1. Using radii from Resource section 1 (p.901) and Born-Lande equation, calculate thelattice energy for PbS, which crystallizes in the NaCl structure. Then, use the Born-Haber cycleto obtain the value of lattice energy for PbS. You will need the following data following data:AH Pb(g) = 196 kJ/mol; AHƒ PbS = −98 kJ/mol; electron affinities for S(g)→S¯(g) is -201 kJ/mol;S¯(g)(g) is 640kJ/mol. Ionization energies for Pb are listed in Resource section 2, p.903.Remember that enthalpies of formation are calculated beginning with the elements in theirstandard states (S8 for sulfur). The formation of S2, AHF: S2 (g) = 535 kJ/mol.Compare the two values, and explain the difference.(8 points)

Step 1: We must take into account the following equation in order to use the Born-Mayer equation to…

Answered: 1. Using radii from Resource section 1…

Chemistry: The Molecular Science

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Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter19: The Chemistry Of The Main-group Elements

Section: Chapter Questions

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Although nitrogen trifluoride (NF3) is a thermally stable compound, nitrogen triiodide (Nl3) is known to be a highly explosive material. NI3 can be synthesized according to the equation BN(s)+3IF(g)BF3(g)+NI3(g) a. What is the enthalpy of formation for NI3(s) given the enthalpy of reaction ( 307 kJ) and the enthalpies of formation for BN(s) (254 kJ/mol), IF(g) ( 96 kJ/mol), and BF3(g) ( 1136 kJ/mol)? b. It is reported that when the synthesis of NI3 is conducted using 4 moles of IF for every l mole of BN. one of the by-products isolated is [IF2]+ [BF4]. What are the molecular geometries of the species in this by-product? What are the hybridizations of the central atoms in each species in the by-product?
Calculate the lattice energy of potassium fluoride, KF, using the BornHaber cycle. Use thermodynamic data from Appendix C to obtain the enthalpy changes for each step. (Note: You will obtain a slightly different answer if you use values given in Chapter 8 for the ionization energy and electron affinity, which are energy values at 0 K rather than the enthalpy changes at 298 K.)
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.
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
Calculate the lattice energy of magnesium sulfide from the data given below. Mg(s) Mg(g) AE 148 kJ/mol Mg2g) 8S(g) AE 2232 kJ/mol 2e AE 2186 kJ/mol Mg(g) S8(s) Sig) 2eSg) AE= 450 kJ/mol 8Mg(s)S8(s) -» 8M9S(s) AE = -2744 kJ/mol Mg2+(g) S2g) MgS(s) AElattice = ?
Write the steps (reactions) for the Born-Haber cycle for MgCl2(s). Use the Born-Haber cycle to calculate the lattice energy of MgCl2(s). Some useful data to work with: For Mg: ΔΔHsub = 147 kJ/mol, IE1 and IE2 are 738 kJ/mol and 1450 kJ/mol, respectively. For chlorine: Bond energy = 243 kJ/mol, EA1 = -349 kJ/mol, respectively. The enthalpy of formation of magnesium chloride is -748.8 kJ/mol.
. Calculate the lattice energy of Li₂O(S). (AH(sublimation) K(s) = 77 kJ/mole, and AHƒ (Li₂O(s)) = −361 kJ/mole)
Given the following thermodynamic data, calculate the lattice energy of LiCl:ΔH°f[LiCl(s)] = -409 kJ/molΔH°sublimation [Li] = 161 kJ/molBond energy [Cl-Cl] = 243 kJ/molIE1 (Li) = 520 kJ/molEA1 (Cl) = -349 kJ/mol -1682 kJ/mol -984 kJ/mol -1560 kJ/mol -862 kJ/mol -1213 kJ/mol
Determine 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)
Use the data given below to construct a Born-Haber cycle to determine the lattice energy of CaO. A H°(kJ) Ca(s) → Ca(g) 193 Ca(g) → Cat (g) + e 590 Cat (g) → Ca2+(g) + e 1010 20(g) → O2(g) -498 O(g) + e O(g) -141 O(g) + e → O2(g) 878 Ca(s) + O2(g) → CaO(s) -> -635 O-2667 kJ O-3414 kJ O +1397 kJ +3028 kJ O-2144 kJ
Calculate 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)?
(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"!

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