List the individual steps used in constructing a Born–Haber cycle for the formation of BaI 2 from the elements. Which of the steps would you expect to be exothermic?

Hi everyone here we have a question asking us to identify the steps that are expected to be exact thermic in the born haber cycle for the formation of magnesium bromide. So first we have magnesium solid forms magnesium gashes and that is a solid to gas which is expected to be positive. So it is endo thermic. Next we have magnesium gashes forms magnesium With a two plus charge gashes plus two electrons. The ionization energy is expected to be positive. So that is end of thermite. Next we have bro ming too liquid forming, browning too gashes this is a liquid to gas, this is expected to be positive. So this is end of thermite. Next we have browning two gashes to to growing gashes. This adam. Ization needs energy so it is expected to be positive. An endo thermic. Next we have bro. Ming gas plus an electron forms bro me negative. The electron affinity is expected to be negative. So this is expected to be exo thermic. And lastly we have magnesium two plus gashes Plus two Bro. ming negative gashes forms magnesium bromide solid. This lattice energy is expected to be negative. So it is exo thermic. So these are our two eggs are thermic steps and that is our final answer. Thank you for watching. Bye.

Ch.8 - Basic Concepts of Chemical Bonding

Brown - Chemistry: The Central Science 15th Edition

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Ch.8 - Basic Concepts of Chemical Bonding

Problem 30

Chapter 8, Problem 30

List the individual steps used in constructing a Born–Haber cycle for the formation of BaI₂ from the elements. Which of the steps would you expect to be exothermic?

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Write the overall reaction for the formation of BaI_2 from its elements: Ba(s) + I_2(s) -> BaI_2(s).

Sublimation of solid barium to gaseous barium: Ba(s) -> Ba(g). This step requires energy input, so it is endothermic.

Ionization of gaseous barium to form Ba^2+: Ba(g) -> Ba^2+(g) + 2e^-. This step is endothermic as it requires energy to remove electrons.

Dissociation of iodine molecules into iodine atoms: I_2(s) -> 2I(g). This step is endothermic because energy is needed to break the I-I bond.

Formation of iodide ions from iodine atoms: I(g) + e^- -> I^-(g). This step is exothermic as energy is released when an electron is added to an iodine atom.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Born-Haber Cycle

The Born-Haber cycle is a thermodynamic cycle that relates the lattice energy of an ionic compound to the enthalpy changes involved in its formation from the constituent elements. It provides a systematic way to calculate the lattice energy by considering the various steps, including sublimation, ionization, and electron affinity, that occur when forming an ionic compound from its elements.

Lattice Energy

Lattice energy is the energy released when gaseous ions combine to form an ionic solid. It is a crucial factor in determining the stability of ionic compounds. In the context of the Born-Haber cycle, lattice energy is typically a large exothermic value, indicating that the formation of the ionic lattice from gaseous ions is energetically favorable.

Enthalpy Changes

Enthalpy changes refer to the heat absorbed or released during a chemical reaction at constant pressure. In the Born-Haber cycle, various steps involve enthalpy changes, such as the enthalpy of sublimation, ionization energy, and electron affinity. Understanding which steps are exothermic (release heat) or endothermic (absorb heat) is essential for predicting the overall energy change in the formation of the compound.

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Enthalpy of Formation

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Textbook Question

Energy is required to remove two electrons from Ca to form Ca2+, and energy is required to add two electrons to O to form O2 - . Yet CaO is stable relative to the free elements. Which statement is the best explanation? (a) The lattice energy of CaO is large enough to overcome these processes. (b) CaO is a covalent compound, and these processes are irrelevant. (c) CaO has a higher molar mass than either Ca or O. (d) The enthalpy of formation of CaO is small. (e) CaO is stable to atmospheric conditions.

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Textbook Question

Consider the ionic compounds KF, NaCl, NaBr, and LiCl. (a) Use ionic radii (Figure 7.8) to estimate the cation–anion distance for each compound.

Textbook Question

Which of the following trends in lattice energy is due to differences in ionic radii: a. NaCl > RbBr > CsBr, b. BaO > KF, c. SrO > SrCl2?

Textbook Question

Use data from Appendix C, Figure 7.11, and Figure 7.13 to calculate the lattice energy of KI.

Textbook Question

(a) Based on the lattice energies of MgCl2 and SrCl2 given in Table 8.1, what is the range of values that you would expect for the lattice energy of CaCl2?

Textbook Question

(b) Using data from Appendix C, Figure 7.11, Figure 7.13, and the value of the second ionization energy for Ca, 1145 kJ/mol, calculate the lattice energy of CaCl2.

List the individual steps used in constructing a Born–Haber cycle for the formation of BaI2 from the elements. Which of the steps would you expect to be exothermic?

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Key Concepts

Born-Haber Cycle

Lattice Energy

Enthalpy Changes

List the individual steps used in constructing a Born–Haber cycle for the formation of BaI₂ from the elements. Which of the steps would you expect to be exothermic?