Phosphorus, Sulfur, and Silicon

5.03 Inorganic Chemistry Journal of Fluorine Chemistry

5.03 Inorganic Chemistry Fluorine Laboratory Fluorine tank in gold (10% in N2), HF in blue

5.03 Inorganic Chemistry Fluorine Laboratory Steel lines feeding into fume hood

5.03 Inorganic Chemistry Fluorine Laboratory Stainless steel manifold for F2, fluoropolymer plastic line for HF

5.03 Inorganic Chemistry Fluorine Laboratory Suiting up for using the manifold

5.03 Inorganic Chemistry Fluorine Laboratory Diagram of HF manifold

5.03 Inorganic Chemistry Fluorine Laboratory Diagram of F2 manifold

5.03 Inorganic Chemistry Neil Bartlett 1932-2008 Konrad Seppelt, Neil Bartlett obituary DOI: 10.1002/anie.200804715

Linus Pauling predicted the existence of noble gas compounds in the 1930s and stuck to this belief for decades before withdrawing it in 1961 One year later, Neil Bartlett synthesized the first xenon compound, XePtF6 Ironically, the nature of that first xenon compound has not yet been resolved

The reaction of xenon with PtF6 was voted as one of the ten best experiments in the history of chemistry

After the discovery of XePtF6, it took only a matter of weeks and months to isolate XeF2, XeF4, XeF6, XeO3, and KrF2

5.03 Inorganic Chemistry Neil Bartlett 1932-2008 Konrad Seppelt, Neil Bartlett obituary DOI: 10.1002/anie.200804715

Linus Pauling predicted the existence of noble gas compounds in the 1930s and stuck to this belief for decades before withdrawing it in 1961 One year later, Neil Bartlett synthesized the first xenon compound, XePtF6 Ironically, the nature of that first xenon compound has not yet been resolved

The reaction of xenon with PtF6 was voted as one of the ten best experiments in the history of chemistry

After the discovery of XePtF6, it took only a matter of weeks and months to isolate XeF2, XeF4, XeF6, XeO3, and KrF2

5.03 Inorganic Chemistry Neil Bartlett 1932-2008 Konrad Seppelt, Neil Bartlett obituary DOI: 10.1002/anie.200804715

Linus Pauling predicted the existence of noble gas compounds in the 1930s and stuck to this belief for decades before withdrawing it in 1961 One year later, Neil Bartlett synthesized the first xenon compound, XePtF6 Ironically, the nature of that first xenon compound has not yet been resolved

The reaction of xenon with PtF6 was voted as one of the ten best experiments in the history of chemistry

After the discovery of XePtF6, it took only a matter of weeks and months to isolate XeF2, XeF4, XeF6, XeO3, and KrF2

5.03 Inorganic Chemistry Neil Bartlett 1932-2008 Konrad Seppelt, Neil Bartlett obituary DOI: 10.1002/anie.200804715

Linus Pauling predicted the existence of noble gas compounds in the 1930s and stuck to this belief for decades before withdrawing it in 1961 One year later, Neil Bartlett synthesized the first xenon compound, XePtF6 Ironically, the nature of that first xenon compound has not yet been resolved

The reaction of xenon with PtF6 was voted as one of the ten best experiments in the history of chemistry

After the discovery of XePtF6, it took only a matter of weeks and months to isolate XeF2, XeF4, XeF6, XeO3, and KrF2

5.03 Inorganic Chemistry Neil Bartlett 1932-2008 Konrad Seppelt, Neil Bartlett obituary DOI: 10.1002/anie.200804715

Linus Pauling predicted the existence of noble gas compounds in the 1930s and stuck to this belief for decades before withdrawing it in 1961 One year later, Neil Bartlett synthesized the first xenon compound, XePtF6 Ironically, the nature of that first xenon compound has not yet been resolved

The reaction of xenon with PtF6 was voted as one of the ten best experiments in the history of chemistry

After the discovery of XePtF6, it took only a matter of weeks and months to isolate XeF2, XeF4, XeF6, XeO3, and KrF2

