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Why does the lightest halogen, which is also the most chemically reactive, exhibit a decrease in reactivity as you move down the column of halogens in the periodic table? Explain this trend in terms of periodic properties.
10. Periodic Properties of the Elements
Periodic Trend: Electron Affinity
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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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