c) TABLE 2 shows several selected thermochemical data. TABLE 2 AH (kJ moll) Entahlpy Lattice energy of sodium oxide Enthalpy of formation of sodium oxide First ionisation energy of sodium First electron affinity of oxygen Second electron affinity of oxygen Enthalpy of atomization of oxygen -2570.0 -415.9 +495.9 -141.0 +791.0 +247.0 Based on the data in TABLE 2, i. construct the Bom-Haber cycle. ii. calculate the enthalpy of atomisation of sodium

c) TABLE 2 shows several selected thermochemical data. TABLE 2 AH (kJ moll) Entahlpy Lattice energy of sodium oxide Enthalpy of formation of sodium oxide First ionisation energy of sodium First electron affinity of oxygen Second electron affinity of oxygen Enthalpy of atomization of oxygen -2570.0 -415.9 +495.9 -141.0 +791.0 +247.0 Based on the data in TABLE 2, i. construct the Bom-Haber cycle. ii. calculate the enthalpy of atomisation of sodium

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter3: Atomic Shells And Classical Models Of Chemical Bonding

Section: Chapter Questions

Problem 7P

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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"!
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.
Construct 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?
At large interatomic separations, an alkali halide moleculeMX has a lower energy as two neutral atoms, M + X; atshort separations, the ionic form (M+)(X-) has a lowerenergy. At a certain distance, Rc, the energies of the twoforms become equal, and it is near this distance that theelectron will jump from the metal to the halogen atom during a collision. Because the forces between neutral atomsare weak at large distances, a reasonably good approximation can be made by ignoring any variation in potentialV(R) for the neutral atoms between Rc and R - `. For theions in this distance range, V(R) is dominated by theirCoulomb attraction.(a) Express Rc for the first ionization energy of the metalM and the electron affinity of the halogen X.(b) Calculate Rc for LiF, KBr, and NaCl using data fromAppendix F.
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