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Chapter 7: Problem 113

Order the atoms in each of the following sets from the least exothermic electron affinity to the most. a. \(\mathrm{S}, \mathrm{Se}\) b. \(\mathrm{F}, \mathrm{Cl}, \mathrm{Br}, \mathrm{I}\)

Short Answer

Expert verified
a. From least exothermic electron affinity to the most: \(\mathrm{Se} < \mathrm{S}\) b. From least exothermic electron affinity to the most: \(\mathrm{I} < \mathrm{Br} < \mathrm{Cl} < \mathrm{F}\)

Step by step solution

01

Analyze the sets of atoms

We are given two sets of atoms: a. S, Se b. F, Cl, Br, I Set (a) contains sulfur (S) and selenium (Se), which are present in the same group (Group 16). Since they are in the same group, we can use the trend of electron affinity in a group to compare their electron affinities. Set (b) contains fluorine (F), chlorine (Cl), bromine (Br), and iodine (I), which are present in the same group (Group 17). We can also use the trend of electron affinity in a group to compare their electron affinities.
02

Apply the trend of electron affinity in groups

According to the trend, electron affinity becomes less exothermic as we move down a group. Based on this trend, we can now order the given atoms. Set (a): S is above Se in Group 16. So, S has a more exothermic electron affinity than Se. Therefore, the order is Se < S. Set (b): Since F, Cl, Br, and I are in the same group, we can arrange them in the order of least to most exothermic electron affinity from bottom to top: I < Br < Cl < F.
03

Present the final order

Now that we have ordered the atoms in the given sets, here's the final order: a. From least exothermic electron affinity to the most: Se < S b. From least exothermic electron affinity to the most: I < Br < Cl < F

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Most popular questions from this chapter

Assume that we are in another universe with different physical laws. Electrons in this universe are described by four quantum numbers with meanings similar to those we use. We will call these quantum numbers \(p, q, r\), and \(s .\) The rules for these quantum numbers are as follows: \(p=1,2,3,4,5, \ldots\) \(q\) takes on positive odd integers and \(q \leq p\) \(r\) takes on all even integer values from \(-q\) to \(+q\). (Zero is considered an even number.) \(s=+\frac{1}{2}\) or \(-\frac{1}{2}\) a. Sketch what the first four periods of the periodic table will look like in this universe. b. Wh?t are the atomic numbers of the first four elements you would expect to be least reactive? c. Give an example, using elements in the forst four rows, of ionic compounds with the formulas \(\mathrm{XY}, \mathrm{XY}_{2}, \mathrm{X}_{2} \mathrm{Y}, \mathrm{XY}_{3}\), and \(\mathrm{X}_{2} \mathrm{Y}_{3}\) d. How many electrons can have \(p=4, q=3 ?\) e. How many electrons can have \(p=3, q=0, r=0 ?\) f. How many electrons can have \(p=6\) ?

Which of the following sets of quantum numbers are not allowed in the hydrogen atom? For the sets of quantum numbers that are incorrect, state what is wrong in each set. a. \(n=3, \ell=2, m_{\ell}=2\) b. \(n=4, \ell=3, m_{\ell}=4\) c. \(n=0, \ell=0, m_{\ell}=0\) d. \(n=2, \ell=-1, m_{\ell}=1\)

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?

Photogray lenses incorporate small amounts of silver chloride in the glass of the lens. When light hits the AgCl particles, the following reaction occurs: $$ \mathrm{AgCl} \stackrel{h v}{\longrightarrow} \mathrm{Ag}+\mathrm{Cl} $$ The silver metal that is formed causes the lenses to darken. The enthalpy change for this reaction is \(3.10 \times 10^{2} \mathrm{~kJ} / \mathrm{mol}\). Assuming all this energy must be supplied by light, what is the maximum wavelength of light that can cause this reaction?

Three elements have the electron configurations \(1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6}\), \(1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2}\), and \(1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 4 s^{1}\). The first ionization energies of these elements (not in the same order) are \(0.419,0.735\), and \(1.527 \mathrm{MJ} / \mathrm{mol}\). The atomic radii are \(1.60,0.98\), and \(2.35 \AA\). Identify the three elements, and match the appropriate values of ionization energy and atomic radius to each configuration.
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