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AP Chemistry
6.9 Hess’s Law
6.8 Enthalpy of Formation
2.3 Structure of Ionic Solids
1.7 Periodic Trends
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An energy level diagram in grayscale. A single vertical upward arrow on the far left is labeled Enthalpy, H. Six horizontal solid black line segments represent energy levels. Level 0 at mid-height is labeled M(s) + 1/2 X2(g). A lower level below Level 0 is labeled MX(s); a solid downward arrow from Level 0 to this lower level is labeled Step 1: Delta H1 = -560 kJ/mol. Above Level 0, Level 1 is labeled M(g) + 1/2 X2(g); an upward arrow from Level 0 to Level 1 is labeled Step 2: Delta H2 = +90 kJ/mol. Above Level 1, Level 2 is labeled M+(g) + e- + 1/2 X2(g); an upward arrow from Level 1 to Level 2 is labeled Step 3: Delta H3 = +420 kJ/mol. Above Level 2, Level 3 is labeled M+(g) + e- + X(g); an upward arrow from Level 2 to Level 3 is labeled Step 4: Delta H4 = +80 kJ/mol. Just below Level 3, Level 4 is labeled M+(g) + X-(g); a downward arrow from Level 3 to Level 4 is labeled Step 5: Delta H5 = -330 kJ/mol. A dashed downward vertical arrow connects Level 4 directly to the lowest level MX(s) and is labeled Step 6: Delta H_lattice = ?. No other text, lines, or annotations appear.
Enthalpy diagram for the Born-Haber cycle of \(\text{MX(s)}\).
The enthalpy diagram below illustrates a Born-Haber cycle for the formation of the ionic compound \(\text{MX(s)}\) from its elements in their standard states at \(298 \text{ K}\).

Which of the following correctly identifies the thermodynamic process for Step 5 and the lattice enthalpy (\(\Delta H^\circ_{\text{lattice}}\)) for the reaction \(\text{M}^+\text{(g)} + \text{X}^-\text{(g)} \rightarrow \text{MX(s)}\)?

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