Input interpretation
![benzo[a]pyrene-d 12](../image_source/1a7b0ac328f78dceac955fb781c63c01.png)
benzo[a]pyrene-d 12
Chemical names and formulas
![formula | C_20D_12 name | benzo[a]pyrene-d 12 IUPAC name | 1, 2, 3, 4, 5, 6, 7, 8, 9, 10, 11, 12-dodecadeuteriobenzo[b]pyrene alternate names | 1, 2, 3, 4, 5, 6, 7, 8, 9, 10, 11, 12-dodecadeuteriobenzo[b]pyrene | 3, 4-benzopyrene-d12 mass fractions | C (carbon) 0.909% | H (hydrogen) 0.0914%](../image_source/901576e36e177cd878521e7a99a9ff68.png)
formula | C_20D_12 name | benzo[a]pyrene-d 12 IUPAC name | 1, 2, 3, 4, 5, 6, 7, 8, 9, 10, 11, 12-dodecadeuteriobenzo[b]pyrene alternate names | 1, 2, 3, 4, 5, 6, 7, 8, 9, 10, 11, 12-dodecadeuteriobenzo[b]pyrene | 3, 4-benzopyrene-d12 mass fractions | C (carbon) 0.909% | H (hydrogen) 0.0914%
Lewis structure
![Draw the Lewis structure of benzo[a]pyrene-d 12. 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 hydrogen (n_H, val = 1) atoms: 20 n_C, val + 12 n_H, val = 92 Calculate the number of electrons needed to completely fill the valence shells for carbon (n_C, full = 8) and hydrogen (n_H, full = 2): 20 n_C, full + 12 n_H, full = 184 Subtracting these two numbers shows that 184 - 92 = 92 bonding electrons are needed. Each bond has two electrons, so in addition to the 36 bonds already present in the diagram add 10 bonds. To minimize formal charge carbon wants 4 bonds. Identify the atoms that want additional bonds and the number of electrons remaining on each atom: Fill in the 10 bonds by pairing electrons between adjacent highlighted atoms. Note that the six atom rings are aromatic, so that the single and double bonds may be rearranged: Answer: | |](../image_source/e971bdcf31dc286f0739a3b30f9f5619.png)
Draw the Lewis structure of benzo[a]pyrene-d 12. 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 hydrogen (n_H, val = 1) atoms: 20 n_C, val + 12 n_H, val = 92 Calculate the number of electrons needed to completely fill the valence shells for carbon (n_C, full = 8) and hydrogen (n_H, full = 2): 20 n_C, full + 12 n_H, full = 184 Subtracting these two numbers shows that 184 - 92 = 92 bonding electrons are needed. Each bond has two electrons, so in addition to the 36 bonds already present in the diagram add 10 bonds. To minimize formal charge carbon wants 4 bonds. Identify the atoms that want additional bonds and the number of electrons remaining on each atom: Fill in the 10 bonds by pairing electrons between adjacent highlighted atoms. Note that the six atom rings are aromatic, so that the single and double bonds may be rearranged: Answer: | |
3D structure
3D structure
Basic properties
molar mass | 264.39 g/mol phase | solid (at STP) melting point | 178.5 °C boiling point | 495 °C
Units
Non-standard atom properties
H-2 | 12
Chemical identifiers
CAS number | 63466-71-7 PubChem CID number | 12202235 PubChem SID number | 24868654 SMILES identifier | C1=CC=C2C3=C4C(=CC2=C1)C=CC5=C4C(=CC=C5)C=C3 InChI identifier | InChI=1/C20H12/c1-2-7-17-15(4-1)12-16-9-8-13-5-3-6-14-10-11-18(17)20(16)19(13)14/h1-12H/i1D, 2D, 3D, 4D, 5D, 6D, 7D, 8D, 9D, 10D, 11D, 12D MDL number | MFCD00143664