deduce the formula of the ion that has a charge of 2+ with the same electron configuration as krypton.

The formula of the ion is Sr²⁺

From the periodic table, we understood that Krypton (Kr) has 36 electrons.

From the question given above, we were told that the ion has the same electronic configuration as krypton. Thus,

The ion also have 36 electrons.

Finally, we shall determine the number of protons in the ion in order to determine the element that form the ion and also the symbol of the element.

Electrons in the ion = 36

Charge on ion = +2

2 = Proton – 36

Collect like terms

Proton = 2 + 36

Considering the period table, the element with 38 protons (i.e atomic number of 38) is strontium with symbol Sr.

Therefore, the formula of the ion with the same electron configuration as krypton is Sr²⁺

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Sr²⁺

Explanation:

Krypton has 36 electrons and an electron configuration of 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6. An ion with a charge of 2+ and 36 electrons is Sr²⁺. Since it has the same amount of electrons, Sr²⁺ also has an electron configuration of 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6.

i'm pretty sure its b i might be wrong though!

58750.08068 is the answer i think