Question

Why are $s$ orbitals non-directional?

Answer 1

Atomic orbitals, which are mathematical functions, describe the wave nature of electrons or electron pairs in an atom. They have a method for calculating the chances of having an electron in a given area around the nucleus of an atom.

Complete answer:
The atomic orbital model, a modern structure for visualizing the submicroscopic behavior of electrons in matter, is built around atomic orbitals. Based on the orbital's mathematical structure, the term atomic orbital may also refer to the physical region or space in which the electron can be determined to be present.
The $s$ , $p$ , $d$ , and $f$ denote four different forms of orbitals, each with a different shape. Since they are the most significant inorganic and biological chemistry, the $s$ and $p$ orbitals are taken into account. An atom's orbitals are arranged into various layers or electron shells.
The $s$ orbitals are spherically symmetrical and non-directional, which means that the probability of having an electron at a given distance from the nucleus is the same in all directions. Electron density in $s$ orbitals is uniform in all directions. Compare this to a $p$ orbital, which resembles a dumbbell in shape. The chance of finding an electron at a given distance is highest along the $x$ , $y$ , or $z$ axis in a $p$ orbital. The $p$ orbital is a directional orbital.
So, we find that because of their spherical symmetry, $s$ orbitals are non-directional.

Note:
An atom, according to the quantum atomic model, may have any number of orbitals. The size, shape, and orientation of these orbitals can all be classified. For a smaller orbital, there's a better chance of having an electron close to the nucleus.