Input interpretation
iodine heptafluoride
Chemical names and formulas
formula | F_7I_1 Hill formula | F_7I name | iodine heptafluoride IUPAC name | heptafluoro-$l^{7}-iodane mass fractions | F (fluorine) 51.2% | I (iodine) 48.8%
Lewis structure
Draw the Lewis structure of iodine heptafluoride. Start by drawing the overall structure of the molecule: Count the total valence electrons of the fluorine (n_F, val = 7) and iodine (n_I, val = 7) atoms: 7 n_F, val + n_I, val = 56 Calculate the number of electrons needed to completely fill the valence shells for fluorine (n_F, full = 8) and iodine (n_I, full = 8): 7 n_F, full + n_I, full = 64 Subtracting these two numbers shows that 64 - 56 = 8 bonding electrons are needed, which are already accounted for in the structure. Note that the valence shell of iodine has been expanded to 7 bonds. After accounting for the expanded valence, there are 7 bonds and hence 14 bonding electrons in the diagram. Lastly, fill in the remaining unbonded electrons on each atom. In total, there remain 56 - 14 = 42 electrons left to draw: Answer: | |
Basic properties
molar mass | 259.89329 g/mol
Units
Chemical identifiers
PubChem CID number | 85645 SMILES identifier | FI(F)(F)(F)(F)(F)F InChI identifier | InChI=1S/F7I/c1-8(2, 3, 4, 5, 6)7