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9. Quantum Mechanics
Quantum Numbers: Magnetic Quantum Number
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What are the possible values of the magnetic quantum number (m_l) for an electron in a d orbital?
A
-2, -1, 0, +1, +2
B
-3, -2, -1, 0, +1, +2, +3
C
0, +1, +2
D
-1, 0, +1
Verified step by step guidance1
Understand that the magnetic quantum number (m_l) is related to the orientation of the orbital in space and can take integer values from -l to +l, where l is the azimuthal quantum number.
Recognize that for a d orbital, the azimuthal quantum number (l) is equal to 2. This is because the d orbital corresponds to l = 2 in quantum mechanics.
Apply the rule for determining the possible values of m_l: since l = 2 for a d orbital, m_l can take values from -2 to +2.
List the possible values of m_l for a d orbital: -2, -1, 0, +1, +2. These are the integer values within the range determined by the azimuthal quantum number.
Verify that the correct answer is the set of values -2, -1, 0, +1, +2, which corresponds to the possible orientations of a d orbital in space.
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