Question:

Which of the following is not isostructural with \(\text{SiCl}_4\) ?

Updated On: Oct 13, 2023
  • \(\text{SCl}_4\)
  • \(\text{SO}^{2-}_4\)
  • \(\text{PO}^{3-}_4\)
  • \(\text{NH}^+_4\)
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The Correct Option is A

Solution and Explanation

\(\text{SiCl}_4\) adopts a tetrahedral structure due to the four chlorine atoms arranged symmetrically around the silicon atom. On the other hand, \(\text{SCl}_4\)features four chlorine atoms and an additional lone pair on sulfur, causing it to assume a see-saw molecular geometry. The remaining molecules in the list maintain a tetrahedral geometry. Therefore, \(\text{SCl}_4\) does not share the same structural arrangement as \(\text{SiCl}_4\).

So, the correct option is (A): \(\text{SCl}_4\)

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Concepts Used:

P-Block Elements

  • P block elements are those in which the last electron enters any of the three p-orbitals of their respective shells. Since a p-subshell has three degenerate p-orbitals each of which can accommodate two electrons, therefore in all there are six groups of p-block elements.
  • P block elements are shiny and usually a good conductor of electricity and heat as they have a tendency to lose an electron. You will find some amazing properties of elements in a P-block element like gallium. It’s a metal that can melt in the palm of your hand. Silicon is also one of the most important metalloids of the p-block group as it is an important component of glass.

P block elements consist of: