Question

Identify an orbital with the quantum numbers $n = 4$, $l = 3$, $m = 0$.

• A. 4f
• B. 4p
• C. 4s
• D. 4d

Hint:

Always memorize the basic alphabet code for the azimuthal quantum number $l$: 0, 1, 2, 3 maps directly to s, p, d, f. Since $n=4$ and $l=3$, it has to be 4f!

Answer 1

The Correct Option is A

Step 1: Understanding the Question:
The question requires us to identify the specific atomic orbital designation corresponding to a given set of principal ($n$), azimuthal ($l$), and magnetic ($m$) quantum numbers.

Step 2: Detailed Explanation:
Let's decode the electronic subshell notation based on the provided quantum values:

• The principal quantum number $n = 4$ specifies that the orbital belongs to the 4th electron shell.

• The azimuthal quantum number $l$ determines the shape and type of the subshell. The standard mapping is: itemize

• $l = 0 \rightarrow \text{s-orbital}$

• $l = 1 \rightarrow \text{p-orbital}$

• $l = 2 \rightarrow \text{d-orbital}$

• $l = 3 \rightarrow \text{f-orbital}$
Since $l = 3$ is specified, this indicates an f-subshell. The magnetic quantum number $m = 0$ is a valid orientation value for an f-subshell, which contains seven distinct degenerate orbitals ranging from $-3$ to $+3$. itemize Combining the shell number and the subshell letter gives us a 4f orbital.

Step 3: Final Answer: The orbital matching the given quantum numbers is 4f, which corresponds to option (A).