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Chapter 7: Problem 37

Write equations that show the processes that describe the first, second, and third ionization energies of a chlorine atom. Which process would require the least amount of energy?

Short Answer

Expert verified
The first, second, and third ionization energies of a chlorine atom can be represented by the following equations: 1. First ionization energy: \(Cl + e^{-} \rightarrow Cl^{+}\) 2. Second ionization energy: \(Cl^{+} + e^{-} \rightarrow Cl^{2+}\) 3. Third ionization energy: \(Cl^{2+} + e^{-} \rightarrow Cl^{3+}\) The process that requires the least amount of energy is the first ionization process \(Cl + e^{-} \rightarrow Cl^{+}\), as ionization energy typically increases with the charge of the ion.

Step by step solution

01

Write the first ionization energy equation

The first ionization energy corresponds to the removal of one electron from a neutral chlorine atom. The general formula for ionization energy is: \[X^{n+} + e^{-} \rightarrow X^{(n+1)+}\] For the first ionization energy of chlorine, the equation is: \[Cl + e^{-} \rightarrow Cl^{+}\]
02

Write the second ionization energy equation

The second ionization energy corresponds to the removal of another electron from the ion formed after the first ionization. For a chlorine ion with a charge of +1, the equation is: \[Cl^{+} + e^{-} \rightarrow Cl^{2+}\]
03

Write the third ionization energy equation

The third ionization energy corresponds to the removal of yet another electron, this time from the ion formed after the second ionization. For a chlorine ion with a charge of +2, the equation is: \[Cl^{2+} + e^{-} \rightarrow Cl^{3+}\]
04

Determine the process requiring the least energy

In general, the ionization energy increases as the charge of the ion increases since the attraction between the positively charged nucleus and the negatively charged electrons also increases. Therefore, the process requiring the least amount of energy is the first ionization process: \[Cl + e^{-} \rightarrow Cl^{+}\]

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Most popular questions from this chapter

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 measure how 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?

We will see in Chapter 12 that semiconductors are materials that conduct electricity better than nonmetals but not as well as metals. The only two elements in the periodic table that are technologically useful semiconductors are silicon and germanium. Integrated circuits in computer chips today are based on silicon. Compound semiconductors are also used in the electronics industry. Examples are gallium arsenide, GaAs; gallium phosphide, GaP; cadmium sulfide, CdS; and cadmium selenide, CdSe. (a) What is the relationship between the compound semiconductors' compositions and the positions of their elements on the periodic table relative to \(\mathrm{Si}\) and Ge? \((\mathbf{b})\) Workers in the semiconductor industry refer to "II-VI" and "III-V" materials, using Roman numerals. Can you identify which compound semiconductors are II-VI and which are III-V? (c) Suggest other compositions of compound semiconductors based on the positions of their elements in the periodic table.

(a) If the core electrons were totally effective at screening the valence electrons and the valence electrons provided no screening for each other, what would be the effective nuclear charge acting on the \(3 s\) and \(3 p\) valence electrons in P? (b) Repeat these calculations using Slater's rules. (c) Detailed calculations indicate that the effective nuclear charge is \(5.6+\) for the \(3 s\) electrons and \(4.9+\) for the \(3 p\) electrons. Why are the values for the \(3 s\) and \(3 p\) electrons different? (d) If you remove a single electron from a Patom, which orbital will it come from?

Which will experience the greater effect nuclear charge, the electrons in the \(n=2\) shell in \(\mathrm{F}\) or the \(n=2\) shell in \(\mathrm{B}\) ? Which will be closer to the nucleus?

As we move across a period of the periodic table, why do the sizes of the transition elements change more gradually than those of the representative elements?
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