Physical Chemistry
2nd Edition
ISBN: 9781133958437
Author: Ball, David W. (david Warren), BAER, Tomas
Publisher: Wadsworth Cengage Learning,
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Chapter 21, Problem 21.51E
Write Born-Haber cycles showing the relationship between the formation reaction and lattice energy definitions of each of the ionic compounds in exercise 21.49. You may need to review the definition of “formation reaction” from earlier in the text.
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(ii) Construct and label a Born-Haber cycle for strontium difluoride, SrF2. Calculate the
lattice energy of SrF2 using the following data:
First electron affinity of fluoride =–328.0 kJ mol"1
First ionization energy of strontium = 549.0 kJ mol"
Second ionization energy of strontium = 1064.0 kJ mol"!
Enthalpy of atomization of fluoride = 75.3 kJ mol"
Enthalpy of atomization of strontium = 164.0 kJ mol"!
Enthalpy of formation of strontium difluoride = -1224.4 kJ mol"!
16).
Using the thermochemical data below calculate the lattice energy for the formation of Na₂O.
Na(s) → Na(g)
107.3 kJ/mol
Na(g) → Na (g) + 1 e
-
495.9 kJ/mol
-418 kJ/mol
249.1 kJ/mol
-141 kJ/mol
-1484.5 kJ/mol
2 Na(s) + O₂(g) →→→ Na₂O(s)
1/2 O₂(g) → 0(g)
O(g) + 1 e→O(g)
O(g) +1e0²(g)
The ionisation energy of potassium is 4.34 eV and the electron affinity of chlorine is 3.61 eV.
The Madelung constant for the KCl structure is 1.748 and the closest distance between ions of opposite sign is 0.314 nm.
On the basis of these data, calculate the cohesive energy of KCl. Compare this with the observed cohesive energy of 6.42 eV for the ion pair and comment on the reasons for any discrepancy
Chapter 21 Solutions
Physical Chemistry
Ch. 21 - Prob. 21.1ECh. 21 - Boron nitride, BN, is a very hard material, harder...Ch. 21 - Prob. 21.3ECh. 21 - Prob. 21.4ECh. 21 - Figure 21.35 shows a unit cell of diamond....Ch. 21 - Prob. 21.6ECh. 21 - How many different unit cells can a crystal have...Ch. 21 - Prob. 21.8ECh. 21 - Prob. 21.9ECh. 21 - Prob. 21.10E
Ch. 21 - Prob. 21.11ECh. 21 - Prob. 21.12ECh. 21 - Prob. 21.13ECh. 21 - Prob. 21.14ECh. 21 - Prob. 21.15ECh. 21 - Prob. 21.16ECh. 21 - Prob. 21.17ECh. 21 - Prob. 21.18ECh. 21 - Prob. 21.19ECh. 21 - Prob. 21.20ECh. 21 - Prob. 21.21ECh. 21 - Prob. 21.22ECh. 21 - Prob. 21.23ECh. 21 - Prob. 21.24ECh. 21 - Prob. 21.25ECh. 21 - Prob. 21.26ECh. 21 - Prob. 21.27ECh. 21 - Prob. 21.28ECh. 21 - For a simple cubic lattice, what is the ratio of...Ch. 21 - Prob. 21.30ECh. 21 - Prob. 21.31ECh. 21 - Consider Figure 21.21. If the lower rightmost...Ch. 21 - Prob. 21.33ECh. 21 - The aluminum-nickel alloy AlNi has a simple cubic...Ch. 21 - Prob. 21.35ECh. 21 - The first two signals from a powdered sample has X...Ch. 21 - Prob. 21.37ECh. 21 - Prob. 21.38ECh. 21 - Prob. 21.39ECh. 21 - Prob. 21.40ECh. 21 - Prob. 21.41ECh. 21 - Prob. 21.42ECh. 21 - Prob. 21.43ECh. 21 - Prob. 21.44ECh. 21 - Prob. 21.45ECh. 21 - What is the coordination number in the cesium...Ch. 21 - Prob. 21.47ECh. 21 - Which solid phase that is, which allotrope of...Ch. 21 - Prob. 21.49ECh. 21 - Prob. 21.50ECh. 21 - Write Born-Haber cycles showing the relationship...Ch. 21 - Prob. 21.52ECh. 21 - Prob. 21.53ECh. 21 - Prob. 21.54ECh. 21 - The lattice energy for potassium iodide, KI, is...Ch. 21 - Prob. 21.56ECh. 21 - Prob. 21.57ECh. 21 - Prob. 21.58ECh. 21 - Prob. 21.59ECh. 21 - Prob. 21.60ECh. 21 - Prob. 21.61ECh. 21 - Prob. 21.62ECh. 21 - Prob. 21.63ECh. 21 - Prob. 21.64E
