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(D) The Born-Haber cycle relates the standard enthalpy of formation $(\Delta H_f^\circ)$ of an ionic compound to its constituent elements' properties.

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the lattice energy

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(D) The Born-Haber cycle relates the standard enthalpy of formation $(\Delta H_f^\circ)$ of an ionic compound to its constituent elements' properties.The equation is: $\Delta H_f^\circ = \Delta H_{sub} + IE + \Delta H_{diss} + EA + U$Using the values from the cycle:$\Delta H_{sub} = +108 \ kJ/mol$$IE = +496 \ kJ/mol$$\Delta H_{diss} = +122 \ kJ/mol$$EA = -349 \ kJ/mol$$U = -788 \ kJ/mol$Comparing the absolute magnitudes of these energy terms,the lattice energy $(U = -788 \ kJ/mol)$ is the largest in magnitude. This large negative value is the primary driving force for the formation and stability of the solid ionic lattice.

In the Born-Haber cycle for the formation of solid common salt $(NaCl)$,the largest contribution to the stability of the crystal lattice comes from:

Similar Questions

The electronic configurations of four elements $L$,$P$,$Q$,and $R$ are given as: $L (1s^2, 2s^2 2p^4)$; $Q (1s^2, 2s^2 2p^6, 3s^2 3p^5)$; $P (1s^2, 2s^2 2p^6, 3s^1)$; $R (1s^2, 2s^2 2p^6, 3s^2)$. The formulas of the ionic compounds that can be formed between these elements are:

Which pair will form the most stable ionic bond?

Explain the Lattice Enthalpy.

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Element $x$ is strongly electropositive and $y$ is strongly electronegative. Both elements are univalent. The compound formed from their combination will be:

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