dimethylamine, CH3NHCH3

H7
|
H9 - C6H3
| \ /
H8N1 - C2
/ | \
H10H5H4
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

N1 charge=-0.653
C2 charge=-0.122
H3 charge= 0.114
H4 charge= 0.079
H5 charge= 0.063
C6 charge=-0.096
H7 charge= 0.106
H8 charge= 0.059
H9 charge= 0.071
H10 charge= 0.377
with a dipole moment of 1.12638 Debye

Bond Lengths:

between N1 and C2: distance=1.469 ang___ between N1 and C6: distance=1.471 ang___
between N1 and H10: distance=1.024 ang___ between C2 and H3: distance=1.105 ang___
between C2 and H4: distance=1.103 ang___ between C2 and H5: distance=1.116 ang___
between C6 and H7: distance=1.107 ang___ between C6 and H8: distance=1.117 ang___
between C6 and H9: distance=1.104 ang___

Bond Angles:

for H3-C2-N1: angle=109.3 deg___ for H4-C2-N1: angle=109.6 deg___
for H5-C2-N1: angle=114.2 deg___ for C6-N1-C2: angle=113.0 deg___
for H7-C6-N1: angle=109.4 deg___ for H8-C6-N1: angle=114.2 deg___
for H9-C6-N1: angle=109.6 deg___ for H10-N1-C2: angle=109.6 deg___

Top of page.

Bond Orders (Mulliken):

between N1 and C2: order=0.857___ between N1 and C6: order=0.855___
between N1 and H10: order=0.940___ between C2 and H3: order=0.980___
between C2 and H4: order=0.990___ between C2 and H5: order=0.986___
between C6 and H7: order=0.979___ between C6 and H8: order=0.986___
between C6 and H9: order=0.990___

Top of page.

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 N1-C2 with 1.9943 electrons
__has 59.86% N 1 character in a sp2.32 hybrid
__has 40.14% C 2 character in a sp2.75 hybrid

2. A bonding orbital for N1-C6 with 1.9942 electrons
__has 59.87% N 1 character in a sp2.32 hybrid
__has 40.13% C 6 character in a sp2.75 hybrid

3. A bonding orbital for N1-H10 with 1.9837 electrons
__has 67.15% N 1 character in a s0.84 p3 hybrid
__has 32.85% H10 character in a s orbital

4. A bonding orbital for C2-H3 with 1.9932 electrons
__has 58.60% C 2 character in a s0.96 p3 hybrid
__has 41.40% H 3 character in a s orbital

5. A bonding orbital for C2-H4 with 1.9923 electrons
__has 58.80% C 2 character in a s0.96 p3 hybrid
__has 41.20% H 4 character in a s orbital

6. A bonding orbital for C2-H5 with 1.9969 electrons
__has 57.69% C 2 character in a s0.99 p3 hybrid
__has 42.31% H 5 character in a s orbital

7. A bonding orbital for C6-H7 with 1.9932 electrons
__has 58.61% C 6 character in a s0.96 p3 hybrid
__has 41.39% H 7 character in a s orbital

8. A bonding orbital for C6-H8 with 1.9969 electrons
__has 57.71% C 6 character in a s0.99 p3 hybrid
__has 42.29% H 8 character in a s orbital

9. A bonding orbital for C6-H9 with 1.9923 electrons
__has 58.81% C 6 character in a s0.96 p3 hybrid
__has 41.19% H 9 character in a s orbital

13. A lone pair orbital for N1 with 1.9356 electrons
__made from a s0.66 p3 hybrid

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

Top of page.

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 N1 with the antibonding acceptor orbital, 111, for C2-H5 is 46.6 kJ/mol.

The interaction of lone pair donor orbital, 13, for N1 with the antibonding acceptor orbital, 113, for C6-H8 is 46.4 kJ/mol.

Top of page.

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.

17 ----- 2.482

16 ----- 2.191

15 ----- 1.949

14 ----- 1.072


13 -^-v- -4.930


12 -^-v- -8.668
11 -^-v- -8.726

10 -^-v- -9.222


9 -^-v- -10.61
8 -^-v- -10.65


7 -^-v- -11.91


6 -^-v- -15.20


5 -^-v- -17.04


4 -^-v- -22.03


3 -^-v- -266.5
2 -^-v- -266.5


1 -^-v- -376.9

Top of page.

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 = -135.2073081732 Hartrees

Top of page.

-> Return to Molecular Structure Page. -> Return to Chemistry Home Page