Answer:
Helium, neon, argon, krypton, xenon, and radon.
Explanation:
The chemical elements in group 18 of the periodic chart are the noble gases. They have the most valence electrons that their outer shell can support, making them the most stable. As a result of their inherent stability, they rarely interact with other components.
Other characteristics of the noble gases are that they all conduct electricity, fluoresce, are odorless and colorless, and are used in many conditions when a stable element is needed to maintain a safe and constant environment. These are the 6 noble gases:
- Helium
- Neon
- Argon
- Krypton
- Xenon
- Radon
Although the phrase "inert gases" was once used to describe the noble gases, it is not entirely true given that some of them do participate in chemical processes.
Chemical properties:
Under normal circumstances, the noble gases are nonflammable, tasteless, colorless, and odorless. Because it was earlier thought that they had a valence of zero, or that their atoms couldn't mix with those of other elements to create compounds, they were originally given the group 0 designation in the periodic table. However, it was eventually determined that some do in fact combine to create compounds, which led to the label's demise. Full valence electron shells are present in noble gases. The only electrons that often take part in chemical bonding are valence electrons, which are an atom's outermost electrons. Due to their great stability, complete valence electron shell atoms have little to no inclination to gain or lose electrons and do not frequently establish chemical bonds. But unlike lesser noble gases like helium, larger noble gases like radon are bound together by electromagnetic force less tightly, making it simpler to remove outside electrons from hefty noble gases. The noble gases can be combined with the electron configuration notation to create the noble gas notation as a consequence of a complete shell.
To do this, the electron configuration is written starting with the nearest noble gas that comes before the element in issue, and then it is carried from there. For instance, the noble gas notation is [Ne] 3s2 3p3, whereas the electron notation for phosphorus is 1s2 2s2 2p6 3s2 3p3. In addition to being shorter than writing down the whole notation of atomic orbitals, this more condensed notation makes it simpler to identify elements.
Of all the noble gas compounds that have been created, xenon compounds are the most prevalent. [33] Most of them consist of a xenon atom in the +2, +4, +6, or +8 oxidation state coupled to an extremely electronegative element, such fluorine or oxygen, as in xenon difluoride (XeF).
2), xenon tetrafluoride (XeF
4), xenon hexafluoride (XeF
6), xenon tetroxide (XeO
4), and sodium perxenate (Na
4XeO
6). Xenon reacts with fluorine to form numerous xenon fluorides according to the following equations:
Xe + F2 → XeF2
Xe + 2F2 → XeF4
Xe + 3F2 → XeF6
Some of these compounds have found use in chemical synthesis as oxidizing agents; XeF
2, in particular, is commercially available and can be used as a fluorinating agent.
