Hostname: page-component-76fb5796d-25wd4 Total loading time: 0 Render date: 2024-04-27T12:09:55.833Z Has data issue: false hasContentIssue false
  • English
  • Français

The decomposition of PdSi by adding a small amount of Ag

Published online by Cambridge University Press:  31 January 2011

K. Tsumori  and
H. Akimune
K. Tsumori
Affiliation:
Plasma Physics Laboratory, Kyoto University, Gokasho, Uji, Kyoto, 611 Japan
H. Akimune
Affiliation:
Plasma Physics Laboratory, Kyoto University, Gokasho, Uji, Kyoto, 611 Japan
Get access

Abstract

The decomposition of the intermetallic compound PdSi by adding a small amount of Ag has been investigated by thermal analysis, metallographic measurement, and x-ray photoemission spectroscopy (XPS). Within the range of Ag concentration from 0 to 6 at.%, PdSi is decomposed in linear proportion to the concentration of Ag into Si and the ternary compound Pd2Si(Ag), which has the ratio of 16 PdSi molecules per single Ag atom. The PdSi is fully decomposed at Ag 10 at.%. In the ternary alloy included in the Pd–Si–Ag alloy involving Ag below 12 at. %, the atomic ratio of Si to metal atoms, which are Pd plus Ag, is nearly the same as the ratio in Pd-rich Pd2Si. Metallographic and XPS measurements indicate that the Ag atom included in the PdSi behaves as an electron donor with a large radius of the wave function; the Ag electron transfers to the anti-bonding state of PdSi and acts to decompose the compound. The Ag atoms seem to occupy the sites of Pd atoms in Pd2Si(Ag) which has been decomposed from PdSi.

Type
Articles
Information
Journal of Materials Research , Volume 5 , Issue 7 , July 1990 , pp. 1443 - 1452
Copyright
Copyright © Materials Research Society 1990

Access options

Get access to the full version of this content by using one of the access options below. (Log in options will check for institutional or personal access. Content may require purchase if you do not have access.)

References

1Aronsson, B. and Nylund, A., Acta Chem. Scand. 14, 1011 (1960).CrossRefGoogle Scholar
2Nylund, A., Acta Chem. Scand. 20, 2381 (1966).CrossRefGoogle Scholar
3Engström, I., Acta Chem. Scand. 24, 1466 (1970).CrossRefGoogle Scholar
4Buckley, W. and Moss, S. C., Solid-State Electron. 15, 1311 (1971).Google Scholar
5Ho, P. S., Rubloff, G. W., Lewis, J. E., Moruzzi, V. L., and Williams, A. R., Phys. Rev. B 22, 4784 (1980).CrossRefGoogle Scholar
6Langer, H. and Wachtell, E., Z. Metallk. 72, 769 (1981).Google Scholar
7Tsumori, K. and Akimune, H., J. Mater. Sci. (to be published).Google Scholar
8Akimune, H., J. Appl. Phys. 54, 18 (1983).CrossRefGoogle Scholar
9Riley, J. D., Ley, L., Azoulay, J., and Terakura, K., Phys. Rev. B 20, 776 (1976).CrossRefGoogle Scholar
10Ley, L., Knwalczyk, S., Pollak, R., and Shirley, D. A., Phys. Rev. Lett. 29, 1088 (1972).CrossRefGoogle Scholar
11Barrie, A. and Christensen, N. E., Phys. Rev. B 14, 2442 (1976).CrossRefGoogle Scholar
12Rubloff, G. W., Ho, P. S., Freeouf, J. F., and Lewis, J. E., Phys. Rev. B 23, 4183 (1981).CrossRefGoogle Scholar
13Eastman, D. E., Phys. Rev. B 2, 1 (1970).CrossRefGoogle Scholar
14Pauling, L., The Nature of the Chemical Bond (Cornell University Press, Ithaca, NY, 1960), 3rd ed., pp. 391–395.Google Scholar