Input interpretation
dichloroiodide anion | structure diagram
Result
Draw the Lewis structure of dichloroiodide anion. Start by drawing the overall structure of the molecule: Count the total valence electrons of the chlorine (n_Cl, val = 7) and iodine (n_I, val = 7) atoms, including the net charge: 2 n_Cl, val + n_I, val - n_charge = 22 Calculate the number of electrons needed to completely fill the valence shells for chlorine (n_Cl, full = 8) and iodine (n_I, full = 8): 2 n_Cl, full + n_I, full = 24 Subtracting these two numbers shows that 24 - 22 = 2 bonding electrons are needed, which are already accounted for in the structure. Note that the valence shell of iodine has been expanded. After accounting for the expanded valence, 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 22 - 4 = 18 electrons left to draw. Lastly, fill in the formal charges: Answer: | |