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JEE MainChemistryStructure of Atom

Four orbitals in a multi-electron atom are described by their number of nodes as follows: Orbital A: 2 radial nodes, 1 angular node Orbital B: 1 radial node, 2 angular nodes Orbital C: 4 radial nodes, 0 angular nodes Orbital D: 0 radial nodes, 3 angular nodes The correct increasing order of energy for these orbitals is:

Options

  1. AC < A < B < D
  2. BA = B = D < C
  3. CA < C < B < D
  4. DD < B < A < C

Correct answer

C. A < C < B < D

Step-by-step solution

The number of angular nodes is equal to the azimuthal quantum number ( l ). The number of radial nodes is given by the formula (n - l - 1) , where n is the principal quantum number. Let us determine n and l for each orbital: Orbital A: l = 1 . Radial nodes = n - 1 - 1 = 2 n = 4 . This is the 4p orbital. (n+l) = 4 + 1 = 5 . Orbital B: l = 2 . Radial nodes = n - 2 - 1 = 1 n = 4 . This is the 4d orbital. (n+l) = 4 + 2 = 6 . Orbital C: l = 0 . Radial nodes = n - 0 - 1 = 4 n = 5 . This is the 5s orbital. (n+l) = 5 + 0 =

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