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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

Write a balanced equation for the reaction that occurs in each of the following cases: (a) Ozone decomposes to dioxygen. (b) Xenon reacts with fluorine. (Write three different equations.) (c) Sulfur reacts with hydrogen gas. (d) Fluorine reacts with water.

Some ions do not have a corresponding neutral atom that has the same electron configuration. For each of the following ions, identify the neutral atom that has the same number of electrons and determine if this atom has the same electron configuration. If such an atom does not exist, explain why. (b) \(\mathrm{Sc}^{3+}\) (d) \(\mathrm{Zn}^{2+},(\mathrm{e}) \mathrm{Sn}^{4+}\) (a) \(\mathrm{Cl}\) (c) \(\mathrm{Fe}^{2+}\)

(a) What is meant by the terms acidic oxide and basic oxide? (b) How can we predict whether an oxide will be acidic or basic based on its composition?

How are metallic character and first ionization energy related?

Does the reactivity of a metal correlate with its first ionization energy? Explain.
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