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Chapter 7: Problem 43

(a) What is the general relationship between the size of an atom and its first ionization energy? (b) Which element in the periodic table has the largest ionization energy? Which has the smallest?

Short Answer

Expert verified
(a) The general relationship between the size of an atom and its first ionization energy is that as the size of an atom increases, the ionization energy decreases. This is due to the weaker attraction between the nucleus and the outer electrons in larger atoms, as well as increased electron shielding. (b) The element with the largest ionization energy in the periodic table is helium (He) due to its small atomic size and strong attraction between the nucleus and its electrons. The element with the smallest ionization energy is francium (Fr) because of its large atomic size, weak attraction between the nucleus and outer electrons, and substantial electron shielding.

Step by step solution

01

(a) General relationship between atom size and ionization energy.

The ionization energy of an atom is the amount of energy required to remove an electron from the outermost shell of an isolated gaseous atom. In general, as the size of an atom increases, the ionization energy decreases. This is because larger atoms have more electron shells, so the outer electrons are farther away from the nucleus. The positive charge of the nucleus has a weaker hold on the outer electrons, making it easier to remove them, and thus the ionization energy decreases. Additionally, larger atoms have more electron shielding, which also weakens the attraction between the nucleus and the outer electrons, leading to lower ionization energies.
02

(b) Element with the largest ionization energy

The element with the largest ionization energy in the periodic table is helium (He). This is because helium has the smallest atomic size among all the elements and only has two electrons, both of which are in the first electron shell, closest to the nucleus. The strong attraction between the nucleus and the electrons makes it difficult to remove an electron, so helium has the highest ionization energy.
03

(b) Element with the smallest ionization energy

The element with the smallest ionization energy in the periodic table is francium (Fr). This is because francium has the largest atomic size, with many electron shells and weak attraction between the outermost electrons and the nucleus. In addition, the many electron shielding layers in francium further weaken the attraction between the nucleus and the outer electrons. As a result, it requires the least energy to remove an electron from a francium atom, and francium has the smallest ionization energy of all the elements.

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Most popular questions from this chapter

Compare the elements sodium and magnesium with respect to the following properties: (a) electron configuration, (b) most common ionic charge, (c) first ionization energy, (d) reactivity toward water, (e) atomic radius. Account for the differences between the two elements.

Moseley established the concept of atomic number by studying X-rays emitted by the elements. The X-rays emitted by some of the elements have the following wavelengths: \begin{tabular}{ll} \hline Element & Wavelength (?) \\ \hline \(\mathrm{Ne}\) & \(14.610\) \\ \(\mathrm{Ca}\) & \(3.358\) \\ \(\mathrm{Zn}\) & \(1.435\) \\ \(\mathrm{Zr}\) & \(0.786\) \\ \(\mathrm{Sn}\) & \(0.491\) \\ \hline \end{tabular} (a) Calculate the frequency, \(\nu\), of the X-rays emitted by each of the elements, in Hz. (b) Using graph paper (or suitable computer software), plot the square root of \(\nu\) versus the atomic number of the element. What do you observe about the plot? (c) Explain how the plot in part (b) allowed Moseley to predict the existence of undiscovered elements. (d) Use the result from part (b) to predict the X-ray wavelength emitted by iron. (e) \(\mathrm{A}\) particular element emits X-rays with a wavelength of \(0.980 \AA\). What element do you think it is?

Use electron configurations to explain the following observations: (a) The first ionization energy of phosphorus is greater than that of sulfur. (b) The electron affinity of nitrogen is lower (less negative) than those of both carbon and oxygen. (c) The second ionization energy of oxygen is greater than the first ionization energy of fluorine. (d) The third ionization energy of manganese is greater than those of both chromium and iron.

Write a balanced equation for the reaction that occurs in each of the following cases: (a) Chlorine reacts with water. (b) Barium metal is heated in an atmosphere of hydrogen gas. (c) Lithium reacts with sulfur. (d) Fluorine reacts with magnesium metal.

(a) If we arrange the elements of the second period (Li-Ne) in order of increasing first ionization energy, where would hydrogen fit into this series? (b) If we now arrange the elements of the third period (Na-Ar) in order of increasing first ionization energy, where would lithium fit into this series? (c) Are these series consistent with the assignment of hydrogen as a nonmetal and lithium as a metal?
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