The boiling point of NH3 H2O and HF are exceptionally higher explain
The boiling point of NH3 H2O and HF are exceptionally higher explain
Boiling point depends upon the intermolecular forces of attraction ,which in turn depends upon the difference in electronegativities of the combined species.
In case of HF, difference in electronegativity of hydrogen and fluorine is greater. Hence HF molecule is highly polarized, due to this ,molecules are associated strongly by strong intermolecular hydrogen bonds.Thus higher boiling point is recorded for HF.
In NH₃,difference in electronegativity of nitrogen and hydrogen is comparatively lesser.Hence in NH₃,intermolecular hydrogen bonds are relatively weaker.Thus boiling point of NH₃ is lesser than that of HF.
I assume that your question relates to the fact that these three small molecules have boiling points “higher than other small molecules with similar molecular weight.” The answer is that only molecules with hydrogen atoms covalently bonded to O, N, or F can participate in hydrogen bonding. Hydrogen bonding isn’t particularly strong, but when you have a lot of hydrogen bonds it makes a real difference in the energy needed to move the molecules from liquid to the gas phase.
Boiling point depends upon the intermolecular forces of attraction ,which in turn depends upon the difference in electronegativities of the combined species.
In case of HF, difference in electronegativity of hydrogen and fluorine is greater. Hence HF molecule is highly polarized, due to this ,molecules are associated strongly by strong intermolecular hydrogen bonds.Thus higher boiling point is recorded for HF.
In NH₃,difference in electronegativity of nitrogen and hydrogen is comparatively lesser.Hence in NH₃,intermolecular hydrogen bonds are relatively weaker.Thus boiling point of NH₃ is lesser than that of HF.
I assume that your question relates to the fact that these three small molecules have boiling points “higher than other small molecules with similar molecular weight.” The answer is that only molecules with hydrogen atoms covalently bonded to O, N, or F can participate in hydrogen bonding. Hydrogen bonding isn’t particularly strong, but when you have a lot of hydrogen bonds it makes a real difference in the energy needed to move the molecules from liquid to the gas phase.
