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Chapter 7: Problem 39

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

Short Answer

Expert verified
The first, second, and third ionization energies of an aluminum atom are represented by the following equations: 1. First Ionization Energy: \(Al \rightarrow Al^+ + e^-\) 2. Second Ionization Energy: \(Al^+ \rightarrow Al^{2+} + e^-\) 3. Third Ionization Energy: \(Al^{2+} \rightarrow Al^{3+} + e^-\) The process that requires the least amount of energy is the first ionization process: \(Al \rightarrow Al^+ + e^-\).

Step by step solution

01

First Ionization Energy

The first ionization energy corresponds to removing one electron from a neutral aluminum atom: \[Al \rightarrow Al^+ + e^-\] Here, a neutral aluminum atom loses an electron, forming an Al^+ ion and a free electron.
02

Second Ionization Energy

The second ionization energy corresponds to removing another electron from the Al^+ ion formed in the first ionization process: \[Al^+ \rightarrow Al^{2+} + e^-\] In this step, the Al^+ ion loses another electron, forming an Al^2+ ion, and another free electron.
03

Third Ionization Energy

The third ionization energy corresponds to removing yet another electron from the Al^(2+) ion formed in the second ionization process: \[Al^{2+} \rightarrow Al^{3+} + e^-\] In this step, the Al^(2+) ion loses another electron and forms an Al^3+ ion, along with a free electron.
04

Least Energy Requirement

Generally, as more electrons are removed, the ionization energy increases. This means that the first ionization energy requires the least energy, followed by the second ionization energy, and the third ionization energy requires the most energy. Therefore, the process requires the least energy is the first ionization process: \[Al \rightarrow Al^+ + e^-\]

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Most popular questions from this chapter

Zinc in its \(2+\) oxidation state is an essential metal ion for life. \(\mathrm{Zn}^{2+}\) is found bound to many proteins that are involved in biological processes, but unfortunately \(\mathrm{Zn}^{2+}\) is hard to detect by common chemical methods. Therefore, scientists who are interested in studying \(\mathrm{Zn}^{2+}\) -containing proteins will frequently substitute \(\mathrm{Cd}^{2+}\) for \(\mathrm{Zn}^{2+}\), since \(\mathrm{Cd}^{2+}\) is easier to detect. (a) On the basis of the properties of the elements and ions discussed in this chapter and their positions in the periodic table, describe the pros and cons of using \(\mathrm{Cd}^{2+}\) as a \(\mathrm{Zn}^{2+}\) substitute. (b) Proteins that speed up (catalyze) chemical reactions are called enzymes. Many enzymes are required for proper metabolic reactions in the body. One problem with using \(\mathrm{Cd}^{2+}\) to replace \(\mathrm{Zn}^{2+}\) in enzymes is that \(\mathrm{Cd}^{2+}\) substitution can decrease or even eliminate enzymatic activity. Can you suggest a different metal ion that might replace \(\mathrm{Zn}^{2+}\) in enzymes instead of \(\mathrm{Cd}^{2+} ?\) Justify your answer.

Although the electron affinity of bromine is a negative quantity, it is positive for \(\mathrm{Kr}\). Use the electron configurations of the two elements to explain the difference.

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?

Elements in group \(7 \mathrm{~A}\) in the periodic table are the halogens; elements in group \(6 \mathrm{~A}\) are called the chalcogens. (a) What is the most common oxidation state of the chalcogens compared to the halogens? Can you suggest an explanation for the difference? (b) For each of the following periodic properties, state whether the halogens or the chalcogens have larger values: atomic radii; ionic radii of the most common oxidation state; first ionization energy; second ionization energy.

Silver and rubidium both form +1 ions, but silver is far less reactive. Suggest an explanation, taking into account the ground-state electron configurations of these elements and atomic radii.
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