Chlorine Monofluoride (FCl)
The MO Calculations for Chlorine Monofluoride (FCl)
 
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Figure 1: Geometry of FCl using 6-21G calculation

        For Chlorine Monofluoride, the over all best calculated dipole moment was from AM1 calculation while the best calculated dipole moment among the ab initio theory calculation was 621G. The same pattern holds true for the bond length. The 6-21G calculation yield an 28.5% error for the Dipole Moment and an 3.79% error for the Bond Length for chlorine Monofluoride. The data collected from the calculations shows as below.

Table 1: Dipole moment and bond length for the five calculations.

Theory
Dipole Moment(Db) Percent Error (%)
Bond Length(nm) Percent Error (%)
Literature
0.881±.002 5 ---
.16283 6 ---
AM1
0.856872

.165

PM3
1.680765

.158

6-21G
1.132491

.169

6-31G
1.607802

.171

DZV
1.841146

.172


        It is obvious that the results of dipole moment and bond length from  AM1 was the closest to the literature value. However, for ab initio theory, 6-21G had the closest results to the literature value. Therefore, we adopted 6-21G for the rest of the calculation for Chlorine Monofluoride.

        The geometry of chlorine fluoride under 6-21G, 6-31G, DZV, and AM1 were shown from Figure 1 to Figure 4. The bond length was labeled in each figure as well. The bond angle of FCl was not included since it is 180 degrees.
 
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Figure 2: Geometry of FCl using  6-31G calculation
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Figure 3: Geometry of FCl using DZV calculation
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Figure 4: Geometry of FCl using AM1 calculation


        The Highest Occupied Molecular Orbital (HOMO) was at orbital 13. The HOMO was calculated by dividing the sum of the total number of electrons in the molecule by 2. The Lowest Unoccupied Molecular Orbital (LUMO) was at orbital 14. The LUMO was the orbital that would get filled by the excited valence electron(s) from the HOMO if proper excitation occurs.
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Figure 5: Highest Occupied Molecular Orbital for FCl using 6-21G calculation
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Figure 6: Lowest Unoccupied Molecular Orbital for FCl using 6-21G calculation


        The electrostatic potential of FCl using 6-21G calculation was shown in Figure 7. The electrostatic potential used a color spectrum, which uses red to indicate the lowest electrostatic potential and blue to indicate the highest electrostatic potential. 5 The electrostatic potential shows the electron distribution to the molecules. 5

        The partial atomic charge was shown in Figure 8. It was distribute by the asymmetric scatter of the electrons in the molecule. Fluorine was more electronegative than chlorine. Therefore, the fluorine had the negative partial atomic charge since the electrons were more likely to hanging around fluorine.

        The bond stretch was shown in Figure 9.      


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Figure 7: Electrostatic Potential for FCl using 6-21G calculation

 
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FCl Partial Atomic Charge

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FCl bond stretch

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FCl S bonding

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FCl S anti-bonding

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FCl Pi x bonding

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FCl Pi y bonding

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FCl Sigma bonding

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FCl Pi x anti-bonding

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FCl Pi y anti-bonding


 
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FCl Sigma anti-bonding

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Based on template by A. Herráez as modified by J. Gutow
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