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[tex]$MnCl_2$[/tex], [tex]$MnO_2$[/tex], [tex]$Mn_2O_3$[/tex], and [tex]$Mn_2O_7$[/tex] are different compounds of manganese. Complete Table 1.17 by writing the oxidation state of manganese in each of these and also the subshell electronic configuration of each.

\begin{tabular}{|c|c|c|}
\hline
Compound & \begin{tabular}{c}
Oxidation state \\
of [tex]$Mn$[/tex]
\end{tabular} & \begin{tabular}{c}
Subshell electronic \\
configuration of [tex]$Mn$[/tex] ions
\end{tabular} \\
\hline
[tex]$MnCl_2$[/tex] & +2 & [tex]$[Ar] 3d^5$[/tex] \\
[tex]$MnO_2$[/tex] & +4 & - \\
[tex]$Mn_2O_3$[/tex] & +3 & - \\
[tex]$Mn_2O_7$[/tex] & +7 & - \\
\hline
\end{tabular}

Table 1.17

Sagot :

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To complete Table 1.17 with the oxidation state and subshell electronic configuration of manganese in each given compound, we need to fill in the missing information based on the oxidation states and configurations of manganese in these compounds. Here is the detailed step-by-step solution:

Compound: [tex]\( MnCl_2 \)[/tex]
1. Oxidation state of Mn: In [tex]\( MnCl_2 \)[/tex], manganese has an oxidation state of [tex]\( +2 \)[/tex].
2. Subshell electronic configuration of [tex]\( Mn^{2+} \)[/tex]: The configuration is [tex]\( 1s^2 2s^2 2p^6 3s^2 3p^6 3d^5 \)[/tex].

Compound: [tex]\( MnO_2 \)[/tex]
1. Oxidation state of Mn: In [tex]\( MnO_2 \)[/tex], manganese has an oxidation state of [tex]\( +4 \)[/tex].
2. Subshell electronic configuration of [tex]\( Mn^{4+} \)[/tex]: The configuration is [tex]\( 1s^2 2s^2 2p^6 3s^2 3p^6 3d^3 \)[/tex].

Compound: [tex]\( Mn_2O_3 \)[/tex]
1. Oxidation state of Mn: In [tex]\( Mn_2O_3 \)[/tex], manganese has an oxidation state of [tex]\( +3 \)[/tex].
2. Subshell electronic configuration of [tex]\( Mn^{3+} \)[/tex]: The configuration is [tex]\( 1s^2 2s^2 2p^6 3s^2 3p^6 3d^4 \)[/tex].

Compound: [tex]\( Mn_2O_7 \)[/tex]
1. Oxidation state of Mn: In [tex]\( Mn_2O_7 \)[/tex], manganese has an oxidation state of [tex]\( +7 \)[/tex].
2. Subshell electronic configuration of [tex]\( Mn^{7+} \)[/tex]: The configuration is [tex]\( 1s^2 2s^2 2p^6 3s^2 3p^6 \)[/tex].

Given these details, we can fill in the table accordingly:

[tex]\[ \begin{array}{|c|c|c|} \hline \text{Compound} & \begin{array}{c} \text{Oxidation state} \\ \text{of} ~ \text{Mn} \end{array} & \begin{array}{c} \text{Subshell electronic} \\ \text{configuration of Mn ions} \end{array} \\ \hline \text{$MnCl_2$} & +2 & 1s^2 2s^2 2p^6 3s^2 3p^6 3d^5 \\ \text{$MnO_2$} & +4 & 1s^2 2s^2 2p^6 3s^2 3p^6 3d^3 \\ \text{$Mn_2O_3$} & +3 & 1s^2 2s^2 2p^6 3s^2 3p^6 3d^4 \\ \text{$Mn_2O_7$} & +7 & 1s^2 2s^2 2p^6 3s^2 3p^6 \\ \hline \end{array} \][/tex]

This completes Table 1.17 with the oxidation states and subshell electronic configurations of manganese in each compound.
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