For all atoms of the same element, the 2s orbital is larger...

In multielectron atoms many of the periodic trends can be explained in terms of $Z_{\text {eff. Consider the fol- }}$ lowing statements and discuss whether or not the statement is true or false. (a) Electrons in a $p$ orbital are more effective than electrons in the s orbitals in shielding other electrons from the nuclear charge. (b) $\mathrm{Z}_{\text {eff }}$ for an electron in an s orbital is lower than that for an electron in a $p$ orbital in the same shell. (c) $\mathrm{Z}_{\text {eff }}$ is usually less than $\mathrm{Z}$ (d) Electrons in orbitals having $\ell=1$ penetrate better than those with $\ell=2$ (e) $\mathrm{Z}_{\text {eff }}$ for the orbitals of the elements $\mathrm{Na}(3 s)$ $\mathrm{Mg}(3 \mathrm{s}), \mathrm{Al}(3 p), \mathrm{P}(3 p),$ and $\mathrm{S}(3 p)$ are in the order $\mathrm{Z}_{\mathrm{eff}}(\mathrm{Na})<\mathrm{Z}_{\mathrm{eff}}(\mathrm{Mg})>\mathrm{Z}_{\mathrm{eff}}(\mathrm{Al})<\mathrm{Z}_{\mathrm{eff}}(\mathrm{P})>\mathrm{Z}_{\mathrm{eff}}(\mathrm{S})$

Question

For all atoms of the same element, the 2s orbital is larger than the 1s orbital. O True O False

Question

For all atoms of the same element, the 2s orbital is larger than the 1s orbital. O True O False

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