1-dehydro-1-bromoethane radical, CH3CH(•)Br

H3
\
H4 - C1 - C2 - BR6
/ \
H5H7
The multiplicity is 2.

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=-0.228
C2 charge=-0.246
H3 charge= 0.114
H4 charge= 0.119
H5 charge= 0.110
BR6 charge=-0.053
H7 charge= 0.183
with a dipole moment of 1.60665 Debye

Bond Lengths:

between C1 and C2: distance=1.485 ang___ between C1 and H3: distance=1.113 ang___
between C1 and H4: distance=1.106 ang___ between C1 and H5: distance=1.106 ang___
between C2 and BR6: distance=1.908 ang___ between C2 and H7: distance=1.092 ang___

Bond Angles:

for H3-C1-C2: angle=112.6 deg___ for H4-C1-C2: angle=109.7 deg___
for H5-C1-C2: angle=111.9 deg___ for BR6-C2-C1: angle=119.1 deg___
for H7-C2-C1: angle=125.2 deg___

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Bond Orders (Mulliken):

between C1 and C2: order=0.983___ between C1 and H3: order=0.948___
between C1 and H4: order=0.950___ between C1 and H5: order=0.964___
between C2 and BR6: order=1.076___ between C2 and H7: order=0.904___

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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. The Lewis structure is built for the up and down electrons, separately. Note that the up and down structures can be very different.

Hybridization in the Best Lewis Structure

Down Electrons

1. A bonding orbital for C1-C2 with 0.9985 electrons
__has 47.90% C 1 character in a sp2.60 hybrid
__has 52.10% C 2 character in a sp1.53 hybrid

2. A bonding orbital for C1-H3 with 0.9982 electrons
__has 59.21% C 1 character in a s0.92 p3 hybrid
__has 40.79% H 3 character in a s orbital

3. A bonding orbital for C1-H4 with 0.9906 electrons
__has 60.88% C 1 character in a s0.96 p3 hybrid
__has 39.12% H 4 character in a s orbital

4. A bonding orbital for C1-H5 with 0.9956 electrons
__has 60.76% C 1 character in a s0.97 p3 hybrid
__has 39.24% H 5 character in a s orbital

5. A bonding orbital for C2-Br6 with 0.9943 electrons
__has 48.99% C 2 character in a s0.86 p3 hybrid
__has 51.01% Br 6 character in a s0.46 p3 hybrid

6. A bonding orbital for C2-H7 with 0.9946 electrons
__has 63.49% C 2 character in a sp1.89 hybrid
__has 36.51% H 7 character in a s orbital

23. A lone pair orbital for C2 with 0.9746 electrons
__made from a s0.11 p3 hybrid

24. A lone pair orbital for Br6 with 0.9986 electrons
__made from a s0.87 p3 hybrid

25. A lone pair orbital for Br6 with 0.9971 electrons
__made from a sp0.56 hybrid

26. A lone pair orbital for Br6 with 0.9919 electrons
__made from a p3 hybrid

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

Up Electrons

1. A bonding orbital for C1-C2 with 0.9988 electrons
__has 52.99% C 1 character in a sp2.44 hybrid
__has 47.01% C 2 character in a sp1.50 hybrid

2. A bonding orbital for C1-H3 with 0.9829 electrons
__has 63.65% C 1 character in a s0.94 p3 hybrid
__has 36.35% H 3 character in a s orbital

3. A bonding orbital for C1-H4 with 0.9895 electrons
__has 61.73% C 1 character in a s0.92 p3 hybrid
__has 38.27% H 4 character in a s orbital

4. A bonding orbital for C1-H5 with 0.9907 electrons
__has 62.63% C 1 character in a s0.93 p3 hybrid
__has 37.37% H 5 character in a s orbital

5. A bonding orbital for C2-Br6 with 0.9960 electrons
__has 41.60% C 2 character in a s0.94 p3 hybrid
__has 58.40% Br 6 character in a s0.58 p3 hybrid

6. A bonding orbital for C2-H7 with 0.9958 electrons
__has 58.21% C 2 character in a sp1.80 hybrid
__has 41.79% H 7 character in a s orbital

24. A lone pair orbital for Br6 with 0.9977 electrons
__made from a sp0.19 hybrid

25. A lone pair orbital for Br6 with 0.9912 electrons
__made from a p3 hybrid

26. A lone pair orbital for Br6 with 0.9479 electrons
__made from a p3 hybrid

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

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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 bonding donor orbital, 2, for C1-H3 with the lone pair acceptor orbital, 23, for C2 is 29.2 kJ/mol.

The interaction of the third lone pair donor orbital, 26, for Br6 with the lone pair acceptor orbital, 23, for C2 is 85.2 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. Only the spin up electron orbital energies are given.

30 ----- 3.118

29 ----- 2.129

28 ----- 1.599


27 ----- -1.024


26 -^--- -4.525


25 -^-v- -7.023

24 -^-v- -7.837


23 -^-v- -9.103


22 -^-v- -10.40

21 -^-v- -10.62

20 -^-v- -11.43


19 -^-v- -14.69


18 -^-v- -18.35


17 -^-v- -20.64


16 -^-v- -68.43 15 -^-v- -68.43

14 -^-v- -68.68
13 -^-v- -68.72
12 -^-v- -68.80


11 -^-v- -171.6
10 -^-v- -171.7

9 -^-v- -172.0


8 -^-v- -229.1


7 -^-v- -266.6


6 -^-v- -268.1


5 -^-v- -1517.
4 -^-v- -1517.
3 -^-v- -1517.


2 -^-v- -1680.


1 -^-v- -13067

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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 = -2652.5776620924 Hartrees

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