5.03 Inorganic Chemistry Neil Bartlett 1932-2008 Konrad Seppelt, Neil Bartlett obituary DOI: 10.1002/anie.200804715

Linus Pauling predicted the existence of noble gas compounds in the 1930s and stuck to this belief for decades before withdrawing it in 1961 One year later, Neil Bartlett synthesized the first xenon compound, XePtF6 Ironically, the nature of that first xenon compound has not yet been resolved

The reaction of xenon with PtF6 was voted as one of the ten best experiments in the history of chemistry

After the discovery of XePtF6, it took only a matter of weeks and months to isolate XeF2, XeF4, XeF6, XeO3, and KrF2

5.03 Inorganic Chemistry Neil Bartlett 1932-2008 Karl O. Christe, Neil Bartlett obituary DOI: 10.1038/455182a

With one stroke of genius, he destroyed the long-standing dogma that the “noble gases” (also known as the inert or rare gases) are unreactive Attempts to prepare compounds of the noble gases date back to the discovery of argon by William Ramsay in 1894 Walther Kossel in 1916 predicted, on the basis of ionization potentials, that krypton and xenon fluorides should exist Attempts to verify that prediction by various investigators, including Otto Ruff, considered one of the greatest inorganic fluorine chemists of all time, were unsuccessful Ruff pursued only argon and krypton fluorides, and not those of xenon

5.03 Inorganic Chemistry Neil Bartlett 1932-2008 Karl O. Christe, Neil Bartlett obituary DOI: 10.1038/455182a

With one stroke of genius, he destroyed the long-standing dogma that the “noble gases” (also known as the inert or rare gases) are unreactive Attempts to prepare compounds of the noble gases date back to the discovery of argon by William Ramsay in 1894 Walther Kossel in 1916 predicted, on the basis of ionization potentials, that krypton and xenon fluorides should exist Attempts to verify that prediction by various investigators, including Otto Ruff, considered one of the greatest inorganic fluorine chemists of all time, were unsuccessful Ruff pursued only argon and krypton fluorides, and not those of xenon

5.03 Inorganic Chemistry Neil Bartlett 1932-2008 Karl O. Christe, Neil Bartlett obituary DOI: 10.1038/455182a

With one stroke of genius, he destroyed the long-standing dogma that the “noble gases” (also known as the inert or rare gases) are unreactive Attempts to prepare compounds of the noble gases date back to the discovery of argon by William Ramsay in 1894 Walther Kossel in 1916 predicted, on the basis of ionization potentials, that krypton and xenon fluorides should exist Attempts to verify that prediction by various investigators, including Otto Ruff, considered one of the greatest inorganic fluorine chemists of all time, were unsuccessful Ruff pursued only argon and krypton fluorides, and not those of xenon

5.03 Inorganic Chemistry Neil Bartlett 1932-2008 Karl O. Christe, Neil Bartlett obituary DOI: 10.1038/455182a

With one stroke of genius, he destroyed the long-standing dogma that the “noble gases” (also known as the inert or rare gases) are unreactive Attempts to prepare compounds of the noble gases date back to the discovery of argon by William Ramsay in 1894 Walther Kossel in 1916 predicted, on the basis of ionization potentials, that krypton and xenon fluorides should exist Attempts to verify that prediction by various investigators, including Otto Ruff, considered one of the greatest inorganic fluorine chemists of all time, were unsuccessful Ruff pursued only argon and krypton fluorides, and not those of xenon

5.03 Inorganic Chemistry Neil Bartlett 1932-2008 Karl O. Christe, Neil Bartlett obituary DOI: 10.1038/455182a

With one stroke of genius, he destroyed the long-standing dogma that the “noble gases” (also known as the inert or rare gases) are unreactive Attempts to prepare compounds of the noble gases date back to the discovery of argon by William Ramsay in 1894 Walther Kossel in 1916 predicted, on the basis of ionization potentials, that krypton and xenon fluorides should exist Attempts to verify that prediction by various investigators, including Otto Ruff, considered one of the greatest inorganic fluorine chemists of all time, were unsuccessful Ruff pursued only argon and krypton fluorides, and not those of xenon

