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What Forms Hydrogen Bonds
No matter what can form hydrogen bonds
All things in the world, those who form hydrogen bonds must have their own characteristics. Hydrogen atoms need to be connected to atoms with large electronegativity and small radius in order to form hydrogen bonds.
Common atoms such as nitrogen, oxygen, and fluorine have large electronegativity. When hydrogen is connected to nitrogen, such as in ammonia molecules, hydrogen is highly electronegative due to the strong electronegativity of nitrogen, and the electron cloud is biased towards nitrogen, and hydrogen is partially positively charged. At this time, the lone pair of electrons of nitrogen atoms in adjacent ammonia molecules will attract each other with positively charged hydrogen, forming hydrogen bonds.
Water is also a typical example. Hydrogen is connected to oxygen, and oxygen is highly electronegative, so that hydrogen in water molecules is positively charged and oxygen is negatively charged. Between different water molecules, hydrogen and oxygen attract each other, and hydrogen bonds can be formed. This is the source of many unique properties of water, such as the higher boiling point, which enhances the intermolecular force due to hydrogen bonds.
In fluorine-containing compounds, hydrogen and fluorine can also form hydrogen bonds. In hydrofluoric acid, the electronegativity of fluorine is extremely strong, and the polarity of hydrogen-fluorine bonds is very high. Hydrogen can form hydrogen bonds with fluorine atoms of neighboring molecules.
In summary, only when hydrogen is combined with atoms with a specific electronegativity and a small radius, and meets certain spatial orientation conditions, can hydrogen bonds be formed. This is the key to the formation of hydrogen bonds.
All things in the world, those who form hydrogen bonds must have their own characteristics. Hydrogen atoms need to be connected to atoms with large electronegativity and small radius in order to form hydrogen bonds.
Common atoms such as nitrogen, oxygen, and fluorine have large electronegativity. When hydrogen is connected to nitrogen, such as in ammonia molecules, hydrogen is highly electronegative due to the strong electronegativity of nitrogen, and the electron cloud is biased towards nitrogen, and hydrogen is partially positively charged. At this time, the lone pair of electrons of nitrogen atoms in adjacent ammonia molecules will attract each other with positively charged hydrogen, forming hydrogen bonds.
Water is also a typical example. Hydrogen is connected to oxygen, and oxygen is highly electronegative, so that hydrogen in water molecules is positively charged and oxygen is negatively charged. Between different water molecules, hydrogen and oxygen attract each other, and hydrogen bonds can be formed. This is the source of many unique properties of water, such as the higher boiling point, which enhances the intermolecular force due to hydrogen bonds.
In fluorine-containing compounds, hydrogen and fluorine can also form hydrogen bonds. In hydrofluoric acid, the electronegativity of fluorine is extremely strong, and the polarity of hydrogen-fluorine bonds is very high. Hydrogen can form hydrogen bonds with fluorine atoms of neighboring molecules.
In summary, only when hydrogen is combined with atoms with a specific electronegativity and a small radius, and meets certain spatial orientation conditions, can hydrogen bonds be formed. This is the key to the formation of hydrogen bonds.
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