Which of the following statements is true?
A)An orbital that penetrates into the region occupied by core electrons is less shielded from nuclear charge than an orbital that does not penetrate and therefore has a lower energy.
B)An orbital that penetrates into the region occupied by core electrons is more shielded from nuclear charge than an orbital that does not penetrate and therefore has a lower energy.
C)It is possible for two electrons in the same atom to have identical values for all four quantum numbers.
D)Two electrons in the same orbital can have the same spin.
E)None of the above are true.

Question

Quizplus · Accepted Answer

An orbital that penetrates into the region occupied by core electrons experiences more nuclear charge and is therefore less shielded, leading to a higher energy. This is due to the increased attraction between the nucleus and electrons, which makes it more difficult to remove the electron from the atom. Option B is incorrect because an orbital that does not penetrate into the region occupied by core electrons experiences more shielding and therefore has a lower energy. Option C is incorrect because the Pauli exclusion principle states that no two electrons in an atom can have the same set of four quantum numbers. Option D is incorrect because the Pauli exclusion principle also requires that two electrons in the same orbital must have opposite spins.

Which of the Following Statements Is True