Input interpretation
cyanide anion | structure diagram
Result
Draw the Lewis structure of cyanide anion. Start by drawing the overall structure of the molecule, ignoring potential double and triple bonds: Count the total valence electrons of the carbon (n_C, val = 4) and nitrogen (n_N, val = 5) atoms, including the net charge: n_C, val + n_N, val - n_charge = 10 Calculate the number of electrons needed to completely fill the valence shells for carbon (n_C, full = 8) and nitrogen (n_N, full = 8): n_C, full + n_N, full = 16 Subtracting these two numbers shows that 16 - 10 = 6 bonding electrons are needed. Each bond has two electrons, so in addition to the 1 bond already present in the diagram add 2 bonds. Identify the atoms that want additional bonds and the number of electrons remaining on each atom. The net charge has been given to the most electronegative atom, carbon: Fill in the 2 bonds by pairing electrons between adjacent highlighted atoms, noting the formal charges of the atoms: Answer: | |