Physical Chemistry
2nd Edition
ISBN: 9781133958437
Author: Ball, David W. (david Warren), BAER, Tomas
Publisher: Wadsworth Cengage Learning,
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Textbook Question
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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The lattice energy of an ionic compound is defined to be the amount of energy required to completely separate one mole of the solid into is gaseous ions. The lattice energy of Na2O is 2695 kJ/mol. Type the balanced chemical equation, including phase labels [ (s), (l), (g), (aq)] for the reaction that illustrates what happens when 2695 kJ of energy is added to 1 mole of solid Na2O .
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
2 Na(s) + O₂(g) → Na₂O(s)
-418 kJ/mol
1/2 O₂(g) → O(g)
249.1 kJ/mol
O(g) + 1 e→O(g)
-141 kJ/mol
-1484.5 kJ/mol
O(g) + 1 e0²(g)
s) If 115
or pressu
Calculate the lattice energy of TIF (s) using the
following thermodynamic data (all data is in
kJ/mol). Note that the data given has been
perturbed, so looking up the answer is
probably not a good idea.
TI (S)
TI (g)
F - F
(g)
F (g)
TIF
(s)
AHsublimation = 161
kJ/mol
Ionization energy =
569 kJ/mol
Bond energy = 138
kJ/mol
Electron affinity = -348
kJ/mol
AH°f = -345 kJ/mol
kJ/mol
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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- 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_forwardCalculate the standard molar enthalpy of formation of NO(g) from the following data: N2(g)+2O22NO2(g)H298=66.4kJ2NO(g)+O22NO2(g)H298=114.1kJarrow_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_forward
- The 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(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"!arrow_forward16). 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)arrow_forward
- Cation Na+ K+ Al³+ Which one of the following ionic compounds has the largest lattice formation enthalpy (lattice energy) thus making it the most favorable to form a stable lattice? Lattice Formation Enthalpy (kJ/mol) CI- Anion Br- |- -787 -747 -704 0²- -2695 -715 -682 -649 -2360 -5492 -5361 -5217 -15,916 A) NaBr B) KI C) AICI 3 D) Na₂Oarrow_forwardCalculate the lattice energy of AgCl(s) using the following thermodynamic data (all data is in kJ/mol). Note that the data given has been perturbed, so looking up the answer is probably not a good idea. Ag(s) AHsublimation 265 kJ/mol Ag(g) Ionization energy 711 kJ/mol Cl-CI(g) Bond energy = 223 kJ/mol CI(g) Electron affinity = -369 kJ/mol AgCl(s) AH°=-147 kJ/mol kJ/mol Do you expect this value to be larger or smaller than the lattice energy of AgBr(s)?arrow_forwardDetermine the lattice energy of NaCl(s), using the data provided.arrow_forward
- What is electrovalent bond? Explain the term lattice energy as applied to ionic crystal How is enthalpy of formation of NaCl calculated, using Born Habeis cycle?arrow_forwardHow 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_forwardCalculate the lattice energy of CsBr(s) using the following thermodynamic data (all data is in kJ/mol). Note that the data given has been perturbed, so looking up the answer is probably not a good idea. AHsublimation = 57 kJ/mol IE= 356 kJ/mol Cs(s) Cs(g) Br-Br(g) Dar Br = 173 kJ/mol Br(g) EA -345 kJ/mol CsBr(s) AH = -426 kJ/mol wwwww kj/molarrow_forward
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