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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) As one goes from left to right across a row of the periodic table, metallic character decreases. (b) As one goes down a column of the periodic table, metallic character increases. (c) The periodic trends in (a) are different from those for first ionization energy, while the trends in (b) are the same as those for first ionization energy.

Step by step solution

01

Metallic character trends across a row of the periodic table

To find the trend in metallic character across a row of the periodic table, we need to consider the properties of metals and how they change as we move from left to right. Metallic character is defined as how easily an atom can lose an electron. Generally, as we move from left to right across a row in the periodic table, the elements become less metallic, and the metallic character decreases.
02

Metallic character trends down a column of the periodic table

To find the trend in metallic character down a column of the periodic table, we again need to consider the properties of metals and how they change as we move down a column. As we move down a column in the periodic table, the elements become more metallic, and the metallic character increases.
03

First ionization energy trends across a row and down a column

First ionization energy is the energy required to remove the outermost electron from an atom. As we move from left to right across a row in the periodic table, the first ionization energy generally increases. This is because the number of protons increase, making it harder to remove the outermost electron due to stronger attractive forces between the nucleus and the electrons. As we move down a column in the periodic table, the first ionization energy generally decreases, due to the increased number of energy levels, making it easier for the outermost electron to be removed.
04

Comparing metallic character trends to first ionization energy trends

For part (a), the metallic character decreases as we go from left to right across a row, while the first ionization energy increases. These trends are different from each other. For part (b), the metallic character increases as we go down a column, and the first ionization energy decreases. These trends are the same as each other. To summarise: (a) Metallic character decreases as one goes from left to right across a row of the periodic table. (b) Metallic character increases as one goes down a column of the periodic table. (c) The periodic trends in (a) are different from those for first ionization energy, while the trends in (b) are the same as those for first ionization energy.

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Most popular questions from this chapter

Would a neutral \(\mathrm{K}\) atom or a \(\mathrm{K}^{+}\) ion have a more negative value of electron affinity?

It is possible to define metallic character as we do in this book and base it on the reactivity of the element and the ease with which it loses electrons. Alternatively, one could measurehow well electricity is conducted by each of the elements to determine how "metallic" the elements are. On the basis of conductivity, there is not much of a trend in the periodic table: silver is the most conductive metal, and manganese the least. Look up the first ionization energies of silver and manganese; which of these two elements would you call more metallic based on the way we define it in this book?

Use electron configurations to explain the following observa tions: (a) The first ionization energy of phosphorus is greater than that of sulfur. (b) The electron afnity 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 the electron configurations for the following ions, and determine which have noble-gas configurations: \((\mathbf{a})\mathrm{Ru}^{3+}\) \((\mathbf{b}) \mathrm{As}^{3-},(\mathbf{c}) \mathrm{Y}^{3+},(\mathbf{d}) \mathrm{Pd}^{2+},(\mathbf{e}) \mathrm{Pb}^{2+},(\mathbf{f}) \mathrm{Au}^{3+}.\)

Consider the first ionization energy of neon and the electron affinity of fluorine. (a) Write equations, including electron configurations, for each process. (b) These two quantities have opposite signs. Which will be positive, and which will be negative? (c) Would you expect the magnitudes of these two quantities to be equal? If not, which one would you expect to be larger?
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