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Oxygen More Electronegative Than Hydrogen
On the reason why the electronegativity of oxygen is stronger than that of hydrogen
Between heaven and earth, yin and yang help each other, and everything is formed by the combination of elements. Among the elements, oxygen and hydrogen are common, and the electronegativity of oxygen is stronger than that of hydrogen. This is the basic understanding of chemistry, but why is it safe? Try to discuss it.
For oxygen, there are eight protons in the nucleus, which carry a lot of positive charges and are very attractive to electrons outside the nucleus. The number of electron layers is two, and the number of outermost electrons is six. If it wants to reach the stable structure of the octet, it has a strong tendency to acquire electrons. Looking at the distribution of its electron cloud, the electron cloud density in the area near the nucleus is relatively large, which shows that electrons are tightly bound by the nucleus and are not easy
This is not the case with hydrogen. The nucleus has only one proton, less positive charge, and relatively weak attraction to electrons. Although the number of its electron layers is only one layer, and the outermost layer is only one electron, although it also wants to achieve a stable structure, compared with oxygen, its power to acquire electrons is far inferior.
Furthermore, the atomic radius is also a key factor. The radius of the oxygen atom is smaller than that of the hydrogen atom. Although hydrogen has only one layer of electrons, the oxygen atom has a large nuclear charge, which attracts electrons more concentrated, so that the outer electrons are closer to the nucleus and tighter bound. When oxygen and hydrogen combine, oxygen, with its strong electronegativity, pulls the shared electron pair towards itself, causing hydrogen to be slightly positive and oxygen to be negative. In summary, oxygen is more electronegative than hydrogen due to factors such as the large number of nuclear charges, the distribution characteristics of electron clouds, and the relatively small atomic radius. This is a natural principle and plays a crucial role in many chemical reactions and the formation of material structures.
Between heaven and earth, yin and yang help each other, and everything is formed by the combination of elements. Among the elements, oxygen and hydrogen are common, and the electronegativity of oxygen is stronger than that of hydrogen. This is the basic understanding of chemistry, but why is it safe? Try to discuss it.
For oxygen, there are eight protons in the nucleus, which carry a lot of positive charges and are very attractive to electrons outside the nucleus. The number of electron layers is two, and the number of outermost electrons is six. If it wants to reach the stable structure of the octet, it has a strong tendency to acquire electrons. Looking at the distribution of its electron cloud, the electron cloud density in the area near the nucleus is relatively large, which shows that electrons are tightly bound by the nucleus and are not easy
This is not the case with hydrogen. The nucleus has only one proton, less positive charge, and relatively weak attraction to electrons. Although the number of its electron layers is only one layer, and the outermost layer is only one electron, although it also wants to achieve a stable structure, compared with oxygen, its power to acquire electrons is far inferior.
Furthermore, the atomic radius is also a key factor. The radius of the oxygen atom is smaller than that of the hydrogen atom. Although hydrogen has only one layer of electrons, the oxygen atom has a large nuclear charge, which attracts electrons more concentrated, so that the outer electrons are closer to the nucleus and tighter bound. When oxygen and hydrogen combine, oxygen, with its strong electronegativity, pulls the shared electron pair towards itself, causing hydrogen to be slightly positive and oxygen to be negative. In summary, oxygen is more electronegative than hydrogen due to factors such as the large number of nuclear charges, the distribution characteristics of electron clouds, and the relatively small atomic radius. This is a natural principle and plays a crucial role in many chemical reactions and the formation of material structures.
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