Difference between Orbit and Orbital

The following are the points of difference between Orbit and Orbital.

Orbit	Orbital
An orbit is a well defined circular path around the nucleus in which the electron revolves.	An orbital is a three-dimensional space around the nucleus within which the probability of finding an electron is maximum (90.95%).
It represents a planar circular path in which an electron moves.	It represents a three-dimensional region in which electron density is more nearer to the nucleus.
All orbits are circular and disc-like in shape.	Different orbitals have different shapes i.e. s-orbitals are spherically symmetrical, p-orbitals are dum-bell shaped and son on.
Orbits do not have any directional characteristics.	All orbitals except s-orbitals have directional characteristics.
Orbit cannot explain the shape of molecules during bonding.	Orbital explain the shapes of molecules during bonding.
In an orbit, the position as well as the momentum of the electron can be known with certainty.	In an orbital, the position and the momentum of the electron cannot be known with certainty.
Orbit concept reflects the particle nature of the electron.	The orbital concept reflects both particle and wave character of an electron.
The maximum number of the electron in any orbit is given by 2n² where ‘n‘ is the number of orbit.	An orbital cannot accommodate more than two electrons and those too revolving in opposite direction.