Name: noble gases: sources, uses, and reactions
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Noble Gases

The nonmetallic elements categorized under group 18 &ndash; helium, neon, argon, krypton, xenon, and radon &ndash; are called noble gases. These elements occur as monatomic species and exist as gases under room-temperature. Radon is the only radioactive element from group 18.&nbsp;

Moving down the group, the elements exhibit an increase in boiling points, densities, and atomic radii, which consequently leads to the decline of ionization energies of each successive element.&nbsp;

Yet, noble gases have high first ionization energies compared to all other elements in the periodic table. This is because these elements have stable electron configurations with complete octets. The removal of an electron requires the input of a large amount of energy, which is unfavorable.&nbsp;

Noble gases also have positive electron affinity values. Meaning, energy is required to add an additional electron to a gaseous atom. Noble gases resist electron additions as their valence shells are already complete, and the incoming electron needs to enter a higher principal quantum shell.&nbsp;

The high stability of noble gases attests to their chemical inertness, which finds many industrial applications. For instance, argon is used to manufacture gas-filled electric light bulbs to prevent the oxidation of tungsten filaments, prolonging the bulb&rsquo;s life. Helium is used to create an inert atmosphere during the melting and welding of easily oxidizable metals.

Noble gases were Initially thought to be entirely chemically unreactive and were called inert gases. However, in the early sixties Neil Barlett discovered some exceptions. For example, xenon, with the lowest ionization energy from the noble gases, was found to react with the most electronegative element, fluorine.&nbsp;

Xenon difluoride, obtained by heating an excess of xenon gas with fluorine gas, is a stable, crystalline material. Other compounds like xenon tetrafluoride and xenon hexafluoride can also be prepared similarly.

Xenon-compounds with the electronegative element, oxygen, can be produced by replacing fluorine atoms in xenon fluorides with oxygen. For instance, xenon hexafluoride reacts with water, yielding a solution of xenon trioxide.&nbsp;

noble gases

The elements in group 18 are noble gases (helium, neon, argon, krypton, xenon, and radon). They earned the name &ldquo;noble&rdquo; because they were assumed to be nonreactive since they have filled valence shells. In 1962, Dr. Neil Bartlett at the University of British Columbia proved this assumption to be false.

These elements are present in the atmosphere in small amounts. Some natural gas contains 1&ndash;2% helium by mass. Helium is isolated from natural gas by liquefying the condensable components, leaving only helium as a gas. Radon comes from other radioactive elements. More recently, it was observed that this radioactive gas is present in very small amounts in soils and minerals. Its accumulation in well-insulated, tightly sealed buildings, however, constitutes a health hazard, primarily lung cancer.

The boiling points and melting points of the noble gases are extremely low relative to those of other substances of comparable atomic or molecular masses. This is because only weak London dispersion forces are present, and these forces can hold the atoms together only when molecular motion is very slight, as it is a very low temperature.

The full s and p orbitals of the valence shell add stability to the noble gases. These elements have the largest first ionization energies, indicating that the removal of an electron is difficult. Going down the group, atomic radius increases and ionization energy decreases. The positive electron affinity values of these elements reveal that they are unlikely to gain electrons as well. Table 1 summarizes the properties of the noble gases.

Table 1: Properties of the Noble Gases.

