Question

An electron has a spin quantum number, s = +1/2 and a magnetic quantum number, ml = +1. In which of the following orbital will it NOT be present?
A. s-orbital
B. p-orbital
C. d-orbital
D. f-orbital​

Answer 1

A) S- orbital

Magnetic quantum number -1 is possible only when the azimuthal quantum number have value 1 = 1, which is possible for p, d and f-subshells but not for s-subshell because the value of 1 for s-subshell is zero.

Answer 2

Correct option is

B.d− orbital

C.p− orbital

D.f− orbital

For a particular l value there should be m values from −m to +m

For l=0, m value should be 0 indicates s orbital.

For l=1, m value should be −1,0,+1 indicates s,p orbitals.

For l=2, m value should be −2,−1,0,+1,+2 indicates s,p,d orbitals.

Fore l=3, m value should be −3,−2,−1,0,+1,+2,+3 indicates s,p,d orbitals. For l value −1 the electron may present in p or d or f orbital

Hence options B,C,D are correct.