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Chapter 10: Problem 63

Predict the geometry of sulfur dichloride \(\left(\mathrm{SCl}_{2}\right)\) and the hybridization of the sulfur atom.

Short Answer

Expert verified
The geometry of sulfur dichloride \(\mathrm{SCl}_{2}\) is bent shape or V-shaped and the hybridization of the sulfur atom is sp3.

Step by step solution

01

Determine Valence Electrons and draw the Electron Dot Structure

Sulfur has 6 valence electrons, and each Chlorine atom has 7 valence electrons. So, for \(\mathrm{SCl}_{2}\), the total number of valence electrons is \(6 + 2*7 = 20\). The Lewis dot structure can be drawn with Sulfur at the center (as it is less electronegative) and a Chlorine atom on each side, each bonded to the sulfur by a single bond, and the remaining 4 electrons placed as lone pairs on the sulfur atom.
02

Determine the Electron Pair Geometry and Molecular Geometry

The sulfur atom is surrounded by 4 regions of electron density, including 2 single bond pairs and 2 lone pairs. These 4 pairs try to position themselves as far apart as possible to minimize repulsion. Hence, the electron-pair geometry is tetrahedral. However, the molecular geometry is determined by the positions of the atoms only, which forms a V-shape or bent shape.
03

Determine the Hybridization

The hybridization of the atom can be determined from the electron pair geometry. In this case, with 4 regions of electron density around the sulfur atom, the sulfur atom is sp3 hybridized.

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Most popular questions from this chapter

Which of these species are tetrahedral? \(\mathrm{SiCl}_{4}, \mathrm{SeF}_{4}\) \(\mathrm{XeF}_{4}, \mathrm{CI}_{4}, \mathrm{CdCl}_{4}^{2-}\)

What hybrid orbitals are used by nitrogen atoms in these species? (a) \(\mathrm{NH}_{3},\) (b) \(\mathrm{H}_{2} \mathrm{~N}-\mathrm{NH}_{2}\) (c) \(\mathrm{NO}_{3}^{-}\)

What is the angle between these two hybrid orbitals on the same atom? (a) \(s p\) and \(s p\) hybrid orbitals, (b) \(s p^{2}\) and \(s p^{2}\) hybrid orbitals, (c) \(s p^{3}\) and \(s p^{3}\) hybrid orbitals.

Draw the Lewis structure for the \(\mathrm{BeCl}_{4}^{2-}\) ion. Predict its geometry and describe the hybridization state of the Be atom.

Draw the Lewis structure of mercury(II) bromide. Is this molecule linear or bent? How would you establish its geometry?
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