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B
Only of radius of the anion
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C
Cation to anion radius ratio
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D
Sum of the radii of cation and anion
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Solution
The correct option is D
Sum of the radii of cation and anion
The explanation of the correct option:
Option (D): Sum of radii of cation and anion
The entire amount of energy necessary to break or convert one mole of aqueous ionic compounds into one mole of ions is known as lattice energy.
Lattice energy is given by Coulomb's law where Q1 and Q2 are numerical ion charges, r is the distance between ion centers, and K is constant.
Also, lattice energy can be given by where ra is the radius of the anion and rc is the radius of the cation.
The entire distance between two ions in an ionic compound is important in determining the molecule's lattice energy. The weaker the ionic link between two ions, the less lattice energy is required to break the binding and release the compound's ions.
The larger the magnitude of charge in the ions, the more strongly the ions are attracted to one other, necessitating the use of more lattice energy to break the ionic bond.