The lattice dissociation enthalpy is the enthalpy change needed to convert 1 mole of solid crystal into its scattered gaseous ions. Lattice dissociation enthalpies are always positive. The lattice formation enthalpy is the enthalpy change when 1 mole of solid crystal is formed from its scattered gase...
Since the lattice formation enthalpy is electrostatic in nature, too, we can say that it depends on similar factors such as the charges of the ions, their sizes, and their arrangement in the solid. Thus, for a given arrangement of ions, the lattice energy increases as the charges on the...
Hsol The enthalpy change of solution is the energy absorber or released when 1 mole of an ionic solid dissolves in sufficient water to form a very dilute solution E.g. MgCl2(s) + aq → Mg+2(aq) + 2Cl-(aq) +3.9kJ·mol-1 NaCl(s) + aq → Na+(aq) + Cl-(aq) -55kJ·mol-1...
The lattice energy of a compound is defined as the formation of gaseous ions from a solid ionic compound. It depends on the charge present on the ions and the size of the ions. Smaller the size and higher is the charge on ions, larger is the lattice energy of ...
Which of the following will have the smallest lattice energy (bond strength)? a. KCI b. CaS c. MgO d. Na2O Which compound has the highest lattice enthalpy? A. CaO B. CaS C. LiF D. LiI Which of the following shows the correct order of i...
So lattice enthalpy could be described in either of two ways. You could describe it as the enthalpy change when 1 mole of sodium chloride (or whatever) was formed from its scattered gaseous ions. In other words, you are looking at a downward arrow on the diagram. ...