1-18:3-lysophosphatidylethanolamine

1-18:3-lysophosphatidylethanolamine

formula | C_23H_42NO_7P name | 1-18:3-lysophosphatidylethanolamine alternate names | 1-18:3-lysoPE | 1-(9Z, 12Z, 15Z-octadecatrienoyl)-sn-glycero-3-phosphoethanolamine mass fractions | C (carbon) 58.5% | H (hydrogen) 8.32% | N (nitrogen) 2.96% | O (oxygen) 23.7% | P (phosphorus) 6.55%

Draw the Lewis structure of 1-18:3-lysophosphatidylethanolamine. 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), nitrogen (n_N, val = 5), oxygen (n_O, val = 6), and phosphorus (n_P, val = 5) atoms: 23 n_C, val + 39 n_H, val + n_N, val + 7 n_O, val + n_P, val = 183 Calculate the number of electrons needed to completely fill the valence shells for carbon (n_C, full = 8), hydrogen (n_H, full = 2), nitrogen (n_N, full = 8), oxygen (n_O, full = 8), and phosphorus (n_P, full = 8): 23 n_C, full + 39 n_H, full + n_N, full + 7 n_O, full + n_P, full = 334 Subtracting these two numbers shows that 334 - 183 = 151 bonding electrons are expected (in such cases with an odd number, round down to 150 bonding electrons). Each bond has two electrons, so in addition to the 70 bonds already present in the diagram add 5 bonds. To minimize formal charge carbon wants 4 bonds, nitrogen wants 3 bonds, and oxygen wants 2 bonds. Identify the atoms that want additional bonds and the number of electrons remaining on each atom: Fill in the 5 bonds by pairing electrons between adjacent highlighted atoms, noting the formal charges of the atoms. Double bonding phosphorus to the other highlighted oxygen atom would result in an equivalent molecule: Answer: | |

molar mass | 472.54 g/mol

PubChem CID number | 90658600 SMILES identifier | CCC=CCC=CCC=CCCCCCCCC(OCC(COP(OCC[N+])([O-])=O)O)=O