Choose the best response for the following. The ionization...

Choose the best response for the following. The ionization energy for the chlorine atom is equal in magnitude to the electron affinity for a. the $\mathrm{Cl}$ atom. b. the $\mathrm{Cl}^{-}$ ion. c. the $\mathrm{Cl}^{+}$ ion. d. the $\mathrm{F}$ atom. e. none of these. Explain each choice. Justify your choice, and for the choices you did not select, explain what is incorrect about them.

Choose the best response for the following. The ionization energy for the chlorine atom is equal in magnitude to the electron affinity for
a. the $\mathrm{Cl}$ atom.
b. the $\mathrm{Cl}^{-}$ ion.
c. the $\mathrm{Cl}^{+}$ ion.
d. the $\mathrm{F}$ atom.
e. none of these.
Explain each choice. Justify your choice, and for the choices you did not select, explain what is incorrect about them.

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Key Concepts

Reversibility of Electron Transfer Processes

The concept of reversibility in electron transfer processes explains that the energy change for a process is equal in magnitude but opposite in sign to that of its reverse process. For example, the energy released when an electron is added to a neutral atom (electron affinity) is equal in magnitude to the energy required to remove that extra electron from the negative ion (ionization energy or electron detachment energy). This relationship is critical in understanding why the ionization energy of a negative ion, such as Cl?, is equal in magnitude to the electron affinity of its corresponding neutral atom.

Electron Affinity

Electron affinity refers to the energy change when an electron is added to a neutral atom in the gaseous state, forming a negatively charged ion. In many cases, this process releases energy, and the magnitude of electron affinity indicates the tendency of an atom to accept an electron.

Ionization Energy

Ionization energy is defined as the energy required to remove an electron from an atom or ion in the gas phase. It quantifies how strongly an electron is held by the particle; a higher ionization energy indicates that more energy is needed to strip an electron, resulting in the formation of a positively charged ion.

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