Which of the following is a correct set of quantum numbers for an electron in a 3d orbital? A) n = 3, l = 0, m_l = -1 B) n = 3, l = 1, m_l = +3 C) n = 3, l = 2, m_l= 3 D) n = 3, l = 3, m_l = +2 E) n = 3, l = 2, m_l= -2

Question

Quizplus · Accepted Answer

For the given orbital, the value of n (principle quantum number) is 3 since it is a 3d orbital (d orbital corresponds to l = 2). 
The allowed values of l (azimuthal quantum number) for a given value of n are 0 to (n-1). So, l can be either 0, 1, or 2. 
The allowed values of m_l (magnetic quantum number) for a given value of l are -l to +l. So, for l = 2, m_l can be -2, -1, 0, 1, or 2 (two electrons can occupy the same orbital only if they have different spin quantum numbers, so there are two possible values of m_s for each value of m_l). 
Therefore, the correct set of quantum numbers for an electron in a 3d orbital is:
n = 3, l = 2, m_l = -2, -1, 0, 1, or 2
And the correct choice from the given options is E, as it matches these values.

Which of the Following Is a Correct Set of Quantum