Question

which of the orbital electron configurations is not possible?
answer:
a 2s¹
b 3d¹⁰
c 4p⁷
d 4f⁷
e 2p⁴

Explanation:

• The maximum number of electrons in a \(p\) - orbital is \(6\).
• For option C, \(4p^{7}\) violates this rule as it has \(7\) electrons in a \(p\) - orbital.
• Option A (\(2s^{1}\)): The \(s\) - orbital can hold a maximum of \(2\) electrons, so having \(1\) is possible.
• Option B (\(3d^{10}\)): The \(d\) - orbital can hold a maximum of \(10\) electrons, so this is possible.
• Option D (\(4f^{7}\)): The \(f\) - orbital can hold a maximum of \(14\) electrons, so having \(7\) is possible.
• Option E (\(2p^{4}\)): Since the \(p\) - orbital can hold up to \(6\) electrons, having \(4\) is possible.

Answer:

C. \(4p^{7}\)