Thermodynamic data for the components for magnesium oxide are
|
Name of enthalpy change
|
Energy change (kJ mol-1)
|
|
Enthalpy of formation of magnesium oxide
|
-602
|
|
Enthalpy of atomisation of magnesium
|
150
|
|
First and second ionisation energy of magnesium
|
2188
|
|
Enthalpy of atomisation of oxygen
|
248
|
|
First and second electron affinity of oxygen
|
702
|
Which of the following is used to calculate the lattice enthalpy of magnesium oxide
-602 - 150 - 2188 - 248 + 702
-602 - 150 - 2188 - 248 - 702
-602 - 150 - 2188 -
- 702
-602 - 150 - 2188 - (2 x 248) - 702
Using the information in the table to answer the question
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Enthalpy Change
|
Value (kJ mol-1)
|
|
ΔHӨlatt CaF2
|
2651
|
|
ΔHӨhyd Ca2+
|
-1616
|
|
ΔHӨhyd F-
|
-504
|
Which of the following is the correct value for the enthalpy change of solution, ΔHӨsol, of calcium fluoride, CaF2?
+2651 + [(-1616) + (-504)]
+2651 - [(-1616) + (-504)]
+2651 + [(-1616) + (-1008)]
+2651 - [(-1616) + (-1008)]
Which of the following ionic compounds has the greatest lattice enthalpy?
Which of the following changes is not endothermic?
Which statements are correct for ionic compounds?
- Solubility in water depends on the relative magnitude of the lattice energy compared to the hydration energy
- Melting points of ionic compounds increase as the size of the cation increases
- The enthalpy of solution for calcium chloride is represented by CaCl2 (s) → CaCl2 (aq)
