[cs_content][cs_section parallax=”false” separator_top_type=”none” separator_top_height=”50px” separator_top_angle_point=”50″ separator_bottom_type=”none” separator_bottom_height=”50px” separator_bottom_angle_point=”50″ style=”margin: 0px;padding: 45px 0px;”][cs_row inner_container=”true” marginless_columns=”false” style=”margin: 0px auto;padding: 0px;”][cs_column fade=”false” fade_animation=”in” fade_animation_offset=”45px” fade_duration=”750″ type=”1/1″ style=”padding: 0px;”][cs_text]Organic Chemistry > Alcohols >[/cs_text][cs_text]
- Alcohols form stronger intramolecular and intermolecular hydrogen bonds which is the reason of their elevated boiling points.
- The oxygen atom of the strongly polarized O―H bond of an alcohol pulls electron density away from the hydrogen atom. This polarized hydrogen, which bears a partial positive charge, can form a hydrogen bond with a pair of nonbonding electrons on another oxygen atom.
- Because alcohols possess a hydrophilic ―OH group, they have tendencies to form hydrogen bonds with water which allows them to dissolve in water.
- Alcohols with higher molecular weights tend to be less water-soluble, because the hydrocarbon part of the molecule, which is hydrophobic (“water-hating”), is larger with increased molecular weight.
- Because they are strongly polar, alcohols are better solvents than hydrocarbons for ionic compounds and other polar substances.
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