The four quantum numbers (n, l, m_l, m_s) fully specify an electron in an atom. The magnetic quantum number m_l can take values
A{'text': '0, 1, 2, …, n as positive integers only', 'label': 'A'}
B{'text': '−½ or +½ irrespective of the orbital', 'label': 'B'}
C{'text': 'Only 0 and 1 regardless of the value of l', 'label': 'C'}
D{'text': '−l, −(l−1), …, 0, …, +l a total of 2l+1', 'label': 'D'}
Answer & Solution
Correct answer: D. {'text': '−l, −(l−1), …, 0, …, +l a total of 2l+1', 'label': 'D'}
1. Magnetic quantum number m_l specifies orbital orientation in space.
2. For a given l, m_l takes values −l, −(l−1), … , 0, … , +l — a total of 2l+1 values.
3. Principal n = 1, 2, 3, …; azimuthal l = 0, 1, …, n−1.
4. Spin m_s = ±½; each orbital holds 2 electrons.
_Source: NCERT Class 11 Chemistry, Ch 2 "Structure of Atom", §2.6_
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