chemical physics of discharges - Argonne National Laboratory
chemical physics of discharges - Argonne National Laboratory chemical physics of discharges - Argonne National Laboratory
80 Possible Modes of Fragmentation of Pentaborane etc. + In support of the above mechanism, the data in Table 1 can be cited BH2+ BH3+ Table 1 Abundances of BH2+ and BH3+ in Some Boron Hydrides Diborane7 Tetraborano8 Pentaboraneg 19.1 .59 (These ion intensities were Cbtained with 70 volt electrons, and are given in percent relative to the most intense peak in the mass spectrum for the cmpound in quest ion. ) + Thua, it can be argued that the loss of BH2 is much more likely than the loss of BH3 . The loss of BH3, however, at least from neutral species, is fairly well established in a number of reactions." It should not be too surprising if BH3 can also be readily fragmented from negative ions. - It is tempting to question the necessity of invoking the excited state decay process (4) described above. For example, can the formation of the B3H7- not be simply written as a resonant attachment process with the dissociation of BH3? Although this is certainly possible, one or two points argue against this mechanism. First, at the electron energies used, a resonant process of this type would not be expected to be of primary importance. Secondly, one might inquire why the pair ionization process, ~ + 4 + e ~ + B 1 ~ H ~ ~ + - B H ~ is not observed, especially in view of the fact that the analogous process seems to be the predominant one in diborane. Indeed, the pair ionization process is the one which is expected; it is disturbing that it is not seen in view of the stability of B3Hg in solution and in the solid phase. The structure of B3Hg- is known frran x-ray Work, and there is ample theoretical and experimental justification for its existence.'l On the other hand, we have found no evidence in the literature for B3H;. The question arises as to whether an error can be made in the mass assignments. The marker compounds used were 02 and H20, giving rise to the 02 , OH-, and 0- peaks, which were always present in the background. Considerable care was taken in making the mass assignments, so that unless some unknown instrumental or chemical processes were occurring of which we are unaware, the given assignments are correct. Therefore, granting that the reported observations are valid, and accepting the notion that pair ionization should be $he dominant process at higher electron enprgies, and further noting that the BH2 ion is much more predominant than the BH3 in the positive ion spectrum, it seems necessary to invoke some mechanism analogous to (4). Perhaps further weight can be given to this argument by noting that the parent peak is not observed in tetraborane, suggesting that a loss of hydrogen is a strongly favored process in the electron impact situation. The present work suggests several further experiments which should be carried 7.0 .6 ! 12.2 --
51 out to answer some of the questions which have been raised here. An investigation Of metastable negative ions on a magnetic sector instrument should prove useful in confirming or negating the fragmentation scheme postulated above. A careful study of the diborane spectrum, either in a tandem instrument, or with an ion source in which one could be sure that pyrolysis is not taking place would be necessary to remove the ambiguity in the obseraation of tetraborane-in the diborane sample; whether the peaks above diborane are due to impurities, or whether they do in fact result from ion-molecule reactions. Perhaps most useful initially would be an investigation of the boron hydride spectra at low electron energies, where resonance attachment becomes the dominant process. Ideally, one should study the spectra as a function of energy; the clastogram technique" might prove valuable in sorting out the various processes occurring. We made some attempt to work at low electron energies, but largely without success. Since we are unable to measure the ionizing current, i.e., keep it constant as a function of energy, we would have little con- fidence in an appearance potential measurement, particularly since the background from electrons again becomes a problem at low electron energies, when they can be pushed out of the ionization chamber by the repeller. Reese, Dibeler, and Mohler have reported on the spectrum of pentaborane, in which they observed the resonant attachment process in the parent ion.13 Although their relative intensities are different from those which we observed, this is probably not surprising, in view of the different energies of the ionizing electrons in the two cases. Curiously, however, Dibeler does not report any of the lower fragments for pentaborane. In conclusion, it is evident that the lower boron hydrides do form negative ions. In certain circumstances, the abundance of these ions mag be great enough so that they would have to be taken into consideration in mass spectral, radiation, or gaseous discharge phenomena. It is also clear, however, that more than a mere qual- itative study of these negative ions will be necessary for the complete understand- ing of their roles in these situations. Acknowledment- This work was done under the auspices of the United States Atomic Energy Commission. Figure Captions Fig. 1. Block diagram of the mass spectrometer. Fig. 2. Lower portion of the mass spectrum of the negative ions from pentaborane. Fig. 3. The monoisotopic relative abundances for the negative ions frm diborane, tetraborane, and pentaborane. References 1. F. Fiquet-Fayard, Actions Chimiques et Biologiques des Radiations 11, p. 44 2. (1965 1. J. F. Paulson, Ion Molecule Reactions in the Gas Phase, p. 28, American Chemical 3. 4. Society Publications (1966). G. Jacobs and A. Henglein, Advances in Mass Spectroscopy 2, p. 28, The Institute of Petroleum (1966). M. F. Calcote and D. E. Jensen, Ion Molecule Reactions in the Gas Phase, p. 291, American Chemical Society Publications (1966). 5. 6. V. V. V. Subbanna, L. H. Hall, and W. S. Koski, J. Am. Von Zahn, Rev. Sci. Inst. 34, 1 (1963). Chem. SOC. 86, 1304 (1964). 7. MBS No. 333 Mass Spectra Data, American Petroleum Institute Project 44 (1949). 8. T. P. Fehlner and W. S. Koski, J. Am. Chem. SOC. &, 1905 (1963). 9. NBS No. 33b Mass Spectra Data, American Petroleum Institute Project 44 (1949). 10. T. P. Fehlner and W. S. Koski, J. Am. Chem. SOC., 86, 2733 (1964). 11. W. N. Lipscomb, Boron Hydrides, W. A. Benjamin, Inc. (1963).
