Why Does Xe React with O2PtF6 to Form XePtF6?

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Discussion Overview

The discussion centers around the reaction of xenon (Xe) with O2PtF6 to form XePtF6. Participants explore the underlying chemistry, including the behavior of noble gases, the role of electronegativity, and the stability of the resulting compound.

Discussion Character

  • Exploratory
  • Technical explanation
  • Conceptual clarification
  • Debate/contested

Main Points Raised

  • Some participants suggest that simplistic views of atomic structure and the octet rule are inadequate to explain the reaction between Xe and O2PtF6.
  • It is proposed that fluorine's high electronegativity allows it to draw electrons away from xenon, which may facilitate the reaction.
  • One participant notes that xenon, being the largest stable noble gas, might be more likely to share its electrons compared to other noble gases.
  • There is uncertainty regarding the stability of the compound formed, with one participant mentioning that the theoretical calculation of electron wave functions could provide insights, though it may not have been done.
  • Another participant questions the accuracy of the chemical formula provided, suggesting that a different positively charged element might be involved instead of O2.
  • Concerns are raised about the stability of the compound at higher temperatures, with a mention that elemental xenon could be formed if the compound is disturbed by heat.
  • One participant provides information on the reactivity of xenon fluorides, noting that XeF6 is particularly reactive.
  • Clarifications are made regarding terms such as "homologues," "cation," and the radioactivity of radon.

Areas of Agreement / Disagreement

Participants express various viewpoints on the reactivity and stability of xenon compounds, with no consensus reached on the underlying reasons for the reaction or the specifics of the chemical formulas involved.

Contextual Notes

There are unresolved questions regarding the definitions of terms used in the discussion, the specific conditions under which the compounds are stable, and the theoretical calculations that might clarify the reaction mechanisms.

KingNothing
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Why in the world does [tex]Xe[/tex] react with [itex]O_2PtF_6[/itex] to form [tex]XePtF_6[/tex]?
 
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This is one of those cases where a simplistic view of the atom and and the octet rule are insufficient to describe what is going on.

However, keep in mind that flourine, being the most electronegative element, is going to be the best canidate to draw electrons away from anything. And Xeon, being the largest (stable) noble gas, is going to be the most likely of the noble gases, if any, to share its electrons since there are furthest away from the nucleus.

I realize I didn't really answer your question but gave only plausible explanations for why it might occur. Actually, I'm not sure if anyone really understands why its stable. Theoretically, you could calculate the wave function of every single electron in the bond, but I'm not sure if anyone has done that. What level chemistry are you taking again?
 
The first level. But its really easy so I'm trying to ask harder questions of the subject.
 
KingNothing, I am not sure if you correctly wrote the hexafluoroplatinate; I suppose some other positively charged element like potassium, sodium, etc., to be instead of O2?

So-crates is right about its reactivity, the outmost shell is more prone to electronic modifications than any lower homologues. Radone is too reactive (radioactive) to be so stable, so this is usually not considered as a "stable" noble gas.

Remember again, that the compound formed (including xenon as a cation) is stable only in low temperatures, disturbing it with some heat will cause elemental xenon to be formed. I think in this case, xenon difluoride, elemental xenon, and tetrafluoroplatinate species might occur.
 
What are homologues? Other elements? Lower energy levels? Why is Radon radioactive? Also, what is a Cation? Also, how low are the temperatures?
 
See the following on Webelements:

XeF2
XeF4
XeF6

Apparently XeF6 is so reactive (more so than lower order fluorides), it cannot be contained in dry quartz.

Radon is radioactive because it has a sufficient excess of neutrons. Rn has Z=86. Lighter radioactive neighbors include Polonium (Z=84) and Astatine (Z=85). Bismuth is the heaviest element with a stable isotope (Bi-209).

Cation is a positive ion.
 

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