5.03 Inorganic Chemistry Neil Bartlett 1932-2008 Karl O. Christe, Neil Bartlett obituary DOI: 10.1038/455182a

With one stroke of genius, he destroyed the long-standing dogma that the “noble gases” (also known as the inert or rare gases) are unreactive Attempts to prepare compounds of the noble gases date back to the discovery of argon by William Ramsay in 1894 Walther Kossel in 1916 predicted, on the basis of ionization potentials, that krypton and xenon fluorides should exist Attempts to verify that prediction by various investigators, including Otto Ruff, considered one of the greatest inorganic fluorine chemists of all time, were unsuccessful Ruff pursued only argon and krypton fluorides, and not those of xenon

5.03 Inorganic Chemistry Neil Bartlett 1932-2008 Karl O. Christe, Neil Bartlett obituary DOI: 10.1038/455182a

In 1933, Linus Pauling predicted the existence of H4XeO6, KrF6, and XeF6 His colleagues Don Yost and Albert Kaye used electric discharges of Xe/F2 mixtures in an attempt to verify the prediction They came close to making xenon fluorides but did not succeed in isolating measurable amounts That failure was taken generally as evidence that the noble gases are unreactive, a principle that made its way into essentially all textbooks Bartlett, however, was undeterred

5.03 Inorganic Chemistry Neil Bartlett 1932-2008 Karl O. Christe, Neil Bartlett obituary DOI: 10.1038/455182a

In 1933, Linus Pauling predicted the existence of H4XeO6, KrF6, and XeF6 His colleagues Don Yost and Albert Kaye used electric discharges of Xe/F2 mixtures in an attempt to verify the prediction They came close to making xenon fluorides but did not succeed in isolating measurable amounts That failure was taken generally as evidence that the noble gases are unreactive, a principle that made its way into essentially all textbooks Bartlett, however, was undeterred

5.03 Inorganic Chemistry Neil Bartlett 1932-2008 Karl O. Christe, Neil Bartlett obituary DOI: 10.1038/455182a

In 1933, Linus Pauling predicted the existence of H4XeO6, KrF6, and XeF6 His colleagues Don Yost and Albert Kaye used electric discharges of Xe/F2 mixtures in an attempt to verify the prediction They came close to making xenon fluorides but did not succeed in isolating measurable amounts That failure was taken generally as evidence that the noble gases are unreactive, a principle that made its way into essentially all textbooks Bartlett, however, was undeterred

5.03 Inorganic Chemistry Neil Bartlett 1932-2008 Karl O. Christe, Neil Bartlett obituary DOI: 10.1038/455182a

In 1933, Linus Pauling predicted the existence of H4XeO6, KrF6, and XeF6 His colleagues Don Yost and Albert Kaye used electric discharges of Xe/F2 mixtures in an attempt to verify the prediction They came close to making xenon fluorides but did not succeed in isolating measurable amounts That failure was taken generally as evidence that the noble gases are unreactive, a principle that made its way into essentially all textbooks Bartlett, however, was undeterred

5.03 Inorganic Chemistry Neil Bartlett 1932-2008 Karl O. Christe, Neil Bartlett obituary DOI: 10.1038/455182a

In 1933, Linus Pauling predicted the existence of H4XeO6, KrF6, and XeF6 His colleagues Don Yost and Albert Kaye used electric discharges of Xe/F2 mixtures in an attempt to verify the prediction They came close to making xenon fluorides but did not succeed in isolating measurable amounts That failure was taken generally as evidence that the noble gases are unreactive, a principle that made its way into essentially all textbooks Bartlett, however, was undeterred

