# 8.14.4: Reactions of Nobel Gases

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The noble gases (Group 18) are located in the far right of the periodic table and were previously referred to as the "inert gases" due to the fact that their filled valence shells (octets) make them extremely nonreactive.

## The Chemical Properties

Noble gases are odorless, colorless, nonflammable, and monotonic gases that have low chemical reactivity.

Atomic Number Element Number of Electrons/Shell
2 Helium 2
10 Neon 2,8
18 Argon 2,8,8
36 Krypton 2,8,18,8
54 Xenon 2,8,18,18,8

The full valence electron shells of these atoms make noble gases extremely stable and unlikely to form chemical bonds because they have little tendency to gain or lose electrons. Although noble gases do not normally react with other elements to form compounds, there are some exceptions. Xe may form compounds with fluoride and oxide.

##### Example 1: Xenon Fluorides

Xenon Difluoride ($$XeF_​2$$)

• Dense white crystallized solid
• Powerful fluorinating agent
• Covalent inorganic fluorides
• Stable xenon compound
• Decomposes on contact with light or water vapor
• Linear geometry
• Moisture sensitive
• Low vapor pressure

Xenon Tetrafluoride ($$XeF_4$$)

• Colorless Crystals
• Square planar geometry
• Discovered in 1963

Xenon Hexafluoride ($$XeF_6$$)

• Strongest fluorinating agent
• Colorless solid
• Highest coordination of the three binary fluorides of xenon ($$XeF_2$$ and $$XeF_4$$)
• Formation is exergonic, and the compound is stable at normal temperatures
• Readily sublimes into intense yellow vapors
• Structure lacks perfect octahedral symmetry
##### Example 2: Xenon Oxide

Xenon Tetroxide (XeO​4)

• Yellow crystalline solid
• Relatively stable
• Oxygen is the only element that can bring xenon up to its highest oxidation state of +8

Two other short-lived xenon compounds with an oxidation state of +8, XeO3F2 and XeO2F4, are produced in the reaction of xenon tetroxide with xenon hexafluoride.