Xenon and its compound (with
oxygen and fluorine)
Bartlett’s
Experiment with Xenon
A few chemists
questioned the absolute inertness of the noble gases. Among those scientists
were Walter Kossel in 1916 and Nobel-prize winning chemist Linus Pauling in
1933. They predicted that highly reactive atoms such as fluorine might form
compounds with xenon, the heaviest of the noble elements and whose electrons,
they observed, were not as tightly bound as those of the lighter gases.
In 1961 Neil Bartlett was
teaching chemistry at the University of British Columbia in Vancouver, Canada.
Some years earlier, while experimenting with fluorine and platinum, he had
accidentally produced a deep-red solid whose
exact chemical composition remained a mystery. With the assistance of his
graduate student Derek Lohmann, he vigorously pursued the identity of the red solid. After
much research, they eventually found that the known gaseous
fluoride, platinum hexafluoride (PtF6), was able to oxidize oxygen and produce the red solid, which he
and Lohmann had identified as O2+PtF6-
first
published report, in June 1962, of a noble gas compound was by Neil
Bartlett, who noticed that the highly oxidising
compound platinum hexafluoride ionised O2 to O+ As the
ionisation energy of O2 to O+ 2 (1165 kJ mol−1) is nearly equal to the ionisation energy of Xe
to Xe+ (1170 kJ mol−1), he tried the reaction of Xe with PtF6. This yielded a crystalline product, xenon hexafluoroplatinate, whose formula
was proposed to be Xe+[PtF6]−
It was later shown that the compound is actually more complex, containing both XeFPtF5 and XeFPt2F11 Nonetheless, this was the first real compound of any noble gas.
What was most unusual about this compound was that it contained oxygen in the form of positively charged ions, although oxygen usually has a net negative charge. Oxygen normally pulls electrons from other atoms and is thus called an oxidizing agent or oxidant. But Bartlett believed that in this case, the PtF6 component was a more powerful oxidizing agent than even oxygen and was extracting electrons from oxygen, leaving oxygen with a net positive charge
Xenon difluoride is a powerful fluorinating agent with the chemical formula XeF2, Xenon tetrafluoride is a XeF4. Xenon hexafluoride is a noble gas compound with the formula XeF6. All known are exergonic and stable at normal temperatures. XeF6 is the strongest fluorinating agent of the series. It is a colorless solid that readily sublimes into intensely yellow vapors.
Xenon-oxygen compounds
Xenon tetroxide is XeO4,Xenon formXeO3 is a colourless explosive solid.
XeOF4 is a colourless volatile liquid & some important compounds with oxygen like XeO3, XeOF4 XeO2F2
Geometry of xenon compound 👇 detail description
https://drive.google.com/file/d/1RB8zDXqI1lFPu_xxK3VVQxuuukNtC0LM/view?usp=sharing
1. . Assertion : xenon di fluoride linear geometry molecules of xenon.
Reason : XeF2 have two lone pair & two bonding electron pair due to sp3d hybridisation.
(i) Both assertion and reason are true and the reason is the correct explanation of assertion "
2. xenon tatra fluoride octahedral shaped .
Reason : in xenon tatrafluoride , xenon sp3d2 hybrid state its have two lone pair of electron
(v) Assertion is false but reason is true".
3. Assertion : xenon hexa fluoride octahedral shape molecule of xenon .
Reason : in xenon hexa fluoride ,xenon sp3d3 hybride state its have one lone pair of electron .
:
. (v) Assertion is false but reason is true.".
4. Assertion :xenon tri oxide pyramidal shape molecule of xenon .
Reason : in xenon tri oxide xenon sp3 hybride state and its have one lone pair of electron . :
(i) Both assertion and reason are true and the reason is the correct explanation of assertion ".
5. Assertion : xenon tetra oxide tetrahedral shape molecule of xenon .
Reason : in xenon tetra oxide xenon sp3 hybrid state and its have one lone pair of electron.
(iii) Assertion is true but the reason is false".
6. Assertion : xenon oxydifluoride have T shaped .
Reason : in xenon oxy di fluoride , xenon sp3d hybrid state and two lone pair electron occupied equatorial position ..
(i) Both assertion and reason are true and the reason is the correct explanation of assertion ".
7. Assertion : xenon dioxy difluoride have seesaw shaped .
Reason : in xenon oxy di fluoride xenon sp3d hybrid state and one lone pair electron occupied equatorial position.
(i) Both assertion and reason are true and the reason is the correct explanation of assertion".
8. Assertion : xenon oxy tetra fluoride have distorted ocatedral shaped.
Reason : In xenon oxy tetra fluoride, xenon sp3d2 hybrid state and its have one lone paired electron .
(i) Both assertion and reason are true and the reason is the correct explanation of assertion.".
9. Assertion : :- What inspired N bertlett for carrying out reaction between Xe and PtF6 .
Reason : N Bartlett noticed that PtF6 srong oxidizing agent which react O2 to form dioxygenyl hexafluoro platinate(v) but O2 molecules first ionization enthalpy more than xenon .
(i) Both assertion and reason are true and the reason is the correct explanation of assertion .".
10. Assertion : Xenon is called a stranger gas .
Reason : xenon name derived from the Greek word “Xenos” which translates to 'stranger' .
(i) Both assertion and reason are true and the reason is the correct explanation of assertion".
