## H2CC...HCN, vinylidene HCN complex

 H3 \ C1 = C5 C2 E N7 / / H4 H6
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=-0.744
C2 charge= 0.390
H3 charge= 0.365
H4 charge= 0.361
C5 charge= 0.221
H6 charge=-0.143
N7 charge=-0.450
with a dipole moment of 6.86684 Debye

## Bond Lengths:

between C1 and H3: distance=1.101 ang___ between C1 and H4: distance=1.103 ang___
between C1 and C5: distance=1.298 ang___ between C2 and H6: distance=1.095 ang___
between C2 and N7: distance=1.166 ang___ between H3 and C5: distance=2.105 ang___
between H4 and C5: distance=2.079 ang___ between C5 and H6: distance=2.266 ang___
between H6 and N7: distance=2.261 ang___

## Bond Angles:

for H3-C1-C2: angle=123.9 deg___ for H4-C1-C2: angle=118.2 deg___
for C5-C1-C2: angle=1.523 deg___ for H6-C2-C1: angle=1.443 deg___
for N7-C2-C1: angle=178.3 deg___

## Bond Orders (Mulliken):

between C1 and H3: order=0.856___ between C1 and H4: order=0.849___
between C1 and C5: order=1.536___ between C2 and H6: order=0.777___
between C2 and N7: order=2.911___ between H3 and C5: order=0.091___
between H4 and C5: order=0.097___ between C5 and H6: order=0.090___
between H6 and N7: order=0.053___

## 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-H3 with 1.9618 electrons
__has 62.88% C 1 character in a sp2.34 hybrid
__has 37.12% H 3 character in a s orbital

2. A bonding orbital for C1-H4 with 1.9580 electrons
__has 62.77% C 1 character in a sp2.44 hybrid
__has 37.23% H 4 character in a s orbital

3. A bonding orbital for C1-C5 with 1.9996 electrons
__has 56.58% C 1 character in a p-pi orbital ( 99.74% p 0.26% d)
__has 43.42% C 5 character in a p-pi orbital ( 99.64% p 0.36% d)

4. A bonding orbital for C1-C5 with 1.9967 electrons
__has 57.06% C 1 character in a sp1.40 hybrid
__has 42.94% C 5 character in a sp1.77 hybrid

5. A bonding orbital for C2-H6 with 1.9918 electrons
__has 63.88% C 2 character in a sp0.90 hybrid
__has 36.12% H 6 character in a s orbital

6. A bonding orbital for C2-N7 with 1.9998 electrons
__has 43.86% C 2 character in a p-pi orbital ( 99.71% p 0.29% d)
__has 56.14% N 7 character in a p-pi orbital ( 99.62% p 0.38% d)

7. A bonding orbital for C2-N7 with 1.9998 electrons
__has 43.93% C 2 character in a p-pi orbital ( 99.71% p 0.29% d)
__has 56.07% N 7 character in a p-pi orbital ( 99.61% p 0.38% d)

8. A bonding orbital for C2-N7 with 1.9982 electrons
__has 42.77% C 2 character in a sp1.09 hybrid
__has 57.23% N 7 character in a sp1.15 hybrid

13. A lone pair orbital for C5 with 1.9596 electrons

15. A lone pair orbital for N7 with 1.9783 electrons

-With core pairs on: C 1 C 2 C 5 N 7 -

#### 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-H3 with the second lone pair acceptor orbital, 14, for C5 is 61.2 kJ/mol.

The interaction of bonding donor orbital, 2, for C1-H4 with the second lone pair acceptor orbital, 14, for C5 is 71.0 kJ/mol.

The interaction of lone pair donor orbital, 13, for C5 with the antibonding acceptor orbital, 111, for C2-H6 is 58.0 kJ/mol.

The interaction of lone pair donor orbital, 15, for N7 with the antibonding acceptor orbital, 111, for C2-H6 is 40.1 kJ/mol.

## 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.

18 ----- -0.499
17 ----- -0.578

16 ----- -1.839

15 ----- -4.963

14 -^-v- -7.851

13 -^-v- -8.227

12 -^-v- -8.440 11 -^-v- -8.441

10 -^-v- -8.563

9 -^-v- -12.41

8 -^-v- -13.92

7 -^-v- -14.26

6 -^-v- -20.17

5 -^-v- -22.20

4 -^-v- -267.1

3 -^-v- -267.4

2 -^-v- -269.0

1 -^-v- -377.3

## 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 = -170.7425889106 Hartrees