The first four ionization energies in kJ/mol of a certain second-row element are 801, 2427, 3660,...

The first four ionization energies in kJ/mol of a certain second-row element are 801, 2427, 3660, and 25,025. What is the likely identity of the element?

Expert Solution

Consider the following graph of the ionization energies.

As seen, there is a spike in the 4th ionization energy of the element. This means that after the 3rd ionization, the element reaches a stable configuration. Therefore, the stable ionic form of the element is +3. When considering the second period, the element with the stable +3 ionic form is boron.

The element is BORON

queen_honey_blossom answered 2 years ago

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