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Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074

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BuyFindarrow_forward

Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074
Textbook Problem

Examine the trends in lattice energy in Table 12.1. The value of the lattice energy becomes somewhat more negative on going from NaI to NaBr to NaCl, and all are in the range from −700 to −800 kJ/mol. Suggest a reason for the observation that the lattice energy of NaF (Δlattice U = −926 kJ/mol) is much more negative than those of the other sodium halides.

TABLE 12.1

Lattice Energies of Some Ionic Compounds

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Interpretation Introduction

Interpretation:

The reason behind the lattice energy of sodium fluoride is more negative than the other sodium halides has to be explained.

Concept introduction:

Lattice formation enthalpy is the enthalpy change when one mole of solid crystal is formed from its scattered gaseous ions.

Explanation

The lattice energy of sodium fluoride is more negative than the other sodium halides because, lattice energy is mainly depends on the charge and size of the ions. Lattice built from smaller ions leads to more negative for the lattice energy...

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