Og is the noble gas after rn. to go from [rn] to [og], you must fill four subshells (s, p, d, and f) with a total of 32 electrons. thus, the atomic numbers of 6th and 7th period elements of the same group differ by 32. to go from [og] to the next noble gas, however, you would theoretically fill five subshells (s, p, d, f, and g). how many electrons are needed to fill all five subshells?

Answer : 50 electrons are needed to fill all five subshells

Explanation :

To move from Rn to Og, we need to fill 4 subshells which are s, p d & f.

The maximum number of electrons that can be added to each orbital are given below.

s = 2 e⁻

p = 6 e⁻

d = 10 e⁻

f = 14 e⁻

If we add all these electrons, we get 2 + 6 + 10 + 14 = 32 electrons.

We need to add 32 electrons to the atomic number of Rn to get the atomic number of Og.

Hence we say that the atomic numbers of 6th and 7th period elements of the same group differ by 32.

To go from Og to the next noble gas, we have to theoretically fill 5 subshells.

The maximum electrons that can be added to g orbital are 18.

Therefore in order to go from Og to next element, we would add

2 + 6 + 10 + 14 + 18 = 50 electrons.

50 electrons are needed to fill all five subshells.

a 20-cm-long, cylindrical graphite (pure carbon) rod is inserted into an oxidizing atmosphere at 1145 k and 1.013 x 105 pa pressure. the oxidizing process is limited by the diffu- sion of oxygen counterflow to the carbon monoxide that is formed on the cylindrical surface.