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Chapter 8: Problem 59

Arrange the elements in each of these groups in order of increasing electron affinity: (a) \(\mathrm{Li}, \mathrm{Na}, \mathrm{K}\) (b) \(\mathrm{F}, \mathrm{Cl}, \mathrm{Br}, \mathrm{I}\)

Short Answer

Expert verified
The elements in group (a) arranged in order of increasing electron affinity are \( \mathrm{K} < \mathrm{Na} < \mathrm{Li} \). The elements in group (b) arranged in order of increasing electron affinity are \( \mathrm{I} < \mathrm{Br} < \mathrm{Cl} < \mathrm{F} \).

Step by step solution

01

Identify Trends in Electron Affinity

It should be known that electron affinity increases across a period from left to right and decreases down a group on the periodic table. This is due to the increase in nuclear charge, decrease in atomic radius, and increase in effective nuclear charge across a period.
02

Arrange Group (a) Elements

The elements in group (a) are \( \mathrm{Li}, \mathrm{Na}, \mathrm{K} \). They are located in the same group in the periodic table hence, we would follow the trend rule that electron affinity decreases down a group. So, the order of increasing electron affinity will be \( \mathrm{K} < \mathrm{Na} < \mathrm{Li} \).
03

Arrange Group (b) Elements

The elements in group (b) are \( \mathrm{F}, \mathrm{Cl}, \mathrm{Br}, \mathrm{I} \). They are also located in the same group in the periodic table, so the trend that electron affinity decreases down a group is also applicable here. Thus, the order of increasing electron affinity will be \( \mathrm{I} < \mathrm{Br} < \mathrm{Cl} < \mathrm{F} \).

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Most popular questions from this chapter

On the basis of their positions in the periodic table, select the atom with the larger atomic radius in each of these pairs: (a) \(\mathrm{Na}, \mathrm{Cs} ;\) (b) Be, \(\mathrm{Ba}\); (c) \(\mathrm{N}, \mathrm{Sb}\) (d) \(\mathrm{F}, \mathrm{Br},(\mathrm{e}) \mathrm{Ne}, \mathrm{Xe}\)

A technique called photo electron spectroscopy is used to measure the ionization energy of atoms. A sample is irradiated with ultraviolet (UV) light, and electrons are ejected from the valence shell. The kinetic energies of the ejected electrons are measured. Because the energy of the UV photon and the kinetic energy of the ejected electron are known, we can write \( h v=I E+\frac{1}{2} m u^{2} \) in which \(\nu\) is the frequency of the UV light, and \(m\) and \(u\) are the mass and velocity of the electron, respectively. In one experiment the kinetic energy of the ejected electron from potassium is found to be \(5.34 \times 10^{-19} \mathrm{~J}\) using a UV source of wavelength \(162 \mathrm{nm}\). Calculate the ionization energy of potassium. How can you be sure that this ionization energy corresponds to the electron in the valence shell (that is, the most loosely held electron)?

Explain why the first electron affinity of sulfur is \(200 \mathrm{~kJ} / \mathrm{mol}\) but the second electron affinity is \(-649 \mathrm{~kJ} / \mathrm{mol}\),

For each pair of elements listed here, give three properties that show their chemical similarity: (a) sodium and potassium and (b) chlorine and bromine.

Ammonium nitrate \(\left(\mathrm{NH}_{4} \mathrm{NO}_{3}\right)\) is the most important nitrogen-containing fertilizer in the world. Describe how you would prepare this compound, given only air and water as the starting materials. You may have any device at your disposal for this task.
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