Input interpretation
phosphite anion
Lewis structure
Draw the Lewis structure of phosphite anion. Start by drawing the overall structure of the molecule: Count the total valence electrons of the oxygen (n_O, val = 6) and phosphorus (n_P, val = 5) atoms, including the net charge: 3 n_O, val + n_P, val - n_charge = 26 Calculate the number of electrons needed to completely fill the valence shells for oxygen (n_O, full = 8) and phosphorus (n_P, full = 8): 3 n_O, full + n_P, 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. Fill in the remaining unbonded electrons on each atom. In total, there remain 26 - 6 = 20 electrons left to draw. Lastly, fill in the formal charges: Answer: | |
General properties
formula | (PO_3)^(3-) net ionic charge | -3 alternate names | trioxophosphate | trioxidophosphate | phosphite | phosphite(3-)
Other properties
ion class | anions | oxoanions | polyatomic ions