/*! This file is auto-generated */ .wp-block-button__link{color:#fff;background-color:#32373c;border-radius:9999px;box-shadow:none;text-decoration:none;padding:calc(.667em + 2px) calc(1.333em + 2px);font-size:1.125em}.wp-block-file__button{background:#32373c;color:#fff;text-decoration:none} Problem 58 Explain why aluminum, magnesium,... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 23: Problem 58

Explain why aluminum, magnesium, and sodium metals are obtained by electrolysis instead of by reduction with chemical reducing agents.

Short Answer

Expert verified
Aluminum, magnesium, and sodium metals are obtained by electrolysis instead of by reduction with chemical reducing agents due to their high reactivity and position in the reactivity series. Their strong affinity for oxygen makes direct reduction with chemical reducing agents difficult. Electrolysis allows for the extraction of these metals in a pure form from their respective compounds, such as aluminum from bauxite, magnesium from magnesite or seawater, and sodium from sodium chloride.

Step by step solution

01

Understanding the reactivity series

The reactivity series is a ranking of metals in order of their reactivity, with very reactive metals at the top and less reactive metals at the bottom. It is an essential concept in chemistry and helps us understand which extraction methods are suitable for different metals. Metals above hydrogen in the reactivity series are typically extracted by electrolysis, while metals below hydrogen are extracted by reduction using chemical reducing agents.
02

Discussing the properties of aluminum

Aluminum is a highly reactive metal and is found in the Earth's crust as an ore called bauxite. The bauxite ore contains aluminum oxide (Al2O3), which needs to be extracted and purified to obtain aluminum metal. Aluminum has a high affinity for oxygen, making it difficult to reduce directly with a chemical reducing agent like carbon. Therefore, aluminum is extracted through electrolysis, specifically the Hall-H茅roult process, which allows for the extraction of pure aluminum metal from its oxide.
03

Discussing the properties of magnesium

Magnesium is another highly reactive metal. Magnesium is commonly found as an ore called magnesite (MgCO3) or in seawater as magnesium chloride (MgCl2). Similar to aluminum, magnesium has a strong affinity for oxygen and is not easily reduced by chemical reducing agents. Magnesium is produced using electrolysis, specifically the Dow Process or the electrolysis of magnesium chloride from seawater. The electrolysis process allows for the extraction of pure magnesium metal from its compound.
04

Discussing the properties of sodium

Sodium is a very reactive metal and is usually found in the form of sodium chloride (NaCl), which is the main component of table salt. As a highly reactive metal, sodium cannot be easily reduced by chemical reducing agents. Instead, sodium is extracted using electrolysis in a process known as the Down's Process. In this process, molten sodium chloride is electrolysed to produce sodium metal and chlorine gas. This allows for the extraction of pure sodium metal from its compound.
05

Conclusion

In summary, aluminum, magnesium, and sodium metals are obtained by electrolysis instead of by reduction with chemical reducing agents due to their high reactivity and position in the reactivity series. These metals have a strong affinity for oxygen, which makes direct reduction with chemical reducing agents difficult. Electrolysis allows for the extraction of these metals in a pure form from their respective compounds.

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Over 30 million students worldwide already upgrade their learning with 91影视!

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

What role does each of the following materials play in the chemical processes that occur in a blast furnace: (a) air, (b) limestone, (c) coke (d) water? Write balanced chemical equations to illustrate your answers.

Indicate whether each of the following compounds is expected to be diamagnetic or paramagnetic, and give a reason for your answer in each case: (a) \(\mathrm{NbCl}_{5}\), (b) \(\mathrm{CrCl}_{2}\), (c) \(\mathrm{CuCl}\), (d) \(\mathrm{RuO}_{4}\), (e) \(\mathrm{NiCl}_{2}\).

Based on the chemistry described in this chapter and others, propose balanced chemical equations for the following sequence of reactions involving nickel: (a) The ore millerite, which contains NiS, is roasted in an atmosphere of oxygen to produce an oxide. (b) The oxide is reduced to the metal, using coke. (c) Dissolving the metal in hydrochloric acid produces a green solution. (d) Adding excess sodium hydroxide to the solution causes a gelatinous green material to precipitate. (e) Upon heating, the green material loses water and yields a green powder.

(a) On the atomic level, what distinguishes ferromagnetic, ferrimagnetic, and antiferromagnetic materials from each other? (b) Which one of these types of magnetic materials cannot be used to make a permanent magnet?

(a) Pyrolusite \(\left(\mathrm{MnO}_{2}\right)\) is a commercially important mineral of manganese. What is the oxidation state of \(\mathrm{Mn}\) in this metal? (b) Name some reagents that might be used to reduce this ore to the metal.
See all solutions

Recommended explanations on Chemistry Textbooks

Nuclear Chemistry

Read Explanation

Physical Chemistry

Read Explanation

Kinetics

Read Explanation

Ionic and Molecular Compounds

Read Explanation

Inorganic Chemistry

Read Explanation

The Earths Atmosphere

Read Explanation
View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.