什么烟推荐一下 organic chemistry

The high聽electronegativity聽of fluorine (4.0 for F vs. 2.5 for carbon) gives the carbon鈥揻luorine bond a significant聽polarity/dipole moment. The electron density is concentrated around the fluorine, leing the carbon relatively electron poor. This introduces ionic character to the bond through聽partial charges聽($\ce{C^{未+}鈥擣^{未鈭拀}$). The partial charges on the fluorine and carbon are attractive, contributing to the unusual bond strength of the carbon鈥揻luorine bond. The bond is labeled as "the strongest in organic chemistry," because fluorine forms the strongest single bond to carbon. Carbon鈥揻luorine bonds can he a聽bond dissociation energy聽(BDE) of up to 544 kJ/mol.聽(This is why) The BDE (strength of the bond) is higher than other carbon鈥揾alogen聽and carbon鈥揾ydrogen聽bonds. For example, the molecule represented by $\ce{CH3X}$ has a BDE of 115 kcal/mol for carbon鈥揻luorine while values of 104.9, 83.7, 72.1, and 57.6 kcal/mol represent $\ce{C鈥揦}$ bonds to聽hydrogen,聽chlorine,聽bromine, and聽iodine, respectively.