methyl-tert-butylether, (CH3)3COCH3

H10H12
\ /
H7H11 - C3H17
\ / /
H8 - C1 - C2 - O5 - C6 - H16
/ | \
H9C4 - H14H18
| \
H13H15
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=-0.616
C2 charge= 0.795
C3 charge=-0.677
C4 charge=-0.575
O5 charge=-0.447
C6 charge=-0.101
H7 charge= 0.159
H8 charge= 0.143
H9 charge= 0.154
H10 charge= 0.166
H11 charge= 0.171
H12 charge= 0.161
H13 charge= 0.135
H14 charge= 0.155
H15 charge= 0.134
H16 charge= 0.064
H17 charge= 0.057
H18 charge= 0.118
with a dipole moment of 1.38986 Debye

Bond Lengths:

between C1 and C2: distance=1.543 ang___ between C1 and H7: distance=1.104 ang___
between C1 and H8: distance=1.104 ang___ between C1 and H9: distance=1.105 ang___
between C2 and C3: distance=1.538 ang___ between C2 and C4: distance=1.543 ang___
between C2 and O5: distance=1.463 ang___ between C3 and H10: distance=1.104 ang___
between C3 and H11: distance=1.104 ang___ between C3 and H12: distance=1.104 ang___
between C4 and H13: distance=1.105 ang___ between C4 and H14: distance=1.105 ang___
between C4 and H15: distance=1.104 ang___ between O5 and C6: distance=1.431 ang___
between C6 and H16: distance=1.109 ang___ between C6 and H17: distance=1.109 ang___
between C6 and H18: distance=1.102 ang___

Bond Angles:

for C3-C2-C1: angle=110.4 deg___ for C4-C2-C1: angle=110.8 deg___
for O5-C2-C1: angle=110.2 deg___ for C6-O5-C2: angle=116.4 deg___
for H7-C1-C2: angle=110.1 deg___ for H8-C1-C2: angle=110.5 deg___
for H9-C1-C2: angle=111.7 deg___ for H10-C3-C2: angle=109.5 deg___
for H11-C3-C2: angle=111.3 deg___ for H12-C3-C2: angle=109.9 deg___
for H13-C4-C2: angle=111.7 deg___ for H14-C4-C2: angle=110.6 deg___
for H15-C4-C2: angle=110.1 deg___ for H16-C6-O5: angle=112.1 deg___
for H17-C6-O5: angle=112.4 deg___ for H18-C6-O5: angle=106.1 deg___

Top of page.

Bond Orders (Mulliken):

between C1 and C2: order=0.985___ between C1 and H7: order=0.982___
between C1 and H8: order=0.978___ between C1 and H9: order=0.972___
between C2 and C3: order=0.974___ between C2 and C4: order=0.975___
between C2 and O5: order=0.897___ between C3 and H10: order=0.986___
between C3 and H11: order=0.978___ between C3 and H12: order=0.987___
between C4 and H13: order=0.974___ between C4 and H14: order=0.982___
between C4 and H15: order=0.978___ between O5 and C6: order=0.892___
between C6 and H16: order=0.977___ between C6 and H17: order=0.973___
between C6 and H18: order=0.991___

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 C1-C2 with 1.9899 electrons
__has 49.73% C 1 character in a sp2.53 hybrid
__has 50.27% C 2 character in a sp2.76 hybrid

2. A bonding orbital for C1-H7 with 1.9920 electrons
__has 59.64% C 1 character in a s0.95 p3 hybrid
__has 40.36% H 7 character in a s orbital

3. A bonding orbital for C1-H8 with 1.9886 electrons
__has 59.15% C 1 character in a s0.93 p3 hybrid
__has 40.85% H 8 character in a s orbital

4. A bonding orbital for C1-H9 with 1.9919 electrons
__has 59.03% C 1 character in a s0.95 p3 hybrid
__has 40.97% H 9 character in a s orbital

5. A bonding orbital for C2-C3 with 1.9854 electrons
__has 51.27% C 2 character in a sp2.77 hybrid
__has 48.73% C 3 character in a sp2.54 hybrid

6. A bonding orbital for C2-C4 with 1.9902 electrons
__has 50.24% C 2 character in a sp2.74 hybrid
__has 49.76% C 4 character in a sp2.53 hybrid

