Introduction of Group 18 elements

p-Block Elements: Group 18

General Introduction

The Group 18 elements are called noble gases or inert gases because they rarely combine with other elements. They are found only as uncombined elements in nature and some compounds. Nobel gases are colourless at room temperature. Only neon and helium are not yet prepared from their compounds.

The noble gases were discovered and isolated in the 1890s by William Ramsey, Lord Rayleigh, and Morris Travers. Noble gases had actually been first discovered, but not recognized, by Henry Cavendish in 1766. He passed a sequence of electric sparks through a mixture of air and oxygen and collected the gases that were produced at the end of the reaction.Each time he did the experiment, he noticed that around

In the rest of the periodic table, the number of the group is the same as the number of outer shell electrons in the elements of that group.However, this is not true for the noble gases. Helium only has 2 electrons in its outer shell, while the others all have 8. The group’s number is also referred to as 0 because of this.The values of an atomic number of noble gases strongly suggest that they should be placed after halogens and before alkali metals.

Xenon forms a large no. of compounds with oxygen and fluorine in different oxidation states. These are xenon fluorides, xenon oxides and xenon oxyfluoride. Some compounds are discussed below.


Formula Name Oxidn state Structure VSEPR explanation
XeF2 Xenon difluoride +2 Linear Five electron pairs form trigonal bipyramidal with three lone pairs at equatorial positions
XeF4 Xenon tetra fluoride +4 Square Planner Six electron pairs form octahedron with two positions occupied by lone pairs
XeF6 Xenon hexafluoride +6 Distorted octahedron Pentagonal bipyramidal or capped octahedron with one lone pair
XeO3 Xenon trioxide +6 Pyramidal tetrahedral (one corner unoccupied) Three π bonds so that the remaining four electron pairs form a tetrahedron with one corner occupied by a lone pair.
XeO2F2 Xenon dioxy difluoride +6 Trigonal bipyramidal (with one position unoccupied) Two π bonds so remaining five electron pair form trigonal bipyramid with one equatorial position occupied by a lone pair
XeOF4 Xenon oxy tetrafluoride +6 Square pyramidal (octahedral with one position unoccupied One π bond so remaining six electron pairs form an octahedron with one position occupied by a lone pair.
XeO4 Xenon tetraoxide +8 Tetrahedral Four π bonds so remaining four electron pair form a tetrahedron
XeO3F2 Xenon trioxy difluoride +8 Trigonal bipyramidal Three π bonds so remaining five electron pairs form trigonal bipyramid
Ba2[XeO6]-4 Barium perxenate +8 octahedral Two π bonds so remaining six electron pair form an octahedron.



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