A
The electron configuration of sodium is 2.8.1. The ionization energy of sodium is relatively low because it has a low mass number (hence its valence electron is loosely held by the nucleus) within its period and it only needs to lose only one electron to achieve stable electron configuration of 2.8
Explanation:
Argon (2.8.8) is already a stable element hence low to react.
The electron configuration of sulfur is 2.8.6. It's ionization energy is too high (due it high mass number within it period), hence it will take much energy to lose an electron as opposed to gaining 2 electrons to achieve a stable electron configuration of 2.8.8.
This same principle applies with silicon which has an electron configuration of is 2.8.4.
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Answer:
Sodium
Explanation:
Sodium is alkali metal. All metal form cation by losing their valance electrons.
Sodium is member of group one it has one valance electron. It easily lose the electron and get stable electronic configuration by completing the octet.
When an atom lose electron cation is formed and when it gain electron anion is formed.
So sodium atom when lose its one valance electron it form cation with charge of +1.
While argon already have complete octet it can not form ion.
while valency of silicon is four and it form four covalent bond easily.
While sulfur form anion by gaining the electrons.
