Which has the more negative electron affinity, Br or Br⁻?

Verified step by step guidance

Step 1: 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.

Step 2: Consider the electron affinity of a neutral bromine atom (Br). When a neutral bromine atom gains an electron, it becomes a bromide ion (Br⁻), and this process releases energy, indicating a negative electron affinity.

Step 3: Analyze the electron affinity of the bromide ion (Br⁻). Adding an electron to an already negatively charged ion (Br⁻) is less favorable because of electron-electron repulsion, and it requires energy input, resulting in a positive or less negative electron affinity.

Step 4: Compare the two scenarios. The neutral bromine atom (Br) has a more negative electron affinity because it releases energy when gaining an electron, whereas the bromide ion (Br⁻) would require energy to gain an additional electron.

Step 5: Conclude that the neutral bromine atom (Br) has a more negative electron affinity compared to the bromide ion (Br⁻) due to the energy release when forming Br⁻ from Br.

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.

Comparison of Atoms and Ions

When comparing the electron affinity of a neutral atom like bromine (Br) to that of its anion (Br⁻), it is essential to consider the electronic structure. The addition of an electron to Br results in Br⁻, which already has an extra electron, affecting its ability to attract another electron due to increased electron-electron repulsion.

Trends in the Periodic Table

Electron affinity generally increases (becomes more negative) across a period from left to right and decreases down a group in the periodic table. Understanding these trends helps predict the behavior of elements like bromine, as its position in the periodic table influences its electron affinity compared to its anion.

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Textbook Question

Why does ionization energy increase regularly across the periodic table from group 1A to group 8A, whereas electron affinity increases irregularly from group 1A to group 7A and then falls dramatically for group 8A?

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What is the relationship between the electron affinity of a singly charged cation such as Na+ and the ionization energy of the neutral atom?

Textbook Question

Why is energy usually released when an electron is added to a neutral atom but absorbed when an electron is removed from a neutral atom?

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Water superheated under pressure to 200 °C and 750 atm has Kw = 1.5 * 10-11. What is 3H3O+ 4 and 3OH-4 at 200 °C? Is the water acidic, basic, or neutral?