5.03 Inorganic Chemistry Neil Bartlett 1932-2008 Karl O. Christe, Neil Bartlett obituary DOI: 10.1038/455182a

In 1933, Linus Pauling predicted the existence of H4XeO6, KrF6, and XeF6 His colleagues Don Yost and Albert Kaye used electric discharges of Xe/F2 mixtures in an attempt to verify the prediction They came close to making xenon fluorides but did not succeed in isolating measurable amounts That failure was taken generally as evidence that the noble gases are unreactive, a principle that made its way into essentially all textbooks Bartlett, however, was undeterred

5.03 Inorganic Chemistry Neil Bartlett 1932-2008 Karl O. Christe, Neil Bartlett obituary DOI: 10.1038/455182a

He was pursuing the synthesis of PtF2 by reduction of PtF4

He purified PtF4 by heating it in a dilute stream of fluorine in a Pyrex apparatus He obtained a red sublimate which he initially thought was + − PtF4O, but subsequently identified correctly as O2 PtF6 The discovery of this compound was accidental, as Bartlett himself stated, but his subsequent reasoning and experiments were brilliant

He recognized that if PtF6 can oxidize O2 (i.p. = 12.2 eV), then it should also be capable of oxidizing xenon (i.p. = 12.13 eV)

5.03 Inorganic Chemistry Neil Bartlett 1932-2008 Karl O. Christe, Neil Bartlett obituary DOI: 10.1038/455182a

He was pursuing the synthesis of PtF2 by reduction of PtF4

He purified PtF4 by heating it in a dilute stream of fluorine in a Pyrex apparatus He obtained a red sublimate which he initially thought was + − PtF4O, but subsequently identified correctly as O2 PtF6 The discovery of this compound was accidental, as Bartlett himself stated, but his subsequent reasoning and experiments were brilliant

He recognized that if PtF6 can oxidize O2 (i.p. = 12.2 eV), then it should also be capable of oxidizing xenon (i.p. = 12.13 eV)

5.03 Inorganic Chemistry Neil Bartlett 1932-2008 Karl O. Christe, Neil Bartlett obituary DOI: 10.1038/455182a

He was pursuing the synthesis of PtF2 by reduction of PtF4

He purified PtF4 by heating it in a dilute stream of fluorine in a Pyrex apparatus He obtained a red sublimate which he initially thought was + − PtF4O, but subsequently identified correctly as O2 PtF6 The discovery of this compound was accidental, as Bartlett himself stated, but his subsequent reasoning and experiments were brilliant

He recognized that if PtF6 can oxidize O2 (i.p. = 12.2 eV), then it should also be capable of oxidizing xenon (i.p. = 12.13 eV)

5.03 Inorganic Chemistry Neil Bartlett 1932-2008 Karl O. Christe, Neil Bartlett obituary DOI: 10.1038/455182a

He was pursuing the synthesis of PtF2 by reduction of PtF4

He purified PtF4 by heating it in a dilute stream of fluorine in a Pyrex apparatus He obtained a red sublimate which he initially thought was + − PtF4O, but subsequently identified correctly as O2 PtF6 The discovery of this compound was accidental, as Bartlett himself stated, but his subsequent reasoning and experiments were brilliant

He recognized that if PtF6 can oxidize O2 (i.p. = 12.2 eV), then it should also be capable of oxidizing xenon (i.p. = 12.13 eV)

5.03 Inorganic Chemistry Neil Bartlett 1932-2008 Karl O. Christe, Neil Bartlett obituary DOI: 10.1038/455182a

He was pursuing the synthesis of PtF2 by reduction of PtF4

He purified PtF4 by heating it in a dilute stream of fluorine in a Pyrex apparatus He obtained a red sublimate which he initially thought was + − PtF4O, but subsequently identified correctly as O2 PtF6 The discovery of this compound was accidental, as Bartlett himself stated, but his subsequent reasoning and experiments were brilliant

He recognized that if PtF6 can oxidize O2 (i.p. = 12.2 eV), then it should also be capable of oxidizing xenon (i.p. = 12.13 eV)

