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(A) For a hydrogen-like atom or ion,the energy of an orbital depends only on the principal quantum number $n$. However,for multi-electron atoms like l

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Both $A$ and $R$ are true and $R$ is the correct explanation of $A$.

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(A) For a hydrogen-like atom or ion,the energy of an orbital depends only on the principal quantum number $n$. However,for multi-electron atoms like lithium $(Z=3)$,the energy of an orbital depends on both $n$ and the effective nuclear charge $(Z_{eff})$.As the atomic number $(Z)$ increases,the effective nuclear charge increases,which leads to a stronger attraction between the nucleus and the electrons.Consequently,the energy of the same orbital (e.g.,$2s$) decreases as the atomic number increases.Therefore,the energy of the $2s$ orbital in hydrogen $(Z=1)$ is higher than that in lithium $(Z=3)$.Both Assertion $A$ and Reason $R$ are correct,and $R$ correctly explains $A$.

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