Carbon-Fluorine Bond
One of the strongest single bonds in organic chemistry, with a bond energy of approximately 485 kJ/mol. Its high stability is the fundamental reason PFAS are difficult to degrade.
Timeline (last 90 days)
In natural environments, almost no microorganisms have evolved enzyme systems capable of effectively breaking carbon-fluorine bonds, and the degradation half-life of PFAS is measured in decades to hundreds of years.
The carbon-fluorine bond (C—F) is one of the strongest single bonds in organic chemistry, with a bond energy of about 485 kJ/mol, far higher than the carbon-hydrogen bond (about 413 kJ/mol) and the carbon-carbon bond (about 347 kJ/mol).
Fluorine atoms have extremely high electronegativity (4.0) and a small radius, so the C—F bonds they form have low polarizability and are highly stable.
All Facts (3)
In natural environments, almost no microorganisms have evolved enzyme systems capable of effectively breaking carbon-fluorine bonds, and the degradation half-life of PFAS is measured in decades to hundreds of years.
50%UnverifiedThe carbon-fluorine bond (C—F) is one of the strongest single bonds in organic chemistry, with a bond energy of about 485 kJ/mol, far higher than the carbon-hydrogen bond (about 413 kJ/mol) and the carbon-carbon bond (about 347 kJ/mol).
50%UnverifiedFluorine atoms have extremely high electronegativity (4.0) and a small radius, so the C—F bonds they form have low polarizability and are highly stable.
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