The electronic configuration 1s² 2s² 2p⁶ 2d¹ is impossible because:
Athe 2d subshell does not exist
Bthe 2p subshell cannot hold six electrons
Cthe 2s subshell must fill after 2p
Dthe total electron count is odd
Answer & Solution
Correct answer: A. the 2d subshell does not exist
1. The subshells available in a shell are limited by its principal quantum number $n$.
2. For $n=2$ the allowed values of the azimuthal quantum number are 0 and 1, giving only s and p subshells.
3. A d subshell needs an azimuthal quantum number of 2, which first becomes available at $n=3$.
4. So 2d cannot exist, and any configuration naming it is impossible.
5. The 2p subshell holding six electrons is entirely correct, since three orbitals take two electrons each.
_Source: NECTA ACSEE 2023 Chemistry 132/1, Question 4: The Atom_
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