In H2O (water), each molecule has two hydrogen atoms bonded to one oxygen atom. The oxygen atom is highly electronegative compared to hydrogen, so it creates a partial negative charge near the oxygen atom and a partial positive charge near the hydrogen atoms. This unequal distribution of electrons creates a polar molecule.
In HF (hydrogen fluoride), each molecule has one hydrogen atom bonded to one fluorine atom. Similar to water, fluorine is more electronegative than hydrogen, creating a partial negative charge near the fluorine atom and a partial positive charge near the hydrogen atom.
Due to the polar nature of both water and hydrogen fluoride, they can form hydrogen bonds with other molecules. In water, the hydrogen bonds form between the partially positive hydrogen atom of one molecule and the partially negative oxygen atom of another molecule. In hydrogen fluoride, the hydrogen bonds form between the partially positive hydrogen atom of one molecule and the partially negative fluorine atom of another molecule.
Below is a simplified diagram showing the hydrogen bonding in H2O and HF:
H2O:
O---Hδ+···δ-H---Oδ-
HF:
H---Fδ+···δ-H
Show by mean of diagram, the hydrogen bonding in the following H2O HF
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