Consider the first ionization energy of neon and the electron affinity of fluorine. (b) These two quantities have opposite signs. Which will be positive, and which will be negative? (c) Would you expect the magnitudes of these two quantities to be equal? If not, which one would you expect to be larger?

Ionization energy is the energy required to remove an electron from a neutral atom in its gaseous state. For noble gases like neon, this value is typically high due to their stable electron configuration. The process is endothermic, meaning it absorbs energy, resulting in a positive value for ionization energy.

Electron affinity is the energy change that occurs when an electron is added to a neutral atom in the gaseous state. This process can be exothermic, releasing energy, which results in a negative value for electron affinity. For elements like fluorine, which readily gain electrons, the electron affinity is significantly negative, indicating a strong tendency to attract electrons.

While both ionization energy and electron affinity relate to electron interactions, their magnitudes are not expected to be equal. Ionization energy is generally larger than electron affinity because removing an electron from a stable configuration (like neon) requires more energy than adding an electron to a less stable configuration (like fluorine). Thus, the ionization energy of neon will be greater than the electron affinity of fluorine.