Full explanation of applications of hydrogen bonding
Thermodynamic properties.
Hydrogen fluoride is a weak acid and then HCL. Why?
One hydrogen atom is entrapped between two fluorine atoms, and it is not easy to remove a hydrogen atom from the HF molecule.
So Hydrogen fluoride is a weak acid from Hcl
Water molecules have higher boiling points than Hydrogen fluoride and Azane. Why?
In water molecules, two hydrogen atoms are present. So it forms two hydrogen bonds per molecule.
In hydrogen fluoride molecules only one hydrogen atom is present and forms only one hydrogen bond per molecule. Therefore boiling point of water is higher than hydrogen fluoride.
Covalent hydrides of group 4thA have a lower boiling point than the other covalent hydrides. Why?
Electronegativity of the elements of group 4th or lower than the other groups like group 5A, 6A and 7A.
So covalent hydrides of group 4th have lower intermolecular forces than the other covalent hydrides. Due to which boiling points of the covalent hydrides of group 4th is less than the other covalent hydrides.
Water is liquid but Hydrogen sulfide is gas at room temperature. Why?
In water molecules, strong hydrogen bonding is present between the water molecules. Due to which hydrogen sulfide is liquid at room temperature. Hydrogen sulfide has weak intermolecular forces between the molecules. Due to which hydrogen sulfide is gas at room temperature.
Boiling point of hydrogen fluoride is higher than HCL and HBR. Why?
In hydrogen fluoride molecules strong hydrogen bonding is present between the hydrogen fluoride molecules and boiling point of hydrogen fluoride molecules are higher than HCL and HBR.
In Hcl and Hbr molecules, hydrogen bonding is not present but dipole dipole forces are present which are weaker than hydrogen bonding. Due to which Advil and HBR have low boiling point than hydrogen fluoride.
No comments: