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Chapter 21: Problem 20

Almost all metals in nature are found as ionic compounds in ores instead of being in the pure state. Why? What must be done to a sample of ore to obtain a metal substance that has desirable properties?

Short Answer

Expert verified
Metals are mostly found as ionic compounds in ores due to their reactive nature, forming stable compounds with elements like oxygen, sulfur, and carbon. To obtain a metal substance with desirable properties, a sample of ore undergoes smelting, which involves heating the ore in the presence of a reducing agent to extract the pure metal. Additional steps like refining, alloying, and forming may be used to enhance the properties of the pure metal substance to tailor it for specific applications.

Step by step solution

01

Understand the nature of metals

Most metals are found as ionic compounds in ores because they are reactive and readily form stable compounds with other elements. In nature, they combine with oxygen, sulfur, carbon or other elements to create various minerals. For example, iron exists in the form of iron oxide like hematite (Fe2O3) and magnetite (Fe3O4), and copper appears as copper sulfides such as chalcopyrite (CuFeS2) and covellite (CuS).
02

Recognize the purpose of extracting metal from ores

The goal when extracting metals from ores is to obtain a pure metal substance with desirable properties for industrial and commercial applications. These properties include high electrical and thermal conductivity, ductility, malleability, and resistance to corrosion.
03

Extracting metals using smelting

One common process to extract metals from ores is smelting. Smelting involves heating the ore in a furnace in the presence of a reducing agent (usually carbon in the form of coke or charcoal) to reduce the metal oxide/sulfide to its elemental form. This reduction process removes oxygen/sulfur from the metal and produces pure metal and waste slag. For example, in the case of iron, the following reactions take place during the smelting process: \[ Fe2O3(s) + 3CO(g) \rightarrow \ 2Fe(l) + 3CO2(g) \]
04

Obtain the desired metal properties

Once the metal is extracted, additional steps like refining, alloying, and forming may be used to enhance the properties of the pure metal substance. These processes are designed to minimize impurities, change the metal structure, and tailor its properties for specific applications. For example, steel, which is an alloy of iron and carbon, is produced by controlling the amount of carbon in the iron and adding other elements like chromium, nickel, and manganese to impart specific properties like strength and corrosion resistance.

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Most popular questions from this chapter

Which of the following molecules exhibit(s) optical isomerism? a. \(c i s-P t\left(\mathrm{NH}_{3}\right)_{2} \mathrm{Cl}_{2}\) b. trans-Ni(en) \(_{2} \mathrm{Br}_{2}\) (en is ethylenediamine) c. \(c i s-\mathrm{Ni}(\mathrm{en})_{2} \mathrm{Br}_{2}(\text { en is ethylenediamine })\)

Name the following complex ions. a. \(\operatorname{Ru}\left(\mathrm{NH}_{3}\right)_{5} \mathrm{Cl}^{2+}\) b. \(\mathrm{Fe}(\mathrm{CN})_{6}^{4-}\) c. \(\mathrm{Mn}\left(\mathrm{NH}_{2} \mathrm{CH}_{2} \mathrm{CH}_{2} \mathrm{NH}_{2}\right)_{3}^{2+}\) d. \(\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{55} \mathrm{NO}_{2}^{2+}\) e. \(\mathrm{Ni}(\mathrm{CN})_{4}^{2-}\) f. \(\mathrm{Cr}\left(\mathrm{NH}_{3}\right)_{4} \mathrm{Cl}_{2}^{+}\) g. \(\mathrm{Fe}\left(\mathrm{C}_{2} \mathrm{O}_{4}\right)_{3}^{3-}\) h. \(\mathrm{Co}(\mathrm{SCN})_{2}\left(\mathrm{H}_{2} \mathrm{O}\right)_{4}^{+}\)

Ammonia and potassium iodide solutions are added to an aqueous solution of \(\mathrm{Cr}\left(\mathrm{NO}_{3}\right)_{3} .\) A solid is isolated (compound A), and the following data are collected: i. When 0.105 g of compound A was strongly heated in excess \(\mathrm{O}_{2}, 0.0203 \mathrm{g} \mathrm{CrO}_{3}\) was formed. ii. In a second experiment it took 32.93 \(\mathrm{mL}\) of 0.100\(M \mathrm{HCl}\) to titrate completely the \(\mathrm{NH}_{3}\) present in \(0.341 \mathrm{g} \mathrm{com}-\) pound A. iii. Compound A was found to contain 73.53\(\%\) iodine by mass. iv. The freezing point of water was lowered by \(0.64^{\circ} \mathrm{C}\) when 0.601 \(\mathrm{g}\) compound A was dissolved in 10.00 \(\mathrm{g} \mathrm{H}_{2} \mathrm{O}\left(K_{\mathrm{f}}=\right.\) \(1.86^{\circ} \mathrm{C} \cdot \mathrm{kg} / \mathrm{mol} )\) What is the formula of the compound? What is the structure of the complex ion present? (Hints: \(\mathrm{Cr}^{3+}\) is expected to be six-coordinate, with \(\mathrm{NH}_{3}\) and possibly I- - as ligands. The I- ions will be the counterions if needed.)

Would it be better to use octahedral \(\mathrm{Ni}^{2+}\) complexes or octahe- dral \(\mathrm{Cr}^{2+}\) complexes to determine whether a given ligand is a strong-field or weak-field ligand by measuring the number of unpaired electrons? How else could the relative ligand field strengths be determined?

Compounds of \(\mathrm{Sc}^{3+}\) are not colored, but those of \(\mathrm{Ti}^{3+}\) and \(\mathrm{V}^{3+}\) are. Why?
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