LiCl is more covalent than KCl because This is due to a phenomenon called polarization. It causes the formation of partial covalent character in an ionic bond. The anion here is same, Cl-, but the cation Li+ is much smaller than K+ and so more polarization occurs in LiCl, thereby making it more covalent than KCl.

A binary molecular compound is a molecular compound that is composed of two elements. In general, the elements that combine to form binary molecular compounds are both nonmetals….Binary Molecular Compound Names.

There is a couple different ways to determine if a bond is ionic or covalent. By definition, an ionic bond is between a metal and a nonmetal, and a covalent bond is between 2 nonmetals. So you usually just look at the periodic table and determine whether your compound is made of a metal/nonmetal or is just 2 nonmetals.

Smaller the cation, greater is its polarizing power and hence larger is the covalent character. The covalent character decreases as the size of cation increases LiCl > NaCl > KCl > RbCl. Thus LiCl is more covalent than KCl and hence KCl is more soluble in water because of decreased covalent character.

In LiCl and KCl the anions are the same. From the periodic table, we can see that Li+ is smaller than K+.So in LiCl more polarisation occurs and makes it more covalent than KCl.

Rubidium chloride (RbCl) is more ionic than sodium chloride.

BeCl2 is more covalent than LiCl. As per the Fajan’s rule, more the polarisation, more will be the covalent character.

Smaller the cation, greater is its polarizing power and hence larger is the covalent character. Thus LiCl is more covalent than KCl and hence KCl is more soluble in water because of decreased covalent character.

LiCl. Because the Li+ ion is smaller than the Na+ ion, the Coulombic attractions between ions in LiCl are stronger than in NaCl. This results in a greater lattice enthalpy. However, the dissolution of LiCl in water is an exothermic process.

Bond-breaking is an endothermic process. Energy is released when new bonds form. Whether a reaction is endothermic or exothermic depends on the difference between the energy needed to break bonds and the energy released when new bonds form.

The dissolution of ammonium chloride is endothermic.

Dissolution of sodium chloride (table salt) in water is endothermic.

It takes just slightly more energy to separate the ions from one another than is released from the water molecules surrounding the ions. More energy is released into the solution than is required to pull apart the ions; therefore dissolving sodium hydroxide in water is exothermic.

The reaction of HCl(aq), a strong acid, with NaOH(aq), a strong base, is an exothermic reaction.