Consider an ionic compound, MX, composed of generic metal M and generic, gaseous halogen X. • The enthalpy of formation of MX is AH; = -553 kJ/mol. %3D • The enthalpy of sublimation of M is AHsub = 129 kJ/mol. %3D • The ionization energy of M is IE = 491 kJ/mol. • The electron affinity of X is AHEA = -325 kJ/mol. (Refer to the hint). • The bond energy of X, is BE = 219 kJ/mol. Determine the lattice energy of MX.

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Consider an ionic compound, MXMX, composed of generic metal MM and generic, gaseous halogen XX.

  • The enthalpy of formation of MXMX is Δ?∘f=−553Δ⁢Hf∘=−553 kJ/mol.

  • The enthalpy of sublimation of MM is Δ?sub=129Δ⁢Hsub=129 kJ/mol.

  • The ionization energy of MM is IE=491IE=491 kJ/mol.

  • The electron affinity of XX is Δ?EA=−325Δ⁢HEA=−325 kJ/mol. (Refer to the hint).

  • The bond energy of X2X2 is BE=219BE=219 kJ/mol.

Determine the lattice energy of MXMX.

Δ?lattice=Δ⁢Hlattice=           kJ/mol
**Ionic Compound Calculation for Educational Use**

Consider an ionic compound, MX, composed of generic metal M and generic, gaseous halogen X.

- The enthalpy of formation of MX is \( \Delta H_f^\circ = -553 \) kJ/mol.
- The enthalpy of sublimation of M is \( \Delta H_{\text{sub}} = 129 \) kJ/mol.
- The ionization energy of M is IE \(= 491 \) kJ/mol.
- The electron affinity of X is \( \Delta H_{\text{EA}} = -325 \) kJ/mol. (Refer to the hint.)
- The bond energy of \( X_2 \) is BE \( = 219 \) kJ/mol.

**Objective:** Determine the lattice energy of MX.

\[ \Delta H_{\text{lattice}} = \, \boxed{\phantom{\text{input}}} \, \text{kJ/mol} \]

**Explanation of Calculation:**

The lattice energy can be calculated using the Born-Haber cycle, which involves summing the following thermodynamic processes:
1. Sublimation of M.
2. Ionization of M.
3. Atomization of \( X_2 \) (half the bond energy).
4. Electron affinity of X.
5. Formation of MX from gaseous ions. 

The enthalpy change for the formation of MX is equal to the sum of all steps, including the lattice energy, which we need to solve.
Transcribed Image Text:**Ionic Compound Calculation for Educational Use** Consider an ionic compound, MX, composed of generic metal M and generic, gaseous halogen X. - The enthalpy of formation of MX is \( \Delta H_f^\circ = -553 \) kJ/mol. - The enthalpy of sublimation of M is \( \Delta H_{\text{sub}} = 129 \) kJ/mol. - The ionization energy of M is IE \(= 491 \) kJ/mol. - The electron affinity of X is \( \Delta H_{\text{EA}} = -325 \) kJ/mol. (Refer to the hint.) - The bond energy of \( X_2 \) is BE \( = 219 \) kJ/mol. **Objective:** Determine the lattice energy of MX. \[ \Delta H_{\text{lattice}} = \, \boxed{\phantom{\text{input}}} \, \text{kJ/mol} \] **Explanation of Calculation:** The lattice energy can be calculated using the Born-Haber cycle, which involves summing the following thermodynamic processes: 1. Sublimation of M. 2. Ionization of M. 3. Atomization of \( X_2 \) (half the bond energy). 4. Electron affinity of X. 5. Formation of MX from gaseous ions. The enthalpy change for the formation of MX is equal to the sum of all steps, including the lattice energy, which we need to solve.
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