5.03 Inorganic Chemistry Neil Bartlett 1932-2008 Karl O. Christe, Neil Bartlett obituary DOI: 10.1038/455182a

He was pursuing the synthesis of PtF2 by reduction of PtF4

He purified PtF4 by heating it in a dilute stream of fluorine in a Pyrex apparatus He obtained a red sublimate which he initially thought was + − PtF4O, but subsequently identified correctly as O2 PtF6 The discovery of this compound was accidental, as Bartlett himself stated, but his subsequent reasoning and experiments were brilliant

He recognized that if PtF6 can oxidize O2 (i.p. = 12.2 eV), then it should also be capable of oxidizing xenon (i.p. = 12.13 eV)

5.03 Inorganic Chemistry Neil Bartlett 1932-2008 Karl O. Christe, Neil Bartlett obituary DOI: 10.1038/455182a

Bartlett’s classic experiment in preparing XePtF6 confirmed his reasoning and gave rise to worldwide interest in noble gas chemistry Thousands of papers have since been published on the subject We now know that xenon can form bonds not only to fluorine but also to many other elements of the periodic table Noble gas chemistry is not limited to xenon - even argon can form some compounds, such as HArF Although many of them are unstable, they nevertheless exist

5.03 Inorganic Chemistry Neil Bartlett 1932-2008 Karl O. Christe, Neil Bartlett obituary DOI: 10.1038/455182a

Bartlett’s classic experiment in preparing XePtF6 confirmed his reasoning and gave rise to worldwide interest in noble gas chemistry Thousands of papers have since been published on the subject We now know that xenon can form bonds not only to fluorine but also to many other elements of the periodic table Noble gas chemistry is not limited to xenon - even argon can form some compounds, such as HArF Although many of them are unstable, they nevertheless exist

5.03 Inorganic Chemistry Neil Bartlett 1932-2008 Karl O. Christe, Neil Bartlett obituary DOI: 10.1038/455182a

Bartlett’s classic experiment in preparing XePtF6 confirmed his reasoning and gave rise to worldwide interest in noble gas chemistry Thousands of papers have since been published on the subject We now know that xenon can form bonds not only to fluorine but also to many other elements of the periodic table Noble gas chemistry is not limited to xenon - even argon can form some compounds, such as HArF Although many of them are unstable, they nevertheless exist

5.03 Inorganic Chemistry Neil Bartlett 1932-2008 Karl O. Christe, Neil Bartlett obituary DOI: 10.1038/455182a

Bartlett’s classic experiment in preparing XePtF6 confirmed his reasoning and gave rise to worldwide interest in noble gas chemistry Thousands of papers have since been published on the subject We now know that xenon can form bonds not only to fluorine but also to many other elements of the periodic table Noble gas chemistry is not limited to xenon - even argon can form some compounds, such as HArF Although many of them are unstable, they nevertheless exist

5.03 Inorganic Chemistry Neil Bartlett 1932-2008 Karl O. Christe, Neil Bartlett obituary DOI: 10.1038/455182a

Bartlett’s classic experiment in preparing XePtF6 confirmed his reasoning and gave rise to worldwide interest in noble gas chemistry Thousands of papers have since been published on the subject We now know that xenon can form bonds not only to fluorine but also to many other elements of the periodic table Noble gas chemistry is not limited to xenon - even argon can form some compounds, such as HArF Although many of them are unstable, they nevertheless exist

5.03 Inorganic Chemistry Neil Bartlett 1932-2008 Karl O. Christe, Neil Bartlett obituary DOI: 10.1038/455182a

Bartlett’s classic experiment in preparing XePtF6 confirmed his reasoning and gave rise to worldwide interest in noble gas chemistry Thousands of papers have since been published on the subject We now know that xenon can form bonds not only to fluorine but also to many other elements of the periodic table Noble gas chemistry is not limited to xenon - even argon can form some compounds, such as HArF Although many of them are unstable, they nevertheless exist

