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Which of the following species will have the highest ionization energy?
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10. Periodic Properties of the Elements
Periodic Trend: Ionization Energy
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Which of the following best describes the overall trend in ionization energy across the periodic table?
A
Ionization energy remains constant across both periods and groups.
B
Ionization energy increases from right to left across a period and from top to bottom within a group.
C
Ionization energy decreases from left to right across a period and from top to bottom within a group.
D
Ionization energy increases from left to right across a period and from bottom to top within a group.
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Understand that ionization energy is the energy required to remove an electron from a gaseous atom or ion.
Recall that across a period (left to right), the nuclear charge increases while the shielding effect remains relatively constant, causing electrons to be held more tightly and thus increasing ionization energy.
Recognize that down a group (top to bottom), additional electron shells are added, increasing the distance between the nucleus and the outermost electron and increasing shielding, which lowers the ionization energy.
Summarize the trend: ionization energy generally increases from left to right across a period and decreases from top to bottom within a group.
Compare the given options to this understanding and identify the correct description of the trend.
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