7) Consider H;O and H;S. a. What two properties of a molecule are used to predict the intermolecular forces that molecule can participate in? b. What intermolecular forces occur between two molecules of H20? c. What intermolecular forces occur between two molecules of H;S? d. Which molecule has the highest boiling point? e. Are these molecules miscible?
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The intermolecular attractions occur between the molecules of hydrogen is bonded to an electronegative atom such as F, O, and N, and the lone pairs of another electronegative atom are termed as the hydrogen bonding. Example: water, ammonia. When a less electronegative atom is bonded to hydrogen, the electronegative difference between the hydrogen and the other bonded atom results in the formation of dipoles. When the dipoles of two adjacent molecules come in contact with each other, the dipole-dipole interactions enhance the physical properties of the molecule.
c) Dipole-dipole interactions
The electronegativity of sulfur and hydrogen is 2.58 and 2.20 respectively. The difference in electronegativity leads to the formation of a partial negative charge on sulfur and a partial positive charge on hydrogen. When the dipole of one molecule comes with the interaction of dipoles (opposite charge) of another hydrogen sulfide molecule, dipole-dipole interaction is induced. This interaction alters the physical properties such as boiling point of to a greater extent.
d)
In water molecules, oxygen has a greater electronegativity than hydrogen. The formation of dipoles between the atoms and the intermolecular interactions enhances the physical properties of water. Besides, water molecules can form intermolecular hydrogen bonding among other water molecules. Since the strength of hydrogen bonding interactions is greater than the dipole-dipole interactions (in ), the water molecule has a higher boiling point (100°C) than (-60°C).
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