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Chapter 10: Problem 58

Describe the carbon-to-sulfur bond in \(\mathrm{H}_{2} \mathrm{CSF}_{4}\). That is, is it most likely a single, double, or triple bond?

Short Answer

Expert verified
The carbon-to-sulfur bond in \(H_2 CSF_4\) is a single bond.

Step by step solution

01

Identify the total number of valence electrons

Carbon has 4 valence electrons, sulfur has 6, fluorine has 7, and hydrogen has 1. Since there are 1 carbon, 1 sulfur, 4 fluorines, and 2 hydrogens in the compound, we multiply these with their respective valence electrons. So, total valence electrons are \(1*4 (C) + 1*6 (S) + 4*7 (F) + 2*1 (H) = 38 valence electrons.
02

Draw the preliminary Lewis Structure

Sketch the molecule by placing the atoms, putting the least electronegative atom in the center, which is usually the one that can form the most number of bonds. In this case, Carbon is the least electronegative. Hence, Carbon is at the center, surrounded by Sulfur and 2 Hydrogens, and the Sulphur is further surrounded by 4 Fluorines.
03

Distribute initial electrons

Add the valence electrons. First add the number of electrons required to fill the outer shells of the Hydrogen and Fluorine atoms. For each Hydrogen, we add 1 electron and for each Fluorine we add 7 electrons. This will give a preliminary structure of the molecule.
04

Adjust electrons and determine the bond

We have already used \(2*1 (for H) + 4*7 (for F) = 30 electrons\). We're left with 8 electrons. Using these, complete the octets of Carbon and Sulphur. Post this, observe the bond structure between Sulphur and Carbon. Since Sulphur shares two electrons with Carbon which counts as one single bond, the answer is a single bond. As there are left over electrons on sulfur, it has a lone pair as well.

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Most popular questions from this chapter

Hydrogen azide, \(\mathrm{HN}_{3}\), can exist in two forms. One form has the three nitrogen atoms connected in a line; and the nitrogen atoms form a triangle in the other. Construct Lewis structures for these isomers and describe their shapes. Other interesting derivatives are nitrosyl azide ( \(\mathrm{N}_{4} \mathrm{O}\) ) and trifluoromethyl azide \(\left(\mathrm{CF}_{3} \mathrm{N}_{3}\right) .\) Describe the shapes of these molecules based on a line of nitrogen atoms.

The species \(\mathrm{PBr}_{4}^{-}\) has been synthesized and has been described as a tetrahedral anion. Comment on this description.

Use the VSEPR theory to predict the shape of (a) the molecule OSF \(_{2} ;\) (b) the molecule \(\mathrm{O}_{2} \mathrm{SF}_{2} ;\) (c) the ion \(\mathrm{SF}_{5}^{-} ;\) (d) the ion \(\mathrm{ClO}_{4}^{-} ;\) (e) the ion \(\mathrm{ClO}_{3}^{-}\).

Sketch the propene molecule, \(\mathrm{CH}_{3} \mathrm{CH}=\mathrm{CH}_{2}\). Indicate the bond angles in this molecule. What is the maximum number of atoms that can be in the same plane?

Draw Lewis structures for the following species, indicating formal charges and resonance where applicable: (a) \(\mathrm{HCO}_{2}=\) (b) \(\mathrm{HCO}_{3}^{-}\) (c) \(\mathrm{FSO}_{3}^{-}\) (d) \(\mathrm{N}_{2} \mathrm{O}_{3}^{2-}\) (the nitrogen atoms are joined centrally with one oxygen atom on one \(\mathrm{N}\) and two on the other)
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