The principal quantum number can only have positive integer values.

The principal quantum number in hydrogen is related to the atom's total energy.

The increase in the principal quantum number n is the more important as you go from top to bottom, so the atoms get bigger.

Normally, we expect that as the principal quantum number increases, the energies increase.

In X-ray notation, every principal quantum number is given a letter associated with it.

Let's consider the principal quantum number "n" (since it is easier).

The radii also increase down the group due to increase in principal quantum number.

Such atoms have the principal quantum number n among their quantum numbers.

Simply put, the lower the principal quantum number, the higher the ionization energy for the electrons within that shell.

As with the principal quantum number, higher numbers are associated with higher potential energy.

The Rydberg levels depend only on the principal quantum number .

As such the highest principal quantum number is 4 and the most energetic orbital "p" has its full complement of 6.

It is a way for us to remember what are the allowed angular momentum quantum numbers based on the principal quantum number.

It is a group of atomic orbitals with the same value of the principal quantum number n.

The oxidation state for these compounds is +2 and stability increases with principal quantum number (moving down a row in the periodic table).

The principal quantum number n satisfies , or .

The principal quantum number arose in the solution of the radial part of the wave equation as shown below.

We, therefore, surmise that chemical reactivity has everything to do with being able to fill-in these highest principal quantum number.

Rydberg atom (an atom in a state of high principal quantum number)

A Rydberg atom is an excited atom with one or more electrons that have a very high principal quantum number.

The study of high principal quantum number Rydberg states has spawned a number of spectroscopic techniques.

It is possible however for orbitals of different principal quantum numbers to overlap in energy, so that E 3d > E 4s for example.

Combining these two equations leads to Bohr's expression for the orbital radius in terms of the principal quantum number, n:

The assignment of molecular Rydberg states often involves following a Rydberg series from intermediate to high principal quantum numbers.

This fits with intuition: electrons with lower principal quantum numbers will have a higher probability density of being nearer to the nucleus.