nerolights.blogg.se - Lattice energy trend

ΔLatticeU denotes the molar lattice energy.The molar lattice energy of an ionic crystal in terms of molar lattice enthalpy, pressure, and volume change can be expressed as follows: Read More: Chemical Bonding and Molecular Structure Important Questions The smaller the size of the constituent ions, the greater will be the lattice energy.Small atoms have smaller interatomic distances in the ionic lattice and stronger binding forces.The more the distance between the ions in a lattice, the weaker the electrostatic forces, and the lower will be the lattice energy.Lattice Energy is inversely proportional to the distance between the ions.Hence, it is considered that the lattice energy of CaCl2 is greater than that of KCl.Thus, the electrostatic forces of attraction are stronger in calcium chloride than in potassium chloride.

The reason for the same is that the magnitude of the positive charge held by the calcium cation (+2) is greater than that held by the potassium cation (+1).

For instance, the lattice energy of calcium chloride is greater than that of potassium chloride despite the similarity in the crystal arrangements.

The greater the charge, the stronger the force of attraction, and thus the stronger will be the lattice.

The strength of the electrostatic force of attraction is in direct proportion to the magnitude of the charge held by the ions.

The individual ions in an ionic lattice are attracted to each other due to the electrostatic forces between them.

Radius of Ions (Distance Between the Ions).

There are two major factors that affect the lattice energy of an ionic compound which are as follows:

r0 is the internuclear distance of the ions.

Q1 and Q2 are the positive and negative ions of the compound.

U is the Lattice Energy of an Ionic Compound.Lattice Energy of ionic compounds is calculated using the simplified form of Coulomb’s Law.

The exact value of the lattice energy of an ionic compound cannot be determined easily.