Algor Cards

The Born-Haber Cycle and Lattice Enthalpy

Concept Map

Algorino

Edit available

The Born-Haber cycle is a fundamental concept in chemistry that explains the energy changes during the formation of ionic compounds. It uses Hess's Law to calculate lattice enthalpy, a measure of the energy needed to separate one mole of an ionic solid into gaseous ions. Factors like ionic charges and ion sizes impact lattice enthalpy, with greater charges and smaller ions increasing it. The cycle also helps distinguish between ionic and covalent characteristics in bonds, based on the comparison of theoretical and experimental enthalpy values.

Exploring the Born-Haber Cycle for Ionic Compound Formation

The Born-Haber cycle is an indispensable concept in chemistry that elucidates the formation of ionic compounds through a series of energy changes. By invoking Hess's Law, which asserts that the total enthalpy change of a reaction is invariant with respect to the reaction pathway, the cycle facilitates the computation of otherwise challenging enthalpy values, such as lattice enthalpy. Lattice enthalpy, the energy required to dissociate one mole of an ionic solid into its constituent gaseous ions, is calculated using the equation: ∆HΘLE = ∆HΘf - [ (∆HΘat (cation)) + (∆HΘat (anion)) + IE1 + EA1 ], where ∆HΘf denotes the enthalpy of formation, ∆HΘat represents the atomization enthalpy for the cation and anion, IE1 is the first ionization energy, and EA1 is the electron affinity.
3D crystalline model with alternating red and blue spheres representing ions in a cubic lattice, linked by transparent rods on a gray-white gradient background.

Determining Lattice Enthalpy via Born-Haber Cycles

To ascertain the lattice enthalpy of an ionic solid like potassium chloride (KCl), one must construct a Born-Haber cycle, apply Hess's Law to the cycle's steps, and then insert the known enthalpy values for formation, atomization, ionization, and electron affinity. For KCl, the lattice enthalpy is determined by subtracting the sum of the atomization enthalpies of potassium and chlorine, the ionization energy of potassium, and the electron affinity of chlorine from the enthalpy of formation of KCl. This methodology is similarly employed for other ionic compounds, such as magnesium oxide (MgO), where the calculation includes two ionization energies to account for magnesium's divalent charge.

Show More

Want to create maps from your material?

Enter text, upload a photo, or audio to Algor. In a few seconds, Algorino will transform it into a conceptual map, summary, and much more!

Learn with Algor Education flashcards

Click on each Card to learn more about the topic

00

Lattice enthalpy, the energy to break down one mole of an ionic solid into gaseous ions, is determined by the formula: ∆HΘLE = ∆HΘf - [ (∆HΘat (______)) + (∆HΘat (______)) + IE1 + EA1 ].

cation

anion

01

Born-Haber cycle application

Applies Hess's Law to relate lattice enthalpy to other enthalpy changes.

02

Enthalpy values in lattice enthalpy calculation

Includes formation, atomization, ionization, and electron affinity enthalpies.

Q&A

Here's a list of frequently asked questions on this topic

Can't find what you were looking for?

Search for a topic by entering a phrase or keyword