Which of the following combination of statements is true regarding the interpretation of the atomic orbitals?
(a) An electron in an orbital of high angular momentum stays away from the nucleus than an electron in the orbital of lower angular momentum.
(b) For a given value of the principal quantum number, the size of the orbit is inversely proportional to the azimuthal quantum number.
(c) According to wave mechanics, the ground state angular momentum is equal to h/2p.
(d) The plot ψ of vs r for various azimuthal quantum numbers, shows peak shifting towards higher r value.
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Let's analyze each statement:
(a) True. Higher angular momentum (l) means more centrifugal force, so electron is farther from nucleus. For example, 3d orbital (l=2) is farther out than 3s (l=0).
(b) False. Orbit size mainly depends on principal quantum number (n). For a given n, size actually increases slightly with l, not inversely proportional.
(c) False. Wave mechanics gives ground state (1s orbital) angular momentum = 0, not .
(d) True. For higher l values, the radial wavefunction peaks at larger r values, shifting outward.
Thus, both (a) and (d) are correct statements.
Final answer: (a), (d)