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Is NH3 Hydrogen Bonding
On the hydrogen bond of ammonia
Ammonia ($NH_3 $), the nitrogen atom in the molecule has a lone pair of electrons, and the hydrogen atom is connected to the nitrogen atom. The hydrogen atom has a strong electronegativity of nitrogen, and the electron cloud is biased towards nitrogen, causing hydrogen to have a partial positive charge.
When the ammonia molecules are close to each other, the positively charged hydrogen in one molecule and the lone pair of electrons of nitrogen in another molecule attract each other. This attraction is due to the hydrogen bond. The electronegativity of nitrogen is quite high, and the atomic radius is small, which can effectively form hydrogen bonds.
In view of reality, the boiling point of ammonia is relatively high, which is higher than that of the $PH_3 $formed by phosphorus of the same main group. Due to the existence of hydrogen bonds between ammonia molecules, it takes extra energy to overcome hydrogen bonds in order to change it from liquid to gaseous. Another example is that ammonia has great solubility in water, which is also related to hydrogen bonds. Ammonia molecules and water molecules can form hydrogen bonds, enhancing the interaction between the two, so ammonia is easily soluble in water.
From this perspective, there are indeed hydrogen bonds between ammonia molecules, which has a huge impact on their physical and chemical properties.
Ammonia ($NH_3 $), the nitrogen atom in the molecule has a lone pair of electrons, and the hydrogen atom is connected to the nitrogen atom. The hydrogen atom has a strong electronegativity of nitrogen, and the electron cloud is biased towards nitrogen, causing hydrogen to have a partial positive charge.
When the ammonia molecules are close to each other, the positively charged hydrogen in one molecule and the lone pair of electrons of nitrogen in another molecule attract each other. This attraction is due to the hydrogen bond. The electronegativity of nitrogen is quite high, and the atomic radius is small, which can effectively form hydrogen bonds.
In view of reality, the boiling point of ammonia is relatively high, which is higher than that of the $PH_3 $formed by phosphorus of the same main group. Due to the existence of hydrogen bonds between ammonia molecules, it takes extra energy to overcome hydrogen bonds in order to change it from liquid to gaseous. Another example is that ammonia has great solubility in water, which is also related to hydrogen bonds. Ammonia molecules and water molecules can form hydrogen bonds, enhancing the interaction between the two, so ammonia is easily soluble in water.
From this perspective, there are indeed hydrogen bonds between ammonia molecules, which has a huge impact on their physical and chemical properties.
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