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Chapter 9: Problem 28

Use ionization energies and electron affinities listed in the text to determine whether the following reaction is endothermic or exothermic. $$ \mathrm{Mg}(\mathrm{g})+2 \mathrm{F}(\mathrm{g}) \longrightarrow \mathrm{Mg}^{2+}(\mathrm{g})+2 \mathrm{F}^{-}(\mathrm{g}) $$

Short Answer

Expert verified
The reaction is exothermic if the total energy change calculated in step 4 is negative, and endothermic if it's positive. The precise conclusion depends on the specific values of ionization energy for Mg and electron affinity for F.

Step by step solution

01

Understand What Ionization Energy and Electron Affinity Mean

Ionization energy is the energy required to remove the most loosely held electron from an atom in the gaseous state. On the other hand, electron affinity is the energy change of an atom in the gaseous state when it gains an electron.
02

Find Out The Values Of Ionization Energies and Electron Affinities

The ionization energy for Magnesium (Mg) is needed, along with the electron affinity for Fluorine (F). These values are available in textbooks or reliable online resources.
03

Calculate The Energy Changes For Each Part Of The Reaction

In the forward reaction, two electrons are removed from a single Mg atom, which equates to two times the ionization energy for Mg. When these two electrons are accepted by two F atoms, it releases energy equal to two times the electron affinity for F.
04

Calculate The Total Energy Change of The Reaction

The total energy change of the reaction can be calculated by subtracting the total energy released (2 times the electron affinity for F) from the total energy required (2 times the ionization energy of Mg).
05

Determine Whether The Reaction Is Endothermic Or Exothermic

If the total energy change is negative, it means the reaction releases energy and is hence exothermic. If the total energy change is positive, it means the reaction requires energy and is hence endothermic.

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Most popular questions from this chapter

Listed below are two atomic properties of the element germanium. Refer only to the periodic table on the inside front cover and indicate probable values for each of the following elements, expressed as greater than, about equal to, or less than the value for Ge. $$\begin{array}{lcc} \hline \text { Element } & \text { Atomic Radius } & \begin{array}{c} \text { First lonization } \\ \text { Energy } \end{array} \\ \hline \mathrm{Ge} & 122 \mathrm{pm} & 762 \mathrm{kJ} / \mathrm{mol} \\ \mathrm{Al} & ? & ? \\ \mathrm{In} & ? & ? \\ \mathrm{Se} & ? & ? \\ \hline \end{array}$$

Arrange the following in expected order of increasing radius: $\mathrm{Br}, \mathrm{Li}^{+}, \mathrm{Se}, \mathrm{I}^{-} .$ Explain your answer.

Refer only to the periodic table on the inside front cover and indicate which of the atoms, \(\mathrm{Bi}, \mathrm{S}, \mathrm{Ba}, \mathrm{As}\) and \(\mathrm{Ca},\) (a) is most metallic; (b) is most nonmetallic; (c) has the intermediate value when the five are arranged in order of increasing first ionization energy.

Two elements, \(A\) and \(B\), have the electron configurations shown. $$ \mathrm{A}=[\mathrm{Kr}] 4 s^{2} \quad \mathrm{B}=[\mathrm{Ar}] 3 d^{10} 4 s^{2} 4 p^{5} $$ (a) Which element is a metal? (b) Which element has the greater ionization energy? (c) Which element has the larger atomic radius? (d) Which element has the greater electron affinity?

Consider a nitrogen atom in the ground state and comment on whether the following statements are true or false. (a) \(\mathrm{Z}_{\text {eff }}\) for an electron in a 2 s orbital is greater than that for the 1 s orbital. (b) The \(Z_{\text {eff for the } 2 p \text { and } 2 s \text { orbitals is the same. }}\) (c) More energy is required to remove an electron from a 2 s orbital than from the \(2 p\) orbital. (d) The 2 s electron is less shielded than the \(2 p\) electron.
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