Given below are two statements :

Statement (I) : The orbitals having same energy are called as degenerate orbitals.

Statement (II) : In hydrogen atom, 3p and 3d orbitals are not degenerate orbitals.

In the light of the above statements, choose the most appropriate answer from the options given below :

<p><strong>Degenerate Orbitals</strong>: Orbitals that have the same energy are called degenerate orbitals. </p> <p><p><strong>Hydrogen-like Atoms (Single-Electron Systems)</strong>: In a hydrogen atom (or any one-electron system), the energy of an orbital depends <strong>only</strong> on the principal quantum number $n$, <em>not</em> on the azimuthal quantum number $l$. Therefore, all orbitals with the same $n$ (e.g., 3s, 3p, 3d) have the same energy and are <strong>degenerate</strong>. </p></p> <p><p><strong>Multi-electron Atoms</strong>: In atoms with more than one electron, the energy also depends on $l$ (and other factors like screening), so 3s, 3p, and 3d orbitals are <strong>not</strong> all degenerate in multi-electron atoms.</p></p> <p>Now, let us evaluate the given statements:</p> <p><p><strong>Statement (I)</strong>: “The orbitals having same energy are called as degenerate orbitals.” </p> <p>This statement is <strong>true</strong> by definition.</p></p> <p><p><strong>Statement (II)</strong>: “In hydrogen atom, 3p and 3d orbitals are not degenerate orbitals.” </p> <p>In a hydrogen atom, all orbitals with the same principal quantum number $n$ (like 3s, 3p, 3d) <strong>are</strong> degenerate. </p> <p>Hence, this statement is <strong>false</strong>.</p></p> <p>Therefore, the correct option is:</p> <p><strong>Option A: Statement I is true but Statement II is false.</strong></p>