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Chapter 10: Problem 103

A compound consists of \(47.5 \%\) S and \(52.5 \%\) Cl, by mass. Write a Lewis structure based on the empirical formula of this compound, and comment on its deficiencies. Write a more plausible structure with the same ratio of \(\mathrm{S}\) to \(\mathrm{Cl}\).

Short Answer

Expert verified
The empirical formula for the compound is SCl but the molecule is inadequately represented by this as Sulphur only has 7 electrons. A more plausible Lewis structure of the compound would be SCl2 where Sulphur (S) shares an electron with each Chlorine (Cl) atom, forming single bonds. This structure adheres to the octet rule.

Step by step solution

01

Determine the Empirical Formula

As there are no absolute masses provided, it can be deducted that 100 g of the compound is being referred to. This would mean there are \(47.5 g\) of Sulphur and \(52.5 g\) of Chlorine. By dividing these masses with their respective atomic weights (\(32.07 g / mol\) for Sulphur and \(35.45 g / mol\) for Chlorine), the number of moles for each can be found. Hence, the number of moles of Sulphur is \((47.5/32.07) = 1.48\) and Chlorine is \((52.5/35.45) = 1.48\). Therefore, the empirical formula of the compound is SCl.
02

Draw the Lewis Structure Based on the Empirical Formula

Using the empirical formula, a Lewis structure can be drawn. Sulphur is in the center as it is less electronegative. According to its valence electrons, Sulphur (S) has 6 electrons while Chlorine (Cl) has 7. An electron from Sulphur can be shared with Chlorine forming a single bond between them. In this structure, Chlorine will have an octet of electrons but Sulphur will only have 7.
03

Commenting on the deficiences

The produced Lewis structure has Sulphur (S) with only 7 electrons which does not follow the octet rule. Therefore, this structure does not accurately represent the correct geometry of the molecule.
04

Provide a Plausible Lewis Structure

To form a structure where each atom adheres to the octet rule, a second compound of Chlorine should be added. Sulphur can share one of its remaining electrons with another Chlorine atom forming another bond. So, the new Lewis structure will consist of Sulphur single bonded with two Chlorine atoms, making the molecule SCl2.

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Most popular questions from this chapter

Without referring to tables or figures in the text other than the periodic table, indicate which of the following atoms, \(\mathrm{Bi}, \mathrm{S}, \mathrm{Ba}, \mathrm{As},\) or \(\mathrm{Mg},\) has the intermediate value when they are arranged in order of increasing electronegativity.

Construct a concept map illustrating the connections between Lewis dot structures, the shapes of molecules, and polarity.

Comment on the similarities and differences in the molecular structure of the following four-atom species: \(\mathrm{NO}_{3}^{-}, \mathrm{CO}_{3}^{2-}, \mathrm{SO}_{3}^{2-},\) and \(\mathrm{ClO}_{3}^{-}\).

Use VSEPR theory to predict the geometric shapes of the following molecules and ions: (a) \(\mathrm{PCl}_{3} ;\) (b) \(\mathrm{SO}_{4}^{2-}\); (c) \(\mathrm{SOCl}_{2} ;\) (d) \(\mathrm{SO}_{3} ;\) (e) \(\mathrm{BrF}_{4}^{+}\).

Write Lewis symbols for the following atoms. (a) \(\mathrm{Kr}\); (b) Ge; (c) \(\mathrm{N} ;\) (d) Ga; (e) As; (f) Rb.
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