Question:
Identify the orbital having quantum numbers, \(n=4\) and \(l=2\) from following.
Identify the orbital having quantum numbers, \(n=4\) and \(l=2\) from following.
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The value of l tells the subshell: l = 0, 1, 2, 3 correspond to s, p, d, f.
Updated On: Nov 12, 2026
- \(4d\)
- \(4p\)
- \(4f\)
- \(2d\)
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The Correct Option is A
Solution and Explanation
Step 1: Understanding the Concept
The principal quantum number \(n\) gives the shell and the azimuthal quantum number \(l\) gives the subshell.
Step 2: Subshell from \(l\)
\(l=0,1,2,3\) correspond to \(s,p,d,f\) respectively. So \(l=2\) is a \(d\) subshell.
Step 3: Combine
With \(n=4\) the orbital is \(4d\).
Step 4: Compare the options
\(2d\) is not possible because \(l\) must be less than \(n\). The answer is option (A).
Final Answer:
The orbital is \(4d\). \[ \boxed{\text{(A) }4d} \]
The principal quantum number \(n\) gives the shell and the azimuthal quantum number \(l\) gives the subshell.
Step 2: Subshell from \(l\)
\(l=0,1,2,3\) correspond to \(s,p,d,f\) respectively. So \(l=2\) is a \(d\) subshell.
Step 3: Combine
With \(n=4\) the orbital is \(4d\).
Step 4: Compare the options
\(2d\) is not possible because \(l\) must be less than \(n\). The answer is option (A).
Final Answer:
The orbital is \(4d\). \[ \boxed{\text{(A) }4d} \]
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