Open Question
Why is the electron affinity of each group 5A element more positive than that of each corresponding group 4A element? Use the outer electron configurations for these columns to suggest a reason for this observation.
10. Periodic Properties of the Elements
Periodic Trend: Electron Affinity
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Based on general trends in electron affinity, which of the elements listed is most likely to have the most negative electron affinity?
A
Al
B
Si
C
S
D
Cl
Verified step by step guidance1
Understand the concept of electron affinity: Electron affinity is the energy change that occurs when an electron is added to a neutral atom in the gaseous state. A more negative electron affinity indicates a greater tendency to gain an electron.
Identify the general trend in electron affinity across the periodic table: Electron affinity generally becomes more negative as you move from left to right across a period due to increasing nuclear charge, which attracts electrons more strongly.
Consider the position of each element in the periodic table: Al (Aluminum), Si (Silicon), and S (Sulfur) are all in the same period, but Cl (Chlorine) is further to the right in the same period.
Recognize that elements in Group 17 (Halogens) typically have the most negative electron affinities because they are one electron short of a full valence shell, making them highly eager to gain an electron.
Conclude that Cl (Chlorine), being a halogen and located further to the right in the same period as Al, Si, and S, is most likely to have the most negative electron affinity.
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