Xe has a complete filled 5p configuration. As a result when it undergoes bonding with an odd number (3 or 5) of F atoms it leaves behind one unpaired electron. This causes the molecule to become unstable. As a result XeF3 and XeF5 do not exist.
Hence option C is correct answer.
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Similar Questions
Q1
How are xenon fluorides XeF2,XeF4 and XeF6 obtained?
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Q2
Oxidising power of xenon fluorides increases in the order:
XeF6>XeF4>XeF2
If true enter 1, else enter 0.
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Q3
SbF5 reacts with XeF4 and XeF6 to form ionic compounds [XeF+3][SbF6]−and[XeF+5][SbF−6]. The geometry of XeF+3 ion and XeF+5 ion, respectively, is :
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Q4
In XeF2,XeF4andXeF5, the number of lone pairs of Xe is respectively:
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Q5
What is the product formed when XeF4 reacts with SbF5?