Choose the element with the more negative (more exothermic) electron affinity from each pair. b. B or S

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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 negative electron affinity indicates a greater tendency to accept an electron.

Identify the position of each element in the periodic table: Boron (B) is in Group 13 and Period 2, while Sulfur (S) is in Group 16 and Period 3.

Recall the general trend for electron affinity in the periodic table: Electron affinity generally becomes more negative across a period from left to right and less negative down a group.

Compare the elements based on their positions: Since Sulfur (S) is to the right of Boron (B) in the same period, it is expected to have a more negative electron affinity.

Conclude which element has the more negative electron affinity: Based on periodic trends, Sulfur (S) is expected to have a more negative (more exothermic) electron affinity than Boron (B).

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Electron Affinity

Electron affinity is the amount of energy released when an electron is added to a neutral atom in the gas phase. A more negative electron affinity indicates a greater release of energy, meaning the atom has a stronger attraction for the added electron. This property is crucial for understanding how elements interact with electrons and form ions.

Trends in Electron Affinity

Electron affinity varies across the periodic table, generally increasing (becoming more negative) from left to right and decreasing (becoming less negative) from top to bottom. This trend is influenced by atomic size and effective nuclear charge, which affect how tightly an atom can hold onto its electrons. Recognizing these trends helps predict the behavior of elements in chemical reactions.

Comparison of Elements

When comparing elements like boron (B) and sulfur (S), it is essential to consider their positions in the periodic table. Sulfur, being further to the right and lower in the table than boron, typically has a more negative electron affinity due to its higher effective nuclear charge and smaller atomic radius, which allows it to attract additional electrons more effectively.