___ between N2 and H7: order=0.801___
between N6 and H7: order=0.079___

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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-N2 with 1.9939 electrons
__has 37.68% C 1 character in a s0.90 p3 hybrid
__has 62.32% N 2 character in a sp1.98 hybrid

2. A bonding orbital for C1-H3 with 1.9910 electrons
__has 59.04% C 1 character in a sp2.94 hybrid
__has 40.96% H 3 character in a s orbital

3. A bonding orbital for C1-H4 with 1.9909 electrons
__has 59.05% C 1 character in a sp2.94 hybrid
__has 40.95% H 4 character in a s orbital

4. A bonding orbital for C1-H5 with 1.9940 electrons
__has 60.33% C 1 character in a sp2.79 hybrid
__has 39.67% H 5 character in a s orbital

5. A bonding orbital for N2-N6 with 1.9979 electrons
__has 57.59% N 2 character in a sp1.44 hybrid
__has 42.41% N 6 character in a sp2.32 hybrid

6. A bonding orbital for N2-N6 with 1.9882 electrons
__has 74.80% N 2 character in a p-pi orbital ( 99.90% p 0.10% d)
__has 25.20% N 6 character in a p-pi orbital ( 99.51% p 0.49% d)

7. A bonding orbital for N2-H7 with 1.9885 electrons
__has 68.72% N 2 character in a sp2.80 hybrid
__has 31.28% H 7 character in a s orbital

11. A lone pair orbital for N6 with 1.9826 electrons
__made from a sp0.41 hybrid

12. A lone pair orbital for N6 with 1.8482 electrons
__made from a p3 hybrid

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

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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 lone pair donor orbital, 11, for N6 with the antibonding acceptor orbital, 90, for C1-N2 is 22.4 kJ/mol.

The interaction of the second lone pair donor orbital, 12, for N6 with the antibonding acceptor orbital, 90, for C1-N2 is 131. kJ/mol.

The interaction of the second lone pair donor orbital, 12, for N6 with the antibonding acceptor orbital, 96, for N2-H7 is 168. 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 ----- 2.220

15 ----- 1.779

14 ----- 0.310


13 ----- -2.361


12 -^-v- -4.302


11 -^-v- -9.013

10 -^-v- -9.245


9 -^-v- -10.37


8 -^-v- -11.69

7 -^-v- -12.67


6 -^-v- -16.00


5 -^-v- -19.21


4 -^-v- -25.89


3 -^-v- -267.4


2 -^-v- -377.2


1 -^-v- -380.4

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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 = -149.9793027009 Hartrees

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