7. A bonding orbital for C2-O5 with 1.9869 electrons
__has 33.37% C 2 character in a s0.76 p3 hybrid
__has 66.63% O 5 character in a sp2.63 hybrid

8. A bonding orbital for C3-H10 with 1.9912 electrons
__has 59.62% C 3 character in a s0.95 p3 hybrid
__has 40.38% H10 character in a s orbital

9. A bonding orbital for C3-H11 with 1.9898 electrons
__has 58.71% C 3 character in a s0.93 p3 hybrid
__has 41.29% H11 character in a s orbital

10. A bonding orbital for C3-H12 with 1.9916 electrons
__has 59.56% C 3 character in a s0.95 p3 hybrid
__has 40.44% H12 character in a s orbital

11. A bonding orbital for C4-H13 with 1.9919 electrons
__has 59.12% C 4 character in a s0.94 p3 hybrid
__has 40.88% H13 character in a s orbital

12. A bonding orbital for C4-H14 with 1.9920 electrons
__has 59.60% C 4 character in a s0.95 p3 hybrid
__has 40.40% H14 character in a s orbital

13. A bonding orbital for C4-H15 with 1.9885 electrons
__has 59.28% C 4 character in a s0.93 p3 hybrid
__has 40.72% H15 character in a s orbital

14. A bonding orbital for O5-C6 with 1.9932 electrons
__has 66.13% O 5 character in a sp2.66 hybrid
__has 33.87% C 6 character in a s0.98 p3 hybrid

15. A bonding orbital for C6-H16 with 1.9956 electrons
__has 57.46% C 6 character in a sp2.93 hybrid
__has 42.54% H16 character in a s orbital

16. A bonding orbital for C6-H17 with 1.9955 electrons
__has 57.38% C 6 character in a sp2.93 hybrid
__has 42.62% H17 character in a s orbital

17. A bonding orbital for C6-H18 with 1.9917 electrons
__has 58.50% C 6 character in a s0.99 p3 hybrid
__has 41.50% H18 character in a s orbital

24. A lone pair orbital for O5 with 1.9698 electrons
__made from a sp1.20 hybrid

25. A lone pair orbital for O5 with 1.9411 electrons
__made from a p-pi orbital ( 99.97% p)

-With core pairs on: C 1 C 2 C 3 C 4 O 5 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 bonding donor orbital, 3, for C1-H8 with the antibonding acceptor orbital, 182, for C2-O5 is 23.4 kJ/mol.

The interaction of bonding donor orbital, 13, for C4-H15 with the antibonding acceptor orbital, 182, for C2-O5 is 24.2 kJ/mol.

The interaction of bonding donor orbital, 17, for C6-H18 with the antibonding acceptor orbital, 182, for C2-O5 is 20.5 kJ/mol.

The interaction of the second lone pair donor orbital, 25, for O5 with the antibonding acceptor orbital, 176, for C1-C2 is 34.0 kJ/mol.

The interaction of the second lone pair donor orbital, 25, for O5 with the antibonding acceptor orbital, 181, for C2-C4 is 26.9 kJ/mol.

The interaction of the second lone pair donor orbital, 25, for O5 with the antibonding acceptor orbital, 190, for C6-H16 is 41.5 kJ/mol.

The interaction of the second lone pair donor orbital, 25, for O5 with the antibonding acceptor orbital, 191, for C6-H17 is 32.8 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.

29 ----- 1.947
28 ----- 1.887

27 ----- 1.396

26 ----- 0.996


25 -^-v- -5.710


24 -^-v- -7.105


23 -^-v- -8.208
22 -^-v- -8.257

21 -^-v- -8.691

20 -^-v- -8.949

19 -^-v- -9.134

18 -^-v- -9.603

17 -^-v- -9.974

16 -^-v- -10.43

15 -^-v- -11.12

14 -^-v- -11.27

13 -^-v- -11.87


12 -^-v- -13.34


11 -^-v- -16.26

10 -^-v- -16.83

9 -^-v- -17.02


8 -^-v- -19.56


7 -^-v- -25.16


6 -^-v- -265.8

5 -^-v- -265.9
4 -^-v- -266.0


3 -^-v- -267.1

2 -^-v- -267.9


1 -^-v- -506.3

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 = -273.0583433230 Hartrees

Top of page.

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