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Chapter 5: Problem 26

Why are most metals found in nature as ores and not as pure metals?

Short Answer

Expert verified
Most metals are found as ores and not in their pure forms in nature because metals are generally reactive and under natural environmental conditions, they react with other elements like oxygen and sulfur to form more stable compounds, which we refer to as ores. This not only prevents their degradation, but also makes them economically feasible for extraction.

Step by step solution

01

Understanding ores

An ore is a natural source of mineral from which metals are extracted economically. The extraction typically involves processing, such as access, concentration, and reduction of metal compounds into desirable form.
02

Explain metal reactivity

Metals in their pure form tend to be highly reactive to oxygen, moisture, carbon dioxide, and other elements in the environment such as sulfur, thereby easily getting oxidized or corroded. Hence, they generally do not occur in nature in their native state except for gold, silver, platinum which are least reactive.
03

Description of metal-ore formation

During geological processes, while metals are exposed to different environmental elements, they react and form compounds. These compounds, compacted with soil, rocks and other organic compounds, are what is commonly referred to as ores.
04

Explain stability of metals

Minerals with metal elements in ore form are stable in earth’s surface environment, which makes ores’ formation more favourable. The metals' natural tendency to bond with other elements, forming more stable compounds, is a natural defense mechanism to prevent degradation and loss.

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Most popular questions from this chapter

Complete the table below, and then use it to answer the questions that follow. \begin{equation} \begin{array}{l}{\text { Write the formula for the following }} \\ {\text { substances: }} \\ {\text { a. manganese chloride }} \\ {\text { b. chromium(III) fluoride }} \\ {\text { c. barium oxide }}\end{array} \end{equation}

Identify and name the cations and anions that make up the following ionic compounds and indicate the charge on each ion. \begin{equation} \begin{array}{ll}{\text { a. } \mathrm{NaNO}_{3}} & {\text { c. }\left(\mathrm{NH}_{4}\right)_{2} \mathrm{CrO}_{4}} \\ {\text { b. } \mathrm{K}_{2} \mathrm{SO}_{3}} & {\text { d. } \mathrm{Al}_{2}\left(\mathrm{SO}_{4}\right)_{3}}\end{array} \end{equation}

Why can't an ionic bond form between potassium and magnesium?

Why is lattice energy the key to forming an ionic bond?

Explain why the properties of an ion differ from its parent atom.
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