Concept explainers
Interpretation:
The compound expected to have greater lattice energy among
Concept Introduction:
A three-dimensional array of ions constitutes the ionic compound lattice. They are stabilized because of attractive forces oppositely charged ions that lower the potential energy. The lattice energy of strong ionic solids is often very large because of small and densely charged ions.
Lower is the potential energy of interaction and more stable is the ionic solid. Hence the compounds that have high charge density on small space are the most stable ionic solids. For example, the calcium phosphate is made up of
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- 5. Which of the following alkali metal halides has the larger lattice energy, and which has the smaller lattice energy? Explain. (a) (b)arrow_forwardWhich pair will form a compound with the larger lattice energy: Na+ and F- ions or Mg2+ and F- ions? Justify your selection.arrow_forwardUse principles of atomic structure to answer each of the following: (1] (a) The radius of the Ca atom is 197 pm; the radius of the Ca2* ion is 99 pm. Account for the difference. (b) The lattice energy of CaO(s) is –3460 kJ/mol; the lattice energy of K20 is –2240 kJ/mol. Account for the difference. (c) Given these ionization values, explain the difference between Ca and K with regard to their first and second ionization energies. Element First lonization Energy (kJ/mol) Second lonization Energy (kJ/mol) K 419 3050 Ca 590 1140 (d) The first ionization energy of Mg is 738 kJ/mol and that of Al is 578 kJ/mol. Account for this difference.arrow_forward
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