10,16-dihydroxypalmitate

10, 16-dihydroxypalmitate

formula | C_16H_32O_4 name | 10, 16-dihydroxypalmitate mass fractions | C (carbon) 66.9% | H (hydrogen) 10.9% | O (oxygen) 22.3%

Draw the Lewis structure of 10, 16-dihydroxypalmitate. 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), hydrogen (n_H, val = 1), and oxygen (n_O, val = 6) atoms, including the net charge: 16 n_C, val + 31 n_H, val + 4 n_O, val - n_charge = 120 Calculate the number of electrons needed to completely fill the valence shells for carbon (n_C, full = 8), hydrogen (n_H, full = 2), and oxygen (n_O, full = 8): 16 n_C, full + 31 n_H, full + 4 n_O, full = 222 Subtracting these two numbers shows that 222 - 120 = 102 bonding electrons are needed. Each bond has two electrons, so in addition to the 50 bonds already present in the diagram add 1 bond. To minimize formal charge carbon wants 4 bonds and oxygen wants 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, oxygen: Fill in the 1 bond by pairing electrons between adjacent highlighted atoms, noting the formal charges of the atoms. Double bonding carbon to the other highlighted oxygen atom would result in an equivalent molecule: Answer: | |

molar mass | 287.42 g/mol

SMILES identifier | C(CCCCC(=O)[O-])CCCC(CCCCCCO)O