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This thermodynamic cycle describes the formation of an ionic compound MX from a metal element M and nonmetal element X in their standard states. Use it to answer the questions in the table below 900 800 700 600 + X enthalpy 400 300. 200. 100. 0. 100.- kJ/mol M3 What is the lattice enthalpy of MX? 1 kJ/mol What is the enthalpy of formation of MX?kJ/mol Suppose both the heat of sublimation of M and the electron affinity of X were smaller Would MX be more stable? Or less? o More stable. O Less stable. o It is impossible to tell without more information.

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Lattice energy of a solid is defined to be energy released when the cations and anions of the ionic compound combine to form an ionic solid as shown as follows: AH = Lattice energy So, the change in enthalpy for the reaction is equal to lattice energy of the reaction and calculated as follows: AH = Enthalpy of products-Enthalpy of reactants 500 kJ/mol =-100 kJ/mol -600 kJ/mol The enthalpy of formation of a compound is the sum of enthalpy of all the steps occurred in the process So, enthalpy of formation of MX(s) is given as follows: Enthalpy of formation of MX(s)-Enthalpy of atomisation of M+Ionizations enthalpy of M +Enthalpies of atomization of X + Electron gainenthalpy of X +Lattice enthalpy OR

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