Question

Why electronegativity values of inert gases are zero?

Answer 1

Answer:

Explanation:

Because the nobel elements have their outermost orbit completed so they don't want to exchange electron so their electronegativity is zero

Answer 2

Answer:

Electrons within an atom exist in states defined by four quantum numbers: the principle quantum number N, the azimuthal quantum number  l , the magnetic quantum number  ml , and the spin quantum number  ms . The first three define atomic orbitals, and the last ( ms ) is important here because it allows exactly two electrons to occupy one orbital (spin is important for other reasons, but I won’t address them here). Atoms are most stable when they have only unoccupied and fully occupied orbitals. Partially filled orbitals are less stable.

In a noble gas, every orbital from the highest occupied orbital down (up/down refer to energy here) is fully occupied, and every higher energy orbital is completely unoccupied. Gaining an electron changes that so that the highest occupied orbital is only half filled. There are atoms whose highest occupied orbital is a half-filled s orbital: they’re Group 1, called the alkali metals, and very easily ionizable to get to the electron configuration that the noble gas atom started with.

The same properties of orbitals that result in noble gases having 0 electron affinity are also responsible for the octet rule, but understanding which states are more stable is important in order to understand why larger atoms (especially transition metals) don’t necessarily follow the octet rule.

Explanation:

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