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Chapter 22: Problem 74

Explain why \(\mathrm{SCl}_{6}, \mathrm{SBr}_{6},\) and \(\mathrm{SI}_{6}\) cannot be prepared.

Short Answer

Expert verified
Despite sulfur's ability to expand its octet, it cannot form SCl₆, SBr₆, or SI₆ due to the larger atomic sizes of Cl, Br, and I. These larger halogens cannot approach sulfur closely enough to form stable molecules like SF₆, resulting in excessive electron-electron repulsion that prevents the formation of these molecules.

Step by step solution

01

- Concept of Octet Rule and Expanded Octet

The octet rule is a simple chemical guideline which states that atoms tend to combine in such a way that they each have eight electrons in their valence shells, giving them the same electronic configuration as a noble gas. However, certain elements in the 3rd period and beyond like sulfur, phosphorus, silicon etc., can expand their valence shell to include more than 8 electrons. This phenomenon is known as the expanded octet.
02

- Understand the Elements Involved

The elements in question here are sulfur (S) and the halogens - chlorine (Cl), bromine (Br), and iodine (I). Sulfur belongs to the 16th group, and it has 6 valence electrons, while the halogens have 7. Due to available d orbitals, sulfur can incorporate more than 8 electrons in its valence shell.
03

- Reasoning for Non-Existence of SCl₆, SBr₆, and SI₆

Although sulfur can expand its octet to form SF₆, it cannot form SCl₆, SBr₆, or SI₆. This can be attributed to the larger sizes of chlorine, bromine, and iodine compared to fluorine. The larger atomic radii of Cl, Br, or I do not allow them to approach sulfur closely enough to form stable SF₆-like species. Because of these increased atomic sizes and their resultant shielding effects, the electron-electron repulsion in the hypothetical SCl₆, SBr₆, and SI₆ molecules would be too high to allow these molecules to exist.

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