5.03 Inorganic Chemistry Neil Bartlett 1932-2008 Karl O. Christe, Neil Bartlett obituary DOI: 10.1038/455182a

Bartlett’s discovery was hailed as “one of the most important developments in inorganic chemistry in modern times” It was not a one-off stroke of luck Throughout his career, Bartlett continually demonstrated the same keen sense of reasoning and mastery as an experimentalist, particularly in the area of xenon fluoride cations and molecular adducts of xenon fluorides with other molecules He worked on the creation of synthetic metals from graphite and graphite-like boron nitride, and salts of perfluoroaromatic cations He worked on unstable compounds at the limits of oxidation, such as NiF4 and AgF3, both ideal sources of fluorine radicals under very mild conditions

5.03 Inorganic Chemistry Neil Bartlett 1932-2008 Karl O. Christe, Neil Bartlett obituary DOI: 10.1038/455182a

Bartlett’s discovery was hailed as “one of the most important developments in inorganic chemistry in modern times” It was not a one-off stroke of luck Throughout his career, Bartlett continually demonstrated the same keen sense of reasoning and mastery as an experimentalist, particularly in the area of xenon fluoride cations and molecular adducts of xenon fluorides with other molecules He worked on the creation of synthetic metals from graphite and graphite-like boron nitride, and salts of perfluoroaromatic cations He worked on unstable compounds at the limits of oxidation, such as NiF4 and AgF3, both ideal sources of fluorine radicals under very mild conditions

5.03 Inorganic Chemistry Neil Bartlett 1932-2008 Karl O. Christe, Neil Bartlett obituary DOI: 10.1038/455182a

Bartlett’s discovery was hailed as “one of the most important developments in inorganic chemistry in modern times” It was not a one-off stroke of luck Throughout his career, Bartlett continually demonstrated the same keen sense of reasoning and mastery as an experimentalist, particularly in the area of xenon fluoride cations and molecular adducts of xenon fluorides with other molecules He worked on the creation of synthetic metals from graphite and graphite-like boron nitride, and salts of perfluoroaromatic cations He worked on unstable compounds at the limits of oxidation, such as NiF4 and AgF3, both ideal sources of fluorine radicals under very mild conditions

5.03 Inorganic Chemistry Neil Bartlett 1932-2008 Karl O. Christe, Neil Bartlett obituary DOI: 10.1038/455182a

Bartlett’s discovery was hailed as “one of the most important developments in inorganic chemistry in modern times” It was not a one-off stroke of luck Throughout his career, Bartlett continually demonstrated the same keen sense of reasoning and mastery as an experimentalist, particularly in the area of xenon fluoride cations and molecular adducts of xenon fluorides with other molecules He worked on the creation of synthetic metals from graphite and graphite-like boron nitride, and salts of perfluoroaromatic cations He worked on unstable compounds at the limits of oxidation, such as NiF4 and AgF3, both ideal sources of fluorine radicals under very mild conditions

5.03 Inorganic Chemistry Neil Bartlett 1932-2008 Karl O. Christe, Neil Bartlett obituary DOI: 10.1038/455182a

Bartlett’s discovery was hailed as “one of the most important developments in inorganic chemistry in modern times” It was not a one-off stroke of luck Throughout his career, Bartlett continually demonstrated the same keen sense of reasoning and mastery as an experimentalist, particularly in the area of xenon fluoride cations and molecular adducts of xenon fluorides with other molecules He worked on the creation of synthetic metals from graphite and graphite-like boron nitride, and salts of perfluoroaromatic cations He worked on unstable compounds at the limits of oxidation, such as NiF4 and AgF3, both ideal sources of fluorine radicals under very mild conditions

5.03 Inorganic Chemistry Neil Bartlett 1932-2008 Karl O. Christe, Neil Bartlett obituary DOI: 10.1038/455182a

Bartlett’s discovery was hailed as “one of the most important developments in inorganic chemistry in modern times” It was not a one-off stroke of luck Throughout his career, Bartlett continually demonstrated the same keen sense of reasoning and mastery as an experimentalist, particularly in the area of xenon fluoride cations and molecular adducts of xenon fluorides with other molecules He worked on the creation of synthetic metals from graphite and graphite-like boron nitride, and salts of perfluoroaromatic cations He worked on unstable compounds at the limits of oxidation, such as NiF4 and AgF3, both ideal sources of fluorine radicals under very mild conditions

5.03 Inorganic Chemistry

A Decade of Noble Gas Chemistry

Claasen, Malm, and Selig at Argonne National Lab conducted a now-famous experiment on Aug. 2, 1962 Xenon and fluorine (1:5 ratio) were heated in a nickel can at 400 ◦C and 6 atm for 1 h. Xe consumption was essentially complete! The can contents readily sublimed into a glass vessel as brilliant colorless XeF4 crystals Xenon di and hexafluorides were also quickly synthesized from the elements Xenon-oxygen compounds cannot yet be directly synthesized

5.03 Inorganic Chemistry A Decade of Noble Gas Chemistry

Claasen, Malm, and Selig at Argonne National Lab conducted a now-famous experiment on Aug. 2, 1962 Xenon and fluorine (1:5 ratio) were heated in a nickel can at 400 ◦C and 6 atm for 1 h. Xe consumption was essentially complete! The can contents readily sublimed into a glass vessel as brilliant colorless XeF4 crystals Xenon di and hexafluorides were also quickly synthesized from the elements Xenon-oxygen compounds cannot yet be directly synthesized

5.03 Inorganic Chemistry A Decade of Noble Gas Chemistry

Claasen, Malm, and Selig at Argonne National Lab conducted a now-famous experiment on Aug. 2, 1962 Xenon and fluorine (1:5 ratio) were heated in a nickel can at 400 ◦C and 6 atm for 1 h. Xe consumption was essentially complete! The can contents readily sublimed into a glass vessel as brilliant colorless XeF4 crystals Xenon di and hexafluorides were also quickly synthesized from the elements Xenon-oxygen compounds cannot yet be directly synthesized

5.03 Inorganic Chemistry A Decade of Noble Gas Chemistry

Claasen, Malm, and Selig at Argonne National Lab conducted a now-famous experiment on Aug. 2, 1962 Xenon and fluorine (1:5 ratio) were heated in a nickel can at 400 ◦C and 6 atm for 1 h. Xe consumption was essentially complete! The can contents readily sublimed into a glass vessel as brilliant colorless XeF4 crystals Xenon di and hexafluorides were also quickly synthesized from the elements Xenon-oxygen compounds cannot yet be directly synthesized

5.03 Inorganic Chemistry A Decade of Noble Gas Chemistry

Claasen, Malm, and Selig at Argonne National Lab conducted a now-famous experiment on Aug. 2, 1962 Xenon and fluorine (1:5 ratio) were heated in a nickel can at 400 ◦C and 6 atm for 1 h. Xe consumption was essentially complete! The can contents readily sublimed into a glass vessel as brilliant colorless XeF4 crystals Xenon di and hexafluorides were also quickly synthesized from the elements Xenon-oxygen compounds cannot yet be directly synthesized

5.03 Inorganic Chemistry A Decade of Noble Gas Chemistry

Claasen, Malm, and Selig at Argonne National Lab conducted a now-famous experiment on Aug. 2, 1962 Xenon and fluorine (1:5 ratio) were heated in a nickel can at 400 ◦C and 6 atm for 1 h. Xe consumption was essentially complete! The can contents readily sublimed into a glass vessel as brilliant colorless XeF4 crystals Xenon di and hexafluorides were also quickly synthesized from the elements Xenon-oxygen compounds cannot yet be directly synthesized

5.03 Inorganic Chemistry A Decade of Noble Gas Chemistry

Xenon compounds vary considerably in their stability

XeCl2 can only be prepared by the Nelson-Pimentel matrix isolation technique ◦ XeO3 (∆Hf = 400 kJ/mol) is an explosive comparable with TNT Xenon chemistry based on the even oxidation states closely resembles that of iodine, and to some extent, osmium and tellurium Argon (i.p. = 15.76), Neon (i.p. = 21.56), and helium (i.p. = 24.59), do not react with fluorine using the Pimentel matrix isolation technique