<table style="margin-left: auto; margin-right: auto;">
	<tbody style="border: 1px solid black;">
		<tr>
			<td style="color: black; border: 1px solid black; text-align: center;">Element</td>
			<td style="color: black; border: 1px solid black; text-align: center;">Electron Configuration</td>
			<td style="color: black; border: 1px solid black; text-align: center;">Atomic Radius (pm)</td>
			<td style="color: black; border: 1px solid black; text-align: center;">IE1 (kJ/mol)</td>
			<td style="color: black; border: 1px solid black; text-align: center;">EA (kJ/mol)</td>
			<td style="color: black; border: 1px solid black; text-align: center;">Density at STP (g/L)</td>
		</tr>
		<tr>
			<td style="color: black; border: 1px solid black; text-align: center;">He</td>
			<td style="color: black; border: 1px solid black; text-align: center;">1s2</td>
			<td style="color: black; border: 1px solid black; text-align: center;">32</td>
			<td style="color: black; border: 1px solid black; text-align: center;">2370</td>
			<td style="color: black; border: 1px solid black; text-align: center;">+20</td>
			<td style="color: black; border: 1px solid black; text-align: center;">0.18</td>
		</tr>
		<tr>
			<td style="color: black; border: 1px solid black; text-align: center;">Ne</td>
			<td style="color: black; border: 1px solid black; text-align: center;">[He] 2s22p6</td>
			<td style="color: black; border: 1px solid black; text-align: center;">70</td>
			<td style="color: black; border: 1px solid black; text-align: center;">2080</td>
			<td style="color: black; border: 1px solid black; text-align: center;">&minus;30</td>
			<td style="color: black; border: 1px solid black; text-align: center;">0.90</td>
		</tr>
		<tr>
			<td style="color: black; border: 1px solid black; text-align: center;">Ar</td>
			<td style="color: black; border: 1px solid black; text-align: center;">[Ne] 3s23p6</td>
			<td style="color: black; border: 1px solid black; text-align: center;">98</td>
			<td style="color: black; border: 1px solid black; text-align: center;">1520</td>
			<td style="color: black; border: 1px solid black; text-align: center;">+35</td>
			<td style="color: black; border: 1px solid black; text-align: center;">1.78</td>
		</tr>
		<tr>
			<td style="color: black; border: 1px solid black; text-align: center;">Kr</td>
			<td style="color: black; border: 1px solid black; text-align: center;">[Ar] 4s24p6</td>
			<td style="color: black; border: 1px solid black; text-align: center;">112</td>
			<td style="color: black; border: 1px solid black; text-align: center;">1350</td>
			<td style="color: black; border: 1px solid black; text-align: center;">+40</td>
			<td style="color: black; border: 1px solid black; text-align: center;">3.74</td>
		</tr>
		<tr>
			<td style="color: black; border: 1px solid black; text-align: center;">Xe</td>
			<td style="color: black; border: 1px solid black; text-align: center;">[Kr] 5s25p6</td>
			<td style="color: black; border: 1px solid black; text-align: center;">130</td>
			<td style="color: black; border: 1px solid black; text-align: center;">1170</td>
			<td style="color: black; border: 1px solid black; text-align: center;">+40</td>
			<td style="color: black; border: 1px solid black; text-align: center;">5.90</td>
		</tr>
	</tbody>
</table>

Argon is useful in the manufacture of gas-filled electric light bulbs, where its lower heat conductivity and chemical inertness made it preferable to nitrogen for inhibiting the vaporization of the tungsten filament and prolonging the life of the bulb. Fluorescent tubes commonly contain a mixture of argon and mercury vapor. Argon is the third most abundant gas in dry air.

Helium is used for filling balloons and lighter-than-air craft because it does not burn, making it safer to use than hydrogen. Liquid helium (boiling point, 4.2 K) is an important coolant to reach the low temperatures necessary for cryogenic research, and it is essential for achieving the low temperatures necessary to produce superconduction in traditional superconducting materials used in powerful magnets and other devices.

Neon is a component of neon lamps and signs.&nbsp;Passing an electric spark through a tube containing neon at low pressure generates the familiar red glow of neon. It is possible to change the color of the light by mixing argon or mercury vapor with the neon or by utilizing glass tubes of a special color.

Krypton-xenon flash tubes are used to take high-speed photographs. An electric discharge through such a tube gives a very intense light that lasts only 1/50,000 of a second. Krypton forms a difluoride, which is thermally unstable at room temperature.

Stable compounds of xenon form when xenon reacts with fluorine. Xenon difluoride, XeF2, forms after heating an excess of xenon gas with fluorine gas and then cooling. The material forms colorless crystals, which are stable at room temperature in a dry atmosphere. Xenon tetrafluoride, XeF4, and xenon hexafluoride, XeF6, are prepared in an analogous manner, with a stoichiometric amount of fluorine and an excess of fluorine, respectively. Compounds with oxygen are prepared by replacing fluorine atoms in the xenon fluorides with oxygen.

When XeF6 reacts with water, a solution of XeO3 results and the xenon remains in the +6&nbsp;oxidation state. Dry, solid xenon trioxide, XeO3, is extremely explosive &mdash; it will spontaneously detonate.

Unstable compounds of argon form at low temperatures, but stable compounds of helium and neon are not known.

This text is adapted from <a href="https://openstax.org/books/chemistry-2e/pages/18-12-occurrence-preparation-and-properties-of-the-noble-gases">Openstax, Chemistry 2e, Section 18.2: Occurrence, Preparation, and the Properties of Noble Gases.</a>


The elements in group 18 are noble gases (helium, neon, argon, krypton, xenon, and radon). They earned the name &ldquo;noble&rdquo; because they were ...

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noble gases: sources, uses, and reactions

Noble gases are the group 18 elements helium, neon, argon, krypton, xenon, and radon. They were called “noble” because they were once thought to be nonreactive. That idea changed in 1962, when Dr. Neil Bartlett at the University of British Columbia showed that this assumption was not fully correct.

These gases occur in very small amounts in the atmosphere. Some natural gas contains 1–2% helium by mass. Helium is separated from natural gas by removing the condensable components, which leaves helium behind as a gas. Radon is produced from other radioactive elements. It has also been found in tiny amounts in soils and minerals. When radon builds up in tightly sealed, well-insulated buildings, it becomes a health hazard. The main risk is lung cancer.

Noble gases also have very low boiling points and melting points compared with other substances of similar atomic or molecular mass. This happens because only weak London dispersion forces hold their atoms together. Those weak forces can only keep the atoms together when motion is very low, which is why very low temperatures are needed. Their filled s and p valence orbitals also add stability. These elements have the largest first ionization energies, so removing an electron is difficult. As you move down the group, atomic radius increases and ionization energy decreases. Their positive electron affinity values show that they are also unlikely to gain electrons.

Table 1 summarizes the noble gas properties. Helium has an atomic radius of 32 pm, an ionization energy of 2370 kJ/mol, and a density of 0.18 g/L at STP. Neon, argon, krypton, and xenon show increasing atomic radius and density, while first ionization energy decreases from 2080 to 1170 kJ/mol. Their electron configurations also show full valence shells.

Argon is useful in gas-filled electric light bulbs because it has lower heat conductivity and is chemically inert. It helps reduce tungsten filament vaporization and extend bulb life. Fluorescent tubes often contain argon and mercury vapor, and argon is the third most abundant gas in dry air. Helium is used in balloons and lighter-than-air craft because it does not burn, which makes it safer than hydrogen. Liquid helium, with a boiling point of 4.2 K, is an important coolant for cryogenic research and for producing superconductivity in traditional superconducting materials used in powerful magnets and other devices.

Neon is used in neon lamps and signs. When an electric spark passes through low-pressure neon, it produces the familiar red glow. The color can be changed by mixing in argon or mercury vapor or by using glass tubes of a special color. Krypton-xenon flash tubes are used for high-speed photography. Their electric discharge gives a very intense light that lasts only 1/50,000 of a second.

Noble gases can also form compounds under the right conditions. Krypton forms a difluoride, but it is thermally unstable at room temperature. Stable xenon compounds form when xenon reacts with fluorine. Xenon difluoride, XeF2, forms when excess xenon gas is heated with fluorine gas and then cooled. Xenon tetrafluoride, XeF4, and xenon hexafluoride, XeF6, are made in similar ways using the right fluorine amounts. Compounds with oxygen can be made by replacing fluorine atoms in xenon fluorides with oxygen. When XeF6 reacts with water, it gives a solution of XeO3, while xenon stays in the +6 oxidation state. Dry solid xenon trioxide, XeO3, is extremely explosive and can detonate on its own. Unstable argon compounds can form at low temperatures, but stable compounds of helium and neon are not known.

Noble Gases: Sources, Uses, and Reactions

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Noble gases are the group 18 elements helium, neon, argon, krypton, xenon, and radon. They were called “noble” because they were once thought to be nonreactive. That idea changed in 1962, when Dr. Neil Bartlett at the University of British Columbia showed that this assumption was not fully correct. These gases occur in very small amounts in the atmosphere. Some natural gas contains 1–2% helium by mass. Helium is separated from natural gas by removing the condensable components, which leaves...

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Noble Gases: Sources, Uses, and Reactions

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