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Fluorocarbon gases are generally greenhouse gases with global-warming potentials 100 to 23,500 times that of carbon dioxide, and SF 6 has the highest global warming potential of any known substance. Organofluorine compounds often persist in the environment due to the strength of the carbon–fluorine bond.
The compound readily decomposes into oxygen and fluorine. Even at a temperature of −160 °C (113 K), 4% decomposes each day [1] by this process: O 2 F 2 → O 2 + F 2. The other main property of this unstable compound is its oxidizing power, although most experimental reactions have been conducted near −100 °C (173 K). [10]
The carbon–fluorine bond of the smaller molecules is formed in three principal ways: Fluorine replaces a halogen or hydrogen, or adds across a multiple bond. The direct reaction of hydrocarbons with fluorine gas can be dangerously reactive, so the temperature may need to be lowered even to −150 °C (−240 °F). [115] "
For gases, departure from 3 R per mole of atoms is generally due to two factors: (1) failure of the higher quantum-energy-spaced vibration modes in gas molecules to be excited at room temperature, and (2) loss of potential energy degree of freedom for small gas molecules, simply because most of their atoms are not bonded maximally in space to ...
Nitrogen dioxide: Gas NO 2: 33.2 Hydrazine: Gas N 2 H 4: 95.4 Hydrazine: Liquid N 2 H 4: 50.6 Nitrous oxide: Gas N 2 O 82.05 Nitric oxide: Gas NO 90.29 Dinitrogen tetroxide: Gas N 2 O 4: 9.16 Dinitrogen pentoxide: Solid N 2 O 5: −43.1 Dinitrogen pentoxide: Gas N 2 O 5: 11.3 Nitric acid: Aqueous HNO 3: −207 Monatomic oxygen Gas O 249 Oxygen ...
Examples are gases carbon monoxide (CO), nitric oxide (NO), and hydrogen chloride (HCl). Many 1:1 binary compounds are not normally considered diatomic because they are polymeric at room temperature, but they form diatomic molecules when evaporated, for example gaseous MgO, SiO, and many others.
The standard Gibbs free energy of formation (G f °) of a compound is the change of Gibbs free energy that accompanies the formation of 1 mole of a substance in its standard state from its constituent elements in their standard states (the most stable form of the element at 1 bar of pressure and the specified temperature, usually 298.15 K or 25 °C).
Perfluoroalkanes are very stable because of the strength of the carbon–fluorine bond, one of the strongest in organic chemistry. [4] Its strength is a result of the electronegativity of fluorine imparting partial ionic character through partial charges on the carbon and fluorine atoms, which shorten and strengthen the bond (compared to carbon-hydrogen bonds) through favorable covalent ...