Choose the element with the more negative (more exothermic) electron affinity in each pair. a. Mg or S b. K or Cs c. Si or P d. Ga or Br

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1. Electron affinity is the energy change that occurs when an electron is added to a neutral atom to form a negative ion. Generally, atoms with a larger atomic radius have a less negative (less exothermic) electron affinity because the added electron is further from the nucleus and therefore less strongly attracted to it.

2. For pair a (Mg or S), Sulfur (S) is to the right of Magnesium (Mg) on the periodic table, which means it has a smaller atomic radius and therefore a more negative electron affinity.

3. For pair b (K or Cs), Potassium (K) is above Cesium (Cs) on the periodic table, which means it has a smaller atomic radius and therefore a more negative electron affinity.

4. For pair c (Si or P), Phosphorus (P) is to the right of Silicon (Si) on the periodic table, which means it has a smaller atomic radius and therefore a more negative electron affinity.

5. For pair d (Ga or Br), Bromine (Br) is to the right of Gallium (Ga) on the periodic table, which means it has a smaller atomic radius and therefore a more negative electron affinity.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Electron Affinity

Electron affinity is the amount of energy released when an electron is added to a neutral atom in the gas phase, forming a negative ion. A more negative electron affinity indicates a greater tendency for an atom to gain an electron, which is often associated with the stability of the resulting anion. Understanding this concept is crucial for comparing elements, as it helps predict their reactivity and the energy changes involved in electron transfer.

Trends in the Periodic Table

Periodic trends refer to the predictable patterns observed in the properties of elements as you move across a period or down a group in the periodic table. For electron affinity, elements on the right side of the table (like halogens) generally have more negative values compared to those on the left (like alkali metals). Recognizing these trends allows for informed predictions about the electron affinity of different elements.

Comparison of Elements

When comparing elements, it is essential to consider their positions in the periodic table, as this influences their electron configurations and, consequently, their chemical properties. For example, elements in the same group may exhibit similar behaviors, while those in different groups can show significant differences. This comparative analysis is vital for determining which element in a pair has a more negative electron affinity.