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Chapter 7: Problem 55

(a) Does metallic character increase, decrease, or remain unchanged as one goes from left to right across a row of the periodic table? (b) Does metallic character increase, decrease, or remain unchanged as one goes down a column of the periodic table? (c) Are the periodic trends in (a) and (b) the same as or different from those for first ionization energy?

Short Answer

Expert verified
(a) Metallic character decreases as one goes from left to right across a row of the periodic table, due to the increase in effective nuclear charge experienced by the valence electrons. (b) Metallic character increases as one goes down a column of the periodic table, due to the increase in atomic size and electron shielding. (c) The periodic trends for metallic character are opposite those for first ionization energy, meaning they are inversely related.

Step by step solution

01

Define Metallic Character

Metallic character refers to an element's ability to lose its electrons and form a positive ion or cation. Elements displaying a high metallic character tend to donate electrons more readily, allowing them to have stronger electrical conductivity and metallic properties. In the periodic table, metallic character is found to generally increase down a group and decrease across a period.
02

Metallic Character Trend across a Period (Left to Right)

Generally, the metallic character decreases as we move from left to right across a period in the periodic table. This is due to the increase in the effective nuclear charge experienced by the valence or outer shell electrons. As we move from left to right in a period, the number of protons increases, and the electrons experience a stronger attraction to the nucleus. This increased attraction makes it more challenging for the atom to lose electrons, hence decreasing the metallic character. Answer (a): Metallic character decreases as one goes from left to right across a row of the periodic table.
03

Metallic Character Trend down a Group (Column)

As we move down a group in the periodic table, the metallic character tends to increase. This is due to the increase in atomic size and electron shielding. Since electron shielding increases as we go down the group due to the addition of electron shells, the effective nuclear charge experienced by the outer electrons decreases. This decreased attraction to the nucleus allows the outer electrons to be more easily lost, resulting in increased metallic character. Answer (b): Metallic character increases as one goes down a column of the periodic table.
04

Compare Trends of Metallic Character with First Ionization Energy

The first ionization energy is the energy required to remove an electron from a neutral atom in its gaseous state. In general, first ionization energy increases from left to right across a period and decreases as we go down a group. This is due to the same factors that affect the metallic character: effective nuclear charge and atomic size. When comparing the trends of metallic character and first ionization energy, it can be seen that they are inversely related. This means that when metallic character increases, the first ionization energy tends to decrease, and vice versa. Answer (c): The periodic trends for metallic character are opposite those for first ionization energy.

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Most popular questions from this chapter

One way to measure ionization energies is ultraviolet photoelectron spectroscopy (PES), a technique based on the photoelectric effect. \(\infty \infty\) (Section 6.2) In PES, monochromatic light is directed onifference between the energy of the photons and the kinetic energy of the electrons corresponds to the to a sample, causing electrons to be emitted. The kinetic energy of the emitted electrons is measured. The denergy needed to remove the electrons (that is, the ionization energy). Suppose that a PES experiment is performed in which mercury vapor is irradiated with ultraviolet light of wavelength \(58.4 \mathrm{~nm}\). (a) What is the energy of a photon of this light, in \(\mathrm{eV}\) ? (b) Write an equation that shows the process corresponding to the first ionization energy of Hg. (c) The kinetic energy of the emitted electrons is measured to be \(10.75 \mathrm{eV}\). What is the first ionization energy of \(\mathrm{Hg}\), in \(\mathrm{kJ} / \mathrm{mol}\) ? (d) Using Figure 7.10, determine which of the halogen elements has a first ionization energy closest to that of mercury.

(a) As described in Section 7.7, the alkali metals react with hydrogen to form hydrides and react with halogens to form halides. Compare the roles of hydrogen and halogens in these reactions. How are the forms of hydrogen and halogens in the products alike? (b) Write balanced equations for the reaction of fluorine with calcium and for the reaction of hydrogen with calcium. What are the similarities among the products of these reactions?

Write the electron configurations for the following ions, and determine which have noble-gas configurations: (a) \(\mathrm{Ru}^{3+}\), (b) \(\mathrm{As}^{3-}\), (c) \(\mathrm{Y}^{3+}\), (d) \(\mathrm{Pd}^{2+}\), (e) \(\mathrm{Pb}^{2+}\), (f) \(\mathrm{Au}^{3+}\).

Using only the periodic table, arrange each set of atoms in order of increasing radius: (a) \(\mathrm{Ba}, \mathrm{Ca}, \mathrm{Na}\); (b) In, \(\mathrm{Sn}, \mathrm{As}\); (c) \(\mathrm{Al}, \mathrm{Be}, \mathrm{Si}\).

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: $$ \begin{array}{lc} \hline \text { Element } & \text { Wavelength } \\ \hline \mathrm{Ne} & 14.610 \\ \mathrm{Ca} & 3.358 \\ \mathrm{Zn} & 1.435 \\ \mathrm{Zr} & 0.786 \\ \mathrm{Sn} & 0.491 \\ \hline \end{array} $$ (a) Calculate the frequency, \(\nu\), of the \(\mathrm{X}\) rays emitted by each of the elements, in Hz. (b) 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 \(\mathrm{X}\)-ray wavelength emitted by iron. (e) A particular element emits X rays with a wavelength of \(0.980 \AA\). What element do you think it is?
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