A particular element has the following values for its first four ionization energies: 900, 1760, 14,800 and 21,000kJ/mol

A particular element has the following values for its first four ionization energies: 900, 1760, 14,800 and 21,000kJ/mol. Without consulting a list of ionization energy values, determine what group in the periodic table this element belong in.

Expert Solution

Since the third ionisation energy is quite large as compared to second ionisation energy, it means that before removing the third electron, configuration must be stable. So, the two electrons can be easily taken out from the shell, this means that the element is in the second group.

queen_honey_blossom answered 2 years ago

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