Uploaded September 2024 | Updated September 2026, 2 weeks ago
In this video, we discuss how lattice energy and hydration energy affect the dissolving process of ionic compounds like sodium chloride (NaCL) in water. Breaking the ionic bonds (lattice energy) requires energy (endothermic), while the hydration of ions releases energy (exothermic). The overall temperature change depends on which energy is greater.
While it is not covered in this video: ... predicting whether dissolution is endothermic or exothermic isn't always easy, but some general factors can help:
Higher Charge and Smaller Ions: Ions with higher charges and smaller sizes typically have higher lattice energies, making them harder to dissolve. However, they also have higher hydration energies.
Solubility Trends: Compounds that are highly soluble often have hydration energies that offset their lattice energies.
In this video, we discuss how lattice energy and hydration energy affect the dissolving process of ionic compounds like sodium chloride (NaCL) in water. Breaking the ionic bonds (lattice energy) requires energy (endothermic), while the hydration of ions releases energy (exothermic). The overall temperature change depends on which energy is greater.
While it is not covered in this video: ... predicting whether dissolution is endothermic or exothermic isn't always easy, but some general factors can help:
Higher Charge and Smaller Ions: Ions with higher charges and smaller sizes typically have higher lattice energies, making them harder to dissolve. However, they also have higher hydration energies.
Solubility Trends: Compounds that are highly soluble often have hydration energies that offset their lattice energies.
