The outer, or valence, shells of the noble gases are completely filled, so that they neither donate to nor accept electrons from other atoms. As a result, noble gas atoms cannot form chemical bonds, so they remain pure. Most elements do not have filled outer shells. Atoms that have nearly full outer shells readily accept electrons, and those with nearly empty outer shells readily donate electrons. "Donated" electrons and "accepted" electrons are simply electrons that are attracted to the nuclei of two atoms. That shared attraction holds the two atoms together. Thus most elements can form chemical bonds.
On the contrary, noble gases are not likley to form bonds.
Noble gases have an octet of electrons in their outer shell.
Some compounds of Ar, Kr, Xe and Rn are known but these are very reactive and in some cases very unstable.
the tendency toward a complete octet of electrons in a bonded atom reflects the natural tendency for a system to move to the lowest energy state possible.
Because of their electronic structure that makes them unreactive
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Metals , generally, have electronic configuration: with outermost electron having 1,2 or 3. Since, they can easily attain noble gas configuration to attain stability; they readily loose electron.
The noble gas electron configuration of radon is [Xe]4f145d106s26p6.
Calcium loses two electrons to obtain a noble-gas electron configuration.
Well first of all your question does not make any sense due to the fact that Electron configuration and Noble gass configuration are two completely different things Electron configuration: 1s22s22p63s23p64s23d104p65s24d105p66s24f145d106p67s2 Noble gas configuration: [Rn] 7s2
The electron configuration of ununoctium is: [Ra] 5f14 6d10 7s2.
Although the formation of an octet is the most stable electron configuration, other electron configurations provide stability. These relatively stable electron arrangements are referred to a pseudo-noble gas configuration. Although the formation of an octet is the most stable electron configuration, other electron configurations provide stability. These relatively stable electron arrangements are referred to a pseudo-noble gas configuration.
The "Noble gas electron configuration," or the condensed electron configuration, for F is [He] 2s2 3p5.
Metals , generally, have electronic configuration: with outermost electron having 1,2 or 3. Since, they can easily attain noble gas configuration to attain stability; they readily loose electron.
The noble gas electron configuration of radon is [Xe]4f145d106s26p6.
Losing an electron cesium has a noble gas configuration.
The electron configuration of boron is: [He]2s2.2p1.
Calcium loses two electrons to obtain a noble-gas electron configuration.
By acquiring noble gas configuration elements become stable .
Well first of all your question does not make any sense due to the fact that Electron configuration and Noble gass configuration are two completely different things Electron configuration: 1s22s22p63s23p64s23d104p65s24d105p66s24f145d106p67s2 Noble gas configuration: [Rn] 7s2
[noble gas]ns2 np6
The electron configuration of ununoctium is: [Ra] 5f14 6d10 7s2.
The electron configuration and noble gas core for Li+ is that of He: Li+: (1s2, 2s0)