Question

Which subshell has no orbital?

Answer 1

1. An atomic orbital is the wave function, $\psi$ for an electron in an atom. If we define an electron by a wave function, it means that an electron occupies that orbital.
2. Bohr's atomic model stated that electrons revolve around the nucleus in a particular circular path called a shell.
3. A shell includes one or more subshells.
4. Each orbital in an atom is defined by several quantum numbers.
5. These are principal quantum number( $n$), azimuthal quantum number($l$), and magnetic orbital quantum number ($m_l$).
6. The principal quantum number n defines the size and energy of the orbital.
7. Azimuthal quantum number, l depicts the 3-D structure of the orbital. Each subshell has an azimuthal quantum number.
   For $l=0$, s-subshell.
   For $l=1$, p-subshell
   For $l=2$, d-subshell
   For $l=3$, f-subshell, etc.,
8. Magnetic orbital quantum number, m depicts the orientation of the orbital in space involving a standard set of co-ordinate axis.
9. It gives the number of orbitals.
   $m_l=2l+1$
   For example:- For $l=0$, the only allowed value of $m_l=(2\times 0)+1=1$. So, the s-subshell has one orbital.
   For $l=1$, $m_l=(2\times 1)+1=3$. So, p-subshell has three p orbitals.

Hence, every subshell has at least one orbital. No subshell has zero orbitals.