Di-t-butyl Peroxide

    Shown below is the geometry optimization of Di-t-butyl Peroxide. The information show are the bond lengths and bond angles.


    The lowest level of theory belongs to the AM1 theory for geometry optimization.
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Shows the bond angle for AM1 theory.

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Shows the bond length for the AM1 theory.
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Shows the bond angles for the 6-21G theory.
    The second lowest level of theory belongs to the 6-21G for the geometry optimization.
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Shows the bond length of the 6-21G theory.

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Shows the bond length of the 6-31G theory.
      The second highest level of theory belongs to the 6-31G theory for geometry optimization.
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Shows the bond angles of the 6-31G theory.

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Shows the bond angles for DZV theory.
The highest level of theory used to determine the geometry optimization is DZV. This theory was the best according to literature values from the below table.
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Shows the bond length for DZV theory.




















    The bond lengths and angles are compared to the literature(1) and literature(4) is shown below in table 1 and table 2.
    Table 1:  Bond lengths from the literature(1) and literature(4).
Bond type
Bond length Angstroms
O-O
1.4552
C-O
1.4308
C-H
1.0791
C-C
1.5052
   
    Table 2: Bond angles from the literature(1) and (4).
Type of bond
Bond angle in degrees
C-O-O
105.978
C-C-O
122-130
C-C-C
111.246
H-C-H
107.691
H-C-C
111.198

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Shows how the molecular orbitals look in its LUMO state.
    The lowest unoccupied molecular orbital is at 42. When excited the molecule will become occupied.
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Shows how the molecular orbitals look in its LUMO state.
    The highest ocupied molecular orbital is at 41. Di-t-butyl peroxide has 82 electrons and when divided in two, the estimated number of orbitals is 41.
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Shows the electrostatic potential.
    The electrostatic potential of the molecule can is represented in red, blue, yellow and green. Red represents the lowest electrostatic potential and blue represents the highest. The green and yellow represents intermediate potentials.













    Partial atomic charges are created by asymmetric distribution of electrons in a chemical bond.
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Shows the partial atomic charges.
Image shows the IR spectrum
    Shows the Infrared Spectrum for Di-t-butyl Peroxide(2).
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Shows the visual at peak 2980.
    The vibrational frequencies were calculated using DZV. Each visual shows what the IR sees when it hits certain peaks.
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Shows the visual at peak 2930.

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Shows the visual at peak 1548.

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Shows the visual at peak 1480.

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Shows the visual at peak 1380.

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Shows the visual at peak 1250.

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Shows the visual at peak 1180.

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Shows the visual at peak 880.

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Shows the vibration at the 750 cm-1 peak in the IR spectrum.

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Shows the vibration at the 530 cm-1 peak in the IR spectrum.

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Shows the vibration at the 460 cm-1 peak in the IR spectrum.




















   
    Table 3: The IR chart is taken from the website(3).
IR Peak for bond Type
Frequency (cm-1)
C-H alkane medium
3000-2840
C-H Alkane bending
1465-1375, 880-700
C-O Stretching
1205-1124

    Table 4: These are the experimental values taken from the theories.
Basis Set
Dipole moment (Debye)
AM1
1.022739
6-21G RHF
0.332934
6-31G RHF
0.170910
DVZ RHF
0.133531
DVZ UHF
0.123887
    Di-t-butyl Peroxide does not have a dipole moment due to its symmetrical geometry. AM1 shows it at one, but the others were close to zero,


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