Difference between Orbit and Orbital(Orbit vs Orbital)

Electrons revolve around the nucleus of the atom and thus we can identify regions of space around the nucleus where there is high probability of finding an electron. This leads to the concept of orbitals in place of definite orbits proposed by Bohr. An orbital may be defined as the region of space around the nucleus where there is maximum probability of finding an electron. Diagrammatic representation of orbitals is difficult.
The electrons revolve around the nucleus only in certain selected circular paths called orbits. These orbits are associated with definite energies and are called energy levels or energy shells or quantum levels. These are numbered as 1, 2, 3, 4 etc. or designated as K, L, M, N etc.
Orbit vs Orbital
It is well defined circular path followed by revolving electron around the nucleus.
It is a region of space around the nucleus where the electron is most likely to be found.
It represents planar motion of an electron.
It represents three dimensional motion of an electron around the nucleus.
The maximum number of electrons is an orbit is 2n2 where n stands for number of the orbit.
An orbital cannot accommodate mote than two electrons.
Orbit are circular in shape.
Bohr's Orbit

Orbital have different shapes.
Orbital Shape

Orbits are non directional in character hence they cannot explain shape of molecules.
Orbitals have directional character and hence they can account for shapes of molecules.
Concept of well defined orbit is against Heisenberg’s principle.
Concept of orbital is in accordance with Heisenberg’s principle.
Heisenberg’s Uncertainty Principle: He pointed out that it is not possible to determine simultaneously the position and momentum of a small moving particle, such as electron, with entire certainty.
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