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80<br />
Possible Modes <strong>of</strong> Fragmentation <strong>of</strong> Pentaborane<br />
etc.<br />
+<br />
In support <strong>of</strong> the above mechanism, the data in Table 1 can be cited<br />
BH2+<br />
BH3+<br />
Table 1<br />
Abundances <strong>of</strong> BH2+ and BH3+ in Some Boron Hydrides<br />
Diborane7 Tetraborano8 Pentaboraneg<br />
19.1<br />
.59<br />
(These ion intensities were Cbtained with 70 volt electrons, and are given in<br />
percent relative to the most intense peak in the mass spectrum for the cmpound in<br />
quest ion. )<br />
+<br />
Thua, it can be argued that the loss <strong>of</strong> BH2 is much more likely than the loss <strong>of</strong><br />
BH3 . The loss <strong>of</strong> BH3, however, at least from neutral species, is fairly well<br />
established in a number <strong>of</strong> reactions." It should not be too surprising if BH3 can<br />
also be readily fragmented from negative ions.<br />
- It is tempting to question the necessity <strong>of</strong> invoking the excited state decay<br />
process (4) described above. For example, can the formation <strong>of</strong> the B3H7- not be<br />
simply written as a resonant attachment process with the dissociation <strong>of</strong> BH3?<br />
Although this is certainly possible, one or two points argue against this mechanism.<br />
First, at the electron energies used, a resonant process <strong>of</strong> this type would not be<br />
expected to be <strong>of</strong> primary importance. Secondly, one might inquire why the pair<br />
ionization process,<br />
~<br />
+<br />
4 + e ~ + B 1 ~ H ~ ~ + - B H ~<br />
is not observed, especially in view <strong>of</strong> the fact that the analogous process seems to<br />
be the predominant one in diborane. Indeed, the pair ionization process is the one<br />
which is expected; it is disturbing that it is not seen in view <strong>of</strong> the stability <strong>of</strong><br />
B3Hg in solution and in the solid phase. The structure <strong>of</strong> B3Hg- is known frran<br />
x-ray Work, and there is ample theoretical and experimental justification for its<br />
existence.'l On the other hand, we have found no evidence in the literature for<br />
B3H;. The question arises as to whether an error can be made in the mass assignments.<br />
The marker compounds used were 02 and H20, giving rise to the 02 , OH-, and<br />
0- peaks, which were always present in the background. Considerable care was taken<br />
in making the mass assignments, so that unless some unknown instrumental or <strong>chemical</strong><br />
processes were occurring <strong>of</strong> which we are unaware, the given assignments are<br />
correct. Therefore, granting that the reported observations are valid, and accepting<br />
the notion that pair ionization should be $he dominant process at higher electron<br />
enprgies, and further noting that the BH2 ion is much more predominant than<br />
the BH3 in the positive ion spectrum, it seems necessary to invoke some mechanism<br />
analogous to (4). Perhaps further weight can be given to this argument by noting<br />
that the parent peak is not observed in tetraborane, suggesting that a loss <strong>of</strong><br />
hydrogen is a strongly favored process in the electron impact situation.<br />
The present work suggests several further experiments which should be carried<br />
7.0<br />
.6<br />
!<br />
12.2<br />
--