Calculating Lattice Energy: LiF vs. CsF

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The discussion focuses on calculating the lattice energy of LiF and CsF, emphasizing the use of Coulomb's law. The user initially struggles with determining the distance (r) between ion centers. It is clarified that larger ions result in a greater r value, leading to lower lattice energy due to inverse proportionality. Consequently, LiF, with smaller ions, has a more exothermic lattice energy compared to CsF. Understanding the relationship between ion size and lattice energy is crucial for accurate calculations.
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I'm having some problems with the calculations associated with this problem:

Which compound in each of the following pairs of ionic substances has the most exothermic lattice energy?

(a) LiF
CsF

I know I need to use Coulomb's law, but I don't know how to calculate r (the distance between the ion centers)

Any help is greatly appreciated. Thanks
 
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nevermind, I have found out that bigger ions have a bigger r value and thus via the inverse proportionality the higher lattice energy corresponds to the lower r value
 

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