Given the following thermodynamic data, calculate the lattice energy of CaBr2 (s). Term Value (kJ/mol) AĦ[CaBr2 (s)] -675 AH[Ca(g)] 178 AĘ Br(g)] 112 n(Ca) 590. I2 (Ca) 1145 EA(Br) -325 Express your answer to four significant figures, and include the appropriate units.

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Please answer question 17 part A and B

**Understanding Lattice Energy Through the Born-Haber Cycle**

By convention, the *lattice energy* is the energy required to form one mole of a solid ionic crystalline lattice from its gaseous ions. Since we cannot directly measure lattice energies, we generally use the Born-Haber cycle to calculate the lattice energy from other measurable quantities. For instance, the Born-Haber cycle of sodium chloride is shown below.

***Figure 1 Explanation***

In the Born-Haber cycle, the lattice energy is calculated using the following parameters. The associated reaction for each is shown in Figure 1:

- \( \Delta H_f^\circ [\text{NaCl}(s)] \): Enthalpy of formation of NaCl.
- \( \Delta H_f^\circ [\text{Cl}(g)] \): Enthalpy of formation of gaseous Cl.
- \( \Delta H_f^\circ [\text{Na}(g)] \): Enthalpy of formation of gaseous Na.
- \( I_1 (\text{Na}) \): First ionization energy of Na.
- \( EA (\text{Cl}) \): Electron affinity of Cl.

**Born-Haber Cycle Diagram Explanation**

The diagram illustrates the Born-Haber cycle for NaCl:

1. \( \text{Na}(s) \) is converted into \( \text{Na}(g) \).
2. \( \text{Cl}_2(g) \) is dissociated into 2 \( \text{Cl}(g) \).
3. \( \text{Na}(g) \) is ionized to \( \text{Na}^+(g) \) plus an electron.
4. The electron is added to \( \text{Cl}(g) \) to form \( \text{Cl}^-(g) \).
5. The gaseous ions \( \text{Na}^+(g) \) and \( \text{Cl}^-(g) \) form the ionic lattice of \( \text{NaCl}(s) \) releasing the lattice energy.

**Part A: Ranking Ionic Compounds by Lattice Energy**

Rank the following ionic compounds by the magnitude of their lattice energy. Rank from highest to lowest magnitude of lattice energy:

- BeO
- Na\(_2\)O
- LiCl
- MgO
- Na\(_2\)S

[Interactive box for ranking, with options to reset
Transcribed Image Text:**Understanding Lattice Energy Through the Born-Haber Cycle** By convention, the *lattice energy* is the energy required to form one mole of a solid ionic crystalline lattice from its gaseous ions. Since we cannot directly measure lattice energies, we generally use the Born-Haber cycle to calculate the lattice energy from other measurable quantities. For instance, the Born-Haber cycle of sodium chloride is shown below. ***Figure 1 Explanation*** In the Born-Haber cycle, the lattice energy is calculated using the following parameters. The associated reaction for each is shown in Figure 1: - \( \Delta H_f^\circ [\text{NaCl}(s)] \): Enthalpy of formation of NaCl. - \( \Delta H_f^\circ [\text{Cl}(g)] \): Enthalpy of formation of gaseous Cl. - \( \Delta H_f^\circ [\text{Na}(g)] \): Enthalpy of formation of gaseous Na. - \( I_1 (\text{Na}) \): First ionization energy of Na. - \( EA (\text{Cl}) \): Electron affinity of Cl. **Born-Haber Cycle Diagram Explanation** The diagram illustrates the Born-Haber cycle for NaCl: 1. \( \text{Na}(s) \) is converted into \( \text{Na}(g) \). 2. \( \text{Cl}_2(g) \) is dissociated into 2 \( \text{Cl}(g) \). 3. \( \text{Na}(g) \) is ionized to \( \text{Na}^+(g) \) plus an electron. 4. The electron is added to \( \text{Cl}(g) \) to form \( \text{Cl}^-(g) \). 5. The gaseous ions \( \text{Na}^+(g) \) and \( \text{Cl}^-(g) \) form the ionic lattice of \( \text{NaCl}(s) \) releasing the lattice energy. **Part A: Ranking Ionic Compounds by Lattice Energy** Rank the following ionic compounds by the magnitude of their lattice energy. Rank from highest to lowest magnitude of lattice energy: - BeO - Na\(_2\)O - LiCl - MgO - Na\(_2\)S [Interactive box for ranking, with options to reset
## Thermodynamic Data and Lattice Energy Calculation of CaBr₂(s)

### Given Data

The following thermodynamic values are provided to calculate the lattice energy of calcium bromide (CaBr₂) in solid form:

| Term                      | Value (kJ/mol) |
|---------------------------|----------------|
| \( \Delta H_f^\circ [\text{CaBr}_2(s)] \)  | -675          |
| \( \Delta H_f^\circ [\text{Ca}(g)] \)      | 178           |
| \( \Delta H_f^\circ [\text{Br}(g)] \)      | 112           |
| \( I_1 (\text{Ca}) \)     | 590            |
| \( I_2 (\text{Ca}) \)     | 1145           |
| \( EA (\text{Br}) \)      | -325           |

### Calculation Requirement

Using the above data, calculate the lattice energy of CaBr₂(s) and express your answer to four significant figures, including the appropriate units.

**Note:** You may refer to available hints for further guidance on solving the problem.

### Input Fields

- \( \Delta H_{\text{latt}} = \) [Value] [Units]

Ensure that all data inputs are accurate and consistent with the given thermodynamic values.
Transcribed Image Text:## Thermodynamic Data and Lattice Energy Calculation of CaBr₂(s) ### Given Data The following thermodynamic values are provided to calculate the lattice energy of calcium bromide (CaBr₂) in solid form: | Term | Value (kJ/mol) | |---------------------------|----------------| | \( \Delta H_f^\circ [\text{CaBr}_2(s)] \) | -675 | | \( \Delta H_f^\circ [\text{Ca}(g)] \) | 178 | | \( \Delta H_f^\circ [\text{Br}(g)] \) | 112 | | \( I_1 (\text{Ca}) \) | 590 | | \( I_2 (\text{Ca}) \) | 1145 | | \( EA (\text{Br}) \) | -325 | ### Calculation Requirement Using the above data, calculate the lattice energy of CaBr₂(s) and express your answer to four significant figures, including the appropriate units. **Note:** You may refer to available hints for further guidance on solving the problem. ### Input Fields - \( \Delta H_{\text{latt}} = \) [Value] [Units] Ensure that all data inputs are accurate and consistent with the given thermodynamic values.
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