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Which of the pair is linear in shape and with three lone pairs?

$\begin{array}{1 1}(a)\;CO_2, SO_2&(b)\; XeF_2, SCl_2\\(c)\; HgCl_2, BeF_2&(d). XeF_2, I_3^-\end{array}$

1 Answer

$XeF_2, I_3^-$
In $XeF_2$,the central Xe-atom is surrounded by five electron pairs.Out of the five electron pairs,two are bond pairs and three are lone pairs.Five electron pairs form trigonal bipyramoidal shape with three lone pairs occupied in equotorial positions.Due to the presence of three lone pairs,$XeF_2$ molecule assumes linear shape with F–Xe–F bond angle equal to $180^{\circ}$
The ion is linear and symmetrical. According to VSEPR theory, the central iodine atom has three equatorial lone pairs, and the terminal iodines are bonded axially in a linear fashion, due to the three lone pairs bonding to the central iodine-atom.
Hence (d) is the correct option.
answered Dec 9, 2013 by sreemathi.v
edited Nov 18, 2017 by sharmaaparna1

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