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Answer :
The correct relationship of the elements beryllium, calcium, and strontium regarding their ionization energy is option E: Ca < Sr < Be.
Ionization energy refers to the energy required to remove an electron from an atom or ion in the gas phase. It generally increases from left to right across a period and decreases from top to bottom within a group on the periodic table.
In this case, beryllium (Be), calcium (Ca), and strontium (Sr) all belong to Group 2, also known as the alkaline earth metals. As we move down Group 2, the atomic radius increases, and the outermost electrons are farther away from the nucleus. This results in a decrease in the effective nuclear charge experienced by the valence electrons.
As a consequence, the ionization energy tends to decrease as we move down the group. Among the given options, the correct relationship is Ca < Sr < Be, with calcium having the lowest ionization energy, followed by strontium, and then beryllium having the highest ionization energy.
This trend is in line with the general periodic trend of ionization energy for elements within the same group on the periodic table. option(E)
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