Question

Can any elements go beyond the 5th principal energy level? Explain why or why not.

Answer 1

Yes, elements can have electrons beyond the 5th principal energy level, as higher energy levels are associated with higher principal quantum numbers and can accommodate more electrons due to an increased number of orbitals.

Step-by-step explanation:

Yes, elements can go beyond the 5th principal energy level. The principal quantum number (n) defines the energy level in which an electron resides, with n=1 being the lowest energy level. The Pauli exclusion principle dictates that no two electrons can have the same set of quantum numbers, which means they have to occupy higher energy levels once the lower ones are filled. Electrons fill in energy levels in a specific order, and as we move higher in the periodic table, we encounter elements with electrons in higher principal energy levels, such as n=6 for Cesium (Cs) and n=7 for elements like Uranium (U).

Higher principal quantum numbers correspond to higher energy levels and can house more electrons due to the increased number of available orbitals. Furthermore, Bohr's model of the atom illustrates that electrons can jump to higher energy levels when they absorb a precise amount of energy, defining these energy jumps as quantized.

Regarding the n values corresponding to the distribution of electrons across the periodic table, for example, an atom of sodium (Na) with 11 electrons, would have two electrons in the first energy level (n=1), eight in the second (n=2), and one electron in the third energy level (n=3), making sodium highly reactive due to having only one electron in its outer shell.

Answer 2

Yes, the elements can go beyond the 5th principal energy level.

As the filling of electrons in the orbital depends on the atomic number of atom. The orbitals are filled with electrons in increasing order of energy of the orbitals. The increasing order of the energy of the orbitals is shown in the image.

From the image it is clear that when the
`5p` orbital is completely filled, the next electron will go to
`6s` orbital.

For example:

The electronic configuration of ruthenium,
`Ru` is
`Kr4d^(7)5s^(1)`

The electronic configuration of polonium,
`Po` is
`Xe6s^(2)4f^(14)5d^(10)6p^(4)`.