An element has the following first through fourth ionization energies (in kJ/mol): 700; 1500; 7700; 10500....

An element has the following first through fourth ionization energies (in kJ/mol): 700; 1500; 7700; 10500. Deduce to which column of the periodic table it porbably belongs. Give your reasoning

Solutions

Expert Solution

Given that first to fourth ionization energies (in kJ/mol): 700 ; 1500; 7700; 10500

These values corresponds to 2nd column of periodic table i.e. IIA group.

Reason:

The outer electronic configuration of IIA group is ns2.

The two outer 's' electrons require less energy for removal. So 1st and 2nd IP values are less.

After removal of two electrons, IIA group elements attain noble gas configuration.

Therefore, 3rd and 4th ionization energie values are higher than 1st and 2nd ionization energies.

Hence, given ionization energy values corresponds to 2nd column of periodic table i.e. IIA group.

Exactly, the above ionization energies are of Magnesium.

queen_honey_blossom answered 1 year ago

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