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Mengapa jarak ikatan C≡C pada asetilena lebih pendek daripada jarak ikatan C=C? Rahasia molekuler yang akan mengejutkan Anda!
Acetylene, with the chemical formula C2H2, is the simplest alkyne and a hydrocarbon molecule with a triple bond. Compared with the well-known double-bond olefins (such as ethylene, C2H4), the C≡C bond distance of acetylene is more compact, even tighter than that of C=C The key pitch is even shorter. This phenomenon not only reflects the structure and stability of atoms in molecules, but also has a close relationship with their bonding properties and electron distribution.
Structural differences between double bonds and triple bonds
In the acetylene molecule, the C≡C bond length is about 118 picometers, while the C=C bond length in ethylene is 132 picometers.
Why is there such a difference? The key lies in the mix of carbon atoms and the nature of the bonds they form. The carbon atoms of acetylene are sp hybridized, which means that each carbon atom has two unhybridized p orbitals to form two π bonds and one sp orbital to form a σ bond. This structure makes the formation of a triple bond very difficult. The structure is stronger than double bonds. As we all know, the stronger the chemical bond, the shorter the distance is usually.
Strength and its influencing factors
The bond energy of a triple bond is 839 kJ/mol, while the bond energy of a double bond is approximately 610 kJ/mol.
In addition to the bond distance, the strength of these bonds is also a factor we need to consider. Ikatan asetilena, daya tarik antara atom karbon semakin ditingkatkan melalui pembentukan ikatan rangkap tiga, membuat ikatan ini tidak mudah rusak. Selama hidrogenasi parsial, asetilen dapat menyerap dua molekul hidrogen dan akhirnya berubah menjadi etilena. benar -benar berbeda.
