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.
Please note that your structure can't be well described by a single
Lewis structure, because of extensive delocalization.
Hybridization in the Best Lewis Structure
1. A bonding orbital for N1-N2 with 1.9657 electrons
__has 67.80% N 1 character in a s0.83 p3 hybrid
__has 32.20% N 2 character in a s0.07 p3 hybrid
2. A bonding orbital for N1-O3 with 1.9941 electrons
__has 49.26% N 1 character in a sp1.47 hybrid
__has 50.74% O 3 character in a s0.93 p3 hybrid
3. A bonding orbital for N1-O3 with 1.9962 electrons
__has 31.73% N 1 character in a p-pi orbital ( 99.58% p 0.42% d)
__has 68.27% O 3 character in a p-pi orbital ( 99.83% p 0.17% d)
4. A bonding orbital for N1-O4 with 1.9938 electrons
__has 48.93% N 1 character in a sp1.53 hybrid
__has 51.07% O 4 character in a s0.94 p3 hybrid
5. A bonding orbital for N2-O5 with 1.9986 electrons
__has 37.83% N 2 character in a p-pi orbital ( 99.36% p 0.64% d)
__has 62.17% O 5 character in a p-pi orbital ( 99.67% p 0.33% d)
6. A bonding orbital for N2-O5 with 1.9950 electrons
__has 41.17% N 2 character in a sp2.63 hybrid
__has 58.83% O 5 character in a sp2.08 hybrid
12. A lone pair orbital for N2 with 1.9945 electrons
__made from a sp0.39 hybrid
13. A lone pair orbital for O3 with 1.9821 electrons
__made from a sp0.31 hybrid
14. A lone pair orbital for O3 with 1.8775 electrons
__made from a p3 hybrid
15. A lone pair orbital for O4 with 1.9834 electrons
__made from a sp0.31 hybrid
16. A lone pair orbital for O4 with 1.8590 electrons
__made from a p3 hybrid
17. A lone pair orbital for O4 with 1.5340 electrons
__made from a p-pi orbital ( 99.85% p 0.15% d)
18. A lone pair orbital for O5 with 1.9934 electrons
__made from a sp0.46 hybrid
19. A lone pair orbital for O5 with 1.7262 electrons
__made from a p3 hybrid
115. A antibonding orbital for N1-N2 with 0.4562 electrons
__has 32.20% N 1 character in a s0.83 p3 hybrid
__has 67.80% N 2 character in a s0.07 p3 hybrid
117. A antibonding orbital for N1-O3 with 0.4560 electrons
__has 68.27% N 1 character in a p-pi orbital ( 99.58% p 0.42% d)
__has 31.73% O 3 character in a p-pi orbital ( 99.83% p 0.17% d)
-With core pairs on: N 1 N 2 O 3 O 4 O 5 -
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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, 1, for N1-N2 with
the antibonding acceptor orbital, 116, for N1-O3 is 25.8 kJ/mol.
The interaction of bonding donor orbital, 1, for N1-N2 with
the antibonding acceptor orbital, 118, for N1-O4 is 26.4 kJ/mol.
The interaction of lone pair donor orbital, 13, for O3 with
the antibonding acceptor orbital, 118, for N1-O4 is 31.2 kJ/mol.
The interaction of the second lone pair donor orbital, 14, for O3 with
the antibonding acceptor orbital, 115, for N1-N2 is 187. kJ/mol.
The interaction of the second lone pair donor orbital, 14, for O3 with
the antibonding acceptor orbital, 118, for N1-O4 is 77.3 kJ/mol.
The interaction of lone pair donor orbital, 15, for O4 with
the antibonding acceptor orbital, 116, for N1-O3 is 30.1 kJ/mol.
The interaction of the second lone pair donor orbital, 16, for O4 with
the antibonding acceptor orbital, 115, for N1-N2 is 206. kJ/mol.
The interaction of the second lone pair donor orbital, 16, for O4 with
the antibonding acceptor orbital, 116, for N1-O3 is 74.3 kJ/mol.
The interaction of the third lone pair donor orbital, 17, for O4 with
the second antibonding acceptor orbital, 117, for N1-O3 is 1048 kJ/mol.
The interaction of the second lone pair donor orbital, 19, for O5 with
the antibonding acceptor orbital, 115, for N1-N2 is 630. 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.
23 ----- 3.418
22 ----- -3.292
21 ----- -3.340
20 ----- -5.710
19 -^-v- -6.611
18 -^-v- -8.061
17 -^-v- -8.781
16 -^-v- -11.39
15 -^-v- -13.05
14 -^-v- -13.35
13 -^-v- -13.47
12 -^-v- -14.36
11 -^-v- -14.59
10 -^-v- -16.02
9 -^-v- -18.11
8 -^-v- -27.44
7 -^-v- -31.28
6 -^-v- -32.71
5 -^-v- -382.9
4 -^-v- -383.4
3 -^-v- -508.5
2 -^-v- -508.6
1 -^-v- -511.3
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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 = -335.1472341905 Hartrees
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