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Both ammonia and water exhibit hydrogen bonding. This is an intermolecular force that holds molecules together to increase their melting and boiling points. Water is a small molecule and really should be a gas at room temperature if you compare it to its nearest chemical relative, hydrogen sulfide. Water is not a gas, thank goodness, but a liquid due to hydrogen bonding.

Hydrogen bonding is the interaction of a slightly positively charged hydrogen nucleus with a neighboring slightly negatively charged small electronegative atom like nitrogen, oxygen or fluorine.


Ammonia, NH3 and water, H2O both have higher melting points due to hydrogen bonding. In chemistry the general rule is the bigger the molecule the higher its melting point.
Ammonia melts at -77oC whereas its bigger relative phosphorus trihydride, PH3, melts at a lower temperature of -133oC.
Similarly, water melts at 0oC but rotten egg gas, H2S, melts at -82oC.


Both ammonia and water owe their unusually high melting and boiling points to hydrogen bonding.


Another similarity between them is that both nitrogen and oxygen have electrons in their outer energy level that are not used to make a bond in water and ammonia. These are called lone pairs or non bonding pairs. Oxygen has two non bonding pairs and nitrogen has one non bonding pairs. This makes both water and ammonia attractive to hydrogen ions, H+(also called protons).

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Q: It what ways are ammonia salt and water alike?
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