A hypothetical element, X, has the following ionization energy values: First ion

Question

A hypothetical element, X, has the following ionization energy values:
First ionization energy: 900 kJ/mol
Second ionization energy: 1750 kJ/mol
Third ionization energy: 14,900 kJ/mol
Fourth ionization energy: 21,000 kJ/mol

Another element, Y, has the following ionization energy values:
First ionization energy: 1200 kJ/mol
Second ionization energy: 2500 kJ/mol
Third ionization energy: 19,900 kJ/mol
Fourth ionization energy: 26,000 kJ/mol

What charge would you expect element X to have when it forms an ion?

Would an atom of Y be smaller or larger than an atom of X? Explain your reasoning.

Explanation / Answer

X has +2 charge It has low first and second ionization energies. Hence it can give 2 electrons easily. Hence it will have +2 charge Y has larger ionization energy than X Hence atom of Y is smaller than that of X(Same group)

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