CH2NF3

H3F6
\ /
C1 = N2 - F7
/ \
H4F5
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=-0.522
N2 charge= 0.443
H3 charge= 0.295
H4 charge= 0.295
F5 charge=-0.066
F6 charge=-0.066
F7 charge=-0.379
with a dipole moment of 4.40866 Debye

Bond Lengths:

between C1 and N2: distance=1.297 ang___ between C1 and H3: distance=1.090 ang___
between C1 and H4: distance=1.090 ang___ between C1 and F7: distance=2.686 ang___
between N2 and F5: distance=1.405 ang___ between N2 and F6: distance=1.408 ang___
between N2 and F7: distance=1.765 ang___ between F5 and F7: distance=2.330 ang___
between F6 and F7: distance=2.325 ang___

Bond Angles:

for H3-C1-N2: angle=117.1 deg___ for H4-C1-N2: angle=116.7 deg___
for F5-N2-C1: angle=116.6 deg___ for F6-N2-C1: angle=117.1 deg___
for F7-N2-C1: angle=121.9 deg___

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Bond Orders (Mulliken):

between C1 and N2: order=1.627___ between C1 and H3: order=0.955___
between C1 and H4: order=0.956___ between C1 and F7: order=0.147___
between N2 and F5: order=0.854___ between N2 and F6: order=0.853___
between N2 and F7: order=0.452___ between F5 and F7: order=-0.064___
between F6 and F7: order=-0.064___

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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 1.9967 electrons
__has 34.67% C 1 character in a sp2.55 hybrid
__has 65.33% N 2 character in a sp1.00 hybrid

2. A bonding orbital for C1-N2 with 1.9948 electrons
__has 41.62% C 1 character in a s0.06 p3 hybrid
__has 58.38% N 2 character in a p3 hybrid

3. A bonding orbital for C1-H3 with 1.9757 electrons
__has 61.42% C 1 character in a sp1.85 hybrid
__has 38.58% H 3 character in a s orbital

4. A bonding orbital for C1-H4 with 1.9752 electrons
__has 61.41% C 1 character in a sp1.86 hybrid
__has 38.59% H 4 character in a s orbital

5. A bonding orbital for N2-F5 with 1.9903 electrons
__has 42.27% N 2 character in a s0.97 p3 hybrid
__has 57.73% F 5 character in a s0.41 p3 hybrid

6. A bonding orbital for N2-F6 with 1.9902 electrons
__has 42.36% N 2 character in a s0.97 p3 hybrid
__has 57.64% F 6 character in a s0.41 p3 hybrid

12. A lone pair orbital for F5 with 1.9930 electrons
__made from a sp0.25 hybrid

13. A lone pair orbital for F5 with 1.9846 electrons
__made from a s0.22 p3 hybrid

14. A lone pair orbital for F5 with 1.9718 electrons
__made from a p3 hybrid

15. A lone pair orbital for F6 with 1.9930 electrons
__made from a sp0.25 hybrid

16. A lone pair orbital for F6 with 1.9848 electrons
__made from a s0.23 p3 hybrid

17. A lone pair orbital for F6 with 1.9719 electrons
__made from a p3 hybrid

18. A lone pair orbital for F7 with 1.9968 electrons
__made from a sp0.07 hybrid

19. A lone pair orbital for F7 with 1.9957 electrons
__made from a s0.08 p3 hybrid

20. A lone pair orbital for F7 with 1.9912 electrons
__made from a p-pi orbital (100.00% p)

21. A lone pair orbital for F7 with 1.6164 electrons
__made from a s0.14 p3 hybrid

128. A antibonding orbital for C1-N2 with 0.3077 electrons
__has 58.38% C 1 character in a s0.06 p3 hybrid
__has 41.62% N 2 character in a p3 hybrid

132. A antibonding orbital for N2-F6 with 0.1027 electrons
__has 57.64% N 2 character in a s0.97 p3 hybrid
__has 42.36% F 6 character in a s0.41 p3 hybrid

-With core pairs on: C 1 N 2 F 5 F 6 F 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 the second bonding donor orbital, 2, for C1-N2 with the second antibonding acceptor orbital, 128, for C1-N2 is 33.7 kJ/mol.

