Orbit vs Orbital key differences. Clear Explanation for Students

Most of the students are confusing to understand the key differences between orbit and orbital.

Orbit:

1. Orbit is a circular path in which electron is  revolving around the nucleus.

2. It represents 2-D motion of an electron. It has no directional properties.

3.  Maximum number of electrons can be accommodated in an orbit is  2n².

4. According to Neis Bohr,  Shape of an orbit is circular.

5. position  and velocity of an electron can be found precisely at any instant.

6.  Determination of the position and momentum of a revolving electron in circular or elliptical orbit is possible.

Orbital

1. Orbital is a space or region around the nucleus where electron probability of finding an electron is maximum

2. It represents 3-D motion of an electron. It has directional properties except s- orbital

3. It can accommodate maximum of 2 electrons.

4. Shape of s – orbital is spherical, p-orbital is  dumb bell, d- orbital is double dumbbell and the shape of f- orbital is four fold dumbell.

5. position and velocity of ecan not be found at any instant simultaneously.

6.  It indicates the overall position of the electron, but not suggest its position at a particular moment