Why do noble gases rarely form bonds with other atoms?

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Dec 19, 2017

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All noble gases have the perfect amount of electrons needed to be stable already.

Explanation:

All noble gases have the perfect amount of electrons to be stable (2, 10, 18, 36, 54...). There would, therefore, be no need to react with any other atom, as it would involve giving up or gaining electrons, making them unstable again. It is possible to bond a noble gas with another atom. But it would immediately decompose back into its previous state (alone).

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Paul G. Share
Dec 19, 2017

Answer:

noble gases have a stable electronic configuration and don't form bonds * with any other element due to their stable octet.

Explanation:

The outermost electron shell (ie. valence shell) is the region where elements will hybridize and share electrons in order to achieve a stable octet.

Noble gases possess an octet in their ground state, as such they will not bond to other elements.

    • highly electronegative elements such as fluorine (highly unstable element) are able to force heavier noble gases such as Xenon to hybridize into the d-shell and allow for bonds to form - this usually involves an exception to the octet rule whereby more than 4 pairs of electrons are found around the Xenon atom.
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