When a sodium atom reacts with a chlorine atom to form a compound, the electron configuration the ions forming the compound are the same as those in which noble gases?

Md Ariful Islam

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Md Ariful Islam

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The of metals tend to be lost, and for this reason metals TEND to be reducing. And non-metals are electron poor. And as a result they tend to be oxidizing. (This tendency is another manifestation of electronic structure.)

Sodium metal and dichlorine thus tend to be involved in redox phenomena:

$Na(s) + 1/2Cl_2 rarr Na^(+)Cl^(-)$

Given the electronic configuration of the reactants, this redox transfer means that each species shares the electronic configuration of it nearest inert gas neighbourL i.e. $Na^(+)-=[Ne] $; $Cl^(-)-=[Ar] $. Each species is still a charged ion, clearly capable of electrostatic interaction, yets its valence electronic shell has been filled and stabilized.

And please look at to confirm these configurations.

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