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Chapter 10: Problem 77

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 (SCl2) is bent or V-shaped, and the sulfur atom is sp3 hybridized.

Step by step solution

01

Determine the Total Number of Valence Electrons

Sulfur (S) is in Group 6 and so has 6 valence electrons. Chlorine (Cl), being in Group 7, has 7 valence electrons. Therefore, in \( \mathrm{SCl}_{2} \), there are a total of \((1 \times 6) + (2 \times 7) = 20\) valence electrons.
02

Determinte The Lewis Structure

Assign S as the central atom. The Lewis structure will show that sulfur forms single bonds with the two chlorine atoms, with two pairs of nonbonding electrons left on the sulfur atom. This uses up 8 out of 20 available electrons, as each bond uses two electrons. The remaining 12 electrons are then allocated to the Cl atoms, six to each (in accordance with the octet rule), completing the Lewis structure.
03

Predict the Geometry Using VSEPR Theory

The sulfur atom in \( \mathrm{SCl}_{2} \) is surrounded by two bond pairs and two lone pairs. According to the VSEPR theory, the repulsion between lone pairs and bond pairs of electrons around the central atom will cause these groups to arrange themselves as far apart as possible. This arrangement results in a bent or V-shaped molecular geometry.
04

Determine the Hybridization

The sulfur atom is surrounded by four groups of electrons: two single bonds and two lone pairs. According to the theory of hybridization, this configuration corresponds to sp3 hybridization. So, the sulfur atom in \( \mathrm{SCl}_{2} \) is sp3 hybridized.

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Most popular questions from this chapter

The geometries discussed in this chapter all lend themselves to fairly straightforward elucidation of bond angles. The exception is the tetrahedron, because its bond angles are hard to visualize. Consider the \(\mathrm{CCl}_{4}\) molecule, which has a tetrahedral geometry and is nonpolar. By equating the bond moment of a particular \(\mathrm{C}-\mathrm{Cl}\) bond to the resultant bond \(\mathrm{mo}-\) ments of the other three \(\mathrm{C}-\mathrm{Cl}\) bonds in opposite directions, show that the bond angles are all equal to \(109.5^{\circ}\)

Predict the geometry of the following molecules and ion using the VSEPR model: (a) \(\mathrm{CBr}_{4},\) (b) \(\mathrm{BCl}_{3}\) (c) \(\mathrm{NF}_{3}\), (d) \(\mathrm{H}_{2} \mathrm{Se},\) (e) \(\mathrm{NO}_{2}^{-}\).

What are the hybrid orbitals of the carbon atoms in the following molecules? (a) \(\mathrm{H}_{3} \mathrm{C}-\mathrm{CH}_{3}\) (b) \(\mathrm{H}_{3} \mathrm{C}-\mathrm{CH}=\mathrm{CH}_{2}\) (c) \(\mathrm{CH}_{3}-\mathrm{C} \equiv \mathrm{C}-\mathrm{CH}_{2} \mathrm{OH}\) (d) \(\mathrm{CH}_{3} \mathrm{CH}=\mathrm{O}\) (e) \(\mathrm{CH}_{3} \mathrm{COOH}\)

For each pair listed here, state which one has a higher first ionization energy and explain your choice: (a) \(\mathrm{H}\) or \(\mathrm{H}_{2},\) (b) \(\mathrm{N}\) or \(\mathrm{N}_{2},\) (c) \(\mathrm{O}\) or \(\mathrm{O}_{2},\) (d) \(\mathrm{F}\) or \(\mathrm{F}_{2}\).

Predict the geometries of the following species: (a) \(\mathrm{AlCl}_{3},\) (b) \(\mathrm{ZnCl}_{2}\), (c) \(\mathrm{ZnCl}_{4}^{2-}\).
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