The azimuthal quantum number, denoted by \( l \), characterizes the shape of an atomic orbital. Specifically: - A value of \( l = 0 \) corresponds to an s orbital, which is spherical. - A value of \( l = 1 \) corresponds to a p orbital, exhibiting a dumbbell shape. - A value of \( l = 2 \) corresponds to a d orbital, which has a cloverleaf structure. - A value of \( l = 3 \) corresponds to an f orbital, characterized by a complex shape. (a) The principal quantum number, \( n \), dictates the energy level and size of the orbital.
(c) The magnetic quantum number, \( m \), specifies the orientation of the orbital in space.
(d) The spin quantum number, \( s \), represents the intrinsic angular momentum of an electron, taking values of \( \pm \frac{1}{2} \).