Once the molecule file is fully loaded, the image at right will become live. At that time the "activate 3-D" icon will disappear.
Nitrobenzene

    Nitrobenzene is an aromatic organic molecule with a nitro-substituent group.  The combustion of the compound produces toxic nitrogen oxides, which can cause carcinogenic effects when inhaled.  As shown in the figures to the right, the chemical structure and properties that classify this molecule demonstrate its potential reactivity and ability to form other compounds, such as aniline.  The Lewis structure of the molecule is shown below.


                                                    Nitrobenzene Lewis structure

    To better understand the nature of the bonding and anti-bonding molecular orbitals, three levels of theory were performed on an initial guess of the molecular structure.  These three levels (Molecular Mechanics, MOPAC3, and Ab initio) served as the predication of the quantum mechanical system for nitrobenzene.


By clicking on the button below, a figure of the molecule can be viewed that shows the physical dimensions of the molecule.



    The geometry of the molecule shows bond lengths between carbon and hydrogen atoms as well as the bonding relationship with the nitro-group.  The partial negative charge on one of the oxygen atoms and a partial positive charge on the nitrogen atom depict the various molecular dipole moments calculated via the ab initio level of theory.  These dipole moments can be correlated with UV-Vis transition energy as shown below in the table of dipole moments from ground state to excited states.

 

Table 1.  Cis-transition dipole moments of nitrobenzene from ground state to excited states.  The calculations were performed using the optimized geometry of the molecule along with the double zeta valence (DZV) basis set.  The unit of energy is Debye.


Excited state

Transition energy (Debye)

1

0.012 635

2

0.124 501

3

1.227 428

4

2.899 312

5

2.283 397

6

5.232 152

7

4.333 443

8

0.241 692

9

3.578 363

10

4.580 314


    The molecular dipole moments were initially calculated using an optimized geometry calculation and a variety of basis sets using ab initio level of theory.  An experimental value, obtained from the NIST database, was found to be a value of 4.220 Debye.  A table of the initial dipole moments prior to optimization is shown below.

Table 2.  Initial dipole moments before optimization.

Basis set

Dipole moment (Debye)

DZV

5.853 971

6-21G

5.229 080

6-31G

5.813 726

AM1

5.147 224

PM3

5.248 982

 

    Given the discrepancies between the experimental and calculated values, the dipole moments were improved by adding a combination of the following diffuse functions:  D-heavy atom polarization, F-heavy atom polarization, light atom polarization.  The best optimization was determined to be a combination of one D-heavy atom polarization and one light atom polarization with a dipole moment of 5.087 767 Debye. 

 

 

By clicking on the button below, a visual representation of the electrostatic potential field surrounding the molecule can be viewed.


    The electrostatic potential is shown as an all-encompassing electric field surrounding the molecule.  The color gradient of the field represents the changes in the potential energy in relation to the charge distribution.  This attribute coincides with the partial atomic charges on the nitro-substituent group. 

 

    The lowest unoccupied molecular orbital (LUMO) is shown using the optimized geometry and DZV basis set.  Molecular orbitals are shown surrounding all atoms in the molecule, which is consistent with the molecular orbital (MO) theory, where the LUMO is the lowest energy state of unoccupied orbitals.  According to the MO theory, delocalized electrons become excited and transition from the HOMO to the LUMO.  This transition energy can be approximated using the ab initio level of theory.


By clicking on the button below, a figure of the molecule can be viewed that shows a visual representation of the lowest unoccupied molecular orbital (LUMO).



    The optimized geometry and double zeta valence (DZV) basis set were used to obtain the highest occupied molecular orbital (HOMO) for the molecule.  The balloon-like surfaces above and below each sulfur atom represent electron occupied pi-orbitals. 

 

By clicking on the button below, a figure of the molecule can be viewed that shows a visual representation of the highest occupied molecular orbital (HOMO).



    The figure represents the stage when the valence electrons are in the highest energy state.  The red and blue-colored orbitals represent the difference in phases for the pi and sigma orbitals.

 


Click here to view an animation of nitrobenzene.
Vibrational Motions

References:

1.     Mihalick, J. Gutow, J. Quantum Calculations 2016, p 1-12.  

 

2.     Chlorine. Chlorine, http://webbook.nist.gov/cgi/cbook.cgi?id=7782-50-5 (accessed Mar 3, 2016).

 

3.     Carbon disulfide. Carbon disulfide, http://webbook.nist.gov/cgi/cbook.cgi?id=75-15-0 (accessed Mar 2, 2016).

 

4.     Benzene, nitro-. Benzene, nitro-, http://webbook.nist.gov/cgi/cbook.cgi?id=c98953 (accessed Mar 3, 2016).


Based on template by A. Herráez as modified by J. Gutow
Page skeleton and JavaScript generated by export to web function using Jmol 14.2.15_2015.07.09 2015-07-09 22:22 on Mar 4, 2016.
This will be the viewer still of jmol image
If your browser/OS combination is Java capable, you will get snappier performance if you use Java
Vibrational motions