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Why Hydrogen Lithium Sodium Are Reactive Elements
On why hydrogen, lithium, and sodium are active elements
Hydrogen, lithium, and sodium are often classified as active elements among chemical elements. This is not for no reason. The reason can be explored from its atomic structure and electronic properties.
First talk about the atomic structure. The atom of hydrogen has only one proton and one electron, and its electron layer has only one layer. The lithium atom has three protons, and the extrinuclear electrons are arranged in two layers, and the outermost electron number is one. The sodium atom contains eleven protons, and the electrons are divided into three layers, and the outermost layer has only one electron. The outermost electrons of these three are all small, only one. In chemistry, if an atom wants to achieve a stable structure, the outer electron often seeks the state of an octet (hydrogen is a two-electron stable state). Therefore, they all have a strong tendency, or lose this electron, in order to achieve a stable structure.
Looking at the electronic properties again. The atomic radii of hydrogen, lithium, and sodium are different, but all because there is only one electron in the outermost layer, the force of this electron bound by the nucleus is relatively weak. Take sodium as an example, it has a large number of electron layers and a large atomic radius. The outermost electron is far away from the nucleus, and its attractiveness is small. Although lithium has a small number of electron layers and a relatively small atomic radius, the outermost electron is also easily separated due to external influences. Although the hydrogen atom has only one electron, it is easy to lose or gain electrons when it wants to reach the stable state of two electrons, showing reactivity.
From the chemical reaction performance, all three are very easy to participate in many chemical reactions. If it reacts with oxygen, sodium is heated in the air slightly, and it burns violently, emitting a dazzling yellow light, forming products such as sodium peroxide; lithium can also react with oxygen to form corresponding oxides when heated; when hydrogen is mixed with oxygen, it reacts quickly when exposed to an open flame, and even explodes to form water. The intensity of such reactions is sufficient to prove its reactivity. Another example is the reaction with water, when sodium is thrown into the water, it immediately melts into small balls, swims around, hisses, and generates sodium hydroxide and hydrogen; although the reaction between lithium and water is relatively mild, it can continue to produce lithium hydroxide and hydrogen. This is because the three are prone to lose their outermost electrons and undergo redox reactions with water molecules.
To sum up, hydrogen, lithium, and sodium are classified as active elements due to their unique atomic structures, the volatile properties of outer electrons, and their reactivity in chemical reactions. Therefore, they are classified as active elements, showing their unique and important positions in the world of chemistry.
Hydrogen, lithium, and sodium are often classified as active elements among chemical elements. This is not for no reason. The reason can be explored from its atomic structure and electronic properties.
First talk about the atomic structure. The atom of hydrogen has only one proton and one electron, and its electron layer has only one layer. The lithium atom has three protons, and the extrinuclear electrons are arranged in two layers, and the outermost electron number is one. The sodium atom contains eleven protons, and the electrons are divided into three layers, and the outermost layer has only one electron. The outermost electrons of these three are all small, only one. In chemistry, if an atom wants to achieve a stable structure, the outer electron often seeks the state of an octet (hydrogen is a two-electron stable state). Therefore, they all have a strong tendency, or lose this electron, in order to achieve a stable structure.
Looking at the electronic properties again. The atomic radii of hydrogen, lithium, and sodium are different, but all because there is only one electron in the outermost layer, the force of this electron bound by the nucleus is relatively weak. Take sodium as an example, it has a large number of electron layers and a large atomic radius. The outermost electron is far away from the nucleus, and its attractiveness is small. Although lithium has a small number of electron layers and a relatively small atomic radius, the outermost electron is also easily separated due to external influences. Although the hydrogen atom has only one electron, it is easy to lose or gain electrons when it wants to reach the stable state of two electrons, showing reactivity.
From the chemical reaction performance, all three are very easy to participate in many chemical reactions. If it reacts with oxygen, sodium is heated in the air slightly, and it burns violently, emitting a dazzling yellow light, forming products such as sodium peroxide; lithium can also react with oxygen to form corresponding oxides when heated; when hydrogen is mixed with oxygen, it reacts quickly when exposed to an open flame, and even explodes to form water. The intensity of such reactions is sufficient to prove its reactivity. Another example is the reaction with water, when sodium is thrown into the water, it immediately melts into small balls, swims around, hisses, and generates sodium hydroxide and hydrogen; although the reaction between lithium and water is relatively mild, it can continue to produce lithium hydroxide and hydrogen. This is because the three are prone to lose their outermost electrons and undergo redox reactions with water molecules.
To sum up, hydrogen, lithium, and sodium are classified as active elements due to their unique atomic structures, the volatile properties of outer electrons, and their reactivity in chemical reactions. Therefore, they are classified as active elements, showing their unique and important positions in the world of chemistry.
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