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The pairs of species of oxygen and their magnetic behaviours are noted below. Which of the following presents the correct description?
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Verified Answer
The correct answer is:
$\mathrm{O}_2^{+}, \mathrm{O}_2$ - Both paramagnetic
The molecular orbital configurations of $\mathrm{O}_2^{+}, \mathrm{O}_2^{-}, \mathrm{O}_2^{2-}$ and $\mathrm{O}_2$ are
$$
\begin{aligned}
& \mathrm{O}_2^{+}=\sigma 1 s^2, \sigma 1 s^2, \sigma 2 s^2, \sigma 2 s^2, \sigma 2 p_z^2, \pi 2 p_x^2 \approx \pi 2 p_y^2, \\
& \pi 2 p_x^1 \approx \pi 2 p_y^0 \\
& \mathrm{O}_2^{-}=\sigma 1 s^2, \sigma \cdot \% 1 s^2, \sigma 2 s^2, \sigma 2 s^2, \sigma 2 p_z^2, \pi 2 p_x^2 \\
& \approx \pi 2 p_y^2, \pi 2 p_x^2 \approx \pi 2 p_y^1 \\
& \mathrm{O}_2^{2-}=\sigma 1 s^2, \sigma \cdot s^2, \sigma 2 s^2, \sigma 2 s^2, \sigma 2 p_z^2, \pi 2 p_x^2 \\
& \approx \pi 2 p_y^2, \pi 2 p_x^2 \approx \pi 2 p_y^2 . \\
& \mathrm{O}_2=\sigma 1 s^2, \sigma 1 s^2, \sigma 2 s^2, \sigma^* 2 s^2, \sigma 2 p_z^2, \pi 2 p_x^2 \\
& \approx \pi 2 p_y^2, \pi 2 p_x^1 \approx \pi 2 p_y^1
\end{aligned}
$$
And the electronic configuration of $\mathrm{O}$ and $\mathrm{O}^{+}$ are
$$
\begin{array}{r}
\mathrm{O}=1 s^2, 2 s^2, 2 p_x^2, 2 p_y^1, 2 p_z^1 \\
\mathrm{O}^{+}=1 s^2, 2 s^2, 2 p_x^1, 2 p_y^1, 2 p_z^1
\end{array}
$$
As $\mathrm{O}_2^{+}, \mathrm{O}_2, \mathrm{O}_2^{-}, \mathrm{O}$ and $\mathrm{O}^{+}$have unpaired electrons, hence are paramagnetic.
$$
\begin{aligned}
& \mathrm{O}_2^{+}=\sigma 1 s^2, \sigma 1 s^2, \sigma 2 s^2, \sigma 2 s^2, \sigma 2 p_z^2, \pi 2 p_x^2 \approx \pi 2 p_y^2, \\
& \pi 2 p_x^1 \approx \pi 2 p_y^0 \\
& \mathrm{O}_2^{-}=\sigma 1 s^2, \sigma \cdot \% 1 s^2, \sigma 2 s^2, \sigma 2 s^2, \sigma 2 p_z^2, \pi 2 p_x^2 \\
& \approx \pi 2 p_y^2, \pi 2 p_x^2 \approx \pi 2 p_y^1 \\
& \mathrm{O}_2^{2-}=\sigma 1 s^2, \sigma \cdot s^2, \sigma 2 s^2, \sigma 2 s^2, \sigma 2 p_z^2, \pi 2 p_x^2 \\
& \approx \pi 2 p_y^2, \pi 2 p_x^2 \approx \pi 2 p_y^2 . \\
& \mathrm{O}_2=\sigma 1 s^2, \sigma 1 s^2, \sigma 2 s^2, \sigma^* 2 s^2, \sigma 2 p_z^2, \pi 2 p_x^2 \\
& \approx \pi 2 p_y^2, \pi 2 p_x^1 \approx \pi 2 p_y^1
\end{aligned}
$$
And the electronic configuration of $\mathrm{O}$ and $\mathrm{O}^{+}$ are
$$
\begin{array}{r}
\mathrm{O}=1 s^2, 2 s^2, 2 p_x^2, 2 p_y^1, 2 p_z^1 \\
\mathrm{O}^{+}=1 s^2, 2 s^2, 2 p_x^1, 2 p_y^1, 2 p_z^1
\end{array}
$$
As $\mathrm{O}_2^{+}, \mathrm{O}_2, \mathrm{O}_2^{-}, \mathrm{O}$ and $\mathrm{O}^{+}$have unpaired electrons, hence are paramagnetic.
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