contestada

Which explains the change in ionization energy that occurs between removing
the first and second electrons from an
atom?
O The ionization energy decreases because the ratio of the protons to electrons increases.
O The ionization energy increases because the ratio of the protons to electrons increases.
O The ionization
energy decreases because the ratio of the protons to electrons decreases.
O The ionization energy increases because the ratio of the protons to electrons decreases.

Respuesta :

bharathparasad577

The ionization energy increases as the ration of protons to electrons increases.

On the periodic table, as we move from left to right through a period, the initial ionization energy rises. This is due to the outermost electron becoming more closely bound to the nucleus as the nuclear charge increases.

Ionization energy - the energy needed to remove an electron from a gaseous atom, is the one that best exemplifies periodic behavior.

The energy needed to remove each additional electron from an atom grows gradually, with the removal of an electron from a filled inner shell causing a significant increase.

A stable atom becomes electrically imperfect or imbalanced if we remove one of its electrons. In other words, the nucleus's protons (positive charges) outnumber its electrons (negative charges). It is a positive ion because the atom has a plus-one charge after losing an electron.

Therefore on removing the second electron more ionization energy will be required than first. So option D is correct.

To learn more about ionization energy refer- https://brainly.com/question/5880605

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