Lattice energy

Lattice energy is the energy change associated with forming an ionic solid from its separated gaseous ions. Its value depends on the ions’ charges, sizes, and arrangement in the crystal.

Coulomb's law: The law relating the electrostatic force between two point charges to their charges and separation. It explains why stronger ionic charges and shorter interionic distances increase lattice energy.
Ionic bond: An electrostatic attraction between oppositely charged ions. Lattice energy measures the collective stabilization from ionic attractions in a solid.
Born–Haber cycle: A Hess's law cycle that relates an ionic solid's formation enthalpy to atomization, ionization, electron affinity, and lattice terms. It uses lattice energy to close a thermochemical cycle and infer otherwise inaccessible values.
Lattice enthalpy: An enthalpy change associated with forming an ionic crystal from gaseous ions, or the reverse process, depending on convention. Its sign and sometimes its meaning differ because sources use opposite formation and separation conventions.
Born–Landé equation: An equation estimating ionic-crystal lattice energy from electrostatic attraction and short-range repulsion. It translates ion charges, crystal spacing, and structure into an energy estimate.
Enthalpy: A thermodynamic state function equal to a system's internal energy plus pressure–volume product. Lattice energy is commonly reported as an enthalpy change at constant pressure.
Hess's law: The principle that a reaction's enthalpy change is independent of the route between the same initial and final states. It makes indirect calculation of lattice energy possible through a Born–Haber cycle.
Lattice dissociation energy: The energy required to separate an ionic solid into its gaseous ions. It describes the reverse process, so its sign is opposite under a consistent energy convention.
Madelung constant: A dimensionless factor expressing the summed electrostatic interactions in an ionic crystal's lattice. It captures how the crystal's geometry changes the net attraction between ions.
Standard enthalpy change of formation: The enthalpy change when one mole of a substance forms from its elements in standard states. It appears in Hess cycles used to infer lattice energy from measurable reactions.

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