Multiple Choice
Determine which atom in the following set has the largest electron affinity: N, O, C, B, Ne
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3. Ionic Compounds
Periodic Trend: Electron Affinity (Simplified)
Multiple Choice
Rank the following elements in order of increasing electron affinity: Cs, Hg, F, S
A
Hg < S < F < Cs
B
Hg < F < S < Cs
C
Cs < S < F < Hg
D
Cs < S < Hg < F
E
Cs < Hg < S < F
Verified step by step guidance1
Understand the concept of electron affinity: Electron affinity is the amount of energy released when an electron is added to a neutral atom in the gaseous state to form a negative ion. Generally, elements with higher electron affinity values are more likely to gain electrons.
Recall the periodic trend: Electron affinity generally increases across a period from left to right and decreases down a group in the periodic table. This is because atoms become smaller across a period, allowing them to attract additional electrons more strongly.
Identify the positions of the given elements in the periodic table: Cs (Cesium) is in Group 1, Period 6; Hg (Mercury) is in Group 12, Period 6; S (Sulfur) is in Group 16, Period 3; F (Fluorine) is in Group 17, Period 2.
Apply the periodic trend to the given elements: Since Cs is in Group 1, it has a low electron affinity. Hg, being a transition metal, also has a relatively low electron affinity. S and F, being nonmetals, have higher electron affinities, with F having the highest due to its position in Group 17.
Rank the elements based on the trend: Cs, being in Group 1, has the lowest electron affinity, followed by Hg. S, being a nonmetal, has a higher electron affinity than Hg, and F, being in Group 17, has the highest electron affinity. Therefore, the order is Cs < Hg < S < F.
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