1,2-Difluoroethane

Ethylene reacts explosively with fluorine yielding a mixture of 1,2-difluoroethane and vinyl fluoride. With solid fluorine it will react when triggered by near-infrared radiation.^[7]

The critical temperature of 1,2-difluoroethane is 107.5 Â°C.^[2]

If a C–H bond is over excited with too much vibration, the intramolecular vibrational relaxation takes 490 picoseconds.^[9]

The F–C–C–F dihedral angle is about 72°.^[10] Natural bond orbital deletion bond calculations show that 1,2-difluoroethane prefers the gauche conformation due to hyperconjugation effects. Since F is much more electronegative than the C atom, it will have greater electron density for the bonding orbital (carbon–fluorine bond). Thus, C will have larger σ* orbital, which is stabilized through C–H hyperconjugation. Thus cis C–H bonds and the C–F σ* interactions are significant. The dihedral angle of about 72° is a result of decreasing hyper conjugative stability and decreasing steric destabilization.^[11]

CH₂FCH₂F reacts with chlorine when treated with light. Two products are formed: CH₂FCCl₂F and CHClFCHClF. The proportions of each depends on the solvent.^[3]

1,2-Difluoroethane is primarily used in refrigerants (39%), foam blowing agents (17%), solvents (14%), fluoropolymers (14%), sterilant gases (2%), aerosol propellants (2%), food freezants (1%), other (8%), and exports (3%).^[12]

1,2-Difluoroethane is toxic when inhaled or when it comes into direct contact with the skin. Fluorocarbons are 4 to 5 times heavier than air, so it tends to concentrate in low-lying areas. This increases the risk of inhalation. 1,2-Difluoroethane is toxic to humans through several mechanisms. First, because it has a high density, it can displace oxygen in the lungs causing suffocation. In addition, inhaled fluorocarbons causes the myocardium to become more sensitive to catecholamines, which results in deadly cardiac arrhythmias.^[13]

When inhaled by rats, 1,2-difluoroethane is converted to fluoroacetate by cytochrome P450 and then to fluorocitrate, both toxic. 100 parts per million in the atmosphere was sufficient to poison rats in 30 minutes and to kill them in four hours. 1,2-Difluoroethane is likely to be similarly toxic to humans.^[14]

1,2-Difluoroethane can enter the environment in various ways. One way is through volatilization from rivers and lakes. Henry's law estimates that the volatilization half life from a model river is about 2.4 hours and 3.2 days from a model lake.^[12] When 1,2-difluoroethane is released to the environment, it will end up in the atmosphere. Here it is degraded by reaction with hydroxyl radicals and oxygen.^[15]

CH₂FCH₂F + OH → CH₂FCHF + H₂O

CH₂FCHF + O₂ → CH₂FCHFO₂ peroxy radical

CH₂FCHFO₂ + NO → CH₂FCHFO alkoxy radical

When catalysed by chlorine atoms and oxidised by nitrogen oxides the end product is HCOF, which can decompose further to HF and CO.^[15]

The halflife in air is between 140 and 180 days.^[12]

1,2-Difluoroethane is a greenhouse gas when released to the atmosphere. It has a warming equivalent to 140 times that of carbon dioxide. As such it may be controlled by government regulation. The Australian government classifies 1,2-difluoroethane as an exotic synthetic greenhouse gas.^[16]