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 Ge1-Cl2 with 0.9474 electrons
__has 52.91% Ge 1 character in a sp1.00 hybrid
__has 47.09% Cl 2 character in a s0.10 p3 hybrid
2. A bonding orbital for Ge1-Cl3 with 0.9473 electrons
__has 52.92% Ge 1 character in a sp1.00 hybrid
__has 47.08% Cl 3 character in a s0.10 p3 hybrid
27. A lone pair orbital for Ge1 with 0.9969 electrons
__made from a p-pi orbital (100.00% p)
28. A lone pair orbital for Ge1 with 0.9969 electrons
__made from a p-pi orbital (100.00% p)
29. A lone pair orbital for Cl2 with 0.9989 electrons
__made from a p-pi orbital ( 99.99% p)
30. A lone pair orbital for Cl2 with 0.9989 electrons
__made from a p-pi orbital ( 99.99% p)
31. A lone pair orbital for Cl2 with 0.9892 electrons
__made from a s orbital
32. A lone pair orbital for Cl3 with 0.9989 electrons
__made from a p-pi orbital ( 99.99% p)
33. A lone pair orbital for Cl3 with 0.9989 electrons
__made from a p-pi orbital ( 99.99% p)
34. A lone pair orbital for Cl3 with 0.9892 electrons
__made from a s orbital
-With core pairs on:Ge 1 Ge 1 Ge 1 Ge 1 Ge 1 Ge 1 Ge 1 Ge 1 Ge 1 Ge 1 Ge 1 Ge 1 Ge 1 Ge 1 Cl 2 Cl 2 Cl 2 Cl 2 Cl 2 Cl 3 Cl 3 Cl 3 Cl 3 Cl 3 -
Up Electrons
1. A bonding orbital for Ge1-Cl2 with 0.9963 electrons
__has 22.20% Ge 1 character in a sp1.01 hybrid
__has 77.80% Cl 2 character in a s0.48 p3 hybrid
2. A bonding orbital for Ge1-Cl3 with 0.9963 electrons
__has 22.19% Ge 1 character in a sp1.01 hybrid
__has 77.81% Cl 3 character in a s0.48 p3 hybrid
29. A lone pair orbital for Cl2 with 0.9940 electrons
__made from a sp0.16 hybrid
30. A lone pair orbital for Cl2 with 0.9869 electrons
__made from a p-pi orbital ( 99.96% p)
31. A lone pair orbital for Cl2 with 0.9869 electrons
__made from a p-pi orbital ( 99.96% p)
32. A lone pair orbital for Cl3 with 0.9940 electrons
__made from a sp0.16 hybrid
33. A lone pair orbital for Cl3 with 0.9869 electrons
__made from a p-pi orbital ( 99.96% p)
34. A lone pair orbital for Cl3 with 0.9869 electrons
__made from a p-pi orbital ( 99.96% p)
-With core pairs on:Ge 1 Ge 1 Ge 1 Ge 1 Ge 1 Ge 1 Ge 1 Ge 1 Ge 1 Ge 1 Ge 1 Ge 1 Ge 1 Ge 1 Cl 2 Cl 2 Cl 2 Cl 2 Cl 2 Cl 3 Cl 3 Cl 3 Cl 3 Cl 3 -
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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 the second lone pair donor orbital, 30, for Cl2 with
the lone pair acceptor orbital, 27, for Ge1 is 20.5 kJ/mol.
The interaction of the third lone pair donor orbital, 31, for Cl2 with
the second lone pair acceptor orbital, 28, for Ge1 is 20.5 kJ/mol.
The interaction of the second lone pair donor orbital, 33, for Cl3 with
the lone pair acceptor orbital, 27, for Ge1 is 20.5 kJ/mol.
The interaction of the third lone pair donor orbital, 34, for Cl3 with
the second lone pair acceptor orbital, 28, for Ge1 is 20.5 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.
38 ----- 2.576
37 ----- 2.468
36 ----- -0.274
35 ----- -4.680
34 -^--- -4.529
33 -^--- -7.215
32 -^-v- -8.466
31 -^-v- -8.570
30 -^-v- -8.768
29 -^-v- -8.877
28 -^-v- -10.71
27 -^-v- -13.68
26 -^-v- -20.74
25 -^-v- -20.86
24 -^-v- -32.58
23 -^-v- -32.60
22 -^-v- -32.71
21 -^-v- -32.84
20 -^-v- -32.91
19 -^-v- -116.8
18 -^-v- -117.1
17 -^-v- -117.2
16 -^-v- -165.1
15 -^-v- -190.8 14 -^-v- -190.8
13 -^-v- -190.9 12 -^-v- -190.9
11 -^-v- -191.1 10 -^-v- -191.1
9 -^-v- -249.2 8 -^-v- -249.2
7 -^-v- -1194.
6 -^-v- -1195.
5 -^-v- -1195.
4 -^-v- -1339.
3 -^-v- -2730. 2 -^-v- -2730.
1 -^-v- -10788
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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 = -2997.3459948248 Hartrees
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