Born-Haber Cycle
Chemistry ⇒ Thermochemistry and Energetics
Born-Haber Cycle starts at 12 and continues till grade 12.
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Describe the difference between lattice enthalpy and enthalpy of formation.
Describe the role of electron affinity in the Born-Haber cycle.
Describe the significance of the Born-Haber cycle in understanding the formation of ionic compounds.
Explain why the Born-Haber cycle for Al2O3 includes three ionization energies for aluminum.
Calculate the lattice enthalpy of NaCl given the following data (all values in kJ/mol): Enthalpy of formation = -411, Sublimation of Na = +108, Ionization energy of Na = +496, Bond dissociation energy of Cl2 = +242, Electron affinity of Cl = -349. (Assume bond dissociation energy is for 1 mole of Cl2.)
Given the following data for the formation of CaCl2 (all in kJ/mol): Enthalpy of formation = -795, Sublimation of Ca = +178, First ionization energy of Ca = +590, Second ionization energy of Ca = +1145, Bond dissociation energy of Cl2 = +242, Electron affinity of Cl = -349. Calculate the lattice enthalpy of CaCl2.
Given the following data for the formation of KCl (all in kJ/mol): Enthalpy of formation = -437, Sublimation of K = +89, Ionization energy of K = +419, Bond dissociation energy of Cl2 = +243, Electron affinity of Cl = -349. Calculate the lattice enthalpy of KCl.
Given the following data for the formation of MgO (all in kJ/mol): Enthalpy of formation = -602, Sublimation of Mg = +150, First ionization energy of Mg = +738, Second ionization energy of Mg = +1451, Bond dissociation energy of O2 = +498, First electron affinity of O = -141, Second electron affinity of O = +744. Calculate the lattice enthalpy of MgO.
Which of the following factors increases the lattice enthalpy of an ionic compound? (1) Larger ionic radii, (2) Higher ionic charges, (3) Lower ionic charges, (4) Lower charge density.
Which of the following is a correct statement about the electron affinity step in the Born-Haber cycle? (1) It is always endothermic, (2) It is always exothermic, (3) It can be either exothermic or endothermic, (4) It is not included in the cycle.
Which of the following is NOT a reason for discrepancies between experimental and theoretical lattice enthalpy values? (1) Covalent character in the compound, (2) Inaccurate ionization energy data, (3) Use of Hess's Law, (4) Polarization of ions.
Which of the following is NOT a step in the Born-Haber cycle for NaBr? (1) Sublimation of Na, (2) Ionization of Na, (3) Dissociation of Br2, (4) Hydration of Br−.
Fill in the blank: The Born-Haber cycle is a _______ cycle that applies Hess's Law to ionic compounds.
Fill in the blank: The energy required to remove one electron from a gaseous atom is called _______.
Fill in the blank: The enthalpy change when one mole of an ionic solid is formed from its gaseous ions is called _______.
Fill in the blank: The process of converting a solid metal to gaseous atoms is called _______.
State whether the following statement is true or false: The Born-Haber cycle can be used to calculate the enthalpy of solution of an ionic compound.
State whether the following statement is true or false: The first ionization energy is always an exothermic process.
State whether the following statement is true or false: The lattice enthalpy of CaF2 is greater than that of NaF.
The enthalpy of formation of an ionic compound is the sum of all the enthalpy changes in the Born-Haber cycle. (Yes/No)
