Discussion
Which one of the following molecule/ion has square planar shape?
Answer: E
The square planar species is \(\mathrm{XeF_{4}}\).
Xenon in \(\mathrm{XeF_{4}}\) has 4 bond pairs and 2 lone pairs, six electron pairs in all, arranged octahedrally. The two lone pairs occupy opposite (trans) positions to keep apart, leaving the four fluorines at the corners of a square in one plane.
\(\mathrm{SF_{4}}\) has 4 bond pairs and 1 lone pair, which gives a see-saw shape. \(\mathrm{NH_{4}^{+}}\), \(\mathrm{CH_{4}}\) and \(\mathrm{CH_{2}Cl_{2}}\) each have four bond pairs and no lone pair on the central atom, so all three are tetrahedral.
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