AsO2+ ion

O3 = AS1 = O2
The ion charge is 1.

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

AS1 charge= 1.060
O2 charge=-0.030
O3 charge=-0.030
with a dipole moment of 0.00171 Debye

Bond Lengths:

between AS1 and O2: distance=1.619 ang___ between AS1 and O3: distance=1.619 ang___
between O2 and O3: distance=3.237 ang___

Bond Angles:

for O3-AS1-O2: angle=179.9 deg___

Top of page.

Bond Orders (Mulliken):

between AS1 and O2: order=1.775___ between AS1 and O3: order=1.775___
between O2 and O3: order=0.152___

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. 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 As1-O2 with 1.9465 electrons
__has 37.18% As 1 character in a sp1 hybrid
__has 62.82% O 2 character in a s0.3 p3 hybrid

2. A bonding orbital for As1-O3 with 1.9465 electrons
__has 37.18% As 1 character in a sp1 hybrid
__has 62.82% O 3 character in a s0.30 p3 hybrid

3. A bonding orbital for As1-O3 with 1.9986 electrons
__has 10.73% As 1 character in a p-pi orbital ( 95.08% p 4.92% d)
__has 89.27% O 3 character in a p-pi orbital ( 99.63% p 0.37% d)

4. A bonding orbital for As1-O3 with 1.9986 electrons
__has 10.73% As 1 character in a p-pi orbital ( 95.08% p 4.92% d)
__has 89.27% O 3 character in a p-pi orbital ( 99.63% p 0.37% d)

21. A lone pair orbital for O2 with 1.9728 electrons
__made from a sp0.09 hybrid

22. A lone pair orbital for O2 with 1.8010 electrons
__made from a p-pi orbital ( 99.62% p 0.38% d)

23. A lone pair orbital for O2 with 1.8010 electrons
__made from a p-pi orbital ( 99.62% p 0.38% d)

24. A lone pair orbital for O3 with 1.9728 electrons
__made from a sp0.09 hybrid

71. A antibonding orbital for As1-O3 with 0.1572 electrons
__has 89.27% As 1 character in a p-pi orbital ( 95.08% p 4.92% d)
__has 10.73% O 3 character in a p-pi orbital ( 99.63% p 0.37% d)

72. A antibonding orbital for As1-O3 with 0.1572 electrons
__has 89.27% As 1 character in a p-pi orbital ( 95.08% p 4.92% d)
__has 10.73% O 3 character in a p-pi orbital ( 99.63% p 0.37% d)

-With core pairs on:A A A A A A A A A A A A A A O 2 O 3 -

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, 1, for As1-O2 with the antibonding acceptor orbital, 70, for As1-O3 is 126. kJ/mol.

The interaction of bonding donor orbital, 2, for As1-O3 with the antibonding acceptor orbital, 69, for As1-O2 is 126. kJ/mol.

The interaction of lone pair donor orbital, 21, for O2 with the antibonding acceptor orbital, 70, for As1-O3 is 39.3 kJ/mol.

The interaction of the second lone pair donor orbital, 22, for O2 with the second antibonding acceptor orbital, 71, for As1-O3 is 209. kJ/mol.

The interaction of the third lone pair donor orbital, 23, for O2 with the third antibonding acceptor orbital, 72, for As1-O3 is 209. kJ/mol.

The interaction of lone pair donor orbital, 24, for O3 with the antibonding acceptor orbital, 69, for As1-O2 is 39.3 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.

28 ----- -3.800


27 ----- -11.70 26 ----- -11.70


25 ----- -13.71


24 -^-v- -16.69 23 -^-v- -16.69


22 -^-v- -18.18 21 -^-v- -18.18


20 -^-v- -19.32


19 -^-v- -22.71


18 -^-v- -33.22

17 -^-v- -33.86


16 -^-v- -54.26 15 -^-v- -54.26
14 -^-v- -54.34 13 -^-v- -54.34

12 -^-v- -54.55


11 -^-v- -144.8

10 -^-v- -144.9 9 -^-v- -144.9


8 -^-v- -196.0


7 -^-v- -517.1 6 -^-v- -517.1


5 -^-v- -1308.
4 -^-v- -1308. 3 -^-v- -1308.


2 -^-v- -1459.


1 -^-v- -11533

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 = -2385.7885768667 Hartrees

Top of page.

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