Cations are formed when an atom loses electrons from its valence shell. The electronic configuration of an atom determines how likely it is to lose electrons. Therefore, cations with the same electronic configuration will be formed by elements in the same group of the periodic table.
One such group is Group 2, also known as the alkaline earth metals. The electronic configuration of these elements is ns2, where "n" represents the principal quantum number. The elements in Group 2 are beryllium (Be), magnesium (Mg), calcium (Ca), strontium (Sr), barium (Ba), and radium (Ra).
All these elements form cations with the same electronic configuration as they lose their two valence electrons to achieve the stable configuration of the noble gas that precedes them in the periodic table. Therefore, beryllium cation (Be2+), magnesium cation (Mg2+), calcium cation (Ca2+), strontium cation (Sr2+), barium cation (Ba2+), and radium cation (Ra2+) all have the same electronic configuration: 1s2 2s2 or equivalent.
Hence, the elements in Group 2 of the periodic table form cations with the same electronic configuration.
Highlight the element(s) that form cations with the same electronic configuration as
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