Multiple Choice
Rank the following elements by electron affinity, from most positive to most negative EA value: Na, Cl, S, Ar.
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10. Periodic Properties of the Elements
Periodic Trend: Electron Affinity
Multiple Choice
Determine which atom in the following set has the most exothermic electron affinity:N, O, C, B, Ne
A
N
B
O
C
C
D
B
E
Ne
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 to form a negative ion. A more exothermic electron affinity means the atom releases more energy when gaining an electron.
Consider the periodic trend: Generally, electron affinity becomes more exothermic across a period from left to right due to increasing nuclear charge, which attracts the added electron more strongly.
Analyze the given elements: The elements provided are N, O, C, B, and Ne. These elements are in the second period of the periodic table.
Evaluate the electron configurations: Oxygen (O) has a higher nuclear charge than nitrogen (N), carbon (C), and boron (B), making it more likely to have a more exothermic electron affinity. Neon (Ne) is a noble gas with a full valence shell, so it has a very low or even positive electron affinity.
Conclude based on trends and configurations: Oxygen (O) is expected to have the most exothermic electron affinity among the given elements due to its position in the periodic table and its electron configuration.
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