Question

Write equations corresponding to the following. a. the fourth ionization energy of Se b. the electron affinity of \(\mathrm{S}^{-}\) c. the electron affinity of \(\mathrm{Fe}^{3+}\) d. the ionization energy of \(\mathrm{Mg}\)

Short answer

a. \(Se^{3+} + IE_{4} \rightarrow Se^{4+} + e^{-}\) b. \(S^{-} + e^{-} \rightarrow S^{2-} + EA\) c. \(Fe^{3+} + e^{-} \rightarrow Fe^{2+} + EA\) d. \(Mg + IE \rightarrow Mg^{+} + e^{-}\)

Step-by-step solution

a. The fourth ionization energy of Se

To find the fourth ionization energy of Se, we need to determine the initial and final states of the selenium atom in this process. After three ionizations, we have the Se³⁺ ion (three electrons removed). The fourth ionization implies the removal of another electron from this ion. The general formula for ionization energy is: Atom/ion + Ionization Energy → Atom/ion⁺ + e⁻ Applying this to Se: Se³⁺ + IE₄ → Se⁴⁺ + e⁻

b. The electron affinity of \(\mathrm{S}^{-}\)

Electron affinity refers to the energy change that occurs when an electron is added to a gaseous atom or ion. For this case, we are considering the addition of an electron to a sulfur ion, S⁻. The general formula for electron affinity is: Atom/ion + e⁻ → Atom/ion⁻ + Electron Affinity Applying this to S⁻: S⁻ + e⁻ → S²⁻ + EA

c. The electron affinity of \(\mathrm{Fe}^{3+}\)

In this case, we are considering the electron affinity of an iron ion, Fe³⁺. We need to add an electron to this ion. Using the general formula for electron affinity: Fe³⁺ + e⁻ → Fe²⁺ + EA

d. The ionization energy of \(\mathrm{Mg}\)

For the ionization energy of magnesium, Mg, we need to remove one electron from the gaseous atom. Using the general formula for ionization energy: Mg + IE → Mg⁺ + e⁻