Question:
For a given sub-shell with azimuthal quantum number 'l' the number of magnetic quantum numbers possible is
For a given sub-shell with azimuthal quantum number 'l' the number of magnetic quantum numbers possible is
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For $p$-orbital ($l=1$), $m_l = -1, 0, 1$ (Total 3). Formula: $2(1)+1 = 3$.
Updated On: Apr 27, 2026
- $l(l+1)$
- $l+1$
- $2(l+1)$
- $(l-1)$
- $(2l+1)$
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The Correct Option is
Solution and Explanation
Step 1: Concept
Magnetic quantum number ($m_l$) values range from $-l$ to $+l$, including zero.
Step 2: Meaning
The total count of these values determines the number of orbitals in a subshell.
Step 3: Analysis
Count = $l$ (negative) + $1$ (zero) + $l$ (positive) = $2l + 1$.
Step 4: Conclusion
Hence, correct answer is $(2l + 1)$.
Final Answer: (E)
Magnetic quantum number ($m_l$) values range from $-l$ to $+l$, including zero.
Step 2: Meaning
The total count of these values determines the number of orbitals in a subshell.
Step 3: Analysis
Count = $l$ (negative) + $1$ (zero) + $l$ (positive) = $2l + 1$.
Step 4: Conclusion
Hence, correct answer is $(2l + 1)$.
Final Answer: (E)
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