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Chapter 7: Problem 53

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?

Short Answer

Expert verified
(a) Ionization energy (Neon): Ne (\(1s^2 2s^2 2p^6\)) --> Ne^+ (\(1s^2 2s^2 2p^5\)) + e^-. Electron affinity (Fluorine): F (\(1s^2 2s^2 2p^5\)) + e^- --> F^- (\(1s^2 2s^2 2p^6\)). (b) Ionization energy of neon: positive, electron affinity of fluorine: negative. (c) Magnitudes are not equal; ionization energy of neon is larger.

Step by step solution

01

a) Write equations including electron configurations for each process.

For ionization energy (Neon): Ne --> Ne^+ + e^- Electron configuration of Neon (Ne): \(1s^2 2s^2 2p^6\) Electron configuration of Ne^+ : \(1s^2 2s^2 2p^5\) For electron affinity (Fluorine): F + e^- --> F^- Electron configuration of Fluorine (F): \(1s^2 2s^2 2p^5\) Electron configuration of F^- : \(1s^2 2s^2 2p^6\)
02

b) Identify the signs of the two quantities

Ionization energy shows how much energy is needed to remove an electron from an atom, so it will always be positive. Electron affinity represents the energy change when an electron is added to an atom, and it usually has a negative value, meaning energy is released. So, ionization energy of neon will be positive, while the electron affinity of fluorine will be negative.
03

c) Determine if the magnitudes of the two quantities are equal and, if not, identify which one is larger.

The magnitudes of these two quantities are not equal. The ionization energy of neon would be larger, as neon is a noble gas and has a stable electron configuration; thus, it requires more energy to remove an electron from it. On the other hand, fluorine is one electron away from a full outer shell, and it releases energy when capturing an extra electron, resulting in a negative electron affinity. Since energy is released, the magnitude will be smaller compared to the ionization energy of neon.

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Most popular questions from this chapter

Compare the elements bromine and chlorine with respect to the following properties: (a) electron configuration, (b) most common ionic charge, (c) first ionization energy, (d) reactivity toward water, (e) electron affinity, (f) atomic radius. Account for the differences between the two elements.

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[7.113]When magnesium metal is burned in air (Figure 3.6), two products are produced. One is magnesium oxide, MgO. The other is the product of the reaction of 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 MgO and magnesium nitride after burning is 0.470 g. Water is added to the crucible, further reaction occurs, and the crucible is heated to dryness until the final product is 0.486 g of 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 \(6.3-\mathrm{g}\) 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.

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