## HCN...CH2=O, HCN acetaldehyde complex

 H7 / N3 E C1 - H4 O6 = C2 \ H5
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= 0.231
C2 charge= 0.304
N3 charge=-0.394
H4 charge= 0.109
H5 charge= 0.044
O6 charge=-0.344
H7 charge= 0.049
with a dipole moment of 6.28454 Debye

## Bond Lengths:

between C1 and N3: distance=1.165 ang___ between C1 and H4: distance=1.086 ang___
between C2 and H5: distance=1.119 ang___ between C2 and O6: distance=1.222 ang___
between C2 and H7: distance=1.120 ang___

## Bond Angles:

for N3-C1-C2: angle=176.2 deg___ for H4-C1-C2: angle=3.386 deg___
for H5-C2-C1: angle=126.0 deg___ for O6-C2-C1: angle=4.861 deg___
for H7-C2-C1: angle=116.9 deg___

## Bond Orders (Mulliken):

between C1 and N3: order=2.882___ between C1 and H4: order=0.832___
between C2 and H5: order=0.959___ between C2 and O6: order=1.811___
between C2 and H7: order=0.947___

## 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-N3 with 1.9999 electrons
__has 43.96% C 1 character in a p-pi orbital ( 99.71% p 0.29% d)
__has 56.04% N 3 character in a p-pi orbital ( 99.61% p 0.38% d)

2. A bonding orbital for C1-N3 with 1.9999 electrons
__has 43.97% C 1 character in a p-pi orbital ( 99.71% p 0.29% d)
__has 56.03% N 3 character in a p-pi orbital ( 99.61% p 0.38% d)

3. A bonding orbital for C1-N3 with 1.9981 electrons
__has 42.83% C 1 character in a sp1.08 hybrid
__has 57.17% N 3 character in a sp1.15 hybrid

4. A bonding orbital for C1-H4 with 1.9924 electrons
__has 63.60% C 1 character in a sp0.91 hybrid
__has 36.40% H 4 character in a s orbital

5. A bonding orbital for C2-H5 with 1.9933 electrons
__has 56.84% C 2 character in a sp2.03 hybrid
__has 43.16% H 5 character in a s orbital

6. A bonding orbital for C2-O6 with 1.9999 electrons
__has 30.34% C 2 character in a p-pi orbital ( 99.42% p 0.57% d)
__has 69.66% O 6 character in a p-pi orbital ( 99.82% p 0.18% d)

7. A bonding orbital for C2-O6 with 1.9990 electrons
__has 34.21% C 2 character in a sp1.86 hybrid
__has 65.79% O 6 character in a sp1.46 hybrid

8. A bonding orbital for C2-H7 with 1.9935 electrons
__has 56.82% C 2 character in a sp2.03 hybrid
__has 43.18% H 7 character in a s orbital

13. A lone pair orbital for N3 with 1.9791 electrons
__made from a sp0.85 hybrid

14. A lone pair orbital for O6 with 1.9839 electrons
__made from a sp0.67 hybrid

15. A lone pair orbital for O6 with 1.9122 electrons
__made from a p-pi orbital ( 99.92% p 0.07% d)

-With core pairs on: C 1 C 2 N 3 O 6 -

#### 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, 13, for N3 with the antibonding acceptor orbital, 110, for C1-H4 is 37.4 kJ/mol.

The interaction of lone pair donor orbital, 14, for O6 with the antibonding acceptor orbital, 110, for C1-H4 is 13.5 kJ/mol.

The interaction of the second lone pair donor orbital, 15, for O6 with the antibonding acceptor orbital, 111, for C2-H5 is 108. kJ/mol.

The interaction of the second lone pair donor orbital, 15, for O6 with the antibonding acceptor orbital, 114, for C2-H7 is 108. 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.

19 ----- 1.188

18 ----- -0.717 17 ----- -0.718

16 ----- -3.651

15 -^-v- -7.024

14 -^-v- -8.618 13 -^-v- -8.620
12 -^-v- -8.634

11 -^-v- -10.91

10 -^-v- -11.84

9 -^-v- -12.82

8 -^-v- -14.32

7 -^-v- -16.28

6 -^-v- -22.39

5 -^-v- -27.16

4 -^-v- -267.4

3 -^-v- -269.8

2 -^-v- -377.5

1 -^-v- -507.8

## 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 = -208.0055167518 Hartrees