Chapter 20.1, Problem 8LC

(a)

Interpretation Introduction

Interpretation: The oxidized and reduced species in the given reaction, $2Na\left(s\right)+B{r}_2\left(l\right)\to 2NaBr\left(s\right)$ is to be found out using electron transfer or electron shift method.

Concept Introduction: The chemical reaction in which the electrons move from one species to other is defined as an electron transfer reaction. Redox reaction is also called a type of electron transfer reaction. Electron transfer reactions always contain oxidation and reduction since for gaining electrons there must be something to lose electrons.

Answer to Problem 8LC

The chemical species that oxidized is $Na$ and that is reduced is $B{r}_2$ .

Explanation of Solution

Redox reactions involve oxidation and reduction processes. The chemical species that involves the loss of an electron or removal of the electron is said to be oxidized and the corresponding reaction is oxidation. While the chemical species that involves the gain of electrons or the acceptance of electrons is said to be reduced and the corresponding reaction is reduction.

In the given reaction,

  $2Na\left(s\right)+B{r}_2\left(l\right)\to 2NaBr\left(s\right)$

The compound $NaBr$ contains sodium, $N{a}^{+}$ , and bromide, $B{r}^{-}$ ions. The electron transfer reaction taking place here is,

  $Na\left(s\right)\to N{a}^{+}\left(g\right)+e^{-}$

  $B{r}_2\left(I\right)+2e^{-}\to 2B{r}^{-}\left(g\right)$

Here, sodium is removing one electron from it. While $B{r}_2$ is accepting the removed electrons. Therefore the species that undergo oxidation is $Na$ and that undergo reduction is $B{r}_2$ .

(b)

Interpretation Introduction

Interpretation: The oxidized and reduced species in the given reaction, $H_2\left(g\right)+C{l}_2\left(g\right)\to 2HCl\left(g\right)$ is to be found out using electron transfer or electron shift method.

Concept Introduction: The chemical reaction in which the electrons move from one species to other is defined as an electron transfer reaction. Redox reaction is also called a type of electron transfer reaction. Electron transfer reactions always contain oxidation and reduction since for gaining electrons there must be something to lose electrons.

Answer to Problem 8LC

The chemical species that oxidized is $H_2$ and that is reduced is $C{l}_2$ .

Explanation of Solution

Redox reactions involve oxidation and reduction processes. The chemical species that involves the loss of an electron or removal of the electron is said to be oxidized and the corresponding reaction is oxidation. While the chemical species that involves the gain of electrons or the acceptance of electrons is said to be reduced and the corresponding reaction is reduction.

In the given reaction,

  $H_2\left(g\right)+C{l}_2\left(g\right)\to 2HCl\left(g\right)$

The electron transfer reaction taking place here is,

  $H_2\left(g\right)\to 2H^{+}\left(g\right)+2e^{-}$

  $C{l}_2\left(g\right)+2e^{-}\to 2C{l}^{-}$

Here, dihydrogen, $H_2$ is removing the electron from it. While $C{l}_2$ is accepting the removed electrons. Therefore the species that undergo oxidation is $C{l}_2$ and that undergo reduction is $C{l}_2$ .

(c)

Interpretation Introduction

Interpretation: The oxidized and reduced species in the given reaction, $2Li\left(s\right)+F_2\left(g\right)\to 2LiF\left(s\right)$ is to be found out using electron transfer or electron shift method.

Concept Introduction: The chemical reaction in which the electrons move from one species to other is defined as an electron transfer reaction. Redox reaction is also called a type of electron transfer reaction. Electron transfer reactions always contain oxidation and reduction since for gaining electrons there must be something to lose electrons.

Answer to Problem 8LC

The chemical species that oxidized is $Li$ and that is reduced is $F_2$ .

Explanation of Solution

Redox reactions involve oxidation and reduction processes. The chemical species that involves the loss of an electron or removal of the electron is said to be oxidized and the corresponding reaction is oxidation. While the chemical species that involves the gain of electrons or the acceptance of electrons is said to be reduced and the corresponding reaction is reduction.

In the given reaction,

  $2Li\left(s\right)+F_2\left(g\right)\to 2LiF\left(s\right)$

  $2Li\left(s\right)\to 2L{i}^{+}\left(g\right)+e^{-}$

  $F_2\left(g\right)+2e^{-}\to 2F^{-}$

Here, lithium is removing one electron from it. While $F_2$ is accepting the removed electrons. Therefore, the species that undergo oxidation is $Li$ and those that undergo reduction is $F_2$ .

