geranyl bromide

geranyl bromide

formula | (CH_3)_2C=CHCH_2CH_2C(CH_3)=CHCH_2Br Hill formula | C_10H_17Br name | geranyl bromide IUPAC name | (2E)-1-bromo-3, 7-dimethylocta-2, 6-diene alternate names | 2, 6-octadiene, 1-bromo-3, 7-dimethyl-, (2E)- | 2, 6-octadiene, 1-bromo-3, 7-dimethyl-, (E)- | (2E)-1-bromo-3, 7-dimethyl-2, 6-octadiene | (2E)-1-bromo-3, 7-dimethyl-octa-2, 6-diene | (2E)-1-bromo-3, 7-dimethylocta-2, 6-diene | (E)-1-bromo-3, 7-dimethylocta-2, 6-diene | trans-1-bromo-3, 7-dimethyl-2, 6-octadiene mass fractions | Br (bromine) 36.8% | C (carbon) 55.3% | H (hydrogen) 7.89%

Draw the Lewis structure of geranyl 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 + 10 n_C, val + 17 n_H, val = 64 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 + 10 n_C, full + 17 n_H, full = 122 Subtracting these two numbers shows that 122 - 64 = 58 bonding electrons are needed. Each bond has two electrons, so in addition to the 27 bonds already present in the diagram add 2 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 2 bonds by pairing electrons between adjacent highlighted atoms: Answer: | |

3D structure

molar mass | 217.15 g/mol phase | liquid (at STP) boiling point | 101.5 °C (measured at 1600 Pa) density | 1.094 g/cm^3

density | 1.094 g/cm^3 refractive index | 1.504

CAS number | 6138-90-5 Beilstein number | 1703631 PubChem CID number | 5365867 PubChem SID number | 24859770 SMILES identifier | CC(=CCCC(=CCBr)C)C InChI identifier | InChI=1/C10H17Br/c1-9(2)5-4-6-10(3)7-8-11/h5, 7H, 4, 6, 8H2, 1-3H3/b10-7+ MDL number | MFCD00000243

flash point | 95 °C

DOT numbers | 3334