Using the concepts of shielding and penetration, explain why a ground state configuration of $1 s^{2} 2 s^{1}$ for an Li atom is energetically preferred over $1 s^{2} 2 p^{1}$.
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This means that there are 2 electrons in the 1s orbital and 1 electron in the 2s orbital. Show more…
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The electron configuration of $\mathrm{B}$ is $1 \mathrm{s}^{2} 2 \mathrm{s}^{2} 2 p^{1}$. (a) If each core electron (that is, the 1 s electrons) were totally effective in shielding the valence electrons (that is, the $2 s$ and $2 p$ electrons) from the nucleus and the valence electrons did not shield one another, what would be the shielding constant $(\sigma)$ and the effective nuclear charge, $\left(Z_{\text {eff }}\right)$ for the $2 s$ and $2 p$ electrons? (b) In reality, the shielding constants for the $2 s$ and $2 p$ electrons in $\mathrm{B}$ are slightly different. They are 2.42 and 2.58 , respectively. Calculate $Z_{\mathrm{eff}}$ for these electrons, and explain the differences from the values you determined in part (a).
Use molecular orbital theory to explain in detail why $\mathrm{N}_{2}^{+}$ and $\mathrm{N}_{2}^{-}$ have similar bond strengths and both are very different from neutral $\mathrm{N}_{2}$ .
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