Question

complete the table below by filling in the principal quantum number ( n ) and angular momentum quantum number ( l ) for each electron subshell listed.

Explanation:

Step1: Determine principal quantum number \( n \)

The principal quantum number \( n \) is the number before the letter in the subshell notation. For \( 6d \), \( n = 6 \); for \( 6p \), \( n = 6 \); for \( 5f \), \( n = 5 \); for \( 5s \), \( n = 5 \).

Step2: Determine angular momentum quantum number \( l \)

• For \( s \)-subshell, \( l = 0 \).
• For \( p \)-subshell, \( l = 1 \).
• For \( d \)-subshell, \( l = 2 \).
• For \( f \)-subshell, \( l = 3 \).

So for \( 6d \), \( l = 2 \); for \( 6p \), \( l = 1 \); for \( 5f \), \( l = 3 \); for \( 5s \), \( l = 0 \).

Answer:

subshell	principal quantum number \( n \)	angular momentum quantum number \( l \)
\( 6p \)	\( 6 \)	\( 1 \)
\( 5f \)	\( 5 \)	\( 3 \)
\( 5s \)	\( 5 \)	\( 0 \)