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Chapter 7: Problem 131

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 Mg

Short Answer

Expert verified
a. \(\mathrm{Se}^{3+}(g) \rightarrow \mathrm{Se}^{4+}(g) + e^{-}\) b. \(\mathrm{S}^{-}(g) + e^{-} \rightarrow \mathrm{S}^{2-}(g)\) c. \(\mathrm{Fe}^{3+}(g) + e^{-} \rightarrow \mathrm{Fe}^{2+}(g)\) d. \(\mathrm{Mg}(g) \rightarrow \mathrm{Mg}^{+}(g) + e^{-}\)

Step by step solution

01

Identify initial and final species

For the fourth ionization energy, the initial species is Se with three electrons removed, i.e., \(\mathrm{Se}^{3+}\), and the final species is Se with a total of four electrons removed, i.e., \(\mathrm{Se}^{4+}\).
02

Write the equation

The equation representing the fourth ionization energy of Se can be written as: \[\mathrm{Se}^{3+}(g) \rightarrow \mathrm{Se}^{4+}(g) + e^{-}\] b. The electron affinity of \(\mathrm{S}^{-}\)
03

Identify initial and final species

Here, the initial species is the \(\mathrm{S}^{-}\) ion and the final species is the \(\mathrm{S}^{2-}\) ion.
04

Write the equation

The equation representing the electron affinity of \(\mathrm{S}^{-}\) can be written as: \[\mathrm{S}^{-}(g) + e^{-} \rightarrow \mathrm{S}^{2-}(g)\] c. The electron affinity of \(\mathrm{Fe}^{3+}\)
05

Identify initial and final species

For this equation, the initial species is the \(\mathrm{Fe}^{3+}\) ion and the final species is \(\mathrm{Fe}^{2+}\).
06

Write the equation

The equation representing the electron affinity of \(\mathrm{Fe}^{3+}\) can be written as: \[\mathrm{Fe}^{3+}(g) + e^{-} \rightarrow \mathrm{Fe}^{2+}(g)\] d. The ionization energy of Mg
07

Identify initial and final species

In this case, the initial species is the neutral Mg atom, and the final species is the \(\mathrm{Mg}^{+}\) ion.
08

Write the equation

The equation representing the ionization energy of Mg can be written as: \[\mathrm{Mg}(g) \rightarrow \mathrm{Mg}^{+}(g) + e^{-}\]

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Most popular questions from this chapter

What are the possible values for the quantum numbers \(n, \ell,\) and $m_{\ell} ?$

In defining the sizes of orbitals, why must we use an arbitrary value, such as 90% of the probability of finding an electron in that region?

Which of the following electron configurations correspond to an excited state? Identify the atoms and write the ground-state electron configuration where appropriate. a. 1\(s^{2} 2 s^{2} 3 p^{1}\) b. 1\(s^{2} 2 s^{2} 2 p^{6}\) c. 1\(s^{2} 2 s^{2} 2 p^{4} 3 s^{1}\) d. \([\mathrm{Ar}] 4 s^{2} 3 d^{5} 4 p^{1}\) How many unpaired electrons are present in each of these species?

One bit of evidence that the quantum mechanical model is “correct” lies in the magnetic properties of matter. Atoms with unpaired electrons are attracted by magnetic fields and thus are said to exhibit paramagnetism. The degree to which this effect is observed is directly related to the number of unpaired electrons present in the atom. Consider the ground-state electron configurations for Li, N, Ni, Te, Ba, and Hg. Which of these atoms would be expected to be paramagnetic, and how many unpaired electrons are present in each paramagnetic atom?

The electron affinity for sulfur is more exothermic than that for oxygen. How do you account for this?
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