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Which of the following elements has the highest ionization energy?
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10. Periodic Properties of the Elements
Periodic Trend: Ionization Energy
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Consider the elements bromine and chlorine. Which element has a higher first ionization energy?
A
Neither has a measurable ionization energy
B
Chlorine
C
Bromine
D
Both have the same ionization energy
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Recall that the first ionization energy is the energy required to remove one electron from a neutral atom in the gaseous state.
Understand that ionization energy generally increases across a period (left to right) in the periodic table and decreases down a group (top to bottom) because of increasing atomic radius and electron shielding.
Identify the positions of bromine and chlorine in the periodic table: both are in Group 17 (halogens), but chlorine is in Period 3 and bromine is in Period 4.
Since chlorine is above bromine in the same group, chlorine has a smaller atomic radius and less electron shielding, which means its outer electrons are held more tightly.
Conclude that chlorine has a higher first ionization energy than bromine because it requires more energy to remove an electron from chlorine's smaller, less shielded atom.
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