which of the following is not a valid set of quantum numbers?\no n = 2, l = 1, m = 0\no n = 1, l = 0, m =…

Answer:

C. $n = 3, l=3, m = 3$

Explanation:

Step1: Recall quantum - number rules

The principal quantum number $n$ can take values $n = 1,2,3,\cdots$. The angular - momentum quantum number $l$ can take values $l=0,1,\cdots,n - 1$. The magnetic quantum number $m$ can take values $m=-l,-l + 1,\cdots,0,\cdots,l-1,l$.

Step2: Analyze option A

For $n = 2$, $l$ can be $0$ or $1$. When $l = 1$, $m$ can be $- 1,0,1$. So $n = 2,l = 1,m = 0$ is valid.

Step3: Analyze option B

For $n = 1$, $l$ can only be $0$. When $l = 0$, $m$ can only be $0$. So $n = 1,l = 0,m = 0$ is valid.

Step4: Analyze option C

For $n = 3$, $l$ can take values $l = 0,1,2$ (since $l$ ranges from $0$ to $n - 1$). Here $l=3$ is not allowed for $n = 3$. So $n = 3,l = 3,m = 3$ is not a valid set of quantum numbers.