Question

match each set of quantum numbers to the correct subshell description by typing in the correct number. 1: n = 2, l = 0 2p: 2: n = 3, l = 2 3d: 3: n = 1, l = 0 2s: 4: n = 2, l = 1 4f: 5: n = 4, l = 3 1s:

Explanation:

Step1: Recall quantum - number rules

The principal quantum number $n$ represents the energy level, and the angular - momentum quantum number $l$ determines the subshell type ($l = 0$ is $s$, $l=1$ is $p$, $l = 2$ is $d$, $l=3$ is $f$).

Step2: Match $n = 2,l = 0$

For $n = 2$ and $l = 0$, the subshell is $2s$. So it does not match $2p$.

Step3: Match $n = 3,l = 2$

For $n = 3$ and $l = 2$, the subshell is $3d$. So the answer for $3d$ is $2$.

Step4: Match $n = 1,l = 0$

For $n = 1$ and $l = 0$, the subshell is $1s$. So the answer for $1s$ is $3$.

Step5: Match $n = 2,l = 1$

For $n = 2$ and $l = 1$, the subshell is $2p$. So the answer for $2p$ is $4$.

Step6: Match $n = 4,l = 3$

For $n = 4$ and $l = 3$, the subshell is $4f$. So the answer for $4f$ is $5$.

Answer:

$2p:4$
$3d:2$
$2s:1$
$4f:5$
$1s:3$