5.03 Inorganic Chemistry A Decade of Noble Gas Chemistry

Xenon compounds vary considerably in their stability

XeCl2 can only be prepared by the Nelson-Pimentel matrix isolation technique ◦ XeO3 (∆Hf = 400 kJ/mol) is an explosive comparable with TNT Xenon chemistry based on the even oxidation states closely resembles that of iodine, and to some extent, osmium and tellurium Argon (i.p. = 15.76), Neon (i.p. = 21.56), and helium (i.p. = 24.59), do not react with fluorine using the Pimentel matrix isolation technique

5.03 Inorganic Chemistry A Decade of Noble Gas Chemistry

Xenon compounds vary considerably in their stability

XeCl2 can only be prepared by the Nelson-Pimentel matrix isolation technique ◦ XeO3 (∆Hf = 400 kJ/mol) is an explosive comparable with TNT Xenon chemistry based on the even oxidation states closely resembles that of iodine, and to some extent, osmium and tellurium Argon (i.p. = 15.76), Neon (i.p. = 21.56), and helium (i.p. = 24.59), do not react with fluorine using the Pimentel matrix isolation technique

5.03 Inorganic Chemistry A Decade of Noble Gas Chemistry

Xenon compounds vary considerably in their stability

XeCl2 can only be prepared by the Nelson-Pimentel matrix isolation technique ◦ XeO3 (∆Hf = 400 kJ/mol) is an explosive comparable with TNT Xenon chemistry based on the even oxidation states closely resembles that of iodine, and to some extent, osmium and tellurium Argon (i.p. = 15.76), Neon (i.p. = 21.56), and helium (i.p. = 24.59), do not react with fluorine using the Pimentel matrix isolation technique

5.03 Inorganic Chemistry A Decade of Noble Gas Chemistry

Xenon compounds vary considerably in their stability

XeCl2 can only be prepared by the Nelson-Pimentel matrix isolation technique ◦ XeO3 (∆Hf = 400 kJ/mol) is an explosive comparable with TNT Xenon chemistry based on the even oxidation states closely resembles that of iodine, and to some extent, osmium and tellurium Argon (i.p. = 15.76), Neon (i.p. = 21.56), and helium (i.p. = 24.59), do not react with fluorine using the Pimentel matrix isolation technique

5.03 Inorganic Chemistry A Decade of Noble Gas Chemistry

Xenon compounds vary considerably in their stability

XeCl2 can only be prepared by the Nelson-Pimentel matrix isolation technique ◦ XeO3 (∆Hf = 400 kJ/mol) is an explosive comparable with TNT Xenon chemistry based on the even oxidation states closely resembles that of iodine, and to some extent, osmium and tellurium Argon (i.p. = 15.76), Neon (i.p. = 21.56), and helium (i.p. = 24.59), do not react with fluorine using the Pimentel matrix isolation technique

5.03 Inorganic Chemistry

Xenon Difluoride

5.03 Inorganic Chemistry

Pentafluoroxenate(IV) Anion First example of a pentagonal planar AX5 species, DOI: 10.1021/ja00009a021

5.03 Inorganic Chemistry Pentafluoroxenate(IV) Anion 129Xe is a good NMR nucleus, I = 1/2, abundance 26.44%

5.03 Inorganic Chemistry Pentafluoroxenate(IV) Anion Natural bond orbital analysis: lone pairs are unhybridized

5.03 Inorganic Chemistry Perfluoro Diphenylxenon CCDC code IDUQED, 169453, Bock et al. 2002, Xe–C distance: 2.394 A˚

5.03 Inorganic Chemistry Perfluorophenylxenon Cation, Tetracyanoborate CCDC code MOFJEX, Xe–C distance: 2.08 A˚

5.03 Inorganic Chemistry Perfluorophenylxenon Cation, Chloride Salt CCDC code DAMROY

5.03 Inorganic Chemistry Perfluoro Phenylxenon Benzoate CCDC code WADHIS, 56762, Frohn et al. 1993

5.03 Inorganic Chemistry The Periodic Table

5.03 Inorganic Chemistry