On the basis of quantum numbers, justify that the sixth period of the periodic table should have 32 elements.
Answers
Principal quantum number is the number which determines the principal energy level or shell in which the electron is present.
It gives the normal range of the particle from the nucleus and the value of the energy of the electron.
In the periodical table of the elements, a period symbolizes the value of the principal quantum number (n) for the outermost shells.
Each period begins with the filling of the primary quantum number (n).
The value of n for the sixth period is 6, then for n = 6, azimuthal quantum number (l) can have the benefits of 0, 1, 2, 3, 4.
According to the Aufbau’s principle-electrons are affixed to various orbitals in order of their rising energies.
The power of the 6d subshell is also eminent than that of the 7s subshell.
In the 6th period- electrons can be filled only in 6s, 4f, 5d, and 6 p subshells.
Now, 6s - one orbital, 4f - seven orbitals, 5d - five orbitals, and 6p - three orbitals.
Thus, there are a total of sixteen (1 + 7 + 5 + 3 = 16) orbitals available.
According to Pauli’s exclusion principle, each orbital can accommodate a maximum of 2 electrons.
Thus, 16 orbitals can accommodate maximum of 32 electrons.
Therefore, the sixth period of the periodic table will have 32 elements.