Two statements are given below:Statement I: I | vedclass

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(C) In a hydrogen atom, which is a single-electron system, the energy of orbitals depends only on the principal quantum number $(n)$. Therefore, $2s$

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Statement $I$ is correct but statement $II$ is not correct

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(C) In a hydrogen atom, which is a single-electron system, the energy of orbitals depends only on the principal quantum number $(n)$. Therefore, $2s$ and $2p$ orbitals have the same energy.In multi-electron atoms like $He$, the energy of orbitals depends on both the principal quantum number $(n)$ and the azimuthal quantum number $(l)$. Due to the shielding effect, the $2s$ orbital has lower energy than the $2p$ orbital.Thus, statement $I$ is correct, and statement $II$ is incorrect.

Two statements are given below:
Statement $I$: In $H$ atom, the energy of $2s$ and $2p$ orbitals is same.
Statement $II$: In $He$ atom, the energy of $2s$ and $2p$ orbitals is same.
The correct answer is:

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Two statements are given below:Statement $I$: In $H$ atom, the energy of $2s$ and $2p$ orbitals is same.Statement $II$: In $He$ atom, the energy of $2s$ and $2p$ orbitals is same.The correct answer is: