Input interpretation
hexafluorophosphate
Lewis structure
Draw the Lewis structure of hexafluorophosphate. Start by drawing the overall structure of the molecule: Count the total valence electrons of the fluorine (n_F, val = 7) and phosphorus (n_P, val = 5) atoms, including the net charge: 6 n_F, val + n_P, val - n_charge = 48 Calculate the number of electrons needed to completely fill the valence shells for fluorine (n_F, full = 8) and phosphorus (n_P, full = 8): 6 n_F, full + n_P, full = 56 Subtracting these two numbers shows that 56 - 48 = 8 bonding electrons are needed, which are already accounted for in the structure. Note that the valence shell of phosphorus has been expanded to 6 bonds. After accounting for the expanded valence, there are 6 bonds and hence 12 bonding electrons in the diagram. Fill in the remaining unbonded electrons on each atom. In total, there remain 48 - 12 = 36 electrons left to draw. Lastly, fill in the formal charges: Answer: | |
General properties
net ionic charge | -1
Other properties
ion class | fluorinated group | halogenated group | anion group