Which of the following is not isostructural with \(\text{SiCl}_4\) ?
- \(\text{SCl}_4\)
- \(\text{SO}^{2-}_4\)
- \(\text{PO}^{3-}_4\)
- \(\text{NH}^+_4\)
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:
- Group 13 Elements: Boron family
- Group 14 Elements: Carbon family
- Group 15 Elements: Nitrogen family
- Group 16 Elements: Oxygen family
- Group 17 Elements: Fluorine family
- Group 18 Elements: Neon family