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Chapter 7: Problem 54

What is the relationship between the ionization energy of an anion with a 1 - charge such as \(\mathrm{F}^{-}\) and the electron affinity of the neutral atom, F?

Short Answer

Expert verified
The ionization energy of an anion with a 1- charge, such as F-, is approximately equal to the electron affinity of the neutral atom, F. The energy released when adding an electron to the neutral F atom (electron affinity) is approximately equal to the energy needed to remove an electron from F- (ionization energy). These two energy changes correspond to reverse processes and should have equal magnitudes but opposite signs.

Step by step solution

01

Ionization energy (IE) is defined as the energy needed to remove an electron from an atom or ion. For an anion, the ionization energy corresponds to the electron removal from its negatively-charged state to form a neutral atom. #Step 2: Define Electron affinity#

Electron affinity (EA) is defined as the energy change associated with adding an electron to a neutral atom. The added electron forms a negatively-charged ion. #Step 3: Consider the relationship between ionization energy and electron affinity#
02

In order to understand the relationship between the ionization energy of F- (F minus) and the electron affinity of F (neutral fluorine), we can analyze the following energy changes: 1. Addition of an electron to the neutral F atom to produce F-, which releases the energy equal to the electron affinity of F. 2. Removal of an electron from F- to form the neutral F atom, which requires energy equal to the ionization energy of F-. By considering these energy changes, we can find a relationship between ionization energy and electron affinity. #Step 4: Summarize the relationship between ionization energy and electron affinity#

When we add an electron to a neutral F atom, we release energy (electron affinity), creating F-. If we then remove an electron from F- (ionization), we get the neutral F atom again, and in this process, we need to provide energy (ionization energy). These two energy changes should be approximately equal but with opposite signs because they follow a reverse path. Therefore, we conclude that the ionization energy of F(1-) ion is approximately equal to the electron affinity of the neutral F atom. In the case of similar atoms and ions, we can find a direct relationship between ionization energy and electron affinity.

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Most popular questions from this chapter

Consider \(\mathrm{S}, \mathrm{Cl}\), and \(\mathrm{K}\) and their most common ions. (a) List the atoms in order of increasing size. (b) List the ions in order of increasing size. (c) Explain any differences in the orders of the atomic and ionic sizes.

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.

Explain the following variations in atomic or ionic radii: (a) \(\Gamma>\mathrm{I}>\mathrm{I}^{+},(\mathrm{b}) \mathrm{Ca}^{2+}>\mathrm{Mg}^{2+}>\mathrm{Be}^{2+}\) (c) \(\mathrm{Fe}>\mathrm{Fe}^{2+}>\mathrm{Fe}^{3+}\)

When magnesium metal is burned in air (Figure 3.6 ), two products are produced. One is magnesium oxide, \(\mathrm{MgO}\). The other is the product of the reaction of \(\mathrm{Mg}\) with molecular nitrogen, magnesium nitride. When water is added to magnesium nitride, it reacts to form magnesium oxide and ammonia gas. (a) Based on the charge of the nitride ion (Table 2.5 ), predict the formula of magnesium nitride. (b) Write a balanced equation for the reaction of magnesium nitride with water. What is the driving force for this reaction? (c) In an experiment a piece of magnesium ribbon is burned in air in a crucible. The mass of the mixture of \(\mathrm{MgO}\) and magnesium nitride after burning is \(0.470 \mathrm{~g}\). Water is added to the crucible, further reaction occurs, and the crucible is heated to dryness until the final product is \(0.486 \mathrm{~g}\) of \(\mathrm{MgO}\). What was the mass percentage of magnesium nitride in the mixture obtained after the initial burning? (d) Magnesium nitride can also be formed by reaction of the metal with ammonia at high temperature. Write a balanced equation for this reaction. If a 6.3 -g Mg ribbon reacts with \(2.57 \mathrm{~g} \mathrm{NH}_{3}(g)\) and the reaction goes to completion, which component is the limiting reactant? What mass of \(\mathrm{H}_{2}(g)\) is formed in the reaction? (e) The standard enthalpy of formation of solid magnesium nitride is \(-461.08 \mathrm{~kJ} / \mathrm{mol} .\) Calculate the standard enthalpy change for the reaction between magnesium metal and ammonia gas.

(a) What is the trend in first ionization energies as one proceeds down the group 7 A elements? Explain how this trend relates to the variation in atomic radii. (b) What is the trend in first ionization energies as one moves across the fourth period from \(\mathrm{K}\) to \(\mathrm{Kr}\) ? How does this trend compare with the trend in atomic radii?
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