Question

what is the correct representation for the subshell with n = 2 and l = 1? 2p 1p 1d 2d complete how many subshells are in the n = 4 shell? 4 complete how many orbitals does the n = 4 shell have? done

Explanation:

Step1: Recall the rules for subshell notation

The principal quantum number $n$ is the first number in the subshell notation. The angular - momentum quantum number $l$ determines the type of subshell: $l = 0$ is $s$, $l=1$ is $p$, $l = 2$ is $d$, $l=3$ is $f$.

Step2: Determine the number of subshells in a shell

The number of subshells in a shell with principal quantum number $n$ is equal to $n$. So for $n = 4$, the number of subshells is 4.

Step3: Calculate the number of orbitals in a shell

The number of orbitals in a shell with principal quantum number $n$ is given by $n^{2}$. For $n = 4$, we have $n^{2}=4^{2}=16$.

Answer:

16