Input interpretation
amide anion
Lewis structure
Draw the Lewis structure of amide anion. Start by drawing the overall structure of the molecule: Count the total valence electrons of the hydrogen (n_H, val = 1) and nitrogen (n_N, val = 5) atoms, including the net charge: 2 n_H, val + n_N, val - n_charge = 8 Calculate the number of electrons needed to completely fill the valence shells for hydrogen (n_H, full = 2) and nitrogen (n_N, full = 8): 2 n_H, full + n_N, full = 12 Subtracting these two numbers shows that 12 - 8 = 4 bonding electrons are needed. Each bond has two electrons, so the above diagram has all the necessary bonds. There are 2 bonds and hence 4 bonding electrons in the diagram. Fill in the remaining unbonded electrons on each atom. In total, there remain 8 - 4 = 4 electrons left to draw. Lastly, fill in the formal charges: Answer: | |
General properties
formula | (NH_2)^- net ionic charge | -1 alternate names | amide | amide(1-)
Ionic radius
thermochemical radius | 130 pm
Units
Other properties
ion class | anions | polyatomic ions common sources of ion | sodium amide (1 eq) | lithium nitride (1 eq) | hexaammineruthenium(II) chloride (1 eq) | diamminediiodopalladium(II) (2 eq) | diammonium hexachlororuthenate (2 eq) | ammonium hexachloroosmate(IV) (2 eq)