Which of the subshells below do not exist due to the constraints upon the angular momentum quantum number? a) 2db) 2sc) 2pd) all of the abovee) none of the above

Explanation:

The angular momentum quantum number, identified with the letter l (lowercase L),  number is the second quantum number.

This number identifies the shape of the orbital or kind of subshell.

The possible values of the angular momentum quantum number, l, are constrained by the value of the principal quantum number n: l can take values from 0 to n - 1.

So, you can use this guide:

Principal quantum   Angular momentum         Shape of the orbital

number, n                 quantum number, l

         1                                      0                             s

         2                                     0, 1                          s, p

         3                                     0, 1, 2                      s, p, d

Hence,

your answer would be “dry”

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