Input interpretation
peroxide anion
Lewis structure
Draw the Lewis structure of peroxide anion. Start by drawing the overall structure of the molecule: Count the total valence electrons of the oxygen (n_O, val = 6) atoms, including the net charge: 2 n_O, val - n_charge = 14 Calculate the number of electrons needed to completely fill the valence shells for oxygen (n_O, full = 8): 2 n_O, full = 16 Subtracting these two numbers shows that 16 - 14 = 2 bonding electrons are needed. Each bond has two electrons, so the above diagram has all the necessary bonds. There is 1 bond and hence 2 bonding electrons in the diagram. Fill in the remaining unbonded electrons on each atom. In total, there remain 14 - 2 = 12 electrons left to draw. Lastly, fill in the formal charges: Answer: | |
General properties
formula | (O_2)^(2-) net ionic charge | -2 alternate names | peroxide | peroxide(2-)
Ionic radius
thermochemical radius | 173 pm
Units
Other properties
ion class | anions | oxoanions | polyatomic ions common sources of ion | zinc peroxide (1 eq) | strontium peroxide (1 eq) | magnesium peroxide (1 eq) | lithium peroxide (1 eq) | calcium peroxide (1 eq)