Saffron, Hawa, and Connor are comparing the energy required to remove an electron from different elements. Which of the following sequences corresponds to a correct trend in ionization energy? Rbgt Kgt Nagt Li Clgt Sgt Pgt Al Rbgt Srgt 1gt Xe Srgt Cagt Mggt Be

The correct sequence that corresponds to a trend in ionization energy is:<br /><br />$Sr\gt Ca\gt Mg\gt Be$<br /><br />Ionization energy is the energy required to remove an electron from an atom or ion. It generally increases across a period (left to right) and decreases down a group (top to bottom) in the periodic table.<br /><br />In the given options, the sequence $Sr\gt Ca\gt Mg\gt Be$ follows the correct trend in ionization energy. As we move from Sr to Ca, Mg, and Be, the elements are in the same group (Group 2) of the periodic table, and the ionization energy increases as we move up the group.