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Chapter 23: Problem 12

By means of a chemical equation, give an example to represent the reaction of (a) a transition metal with a nonoxidizing acid; (b) a transition metal oxide with \(\mathrm{NaOH}(\mathrm{aq}) ;(\mathrm{c})\) an inner transition metal with \(\mathrm{HCl}(\mathrm{aq})\).

Short Answer

Expert verified
The chemical equations are: (a) \(Fe(s) + H_2SO_4(aq) \rightarrow FeSO_4(aq) + H_2(g)\), (b) \(Fe_2O_3(s) + 6NaOH(aq) \rightarrow 2Na_3[Fe(OH)_6](aq)\), and (c) \(La(s) + 2HCl(aq) \rightarrow LaCl_2(aq) + H_2(g)\).

Step by step solution

01

Transition metal with a nonoxidizing acid

(a) When a transition metal, say iron (\(Fe\)), reacts with a nonoxidizing acid like sulfuric acid (\(H_2SO_4\)), it forms a corresponding salt and hydrogen gas. The balanced chemical equation for this is: \[Fe(s) + H_2SO_4(aq) \rightarrow FeSO_4(aq) + H_2(g)\]
02

Transition metal oxide with NaOH

(b) A transition metal oxide, such as iron(III) oxide (\(Fe_2O_3\)), reacts with sodium hydroxide (\(NaOH\)) to produce a complex salt and water. The balanced chemical equation for this reaction is: \[Fe_2O_3(s) + 6NaOH(aq) \rightarrow 2Na_3[Fe(OH)_6](aq)\]
03

Inner transition metal with HCl

(c) When an inner transition metal like lanthanum (\(La\)) reacts with hydrochloric acid (\(HCl\)), it forms a corresponding salt and hydrogen gas. The balanced chemical equation for this reaction is: \[La(s) + 2HCl(aq) \rightarrow LaCl_2(aq) + H_2(g)\]

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Most popular questions from this chapter

All of the following elements have an ion displaying the +6 oxidation state except (a) Mo; (b) Cr; (c) Mn; (d) \(\mathrm{V} ;\) (e) S.

Calcium will reduce \(\mathrm{MgO}(\mathrm{s})\) to \(\mathrm{Mg}(\mathrm{s})\) at all temperatures from 0 to \(2000^{\circ} \mathrm{C}\). Use this fact, together with the melting point ( \(839^{\circ} \mathrm{C}\) ) and boiling point \(\left(1484^{\circ} \mathrm{C}\right)\) of calcium, to sketch a plausible graph of \(\Delta G^{\circ}\) as a function of temperature for the reaction \(2 \mathrm{Ca}(\mathrm{s})+\) \(\mathrm{O}_{2}(\mathrm{g}) \longrightarrow 2 \mathrm{CaO}(\mathrm{s})\).

Attempts to make \(\mathrm{CuI}_{2}\) by the reaction of \(\mathrm{Cu}^{2+}(\mathrm{aq})\) and \(\mathrm{I}^{-}(\text {aq })\) produce \(\mathrm{CuI}(\mathrm{s})\) and \(\mathrm{I}_{3}^{-}(\mathrm{aq})\) instead. Without performing detailed calculations, show why this reaction should occur. $$2 \mathrm{Cu}^{2+}(\mathrm{aq})+5 \mathrm{I}^{-}(\mathrm{aq}) \longrightarrow 2 \mathrm{CuI}(\mathrm{s})+\mathrm{I}_{3}^{-}(\mathrm{aq})$$

Describe how the transition elements compare with main-group metals (such as group 2 ) with respect to oxidation states, formation of complexes, colors of compounds, and magnetic properties.

Describe the chemical composition of the material called (a) pig iron; (b) ferromanganese alloy; (c) chromite ore; (d) brass; (e) aqua regia; (f) blister copper; (g) stainless steel.
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