Warning: foreach() argument must be of type array|object, bool given in /var/www/html/web/app/themes/studypress-core-theme/template-parts/header/mobile-offcanvas.php on line 20

Magnesium reacts with acids producing hydrogen and corresponding magnesium salts. In sueh reactions, magnesium undergoes (1) Oxidation (2) Reduction (3) Neither oxidation nor reduction (4) Simple dissolution

Short Answer

Expert verified
Oxidation

Step by step solution

01

- Understand the Reaction

Magnesium reacts with acids to produce hydrogen gas and magnesium salts. This is a redox (oxidation-reduction) reaction.
02

- Determine Oxidation State of Magnesium Before Reaction

In its elemental form, magnesium (Mg) has an oxidation state of 0.
03

- Determine Oxidation State of Magnesium After Reaction

In the reaction with an acid, magnesium forms magnesium salts. For instance, when magnesium reacts with hydrochloric acid (HCl), it forms magnesium chloride (MgCl₂). In MgCl₂, magnesium has an oxidation state of +2.
04

- Identify Change in Oxidation State

Since magnesium's oxidation state changes from 0 to +2, it loses electrons during the reaction.
05

- Conclude the Type of Reaction

Losing electrons corresponds to oxidation. Therefore, in this reaction, magnesium undergoes oxidation.

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 Vaia!

Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Oxidation States
Oxidation states are used to keep track of electron transfers in chemical reactions. They indicate the degree of oxidation of an atom in a compound. The oxidation state of an element in its pure form is always zero. However, when elements form compounds, their oxidation states change.
For example, pure magnesium (Mg) has an oxidation state of 0 because it is not combined with any other element. When magnesium reacts with hydrochloric acid (HCl) to form magnesium chloride (MgCl₂), the oxidation state of magnesium changes. After the reaction, magnesium exists as Mg²⁺, meaning its oxidation state has risen to +2.
Understanding changes in oxidation states is crucial as it helps us identify which elements are oxidized and which are reduced in redox reactions.
Magnesium Reaction with Acids
When magnesium reacts with acids, it typically produces hydrogen gas and magnesium salts. Here's a common reaction with hydrochloric acid (HCl):
\[ \text{Mg} + 2 \text{HCl} \rightarrow \text{MgCl}_2 + \text{H}_2 \]
In this reaction, magnesium (Mg) reacts with hydrochloric acid (HCl) to produce magnesium chloride (MgCl₂) and hydrogen gas (H₂).
Before the reaction, magnesium is in its elemental form (Mg) with an oxidation state of 0. During the reaction, magnesium loses two electrons and forms Mg²⁺ with an oxidation state of +2.
At the same time, hydrogen ions (H⁺) from the acid gain electrons to form hydrogen gas (H₂). This simultaneous oxidation and reduction process defines a redox reaction.
  • Magnesium is oxidized (loses electrons).
  • Hydrogen ions are reduced (gain electrons).
Understanding the specific steps helps to comprehend how magnesium transforms during the reaction with acids.
Electron Transfer
Electron transfer is fundamental to redox reactions. An atom's loss of electrons is called oxidation, while the gain of electrons is called reduction. These two processes occur together in a redox reaction.
In our magnesium reaction example, magnesium atoms lose electrons (are oxidized) when they react with hydrochloric acid, forming Mg²⁺ ions. These lost electrons are gained by hydrogen ions (H⁺) from the acid, converting them into hydrogen gas (H₂).
The steps of electron transfer are:
  • Magnesium atoms (Mg) lose two electrons, forming Mg²⁺ ions.
  • These electrons are gained by hydrogen ions (H⁺) from the acid.
  • The hydrogen ions (H⁺) are reduced to form hydrogen gas (H₂).
Understanding electron transfer helps explain the changes in oxidation states and provides a clearer picture of the redox process in a chemical reaction.
Redox reactions, including electron transfers, are crucial in many chemical processes, from biological systems to industrial applications. Recognizing how electrons move in reactions helps students grasp the fundamental nature of chemical changes.

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

Which of the following cquations is balanced? (1) \(5 \mathrm{BiO}_{3}+2 \mathrm{H}^{+}+\mathrm{Mn}^{2+} \longrightarrow 5 \mathrm{Bi}^{3+}+12 \mathrm{H}_{2} \mathrm{O}+\) \(\mathrm{MnO}_{4}^{-}\) (2) \(5 \mathrm{BiO}_{3}+14 \mathrm{H}^{+}+2 \mathrm{Mn}^{2+} \longrightarrow 5 \mathrm{Bi}^{3+}+7 \mathrm{H}_{2} \mathrm{O}+\) \(2 \mathrm{MnO}_{4}^{-}\) (3) \(2 \mathrm{BiO}_{3}+4 \mathrm{H}^{\prime}+\mathrm{Mn}^{21} \longrightarrow 2 \mathrm{Bi}^{31}+2 \mathrm{H}_{2} \mathrm{O}\) \(+\mathrm{MnO}_{4}\) (4) \(6 \mathrm{BiO}_{3}+12 \mathrm{II}+3 \mathrm{Mn}^{21} \longrightarrow 6 \mathrm{Bi}^{3}+6 \mathrm{II}_{2} \mathrm{O}\) \(+3 \mathrm{MnO}_{4}^{-}\)

Every redox reaction is made up of \(\ldots . .\) that which involves gain in clectrons is called ...... (1) Reduction half-reaction, two half-rcactions (2) Oxidation half-rcaction, two half-reactions (3) Two half-reactions, oxidation reaction (4) Two half-reactions, reduction reaction

\(2 \mathrm{KClO}_{3}+\mathrm{I}_{2} \rightarrow 2 \mathrm{~K} 1 \mathrm{O}_{3}+\mathrm{Cl}_{2}\) Which of the following statements is correct regarding the above reaction? (1) It is a simple displaccment but not a redox reaction (2) Chlorine is reduced by iodine (3) Chlorinc is oxidiscd by iodine (4) It is a metathesis reaction

A metal having negative reduction potential when dipped in the solution of its own jons has a tendency to (1) To pass into solution (2) To be deposited from the solution (3) To become clectrically positive (4) To remain neutral

Standard reduction potential of an clement is cqual to (1) \(+\mathrm{l} \times\) its reduction potential (2) \(-1 \times\) its standard oxidation potential (3) \(0.00\) (4) \(+\mathrm{l} \times\) its standard oxidation potential

See all solutions

Recommended explanations on Chemistry Textbooks

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.

Sign-up for free