What happens to the oxidation number of one of its elements when a compound is oxidized and when it is reduced, must be explained. Concept Introduction: One of the ways to define oxidation and reduction involves gain or loss of electrons by elements during the reaction. Here, Oxidation is loss of electrons. Reduction is gain of electrons. For example, the reaction of magnesium with chlorine shown below: Mg ( s ) + 2 HCl ( g ) → MgCl 2 ( aq ) + H 2 ( g ) Here, the oxidation state of magnesium in Mg(s) is zero and that in MgCl 2 is 2+, thus, oxidation of Mg to Mg 2 + results in increase in oxidation state. Similarly, the oxidation state of hydrogen in HCl is +1 and that in H 2 is zero, reduction of hydrogen from HCl to H 2 results in decrease in oxidation state.

Question

Want to see more full solutions like this?

Answer 1

Question

Chapter 8, Problem 1RQ

Interpretation Introduction

Interpretation:

What happens to the oxidation number of one of its elements when a compound is oxidized and when it is reduced, must be explained.

Concept Introduction:

One of the ways to define oxidation and reduction involves gain or loss of electrons by elements during the reaction.

Here,

Oxidation is loss of electrons.

Reduction is gain of electrons.

For example, the reaction of magnesium with chlorine shown below:

Mg(s)+2HCl(g)→MgCl2(aq)+H2(g)

Here, the oxidation state of magnesium in Mg(s) is zero and that in MgCl₂ is 2+, thus, oxidation of Mg to Mg²+ results in increase in oxidation state. Similarly, the oxidation state of hydrogen in HCl is +1 and that in H₂ is zero, reduction of hydrogen from HCl to H₂ results in decrease in oxidation state.

Expert Solution & Answer

Answer to Problem 1RQ

Solution:

Oxidation number of one of its elements is increased when a compound is oxidized.

Oxidation number of one of its elements is decreased when a compound is reduced.

Explanation of Solution

Oxidation number is defined as the charge present on a simple ion or atom.

In any reaction, reduction results due to gain of electron, if an atom or ion gain electrons it gets negative charge, or its negative charge increases. Thus, oxidation state of that atom decreases. Similarly, oxidation results due to loss of electron, if an atom or ion lose electrons it gets positive charge, or its positive charge increases.

Conclusion

Thus, oxidation number is increased during oxidation and it is decreased during reduction.

Want to see more full solutions like this?

Subscribe now to access step-by-step solutions to millions of textbook problems written by subject matter experts!

Students have asked these similar questions

eks.com/aleksogi/x/sl.exe/1o_u-IgNslkr7j8P3jH-IQs_pBanHhvTCeeBZbufuBYTI0Hz7m7D3ZS17Hd6m-HIl6n52njJN-TXdQA2X9yID-1SWQJTgnjARg30 111 States of Matter Understanding conceptual components of the enthalpy of solution 0/5 Ge A small amount of acetonitrile (CH, CN) is dissolved in a large amount of water. Imagine separating this process into the four stages sketched below. (These sketches show only a portion of the substances, so you can see the density and distribution of atoms and molecules in them.) CH,CN H₂O B 88 C Use these sketches to answer the questions in the table below. The enthalpy of solution AH is negative soln when CH3CN dissolves in water. Use this information to list the stages in order of increasing enthalpy. Would heat be absorbed or released if the system moved from Stage C to D? What force would oppose or favor the system moving from Stage C to D? Check all that apply. 1 absorbed O released neither absorbed nor released. none O ionic bonding force covalent bonding force…

In a system with an anodic overpotential, the variation of ŋ as a function of the current density: 1. at low fields is linear 2. at higher fields, it follows Tafel's law Find the range of current densities for which the overpotential has the same value as when calculated for cases 1 and 2 (maximum relative difference of 5% with respect to the behavior for higher fields). To which overpotential range does this correspond? Data: 10 = 1.5 mA cm², T = 300°C, ẞ = 0.64, R = 8.314 J K 1 mol‍¹ and F = 96485 C mol-1.

Indicate 10.6 with only one significant figure.

Answer 2

Question

Chapter 8, Problem 1RQ

Interpretation Introduction

Interpretation:

What happens to the oxidation number of one of its elements when a compound is oxidized and when it is reduced, must be explained.

Concept Introduction:

One of the ways to define oxidation and reduction involves gain or loss of electrons by elements during the reaction.

Here,

Oxidation is loss of electrons.

Reduction is gain of electrons.

