The reason for the formula of NaF to not be NaF 2 has to be determined. Concept Introduction: Lattice energy is used to determine the bond strength in ionic compounds. It is the heat of formation for ions of opposite charge in the gaseous phase combine to form an ionic solid. Lattice energy is the energy required to separate a mole of an ionic solid into gaseous ions. It cannot be measured empirically but it can be estimated by the Born-Haber cycle. MX ( s ) → M + ( g ) + X − ( g ) The two main factors responsible for the magnitude of the lattice energy are the charge and radius of the bonded ions. The effect of those factors is as follows: 1. If the charge of the ions increases, the lattice energy increases. 2. If the size of the ions increases, the lattice energy decreases.

Question

Want to see the full answer?

Answer 1

Question

Chapter 9, Problem 9.7QE

Interpretation Introduction

Interpretation:

The reason for the formula of NaF to not be NaF2 has to be determined.

Concept Introduction:

Lattice energy is used to determine the bond strength in ionic compounds. It is the heat of formation for ions of opposite charge in the gaseous phase combine to form an ionic solid.

Lattice energy is the energy required to separate a mole of an ionic solid into gaseous ions. It cannot be measured empirically but it can be estimated by the Born-Haber cycle.

MX(s)→M+(g)+X−(g)

The two main factors responsible for the magnitude of the lattice energy are the charge and radius of the bonded ions. The effect of those factors is as follows:

1. If the charge of the ions increases, the lattice energy increases.

2. If the size of the ions increases, the lattice energy decreases.

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Students have asked these similar questions

Use the Born-Haber cycle to calculate the lattice energy of KF. [The heat of sublimation of K is 91.6 kJ·mol−1 and ΔfH(KF) = −567.3 kJ·mol−1. Bond enthalpy for F2 is 158.8 kJ·mol−1. Other data may be found in the Ionization Energies Table and the Electron Affinities Table.]

Using the following data, calculate the lattice energy of calcium chloride: Ca2+(g) + 2Cl– (g) → CaCl2(s) ΔHlattice = ? Sublimation enthalpy of calcium ΔH = 177.8 kJ/mol First ionization energy of calcium ΔH = 590.2 kJ/mol Second ionization energy of calcium ΔH = 1144.2 kJ/mol First electron affinity of chlorine ΔH = –349 kJ/mol Heat of formation of CaCl2(s) ΔH = –795.4 kJ/mol Bond energy of Cl2 (see Table 2) Use Hess’s law to calculate the lattice energy of calcium chloride. set-up must show all the chemical equations and you must show how their H values add up to give your answer.

Write the steps (reactions) for the Born-Haber cycle for MgCl2(s). Use the Born-Haber cycle to calculate the lattice energy of MgCl2(s). Some useful data to work with: For Mg: ΔΔHsub = 147 kJ/mol, IE1 and IE2 are 738 kJ/mol and 1450 kJ/mol, respectively. For chlorine: Bond energy = 243 kJ/mol, EA1 = -349 kJ/mol, respectively. The enthalpy of formation of magnesium chloride is -748.8 kJ/mol.