match each set of quantum numbers to the correct subshell description by typing in the correct number. 1: n…

Explanation:

Step1: Recall quantum - number rules

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

Step2: Analyze each set

For $n = 2,l = 0$

Since $l = 0$, it is an $s$ - subshell and with $n = 2$, it is the $2s$ subshell. So it matches with $2s$.

For $n = 3,l = 2$

Since $l = 2$, it is a $d$ - subshell and with $n = 3$, it is the $3d$ subshell. So it matches with $3d$.

For $n = 1,l = 0$

Since $l = 0$, it is an $s$ - subshell and with $n = 1$, it is the $1s$ subshell. So it matches with $1s$.

For $n = 2,l = 1$

Since $l = 1$, it is a $p$ - subshell and with $n = 2$, it is the $2p$ subshell. So it matches with $2p$.

For $n = 4,l = 3$

Since $l = 3$, it is an $f$ - subshell and with $n = 4$, it is the $4f$ subshell. So it matches with $4f$.

Answer:

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