For example, the reaction of magnesium with chlorine shown below:

Mg(s)+2HCl(g)→MgCl2(aq)+H2(g)

Here, the oxidation state of magnesium in Mg(s) is zero and that in MgCl₂ is 2+, thus, oxidation of Mg to Mg²+ results in increase in oxidation state. Similarly, the oxidation state of hydrogen in HCl is +1 and that in H₂ is zero, reduction of hydrogen from HCl to H₂ results in decrease in oxidation state.

Expert Solution & Answer

Answer to Problem 1RQ

Solution:

Oxidation number of one of its elements is increased when a compound is oxidized.

Oxidation number of one of its elements is decreased when a compound is reduced.

Explanation of Solution

Oxidation number is defined as the charge present on a simple ion or atom.

In any reaction, reduction results due to gain of electron, if an atom or ion gain electrons it gets negative charge, or its negative charge increases. Thus, oxidation state of that atom decreases. Similarly, oxidation results due to loss of electron, if an atom or ion lose electrons it gets positive charge, or its positive charge increases.

Conclusion

Thus, oxidation number is increased during oxidation and it is decreased during reduction.

Want to see more full solutions like this?

Subscribe now to access step-by-step solutions to millions of textbook problems written by subject matter experts!

Answer 3

Question

Chapter 8, Problem 1RQ

Interpretation Introduction

Interpretation:

What happens to the oxidation number of one of its elements when a compound is oxidized and when it is reduced, must be explained.

Concept Introduction:

One of the ways to define oxidation and reduction involves gain or loss of electrons by elements during the reaction.

Here,

Oxidation is loss of electrons.

Reduction is gain of electrons.

For example, the reaction of magnesium with chlorine shown below:

Mg(s)+2HCl(g)→MgCl2(aq)+H2(g)

Here, the oxidation state of magnesium in Mg(s) is zero and that in MgCl₂ is 2+, thus, oxidation of Mg to Mg²+ results in increase in oxidation state. Similarly, the oxidation state of hydrogen in HCl is +1 and that in H₂ is zero, reduction of hydrogen from HCl to H₂ results in decrease in oxidation state.

Expert Solution & Answer

Answer to Problem 1RQ

Solution:

Oxidation number of one of its elements is increased when a compound is oxidized.

Oxidation number of one of its elements is decreased when a compound is reduced.

Explanation of Solution

Oxidation number is defined as the charge present on a simple ion or atom.

In any reaction, reduction results due to gain of electron, if an atom or ion gain electrons it gets negative charge, or its negative charge increases. Thus, oxidation state of that atom decreases. Similarly, oxidation results due to loss of electron, if an atom or ion lose electrons it gets positive charge, or its positive charge increases.

Conclusion

Thus, oxidation number is increased during oxidation and it is decreased during reduction.

Want to see more full solutions like this?

Subscribe now to access step-by-step solutions to millions of textbook problems written by subject matter experts!

Answer 4

Question

Chapter 8, Problem 1RQ

Interpretation Introduction

Interpretation:

What happens to the oxidation number of one of its elements when a compound is oxidized and when it is reduced, must be explained.

Concept Introduction:

One of the ways to define oxidation and reduction involves gain or loss of electrons by elements during the reaction.

Here,

Oxidation is loss of electrons.

Reduction is gain of electrons.

For example, the reaction of magnesium with chlorine shown below:

Mg(s)+2HCl(g)→MgCl2(aq)+H2(g)

Here, the oxidation state of magnesium in Mg(s) is zero and that in MgCl₂ is 2+, thus, oxidation of Mg to Mg²+ results in increase in oxidation state. Similarly, the oxidation state of hydrogen in HCl is +1 and that in H₂ is zero, reduction of hydrogen from HCl to H₂ results in decrease in oxidation state.

Expert Solution & Answer

Answer to Problem 1RQ

Solution:

Oxidation number of one of its elements is increased when a compound is oxidized.

Oxidation number of one of its elements is decreased when a compound is reduced.

Explanation of Solution

Oxidation number is defined as the charge present on a simple ion or atom.

In any reaction, reduction results due to gain of electron, if an atom or ion gain electrons it gets negative charge, or its negative charge increases. Thus, oxidation state of that atom decreases. Similarly, oxidation results due to loss of electron, if an atom or ion lose electrons it gets positive charge, or its positive charge increases.

Conclusion

Thus, oxidation number is increased during oxidation and it is decreased during reduction.

Want to see more full solutions like this?

Subscribe now to access step-by-step solutions to millions of textbook problems written by subject matter experts!

