Talk:Platinum hexafluoride

From Wikipedia, the free encyclopedia
Jump to: navigation, search
WikiProject Chemicals (Rated Start-class, Low-importance)
WikiProject icon This article is within the scope of WikiProject Chemicals, a daughter project of WikiProject Chemistry, which aims to improve Wikipedia's coverage of chemicals. To participate, help improve this article or visit the project page for details on the project.
Start-Class article Start  This article has been rated as Start-Class on the project's quality scale.
 Low  This article has been rated as Low-importance on the project's importance scale.

Melting Point/Boiling Point[edit]

This article currently describes PtF6 as subliming at 56.7°C, however, other sources (, Handbook of Inorganic Compounds) give a melting point of 61.3° and a boiling point of 69.1°. As such, I will change the data in the article to reflect the sources. --Pyrochem (talk) 06:33, 10 February 2008 (UTC)

bond lengths[edit]

The unit of bond lengths "1.85" is not understood.--Akane700 (talk) 14:05, 6 May 2008 (UTC)

ground state and d-electron count[edit]

The ground state cannot be triplet if it has four d-electrons. If this were the case it would be a quintuplet. This means that its two s-electrons are NOT promoted upon ionization, and that is has an electron count of s2d2. —Preceding unsigned comment added by (talk) 23:02, 2 March 2009 (UTC)

It's low-spin, so two of the four electrons in the t2g levels are paired, leaving two unpaired, hence the triplet.--Smokefoot (talk) 23:52, 2 March 2009 (UTC)

Yeah, but it's neither of those. See Phys. Rev. A 77, 034502 (2008) and Inorg. Chem. 2006, 45, 3782-3788. Relativistic spin-orbit coupling results in PtF6 having J=0, so that it's a closed-shell ground state. There's a very weak temperature-independent paramagnetism, but not enough to prevent acquisition of room-temperature 19F and 195Pt NMR spectra. The sentence "With only four d-electrons, it is paramagnetic with a triplet ground state" is totally false, with no basis in experimental measurement. -- (talk) 00:57, 6 April 2012 (UTC)

DOI's for those articles: doi:10.1103/PhysRevA.77.034502 and doi:10.1021/ic052029f. --Ben (talk) 08:17, 6 April 2012 (UTC)

Does PtF6 dissolve in anhydrous HF?[edit]

A Chinese website said that PtF6 can reacts with anhydrous HF, and it produces H[PtF7]. I can't find any references about it. --Makecat (talk) 12:54, 9 July 2011 (UTC)

Probably the most reliable source is a computational analysis of PtF7- in doi:10.1021/ic901967h.--Smokefoot (talk) 15:59, 9 July 2011 (UTC)