Physical Chemistry
2nd Edition
ISBN: 9781133958437
Author: Ball, David W. (david Warren), BAER, Tomas
Publisher: Wadsworth Cengage Learning,
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Chapter 22, Problem 22.38E
Interpretation Introduction
Interpretation:
Whether the relationship trend between the surface energy of ionic compounds and the magnitudes of the charges of the ions exists or not is to be stated.
Concept introduction:
The energy which can quantify the disturbance created by the intermolecular bonds during the creation of the surface is known as surface energy. It is also known as interfacial free energy.
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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"!
Given the following data, calculate the lattice energy of barium chloride, BaCl. IE 1BA= 502.7 kJ mol, IE 2Ba = 965.0 kJ mol, AHsub (Ba) =175.6 kJ moľ, EA = 349.0 kJ mol, BDE (CI - CI) = 243.4 kJ mol, AH(BaCl) = -858.6 kJ mol
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 22 Solutions
Physical Chemistry
Ch. 22 - Using the explanation of unbalanced forces as the...Ch. 22 - Show that the right side of equation 22.1 has...Ch. 22 - The text claims that surface tension varies with...Ch. 22 - Prob. 22.4ECh. 22 - Prob. 22.5ECh. 22 - Prob. 22.6ECh. 22 - Prob. 22.7ECh. 22 - Equation 22.6 defines surface tension in terms of...Ch. 22 - Prob. 22.9ECh. 22 - Prob. 22.10E
Ch. 22 - Prob. 22.11ECh. 22 - Prob. 22.12ECh. 22 - Prob. 22.13ECh. 22 - Prob. 22.14ECh. 22 - Prob. 22.15ECh. 22 - Prob. 22.16ECh. 22 - Prob. 22.17ECh. 22 - Prob. 22.18ECh. 22 - Prob. 22.19ECh. 22 - Determine the pressure difference on a droplet of...Ch. 22 - Prob. 22.21ECh. 22 - Prob. 22.22ECh. 22 - Prob. 22.23ECh. 22 - Prob. 22.24ECh. 22 - Prob. 22.25ECh. 22 - Prob. 22.26ECh. 22 - Prob. 22.27ECh. 22 - The Young-Dupr equation, equation 22.16, is...Ch. 22 - Why are capillary rises and depressions not seen...Ch. 22 - Prob. 22.30ECh. 22 - Prob. 22.31ECh. 22 - Prob. 22.32ECh. 22 - Prob. 22.33ECh. 22 - Prob. 22.34ECh. 22 - Prob. 22.35ECh. 22 - Prob. 22.36ECh. 22 - Prob. 22.37ECh. 22 - Prob. 22.38ECh. 22 - A china cup breaks when the ionic or covalent...Ch. 22 - Satellites in space often suffer from vacuum...Ch. 22 - Prob. 22.41ECh. 22 - Prob. 22.42ECh. 22 - Prob. 22.43ECh. 22 - Are the following processes examples of...Ch. 22 - Prob. 22.45ECh. 22 - Early attempts to coat metals with Teflon, poly...Ch. 22 - Prob. 22.47ECh. 22 - Prob. 22.48ECh. 22 - Prob. 22.49E
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- 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.arrow_forward7.74 In 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 simpler?arrow_forwardDetermine the crystal lattice energy for MgCl2, given the following: Mg(s) + Cl2(g) --> MgCl2(s) triangle Hof= -642 kj/mol (Mg - triangle Hvaporization= 147.7 kj/mol, Mg2+- Eionization= 2188.4 kj/mol, Cl2- Ebond= 248 kj/mol, Cl- - Eionization= -349 kj/mol)arrow_forward
- (a) Imagine that a Born-Haber cycle is being constructed by a colleague, to determine the lattice energy of a hypothetical magnesium halide salt, where X is the halide ion. The colleague makes the following list: First and second ionisations of Mg; 737 and 1451 Sublimation energy of Mg; 147 Electron affinity of X; 200 Atomisation enthalpy of X₂; 400 Enthalpy of formation of MgX₂; -450 2+ 2e+ Mg(+2X (8) b 2+ 2e + Mg( + X2 (8) a + Mg(g) + X₂ (8) 1451 Mg(g) + X₂ (8) Mg(s) + X2 (8) f 147 2+ Mg(g) +2X(g) MgX2 (s) d Sadly the colleague becomes discouraged and leaves the document incomplete, simply drawing boxes around unknown quantities. Complete the calculation by writing down the boxed quantities a-f on your answer paper. You may assume that the units are kJ mol-¹.arrow_forwardConstruct a Born–Haber cycle for the formation of the hypotheticalcompound NaCl2, where the sodium ion has a 2+charge (the second ionization energy for sodium is given inTable 7.2). (a) How large would the lattice energy need to befor the formation of NaCl2 to be exothermic? (b) If we wereto estimate the lattice energy of NaCl2 to be roughly equalto that of MgCl2 (2326 kJ/mol from Table 8.1), what valuewould you obtain for the standard enthalpy of formation,ΔHf°, of NaCl2?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_forward
- Calculate the lattice energy of RbCl using the following data: AH (k) Rb(3) Rb(g) Chig) CI(g) + e Rb(s) + ¾Cl(g} Rb(g) Rb"(g) + e¯ 86 409 2CI(g) CF(g) RÜCI(s) 242 -355 435arrow_forwardWhy catenation property is most remarkable in the case of carbon?arrow_forwardCalculate 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/molarrow_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_forwardWhich substance do you expect to have the greatest lattice energy: MgF2, CaF2, or ZrO2? Why?arrow_forwardDetermine the lattice energy of NaCl(s), using the data provided.arrow_forward
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