farnesyl bromide

trans, trans-farnesyl bromide

formula | (CH_3)_2C=CH[CH_2CH_2C(CH_3)=CH]_2CH_2Br Hill formula | C_15H_25Br name | trans, trans-farnesyl bromide IUPAC name | (2E, 6E)-1-bromo-3, 7, 11-trimethyldodeca-2, 6, 10-triene alternate names | (2E, 6E)-1-bromo-3, 7, 11-trimethyl-dodeca-2, 6, 10-triene | (2E, 6E)-1-bromo-3, 7, 11-trimethyldodeca-2, 6, 10-triene | trans, trans-1-bromo-3, 7, 11-trimethyl-2, 6, 10-dodecatriene mass fractions | Br (bromine) 28% | C (carbon) 63.2% | H (hydrogen) 8.83%

Draw the Lewis structure of trans, trans-farnesyl bromide. Start by drawing the overall structure of the molecule, ignoring potential double and triple bonds: Count the total valence electrons of the bromine (n_Br, val = 7), carbon (n_C, val = 4), and hydrogen (n_H, val = 1) atoms: n_Br, val + 15 n_C, val + 25 n_H, val = 92 Calculate the number of electrons needed to completely fill the valence shells for bromine (n_Br, full = 8), carbon (n_C, full = 8), and hydrogen (n_H, full = 2): n_Br, full + 15 n_C, full + 25 n_H, full = 178 Subtracting these two numbers shows that 178 - 92 = 86 bonding electrons are needed. Each bond has two electrons, so in addition to the 40 bonds already present in the diagram add 3 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 3 bonds by pairing electrons between adjacent highlighted atoms: Answer: | |

3D structure

molar mass | 285.27 g/mol phase | liquid (at STP) boiling point | 105 °C (measured at 2000 Pa) density | 1.052 g/cm^3

density | 1.052 g/cm^3 refractive index | 1.509

CAS number | 28290-41-7 PubChem CID number | 5366048 PubChem SID number | 24860010 SMILES identifier | CC(=CCCC(=CCCC(=CCBr)C)C)C InChI identifier | InChI=1/C15H25Br/c1-13(2)7-5-8-14(3)9-6-10-15(4)11-12-16/h7, 9, 11H, 5-6, 8, 10, 12H2, 1-4H3/b14-9+, 15-11+ MDL number | MFCD00054465

flash point | 110 °C