## S2 triplet

 S1 = S2
The multiplicity is 3.

## Atomic Charges and Dipole Moment

S1 charge= 0.000
S2 charge= 0.000
with a dipole moment of 0 Debye

## Bond Lengths:

between S1 and S2: distance=1.952 ang___

## Bond Orders (Mulliken):

between S1 and S2: order=1.880___

## 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 S1-S2 with 1.0000 electrons
__has 50.00% S 1 character in a s0.44 p3 hybrid
__has 50.00% S 2 character in a s0.44 p3 hybrid

12. A lone pair orbital for S1 with 0.9998 electrons

13. A lone pair orbital for S1 with 0.9968 electrons
__made from a p-pi orbital (100.00% p)

14. A lone pair orbital for S1 with 0.9968 electrons
__made from a p-pi orbital (100.00% p)

15. A lone pair orbital for S2 with 0.9998 electrons

16. A lone pair orbital for S2 with 0.9968 electrons
__made from a p-pi orbital (100.00% p)

17. A lone pair orbital for S2 with 0.9968 electrons
__made from a p-pi orbital (100.00% p)

-With core pairs on: S 1 S 1 S 1 S 1 S 1 S 2 S 2 S 2 S 2 S 2 -

#### Up Electrons

1. A bonding orbital for S1-S2 with 1.0000 electrons
__has 50.00% S 1 character in a s0.60 p3 hybrid
__has 50.00% S 2 character in a s0.60 p3 hybrid

2. A bonding orbital for S1-S2 with 1.0000 electrons
__has 50.00% S 1 character in a p-pi orbital ( 98.81% p 1.19% d)
__has 50.00% S 2 character in a p-pi orbital ( 98.81% p 1.19% d)

3. A bonding orbital for S1-S2 with 1.0000 electrons
__has 50.00% S 1 character in a p-pi orbital ( 98.81% p 1.19% d)
__has 50.00% S 2 character in a p-pi orbital ( 98.81% p 1.19% d)

14. A lone pair orbital for S1 with 0.9995 electrons

15. A lone pair orbital for S2 with 0.9995 electrons

-With core pairs on: S 1 S 1 S 1 S 1 S 1 S 2 S 2 S 2 S 2 S 2 -

## 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.

21 ----- 5.697 20 ----- 5.686

19 ----- 4.159

18 ----- -1.667

17 -^--- -5.951 16 -^--- -5.954

15 -^-v- -9.185 14 -^-v- -9.188

13 -^-v- -10.08

12 -^-v- -15.71

11 -^-v- -20.94

10 -^-v- -156.3 9 -^-v- -156.3 8 -^-v- -156.3 7 -^-v- -156.3

6 -^-v- -156.5
5 -^-v- -156.5

4 -^-v- -209.2 3 -^-v- -209.3

2 -^-v- -2388. 1 -^-v- -2388.

## 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 = -796.4497883429 Hartrees