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Chapter 18: Q48E (page 1043)

Determine the oxidation state of sulfur in each of the following:

(a) \(S{O_3}\)

(b) \(S{O_2}\)

(c) \(SO_3^{2 - }\)

Short Answer

Expert verified

(a) For \({\rm{S}}{{\rm{O}}_3}\), the oxidation number of oxygen is\( - 2\)and for sulfur is\( + 6\).

(b) For \({\rm{S}}{{\rm{O}}_2}\), the oxidation number of oxygen is\( - 2\)and for sulfur is\( + 4\).

(c) For \({\rm{SO}}_3^{2 - }\), the oxidation number of oxygen is\( - 2\)and for sulfur is\( + 4\).

Step by step solution

01

Definition of oxidation state

An oxidation state is classified as a hypothetical charge. It is evaluated by adding the total electrons that are either gained or lost by anatom during bond formation. For a neutral compound, the addition of all oxidation states is zero.

02

Oxidation state of sulfur in each element

In the compounds \({\rm{S}}{{\rm{O}}_3}\) and \({\rm{S}}{{\rm{O}}_2}\), the total sum of the oxidation numbers is zero, while in \({\rm{SO}}_3^{2 - }\), the total sum is \( - 2\).

(a) In \({\rm{S}}{{\rm{O}}_3}\), the oxidation number of oxygen is\( - 2\), so the oxidation number of sulfur is\( + 6\).

(b) In \({\rm{S}}{{\rm{O}}_2}\) the oxidation number of oxygen is\( - 2\), while the oxidation number of sulfur is\( + 4\).

(c) In \({\rm{SO}}_3^{2 - }\) the oxidation number of oxygen is\( - 2\), while the oxidation number of sulfur is\( + 4\).

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Most popular questions from this chapter

A mixture of Xenon and Flourine was heated. A sample of white solid that formed reacted with hydrogen to yield 81 mL of Xenon (at STP) and hydrogen fluoride , which was collected in water, giving a solution of hydrofluoric acid . The hydrofluoric acid solution was titrated , and 68.43 mL of 0.3172 M of Sodium Hydroxide was required to reach the equivalence point. Determine the empirical formula for the white solid and write balanced chemical equations for the reactions involving xenon .

Write balanced chemical equations for the following reactions:

(a) metallic aluminum burned in air

(b) elemental aluminum heated in an atmosphere of chlorine

(c) aluminum heated in hydrogen bromide gas

(d) aluminum hydroxide added to a solution of nitric acid

What is the oxidation state of the halogen in each of the following?

\(\begin{array}{l}(a){{\rm{H}}_5}{\rm{I}}{{\rm{O}}_6}\\(b){\rm{IO}}_4^ - \\(c){\rm{Cl}}{{\rm{O}}_2}\\(d){\rm{IC}}{{\rm{l}}_3}\\(e){F_2}\end{array}\)

Give the hybridization of the metalloid and the molecular geometry for each of the following compounds or ions. You may wish to review the chapters on chemical bonding and advanced covalent bonding for relevant examples.

\((a){\rm{Ge}}{{\rm{H}}_4}\)

\((b){\rm{Sb}}{{\rm{F}}_3}\)

\((c){\rm{Te}}{({\rm{OH}})_6}\)

\((d){{\rm{H}}_2}{\rm{Te}}\)

\((e){\rm{Ge}}{{\rm{F}}_2}\)

\((f){\rm{TeC}}{{\rm{l}}_4}\)

\((g){\rm{SiF}}_6^{2 - }\)

\((h){\rm{SbC}}{{\rm{l}}_5}\)

\((i){\rm{Te}}{{\rm{F}}_6}\)

How many tons of \(C{a_3}{\left( {P{O_4}} \right)_2}\)are necessary to prepare 5.0 tons of phosphorus if the yield is 90 % ?
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