How are orbitals written?

 

When we write an orbital, we use two quantum numbers. One is the principal quantum number (n), and the other is the auxiliary quantum number (l).

The value of the principal quantum number n is 1,2,3,4 ---- etc. On the other hand, the auxiliary quantum numbers are denoted by s, p, d, f.

When writing an orbital, we write the principal quantum number and the auxiliary quantum number together. For example: 1s, 2s, 2p, 3s etc. .

Here, in the case of 1s, 1 is the principal quantum number or the main energy level and s is the auxiliary quantum number or the sub-energy level.

The value of the principal quantum number n = 1,2,3,4 --- etc. refers to the various circular main orbits or main energy levels or orbits outside the nucleus of the atom.

The auxiliary quantum number indicates which sublevel of a main energy level an electron exists in an atom.

The value of the auxiliary quantum number ranges from zero to (n - 1). For example: If n = 1, l = 0. The 1s sublevel will be in the field.

If n = 2, l = 0 and 1. In this case, the 2s and 2p sublevels will be.

That is, if l = 0, the s sublevel will be, if l = 1, the p sublevel will be, if l = 2, the d sublevel will be, and if l = 3, the f sublevel will be.

The electrons in the sublevel of the atom are arranged in a three-dimensional manner. The three-dimensional arrangement of electrons in any sublevel of the atom or the region where the electron density (90% - 95%) is high is called an orbital.