(d)

Interpretation Introduction

Interpretation: The oxidized and reduced species in the given reaction, $S\left(s\right)+C{l}_2\left(g\right)\to SC{l}_2\left(g\right)$ is to be found out using electron transfer or electron shift method.

Concept Introduction: The chemical reaction in which the electrons move from one species to other is defined as an electron transfer reaction. Redox reaction is also called a type of electron transfer reaction. Electron transfer reactions always contain oxidation and reduction since for gaining electrons there must be something to lose electrons.

Answer to Problem 8LC

The chemical species that oxidized is sulfur and that is reduced is $C{l}_2$ .

Explanation of Solution

Redox reactions involve oxidation and reduction processes. The chemical species that involves the loss of an electron or removal of the electron is said to be oxidized and the corresponding reaction is oxidation. While the chemical species that involves the gain of electrons or the acceptance of electrons is said to be reduced and the corresponding reaction is reduction.

In the given reaction,

  $S\left(s\right)+C{l}_2\left(g\right)\to SC{l}_2\left(g\right)$

The electron transfer reaction taking place here is,

  $S\left(s\right)\to S_2{}^{+}\left(g\right)+2e^{-}$

  $C{l}_2\left(g\right)+2e^{-}\to 2C{l}^{-}$

Here, sulfur, $S$ is removing electrons from it. While $C{l}_2$ is accepting the removed electrons. Therefore the species that undergo oxidation is $S$ and those that undergo reduction is $C{l}_2$ .

(e)

Interpretation Introduction

Interpretation: The oxidized and reduced species in the given reaction, $N_2\left(g\right)+2O_2\left(g\right)\to 2N{O}_2\left(g\right)$ is to be found out using electron transfer or electron shift method.

Concept Introduction: The chemical reaction in which the electrons move from one species to other is defined as an electron transfer reaction. Redox reaction is also called a type of electron transfer reaction. Electron transfer reactions always contain oxidation and reduction since for gaining electrons there must be something to lose electrons.

Answer to Problem 8LC

The chemical species that oxidized is $N_2$ and that is reduced is $O_2$ .

Explanation of Solution

Redox reactions involve oxidation and reduction processes. The chemical species that involves the loss of an electron or removal of the electron is said to be oxidized and the corresponding reaction is oxidation. While the chemical species that involves the gain of electrons or the acceptance of electrons is said to be reduced and the corresponding reaction is reduction.

In the given reaction,

  $N_2\left(g\right)+2O_2\left(g\right)\to 2N{O}_2\left(g\right)$

The electron transfer reaction taking place here is,

  $N_2\to 2N_2{}^{+}\left(g\right)+2e^{-}$

  $O_2\left(g\right)+2e^{-}\to 2O^{-}$

Here, dinitrogen, $N_2$ is removing electrons from it. While $O_2$ is accepting the removed electrons. Therefore the species that undergo oxidation is $N_2$ and that undergo reduction are $O_2$ .

(f)

Interpretation Introduction

Interpretation: The oxidized and reduced species in the given reaction, $Mg\left(s\right)+Cu{\left(N{O}_3\right)}_2\left(aq\right)\to Mg{\left(N{O}_3\right)}_2\left(aq\right)+Cu\left(s\right)$ is to be found out using electron transfer or electron shift method.

Concept Introduction: The chemical reaction in which the electrons move from one species to other is defined as an electron transfer reaction. Redox reaction is also called a type of electron transfer reaction. Electron transfer reactions always contain oxidation and reduction since for gaining electrons there must be something to lose electrons.

Answer to Problem 8LC

The chemical species that oxidized is $Mg$ and that is reduced is $C{u}^{2+}$ .

Explanation of Solution

Redox reactions involve oxidation and reduction processes. The chemical species that involves the loss of an electron or removal of the electron is said to be oxidized and the corresponding reaction is oxidation. While the chemical species that involves the gain of electrons or the acceptance of electrons is said to be reduced and the corresponding reaction is reduction.

In the given reaction,

  $Mg\left(s\right)+Cu{\left(N{O}_3\right)}_2\left(aq\right)\to Mg{\left(N{O}_3\right)}_2\left(aq\right)+Cu\left(s\right)$

The electron transfer reaction taking place here is,

  $mg\to M{g}^{2+}\left(g\right)+2e^{-}$

  $C{u}^{2+}+2e^{-}\to 2Cu$

Here, magnesium, $Mg$ is removing electrons from it. While $C{u}^{2+}$ is accepting the removed electrons. Therefore the species that undergo oxidation is $Mg$ and those that undergo reduction is $C{u}^{2+}$ .