Question

# In which of the following compounds, the Fluorine atoms are placed axially in a trigonal bipyramidal geometry?

A
XeOF2
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B
XeOF4
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C
XeF2
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D
XeO2F2
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Solution

## The correct options are A XeOF2 C XeF2 D XeO2F2We had earlier seen that XeF2 has a linear shape. The 3 lone pairs of electrons of central Xe atom lie on the plane perpendicular to the axial Xe – F bonds. The molecule has a trigonal bipyramidal geometry In this molecule, if one oxygen atom takes the place of a lone pair, we get the geometry of XeOF2. Do note that Xenon has a double bond with the oxygen atom. Let us look at the ground state and excited state: Let us look at the geometry: Now try to deduce the shape and geometry of XeO2F2: A logical leap is to assume that the structure would be similar to replacing two of the three lone pairs with two oxygen atoms in the XeF2 structure. It is a good guess! As for the geometry, XeF2, XeOF2 and XeO2F2 all have the same trigonal bipyramidal geometry. XeF2 has a linear shape. XeOF2 is T - Shaped. XeO2F2 is see-saw shaped. Earlier we had seen that the geometry of XeF4 has a square bipyramidal geometry and square planar shape: In the above geometry, if we replace a lone pair with an Oxygen atom such that there is a double bond between Xe and O, then we get the geometry of XeOF4. The four F atoms line in a plane perpendicular to the Xe – O axial sigma bond. This geometry is still the same as XeF4 but the shape will be square pyramidal! So correct options are a c and d

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