The subshell is represented by the principal quantum number(n) followed by the orbital.
Example. 2s subshell represents the principal quantum number as 2 and for the s-orbital angular quantum number(l) is 0.
Name of Subshell | Angular momentum quantum numbers(l) |
s | 0 |
p | 1 |
d | 2 |
f | 3 |
Now,
1) For 5p,
Principal quantum number(n) = 5
Angular momentum quantum number(l) = 1 ; since from the table, for p-subshell l = 1
2) For 4f,
Principal quantum number(n) = 4
Angular momentum quantum number(l) = 3 ; since from the table, for f-subshell l = 3
3) For 6d,
Principal quantum number(n) = 6
Angular momentum quantum number(l) = 2 ; since from the table, for d-subshell l = 2
4) For 2p,
Principal quantum number(n) = 2
Angular momentum quantum number(l) = 1 ; since from the table, for p-subshell l = 1
Thus,
Subshell | Principal quantum number(n) | Angular momentum quantum number(l) |
5p | 5 | 1 |
4f | 4 | 3 |
6d | 6 | 2 |
2p | 2 | 1 |
Complete the table below by filling in the principal quantum number n and angular momentum quantum number / for eac...
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im stuck on this one please help! Part A If an electron has a principal quantum number (n) of 4 and an angular momentum quantum number (1) of 3, the subshell designation is O 31 4p OOO 3s Submit Request Answer