Could someone explain how to solve this for me? We have been studying fluoride in drinking...

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Could someone explain how to solve this for me?
We have been studying fluoride in drinking water. If you were toexamine your toothpaste one of the active ingredient is most likelyto be sodium fluoride. Given theinformation below write theequation associated with each one of the following energies,daw theBorn Haber Cycle and calculate the lattice energy for the formationof Sodiumfluoride.
First Ionization energy of Na: 496 kJ/molFirst
Electron affinity of F: â€“328 kJ/mol
Enthalpy of atomization Na: 108 kJ/molF2
bond energy: 159 kJ/mol
Enthalpy of formation of NaF(s) = â€“574 kJ/mol

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3.9 Ratings (621 Votes)

Given data

First Ionization energy of Na: 496 kJ/molÂ Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Na(g) ------->Na⁺ + e^-

Electron affinity of F: â€“328 kJ/molÂ Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â F(g) + e^- -------------> 2F(g)

Enthalpy of atomization Na: 108 kJ/mol Na(s) -------------> Na(g)

bond energy of fluorine gas: 159 kJ/molÂ Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â F₂(g)------------------> 2F(g)

Enthalpy of formation of NaF(s) = â€“574 kJ/molÂ Â Â Â Â Â Â Â Â Na(s) + 1/2F₂ ---------> NaF

Using Born Haber cycle

Enthalpy of formation of NaF_(s) = Enthalpy of atomization Na + First Ionization energy of Na + bond energy of fluorine gas + Electron affinity of F + Lattice energy of NaF

-574 = 108 + 496 + 159 -328 + Lattice energyÂ Â Â Â Â (all the energies are in kj/mol)

Lattice energy = -574 -108-496-159+328 = -1009 kj/mol

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