The oxygen atom is next to the negative terminal of the dipole vector. This occurs as a result of the atom's electronegative nature and abundance of lone electron pairs. Because it trades up its lone pair electrons to create a hydrogen bond, such oxygen is called the hydrogen bonding donor.
Hydrogen-bonded compounds exhibit abnormally high melting and boiling points. According to the additional energy required to break these bonds, the molecule with hydrogen bonds has a high melting or boiling point.
The dipole moment increases with the difference in electronegativity. Another element affecting the size of the dipole moment was the spacing between the charge separations. The polarity of the molecule is determined by the dipole moment.
Therefore, the oxygen atom is next to the negative terminal of the dipole vector. This occurs as a result of the atom's electronegative nature and abundance of lone electron pairs.
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