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Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Similar questions
- Use a Born-Haber cycle (Sec. 5-13) to calculate the lattice energy of MgF2 using these thermodynamic data. Compare this lattice energy with that of SrF2, −2496 kJ/mol. Explain the difference in the values in structural terms.arrow_forwardThe lattice energy of LiF is 1023 kJ/mol, and the Li—F distance is 200.8 pm. NaF crystallizes in the same structure as LiF but with a Na—F distance of 231 pm. Which of the following values most closely approximates the lattice energy of NaF: 510, 890, 1023, 1175, or 4090 kJ/mol? Explain your choice.arrow_forwardThe lattice energy of KF is 794 kJ/mol, and the interionic distance is 269 pm. The Na—F distance in NaF, which has the same structure as KF, is 231 pm. Which of the following values is the closest approximation of the lattice energy of NaF: 682 kJ/mol, 794 kJ/mol, 924 kJ/mol, 1588 kJ/mol, or 3175 kJ/mol? Explain your answer.arrow_forward
- How can I use the Born Haber cycle to establish the lattice energy of CsCl (s)from the following data: ΔHf° [CsCl(s)] = -442.8 kJ/mol; enthalpy of sublimation of Cesium is 78.2 kJ/mol; enthalpy of dissociation of Cl2 (g) = 243 kJ/mol Cl2 ; IE1 for Cs(g) = 375.7 kJ/mol; electron affinity enthalpy-EA1 for Cl(g) = -349kJ/mol.arrow_forwardIn a lattice, a positive ion is often surrounded by eight negative ions. We might reason, therefore, that the lattice energy should be related to eight times the potential of interaction between these oppositely charged particles. Why is this reasoning too simple?arrow_forwardUse the Born Haber cycle (show relevant steps) to determine the lattice energy of CsCl (s) from the following data:Hf 0 [CsCl(s)] = -442.8 kJ/mol; enthalpy of sublimation of Cesium is 78.2 kJ/mol; enthalpy of dissociation of Cl2 (g) = 243 kJ/mol Cl2 ; IE1 for Cs(g) = 375.7 kJ/mol; electron affinity enthalpy-EA1 for Cl(g) = -349kJ/molarrow_forward
- Calculate the lattice enthalpy of KCI(s) using a Born-Haber cycle and the following data, which are all for 25 °C.arrow_forwardPlease don't provide handwritten solution ....arrow_forwardThe lattice energy of magnesium sulfide is the energy change accompanying the process Mg2*(g) + + S2-(g) → MgS(s) Calculate the lattice energy of MgS using the following data: Mg(s) → Mg(g) AH° = 148 kJ/mol Mg(g) → Mg2*(g) + 2e- AH° = 2186 kJ/mol Sg(s) → 8S(g) AH° = 2232 kJ/mol S(g) + 2e-- s2-(g) AH° = 450 kJ/mol 8Mg(s) + Sg(s) → 8MGS(s) AH° = -2744 kJ/mol Mg2*(g) + S2-(g)→ MgS(s) AH°lattice = ?arrow_forward
- Use the Born Haber cycle (show relevant steps) to determine the lattice energy of CsCl (s) from the following data: ΔHf°[CsCl(s)] = -442.8 kJ/mol; enthalpy of sublimation of Cesium is 78.2 kJ/mol; enthalpy of dissociation of Cl2 (g) = 243 kJ/mol Cl2 ; IE1 for Cs(g) = 375.7 kJ/mol; electron affinityenthalpy-EA1 for Cl(g) = -349kJ/mol.arrow_forwardWhat is the Born–Haber cycle? How can we determine the enthalpy change for the lattice energy?arrow_forwardGive correct detailed Solution with explanation needed..don't give Handwritten answer..don't use Ai for answering thisarrow_forward
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