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JEE MainChemistryStructure of Atom

Consider the following orbital states for a He ⁺ ion: A. n=4, l=0 B. n=3, l=2 C. n=3, l=1 D. n=3, l=0 The correct increasing order of energy of these states is:

Options

  1. AD < C < A < B
  2. BD = C = B < A
  3. CD < A < C < B
  4. DB < C < D < A

Correct answer

B. D = C = B < A

Step-by-step solution

For a single-electron species like the He ⁺ ion, the energy of an orbital depends only on the principal quantum number ( n ) and is independent of the azimuthal quantum number ( l ). This means that all subshells within the same principal shell are degenerate. The given states have the following principal quantum numbers: A. n=4 B. n=3 C. n=3 D. n=3 Since states B, C, and D all have n=3 , they possess the same energy. State A has n=4 , which corresponds to a higher energy level. Therefore, the correct increasing or

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