General Chemistry
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Given the following data, calculate the second electron affinity of sulfur. Is the S2– more stable as a free ion or in CaS?
The lattice energy of CuCl2(s) is 2824 kJ/mol. Use the Born-Haber cycle to determine the ΔH°f for CuCl2(s) from its elements. Compare this with the ΔH°f for CuCl(s) (–137.2 kJ/mol) and determine which compound is more stable.
Using knowledge of the formation of KCl from its elements, construct a Born-Haber cycle for KCl.
Determine the lattice energy of Li2O using a Born-Haber cycle and the information below.
Identify the steps that are expected to be exothermic in the Born–Haber cycle for the formation of MgBr2.
How large must the lattice energy be for the formation of a hypothetical compound MgBr3 (the magnesium ion has a 3+ charge) to be exothermic?
Calculate the lattice energy of NaBr.
The Born–Haber cycle is an approach to studying energy changes during the formation of a crystalline solid. Using the Born–Haber cycle, determine lattice energy for MgCl2. Use the following values:
ΔHsub for magnesium = 148 kJ/molIE1 and IE2 for magnesium = 737 kJ/mol and 1450 kJ/mol, respectivelyBond energy for Cl—Cl = 239 kJ/molEA for chlorine = −348.5 kJ/molEnthalpy of formation (ΔH°f) for MgCl2(s) = −641.3 kJ/mol
In the steps of the Born-Haber cycle for Na2O, how many ionization energies (IE) and how many electron affinities (EA) are there?
The heat of sublimation of strontium (Sr) is 163 kJ/mol and ΔH°f(SrCl2) = –828.9 kJ/mol. Calculate the lattice energy of strontium chloride.
A hypothetical halogen, J, has ΔHdiss,J2 = 166 kJ/mol and EA = −324 kJ/mol. Using the Born-Haber cycle, what is the lattice energy for LiJ? (ΔH°f,LiJ = −587.2 kJ/mol, I.E.1,Li = 519 kJ/mol, ΔHsub,Li = 155.3 kJ/mol.)
Use the Born–Haber cycle and data from Appendix IIB and Table 9.3 to calculate the lattice energy of SrO. (ΔHsub for strontium is 164 kJ/mol; IE1 and IE2 for strontium are 550 kJ/mol and 1064 kJ/mol, respectively; EA1 and EA2 for O are –141 kJ/mol and 744 kJ/mol, respectively.)