Question

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

• A. Statement-I is true but Statement-II is false
• B. Both Statement-I and Statement-II are true
• C. Both Statement-I and Statement-II are false
• D. Statement-I is false but Statement-II is true

Answer 1

The Correct Option is A

To choose the most appropriate answer based on the given statements about degenerate orbitals, let's analyze each statement:

1. Statement-I: The orbitals having same energy are called as degenerate orbitals.
   • This statement is a true fact. Degenerate orbitals are defined in chemistry as orbitals that have the same energy level.
2. Statement-II: In hydrogen atom, 3p and 3d orbitals are not degenerate orbitals.
   • This statement is false. In a hydrogen atom, which has only one electron, all sublevels within a principal energy level (i.e., \(3p, 3d, \text{ and } 3s\)) are indeed degenerate because they all have the same energy.
   • This degeneracy is due to the symmetrical nature of the electron's attraction to the nucleus in a single-electron system like hydrogen.

In light of these analyses:

• Statement-I is true as it correctly defines degenerate orbitals.
• Statement-II is false because, in the hydrogen atom, the 3p and 3d orbitals indeed have the same energy.

Therefore, the correct answer is: Statement-I is true but Statement-II is false.

Answer 2

Step 1. Analyze Statement-I: The definition of degenerate orbitals is accurate, as orbitals with the same energy level are indeed degenerate.
Step 2. Examine Statement-II: In a hydrogen atom, all orbitals in the same principal quantum level (e.g., 3s, 3p, 3d) are degenerate, as they have the same energy. Therefore, Statement-II is incorrect.
Step 3. Conclusion: Statement-I is correct, but Statement-II is incorrect.