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Group 0: Noble gases

Atomic structure and the periodic table • The periodic table

Key concepts

What you'll likely be quizzed about

  • Group 0 elements possess complete outer electron shells: helium has a 1s2 shell, while the others have an ns2 np6 configuration.
  • This arrangement creates electronic stability, minimizing the tendency to gain, lose, or share electrons in chemical reactions.
  • Consequently, these elements primarily exist as uncombined, monatomic gases under standard conditions.
  • High first ionization energies also result from the stability of the configuration; removing an electron disrupts this stability, making electron loss energetically unfavourable.

Flashcards

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Why are noble gases largely unreactive?

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Noble gases are largely unreactive due to their complete outer electron shells, which provide electronic stability and reduce the tendency to gain, lose, or share electrons.

Key notes

Important points to keep in mind

Full outer electron shells lead to very low chemical reactivity.

Atomic radius increases down the group due to added electron shells.

First ionization energy decreases down the group because of increased distance and shielding.

London dispersion forces strengthen down the group as polarizability increases with electron count.

Melting and boiling points increase down the group due to stronger London forces.

Density increases down the group as atomic mass rises faster than volume.

Heavier noble gases can form compounds under extreme conditions; xenon compounds are common lab examples.

Radon is radioactive, limiting experimental study and practical use.

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