Questions: Complete the table below by filling in the principal quantum number n and angular momentum quantum number I for each electron subshell listed. subshell principal quantum number n angular momentum quantum number I --- --- --- 6 f 6 d 3 s 4 d

Complete the table below by filling in the principal quantum number n and angular momentum quantum number I for each electron subshell listed.

subshell principal quantum number n angular momentum quantum number I
--- --- ---
6 f
6 d
3 s
4 d

Transcript text: Complete the table below by filling in the principal quantum number $n$ and angular momentum quantum number / for each electron subshell listed. \begin{tabular}{|c|c|c|} \hline subshell & \begin{tabular}{c} principal \\ quantum number $\boldsymbol{n}$ \end{tabular} & \begin{tabular}{c} angular momentum \\ quantum number I \end{tabular} \\ \hline 6 f & $\square$ & $\square$ \\ \hline 6 d & $\square$ & $\square$ \\ \hline 3 s & $\square$ & $\square$ \\ \hline 4 d & $\square$ & $\square$ \\ \hline \end{tabular}

Solution

Solution Steps

Step 1: Identify the Principal Quantum Number $ n $

The principal quantum number $ n $ is the number that appears before the letter in the subshell notation. For example, in the subshell "6f", the principal quantum number $ n $ is 6.

Step 2: Identify the Angular Momentum Quantum Number $ l $

The angular momentum quantum number $ l $ is determined by the letter in the subshell notation:

$ s $ corresponds to $ l = 0 $
$ p $ corresponds to $ l = 1 $
$ d $ corresponds to $ l = 2 $
$ f $ corresponds to $ l = 3 $

Step 3: Fill in the Table

Using the information from Steps 1 and 2, we can fill in the table as follows:

\[ \begin{array}{|c|c|c|} \hline \text{subshell} & \text{principal quantum number } n & \text{angular momentum quantum number } l \\ \hline 6f & 6 & 3 \\ \hline 6d & 6 & 2 \\ \hline 3s & 3 & 0 \\ \hline 4d & 4 & 2 \\ \hline \end{array} \]

Final Answer

\[ \boxed{ \begin{array}{|c|c|c|} \hline \text{subshell} & \text{principal quantum number } n & \text{angular momentum quantum number } l \\ \hline 6f & 6 & 3 \\ \hline 6d & 6 & 2 \\ \hline 3s & 3 & 0 \\ \hline 4d & 4 & 2 \\ \hline \end{array} } \]

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