Input interpretation
difluorine dioxide
Chemical names and formulas
formula | O_2F_2 Hill formula | F_2O_2 name | difluorine dioxide IUPAC name | hypofluorous acid fluorooxy ester alternate names | dioxygen difluoride | fluorine dioxide | perfluoroperoxide | fluorooxy hypofluorite mass fractions | F (fluorine) 54.3% | O (oxygen) 45.7%
Lewis structure
Draw the Lewis structure of difluorine dioxide. Start by drawing the overall structure of the molecule: Count the total valence electrons of the fluorine (n_F, val = 7) and oxygen (n_O, val = 6) atoms: 2 n_F, val + 2 n_O, val = 26 Calculate the number of electrons needed to completely fill the valence shells for fluorine (n_F, full = 8) and oxygen (n_O, full = 8): 2 n_F, full + 2 n_O, full = 32 Subtracting these two numbers shows that 32 - 26 = 6 bonding electrons are needed. Each bond has two electrons, so the above diagram has all the necessary bonds. There are 3 bonds and hence 6 bonding electrons in the diagram. Lastly, fill in the remaining unbonded electrons on each atom. In total, there remain 26 - 6 = 20 electrons left to draw: Answer: | |
3D structure
3D structure
Basic properties
molar mass | 69.995 g/mol
Units
Chemical identifiers
CAS number | 7783-44-0 PubChem CID number | 123257 SMILES identifier | O(OF)F InChI identifier | InChI=1S/F2O2/c1-3-4-2