Answer 5

Chapter 8, Problem 1RQ

Interpretation Introduction

Interpretation:

What happens to the oxidation number of one of its elements when a compound is oxidized and when it is reduced, must be explained.

Concept Introduction:

One of the ways to define oxidation and reduction involves gain or loss of electrons by elements during the reaction.

Here,

Oxidation is loss of electrons.

Reduction is gain of electrons.

For example, the reaction of magnesium with chlorine shown below:

Mg(s)+2HCl(g)→MgCl2(aq)+H2(g)

Here, the oxidation state of magnesium in Mg(s) is zero and that in MgCl₂ is 2+, thus, oxidation of Mg to Mg²+ results in increase in oxidation state. Similarly, the oxidation state of hydrogen in HCl is +1 and that in H₂ is zero, reduction of hydrogen from HCl to H₂ results in decrease in oxidation state.

Expert Solution & Answer

Answer to Problem 1RQ

Solution:

Oxidation number of one of its elements is increased when a compound is oxidized.

Oxidation number of one of its elements is decreased when a compound is reduced.

Explanation of Solution

Oxidation number is defined as the charge present on a simple ion or atom.

In any reaction, reduction results due to gain of electron, if an atom or ion gain electrons it gets negative charge, or its negative charge increases. Thus, oxidation state of that atom decreases. Similarly, oxidation results due to loss of electron, if an atom or ion lose electrons it gets positive charge, or its positive charge increases.

Conclusion

Thus, oxidation number is increased during oxidation and it is decreased during reduction.

Answer 6

Chapter 8, Problem 1RQ

Interpretation Introduction

Interpretation:

What happens to the oxidation number of one of its elements when a compound is oxidized and when it is reduced, must be explained.

Concept Introduction:

One of the ways to define oxidation and reduction involves gain or loss of electrons by elements during the reaction.

Here,

Oxidation is loss of electrons.

Reduction is gain of electrons.

For example, the reaction of magnesium with chlorine shown below:

Mg(s)+2HCl(g)→MgCl2(aq)+H2(g)

Here, the oxidation state of magnesium in Mg(s) is zero and that in MgCl₂ is 2+, thus, oxidation of Mg to Mg²+ results in increase in oxidation state. Similarly, the oxidation state of hydrogen in HCl is +1 and that in H₂ is zero, reduction of hydrogen from HCl to H₂ results in decrease in oxidation state.

Expert Solution & Answer

Answer to Problem 1RQ

Solution:

Oxidation number of one of its elements is increased when a compound is oxidized.

Oxidation number of one of its elements is decreased when a compound is reduced.

Explanation of Solution

Oxidation number is defined as the charge present on a simple ion or atom.

In any reaction, reduction results due to gain of electron, if an atom or ion gain electrons it gets negative charge, or its negative charge increases. Thus, oxidation state of that atom decreases. Similarly, oxidation results due to loss of electron, if an atom or ion lose electrons it gets positive charge, or its positive charge increases.

Conclusion

Thus, oxidation number is increased during oxidation and it is decreased during reduction.

Answer 7

Chapter 8, Problem 1RQ

Interpretation Introduction

Interpretation:

What happens to the oxidation number of one of its elements when a compound is oxidized and when it is reduced, must be explained.

Concept Introduction:

One of the ways to define oxidation and reduction involves gain or loss of electrons by elements during the reaction.

Here,

Oxidation is loss of electrons.

Reduction is gain of electrons.

For example, the reaction of magnesium with chlorine shown below:

Mg(s)+2HCl(g)→MgCl2(aq)+H2(g)

Here, the oxidation state of magnesium in Mg(s) is zero and that in MgCl₂ is 2+, thus, oxidation of Mg to Mg²+ results in increase in oxidation state. Similarly, the oxidation state of hydrogen in HCl is +1 and that in H₂ is zero, reduction of hydrogen from HCl to H₂ results in decrease in oxidation state.

Answer 8

Expert Solution & Answer

Answer to Problem 1RQ

Solution:

Oxidation number of one of its elements is increased when a compound is oxidized.

Oxidation number of one of its elements is decreased when a compound is reduced.

Answer 9

Expert Solution & Answer

Answer 10

Expert Solution & Answer

Answer 11

Explanation of Solution

Oxidation number is defined as the charge present on a simple ion or atom.

In any reaction, reduction results due to gain of electron, if an atom or ion gain electrons it gets negative charge, or its negative charge increases. Thus, oxidation state of that atom decreases. Similarly, oxidation results due to loss of electron, if an atom or ion lose electrons it gets positive charge, or its positive charge increases.