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Chapter 16: Problem 79

Use Lewis structures to diagram the following reaction in the manner of reaction (16.20) $$\mathrm{H}_{2} \mathrm{O}+\mathrm{SO}_{2} \longrightarrow \mathrm{H}_{2} \mathrm{SO}_{3}$$ Identify the Lewis acid and Lewis base.

Short Answer

Expert verified
In the given reaction \(H_2O + SO_2 \longrightarrow H_2SO_3\), \(SO_2\) is the Lewis acid because it accepts an electron pair, and \(H_2O\) is the Lewis base because it donates an electron pair.

Step by step solution

01

Draw Lewis Structures

Draw the Lewis structures for the reactants, which include water \(H_2O\) and sulfur dioxide \(SO_2\), and the product, which is sulphurous acid \(H_2SO_3\). In water, oxygen shares one electron with each hydrogen, forming 2 bonds, and has 4 non-bonding electrons. In sulfur dioxide, sulfur shares 2 electrons with each oxygen, forming 2 double bonds and has 2 non-bonding electrons. In the sulphurous acid molecule, sulfur shares 2 electrons with one oxygen (double bond) and one with each other atom (single bonds), and has 2 non-bonding electrons.
02

Identify the Lewis Acid and Base

A Lewis acid is a substance that can accept an electron pair, while a Lewis base is a substance that can donate an electron pair. In this reaction, \(H_2O\) is the Lewis base as it donates an electron pair to \(SO_2\), which acts as the Lewis acid by accepting the pair of electrons, forming \(H_2SO_3\).
03

Finalize Reaction Diagram and Check

Finalize your Lewis structures and check to make sure that all atoms obey the octet rule (with up to 8 electrons in their valence shell), and that the overall charges of the reactants and products are balanced. In this case, all the molecules are neutral, so our reaction does not involve any ions.

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Most popular questions from this chapter

The molecular solid \(\mathrm{I}_{2}(\mathrm{s})\) is only slightly soluble in water but will dissolve to a much greater extent in an aqueous solution of \(\mathrm{KI}\), because the \(\mathrm{I}_{3}^{-}\) anion forms. Write an equation for the formation of the \(I_{3}^{-}\) anion, and indicate the Lewis acid and Lewis base.

Complete the following equations in those instances in which a reaction (hydrolysis) will occur. If no reaction occurs, so state. (a) \(\mathrm{NH}_{4}^{+}(\mathrm{aq})+\mathrm{NO}_{3}^{-}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O} \longrightarrow\) (b) \(\mathrm{Na}^{+}(\mathrm{aq})+\mathrm{NO}_{2}^{-}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O} \longrightarrow\) (c) \(\mathrm{K}^{+}(\mathrm{aq})+\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{COO}^{-}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O} \longrightarrow\) (d) \(\mathrm{K}^{+}(\mathrm{aq})+\mathrm{Cl}^{-}(\mathrm{aq})+\mathrm{Na}^{+}(\mathrm{aq})+\mathrm{I}^{-}(\mathrm{aq})+\) (e) \(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{NH}_{3}^{+}(\mathrm{aq})+\mathrm{Cl}^{-}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O} \longrightarrow \mathrm{H}_{2} \mathrm{O} \longrightarrow\)

With which of the following bases will the ionization of acetic acid, \(\mathrm{CH}_{3} \mathrm{COOH},\) proceed furthest toward completion (to the right): (a) \(\mathrm{H}_{2} \mathrm{O} ;\) (b) \(\mathrm{NH}_{3} ;\) (c) \(\mathrm{Cl}^{-}\) (d) \(\mathrm{NO}_{3}^{-} ?\) Explain your answer.

The following four equilibria lie to the right: \(\mathrm{N}_{2} \mathrm{H}_{5}^{+}+\) \(\mathrm{CH}_{3} \mathrm{NH}_{2} \longrightarrow \mathrm{N}_{2} \mathrm{H}_{4}+\mathrm{CH}_{3} \mathrm{NH}_{3}^{+} ; \mathrm{H}_{2} \mathrm{SO}_{3}+\mathrm{F}^{-} \longrightarrow\) \(\mathrm{HSO}_{3}^{-}+\mathrm{HF} ; \mathrm{CH}_{3} \mathrm{NH}_{3}^{+}+\mathrm{OH}^{-} \longrightarrow \mathrm{CH}_{3} \mathrm{NH}_{2}+\) \(\mathrm{H}_{2} \mathrm{O} ;\) and \(\mathrm{HF}+\mathrm{N}_{2} \mathrm{H}_{4} \longrightarrow \mathrm{F}^{-}+\mathrm{N}_{2} \mathrm{H}_{5}^{+}\) (a) Rank all the acids involved in order of decreasing acid strength. (b) Rank all the bases involved in order of decreasing base strength. (c) State whether each of the following two equilibria lies primarily to the right or to the left: (i) \(\mathrm{HF}+\mathrm{OH}^{-} \longrightarrow \mathrm{F}^{-}+\mathrm{H}_{2} \mathrm{O} ;\) (ii) \(\mathrm{CH}_{3} \mathrm{NH}_{3}^{+}+\) \(\mathrm{HSO}_{3}^{-} \longrightarrow \mathrm{CH}_{3} \mathrm{NH}_{2}+\mathrm{H}_{2} \mathrm{SO}_{3}\).

One handbook lists a value of 9.5 for \(\mathrm{p} \mathrm{K}_{\mathrm{b}}\) of quinoline, \(\mathrm{C}_{9} \mathrm{H}_{7} \mathrm{N},\) a weak base used as a preservative for anatomical specimens and to make dyes. Another handbook lists the solubility of quinoline in water at \(25^{\circ} \mathrm{C}\) as \(0.6 \mathrm{g} / 100 \mathrm{mL} .\) Use this information to calculate the \(\mathrm{pH}\) of a saturated solution of quinoline in water.
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