Multiple Choice
Periodic Trend: Ionization Energy (Simplified) Which element has the highest first ionization energy?
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9. Electrons in Atoms and the Periodic Table
Periodic Trend: Ionization Energy (Simplified)
Multiple Choice
Rank the following elements in order of increasing ionization energy:Br, F, Ga, K and Se.
A
Ga < K < Br < Se < F
B
Ga < Br < K < Se < F
C
K < Se < Ga < Br < F
D
K < Ga < Se < Br < F
E
K < Ga < Se < F < Br
Verified step by step guidance1
Understand the concept of ionization energy: Ionization energy is the energy required to remove an electron from an atom in its gaseous state. Generally, ionization energy increases across a period (from left to right) and decreases down a group (from top to bottom) in the periodic table.
Identify the position of each element in the periodic table: K (Potassium) is in Group 1, Ga (Gallium) is in Group 13, Se (Selenium) is in Group 16, Br (Bromine) is in Group 17, and F (Fluorine) is also in Group 17.
Apply the periodic trend: Since ionization energy increases across a period, elements further to the right in the same period will have higher ionization energies. Therefore, F will have a higher ionization energy than Br, and Br will have a higher ionization energy than Se.
Consider the group trend: Ionization energy decreases down a group, so K, being in Group 1 and lower in the periodic table, will have the lowest ionization energy. Ga, being in Group 13, will have a higher ionization energy than K but lower than Se, Br, and F.
Rank the elements based on the trends: Based on the periodic trends, the order of increasing ionization energy is K < Ga < Se < Br < F.
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