Ionic solids often tend to be an extremely stable compounds. The enthalpies of development of the ionic molecules cannot alone account for this stability. This compounds have secondary stability due to the lattice energy of the heavy structure. However, lattice energy cannot be straight measured. The Born-Haber cycle allows us to understand and determine the lattice energies of ionic solids.

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This module will present the idea the lattice energy, as well as one process that allows us to calculation it: the Born-Haber Cycle. In bespeak to usage the Born-Haber Cycle, there room several concepts that us must recognize first.

Lattice Energy

Lattice power is a type of potential energy that may be defined in 2 ways. In one definition, the lattice energy is the energy required to break apart an ionic solid and convert its ingredient atoms right into gaseous ions. This an interpretation causes the value for the lattice energy to constantly be positive, since this will constantly be one endothermic reaction. The other an interpretation says the lattice energy is the reverse process, an interpretation it is the power released when gaseous ions bind to type an ionic solid. Together implied in the definition, this process will always be exothermic, and also thus the value for lattice power will it is in negative. Its values space usually expressed through the systems kJ/mol.

Lattice power is offered to explain the stability of ionic solids. Some could expect together an ordered structure to be less stable because the entropy that the system would be low. However, the crystalline structure permits each ion to communicate with many oppositely fee ions, which causes a highly favorable adjust in the enthalpy the the system. A lot of power is released as the oppositely charged ions interact. It is this that reasons ionic solids to have actually such high melting and boiling points. Some call for such high temperatures the they decompose before they have the right to reach a melting and/or cook point.

Born-Haber Cycle

There are several important principle to understand before the Born-Haber Cycle can be applied to recognize the lattice power of an ionic solid; ionization energy, electron affinity, dissociation energy, sublimation energy, warmth of formation, and Hess"s Law.

Dissociation energy is the energy required to break apart a compound. The dissociation the a link is always an endothermic process, an interpretation it will always require an input of energy. Therefore, the adjust in energy is constantly positive. The size of the dissociation energy depends on the electronegativity that the atoms involved. The heat of formation is the change in energy when developing a compound from the elements. This might be hopeful or negative, depending upon the atoms involved and also how castle interact.

Using the Born-Haber Cycle

The values supplied in the Born-Haber Cycle are all predetermined alters in enthalpy because that the processes explained in the section above. Hess" Law allows us to add or subtract this values, which permits us to identify the lattice energy.


Step 5

Now the metal and nonmetal will be an unified to kind the ionic solid. This will cause a release of energy, which is dubbed the lattice energy. The value for the lattice power is the difference between the worth from action 1 and the worth from action 4.


The diagram listed below is an additional representation the the Born-Haber Cycle.

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Lattice energy: The difference in energy in between the expected experimental value because that the power of the ionic solid and also the actual worth observed. An ext specifically, this is the energy gap in between the energy of the separate gaseous ions and the power of the ionic solid. Ionization energy: The energy readjust associated with the removed of one electron from a neutral atom or ion. Electron affinity: The relax of energy linked with the addition of an electron to a neutral atom or ion. Hess" law states the the as whole energy that a reaction might be determined by breaking under the process into number of steps, then including together the transforms in energy of each step. Lattice Energy= <-436.68-89-(0.5*158)-418.8-(-328)> kJ/mol= -695.48 kJ/mol Lattice Energy= <-641.8-146-243-(737.7+1450.6)-(2*-349)> kJ/mol= -2521.1 kJ/mol MgO. It has actually ions through the biggest charge. AlCl3. Follow to the periodic trends, together the radius the the ion increases, lattice energy decreases.