**Calculate the Lattice Formation Enthalpy (Lattice Energy) of MgF₂(s)**Given the following information, calculate the lattice formation enthalpy of the lattice for MgF₂(s), in kJ/mol.| Process | Change in Energy (ΔH°) ||-------------------------------------|------------------------|| Heat of sublimation for Mg | 146 kJ/mol || First ionization energy for Mg | 738 kJ/mol || Second ionization energy for Mg | 1451 kJ/mol || Electron affinity of F | -328 kJ/mol || Bond dissociation energy of F₂ | 158 kJ/mol || Heat of formation for MgF₂ | -1124 kJ/mol |This table outlines the energy changes associated with each process involved in calculating the lattice energy for magnesium fluoride (MgF₂). The values listed in the table are essential for applying Hess's law to derive the overall lattice energy.

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Calculate the lattice formation enthalpy (lattice energy) of the lattice for MgF₂(s), in kJ/mol, given the following information:

Chemistry

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ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

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Exergonic Reaction

The term exergonic is derived from the Greek word in which ‘ergon’ means work and exergonic means ‘work outside’. Exergonic reactions releases work energy. Exergonic reactions are different from exothermic reactions, the one that releases only heat energy during the course of the reaction. So, exothermic reaction is one type of exergonic reaction. Exergonic reaction releases work energy in different forms like heat, light or sound. For example, a glow stick releases light making that an exergonic reaction and not an exothermic reaction since no heat is released. Even endothermic reactions at very high temperature are exergonic.

Question

**Calculate the Lattice Formation Enthalpy (Lattice Energy) of MgF₂(s)**

Given the following information, calculate the lattice formation enthalpy of the lattice for MgF₂(s), in kJ/mol.

| Process | Change in Energy (ΔH°) |
|-------------------------------------|------------------------|
| Heat of sublimation for Mg | 146 kJ/mol |
| First ionization energy for Mg | 738 kJ/mol |
| Second ionization energy for Mg | 1451 kJ/mol |
| Electron affinity of F | -328 kJ/mol |
| Bond dissociation energy of F₂ | 158 kJ/mol |
| Heat of formation for MgF₂ | -1124 kJ/mol |

This table outlines the energy changes associated with each process involved in calculating the lattice energy for magnesium fluoride (MgF₂). The values listed in the table are essential for applying Hess's law to derive the overall lattice energy.

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