Question

Oxygen molecule $\left(\mathrm{O}_{2}\right)$ is paramagnetic. Explain with the help of MOT.

Answer 1

$\mathrm{O}_{2}$
Total electrons $=8+8=16$
Electronic configuration
$$\begin{aligned} &8^{0}=1 s^{2}, 2 s^{2} 2 p^{4} \\ &8^{0}=1 s^{2}, 2 s^{2} 2 p^{4} \end{aligned}$$
Molecular orbital configuration,
$$\begin{aligned} &\left(\sigma^{b} 1 s\right)^{2} \cdot\left(\sigma^{\prime} 1 s\right)^{2},\left(\sigma^{b} 2 s\right)^{2} \cdot\left(\sigma^{*} 2 s\right)^{2},\left(\sigma^{\prime} 2 \mathrm{px}\right)^{2}, \\ &\left(\pi^{3} 2 p y\right)^{2}\left(\pi^{b} 2 p z\right)^{2},\left(\pi^{2} 2 p y\right)^{\prime}\left(\pi^{\prime} 2 p z\right)^{l},\left(\sigma^{\prime} 2 p x\right)^{0} \end{aligned}$$
Since, there are two unpaired electrons in molecular orbitals of $\mathrm{O}_{2}$ molecule, so it is paramagnetic in nature.

Answer 2

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Answer 3

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