Multiple Choice
Arrange the following elements in order from greatest to least tendency to accept an electron (i.e., from highest to lowest electron affinity): Cl, Na, S, P.
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10. Periodic Properties of the Elements
Periodic Trend: Electron Affinity
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Arrange the following elements in order of increasing electron affinity: Cl, Na, S, P.
A
P < S < Na < Cl
B
S < P < Na < Cl
C
Na < P < S < Cl
D
Cl < S < P < Na
Verified step by step guidance1
Understand that electron affinity (EA) is the energy change when an atom gains an electron; generally, a higher (more negative) EA means the atom more readily accepts an electron.
Recall periodic trends: EA generally increases across a period from left to right and decreases down a group in the periodic table.
Identify the positions of the elements: Na is in Group 1 (alkali metals), P and S are in Period 3 with P in Group 15 and S in Group 16, and Cl is in Group 17 (halogens).
Based on trends, Na (Group 1) will have the lowest EA, Cl (Group 17) the highest, and P and S will be in between, with S typically having a higher EA than P because it is to the right in the same period.
Arrange the elements in order of increasing electron affinity as: Na < P < S < Cl.
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