91Ó°ÊÓ

Radioactive elements are fascinating for their ability to spontaneously emit radiation as they decay. Element 118, known as Oganesson (Og), falls into this category.
Since it's a heavy element with a high atomic number, it is inherently unstable. This instability causes it to decay quickly into lighter elements. These super-heavy elements, like Oganesson, are created artificially in laboratories, and their half-lives often last only a few milliseconds.
Understanding radioactivity is crucial as it impacts the element's stability and existence, which is why most elements beyond Bismuth are radioactive. Radioactivity means that these elements will not exist naturally for long periods because they decay into more stable forms.

Noble gases are located in Group 18 of the periodic table and include elements like Helium, Neon, and Argon. They are known for their unique characteristic of being mostly inert, meaning they do not readily react with other elements.
Oganesson is the newest and heaviest member of this group. Noble gases are distinguished by their full valence electron shells, which contribute to their low reactivity.
At standard conditions, noble gases are colorless, odorless, and have low boiling and melting points, existing as gases. However, the properties can change for heavier noble gases, where Oganesson might deviate slightly due to its higher mass.

The periodic table arranges elements based on their atomic number and similar chemical properties. One notable trend is that elements in the same group share characteristics, like those seen in noble gases.
As you move down any group in the periodic table, atomic size generally increases, and with that, other properties such as ionization energy and electron affinity tend to decrease.
In the case of noble gases, the heavier the gas, the lower its ionization energy. This decrease is because the outermost electrons are further from the nucleus and feel less of an attraction, making them easier to remove.

Ionization energy is the energy required to remove an electron from an atom in its gaseous state. This is a critical concept in understanding an element's reactivity.
For noble gases like Oganesson, ionization energy typically decreases as you move down the group.
The outer electrons are farther from the nucleus, experience less electrostatic force, and thus, are easier to remove. Oganesson, therefore, would have the lowest ionization energy among the noble gases, adhering to this periodic trend.

Reactivity in noble gases is generally low due to their full valence electron shells. Electrons are arranged in such a way that they don't need to gain or lose electrons, leading to few reactions.
However, heavier noble gases like Xenon can form compounds under specific conditions, showing a degree of reactivity. Oganesson, being heavier than Xenon, might exhibit limited reactivity, but it's still expected to be less reactive than Xenon due to its position in the group.
Understanding these reactivity trends helps in predicting and analyzing the chemical behavior of these elements in various scenarios.