The interaction of bonding donor orbital, 3, for C1-H3 with the antibonding acceptor orbital, 131, for N2-F5 is 44.1 kJ/mol.

The interaction of bonding donor orbital, 4, for C1-H4 with the antibonding acceptor orbital, 132, for N2-F6 is 45.0 kJ/mol.

The interaction of bonding donor orbital, 5, for N2-F5 with the antibonding acceptor orbital, 132, for N2-F6 is 24.6 kJ/mol.

The interaction of bonding donor orbital, 6, for N2-F6 with the antibonding acceptor orbital, 131, for N2-F5 is 24.8 kJ/mol.

The interaction of the second lone pair donor orbital, 13, for F5 with the second antibonding acceptor orbital, 128, for C1-N2 is 28.9 kJ/mol.

The interaction of the third lone pair donor orbital, 14, for F5 with the antibonding acceptor orbital, 132, for N2-F6 is 47.7 kJ/mol.

The interaction of the second lone pair donor orbital, 16, for F6 with the second antibonding acceptor orbital, 128, for C1-N2 is 28.7 kJ/mol.

The interaction of the third lone pair donor orbital, 17, for F6 with the antibonding acceptor orbital, 131, for N2-F5 is 47.4 kJ/mol.

The interaction of the second antibonding donor orbital, 128, for C1-N2 with the antibonding acceptor orbital, 131, for N2-F5 is 25.0 kJ/mol.

The interaction of the second antibonding donor orbital, 128, for C1-N2 with the antibonding acceptor orbital, 132, for N2-F6 is 27.0 kJ/mol.

The interaction of lone pair donor orbital, 18, for F7 with the antibonding acceptor orbital, 127, for C1-N2 is 3.68 kJ/mol.

The interaction of lone pair donor orbital, 18, for F7 with the second antibonding acceptor orbital, 128, for C1-N2 is 35.8 kJ/mol.

The interaction of the second lone pair donor orbital, 19, for F7 with the antibonding acceptor orbital, 127, for C1-N2 is 4.43 kJ/mol.

The interaction of the second lone pair donor orbital, 19, for F7 with the antibonding acceptor orbital, 131, for N2-F5 is 2.38 kJ/mol.

The interaction of the second lone pair donor orbital, 19, for F7 with the antibonding acceptor orbital, 132, for N2-F6 is 2.59 kJ/mol.

The interaction of the third lone pair donor orbital, 20, for F7 with the antibonding acceptor orbital, 131, for N2-F5 is 6.90 kJ/mol.

The interaction of the third lone pair donor orbital, 20, for F7 with the antibonding acceptor orbital, 132, for N2-F6 is 6.52 kJ/mol.

The interaction of 4th lone pair donor orbital, 21, for F7 with the second antibonding acceptor orbital, 128, for C1-N2 is 503. kJ/mol.

The interaction of 4th lone pair donor orbital, 21, for F7 with the antibonding acceptor orbital, 131, for N2-F5 is 54.0 kJ/mol.

The interaction of 4th lone pair donor orbital, 21, for F7 with the antibonding acceptor orbital, 132, for N2-F6 is 57.3 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.

25 ----- 1.539


24 ----- -2.466

23 ----- -2.659


22 ----- -4.112


21 -^-v- -7.131

20 -^-v- -7.674

19 -^-v- -7.957


18 -^-v- -10.01

17 -^-v- -10.89

16 -^-v- -11.38

15 -^-v- -11.75

14 -^-v- -12.46


13 -^-v- -14.42

12 -^-v- -14.64


11 -^-v- -16.50


10 -^-v- -18.19


9 -^-v- -24.14


8 -^-v- -26.49


7 -^-v- -31.28


6 -^-v- -33.44


5 -^-v- -268.7


4 -^-v- -385.5


3 -^-v- -653.7


2 -^-v- -658.0
1 -^-v- -658.1

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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 = -393.5134113777 Hartrees

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