Usually, increasing "s" character induces higher electronegativity. sp2 carbon has more s character than sp3 carbon. Therefore, sp2 carbon should have higher XPS binding energy than sp3 carbon ?. In the literature, most of the time sp3 carbon binding energy is greater than sp2. If we compare diamond-like carbon and graphene-like carbon which carbon has a higher binding energy ?. Why ?.
Along the graphite sheets the XPS binding energy is higher. But when the sheets slide or slip, I would give the marks to diamond like carbon.
Thank you for your reply, Prof. Padmanabhan. Is there any way you can rationalize that difference ?. Based on the electronegativity or molecular orbital theory..etc.?
The issue is discussed at length in this paper
DOI: 10.1021/acs.analchem.6b01327
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