Input interpretation
![(2-bromoethyl)benzene](../image_source/1888d11c1eb1107038ea94a7923c3c16.png)
(2-bromoethyl)benzene
Chemical names and formulas
![formula | C_6H_5CH_2CH_2Br Hill formula | C_8H_9Br name | (2-bromoethyl)benzene IUPAC name | 2-bromoethylbenzene alternate names | 1-bromo-2-phenylethane | 2-bromoethylbenzene | 2-phenethyl bromide | 2-phenylethyl bromide | beta-bromoethylbenzene | phenethyl bromide | phenylethyl bromide mass fractions | Br (bromine) 43.2% | C (carbon) 51.9% | H (hydrogen) 4.9%](../image_source/41316aef9264840f45a68a42b40f8f57.png)
formula | C_6H_5CH_2CH_2Br Hill formula | C_8H_9Br name | (2-bromoethyl)benzene IUPAC name | 2-bromoethylbenzene alternate names | 1-bromo-2-phenylethane | 2-bromoethylbenzene | 2-phenethyl bromide | 2-phenylethyl bromide | beta-bromoethylbenzene | phenethyl bromide | phenylethyl bromide mass fractions | Br (bromine) 43.2% | C (carbon) 51.9% | H (hydrogen) 4.9%
Lewis structure
![Draw the Lewis structure of (2-bromoethyl)benzene. 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 + 8 n_C, val + 9 n_H, val = 48 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 + 8 n_C, full + 9 n_H, full = 90 Subtracting these two numbers shows that 90 - 48 = 42 bonding electrons are needed. Each bond has two electrons, so in addition to the 18 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. Note that the six atom ring is aromatic, so that the single and double bonds may be rearranged: Answer: | |](../image_source/680dd8e95cfcdfe6922187fc68193e28.png)
Draw the Lewis structure of (2-bromoethyl)benzene. 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 + 8 n_C, val + 9 n_H, val = 48 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 + 8 n_C, full + 9 n_H, full = 90 Subtracting these two numbers shows that 90 - 48 = 42 bonding electrons are needed. Each bond has two electrons, so in addition to the 18 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. Note that the six atom ring is aromatic, so that the single and double bonds may be rearranged: Answer: | |
3D structure
![3D structure](../image_source/515daed131f220fbb20676b35dfbdea9.png)
3D structure
Basic properties
![molar mass | 185.06 g/mol phase | liquid (at STP) melting point | -56 °C boiling point | 220.5 °C density | 1.355 g/cm^3](../image_source/576cc2a40441e8f2ef390c887f1cd940.png)
molar mass | 185.06 g/mol phase | liquid (at STP) melting point | -56 °C boiling point | 220.5 °C density | 1.355 g/cm^3
Units
Liquid properties (at STP)
![density | 1.355 g/cm^3 vapor pressure | 0.17 mmHg (at 25 °C) surface tension | 0.03923 N/m refractive index | 1.556](../image_source/15bd4f9614ae8796e4cbff26541d6d68.png)
density | 1.355 g/cm^3 vapor pressure | 0.17 mmHg (at 25 °C) surface tension | 0.03923 N/m refractive index | 1.556
Units
Thermodynamic properties
![molar heat of vaporization | 43.8 kJ/mol specific heat of vaporization | 0.237 kJ/g (at STP)](../image_source/1abcb325ee548dae5459db9de5029b62.png)
molar heat of vaporization | 43.8 kJ/mol specific heat of vaporization | 0.237 kJ/g (at STP)
Chemical identifiers
![CAS number | 103-63-9 Beilstein number | 507487 PubChem CID number | 7666 PubChem SID number | 24891921 SMILES identifier | C1=CC=C(C=C1)CCBr InChI identifier | InChI=1/C8H9Br/c9-7-6-8-4-2-1-3-5-8/h1-5H, 6-7H2 RTECS number | CY9032000 MDL number | MFCD00000240](../image_source/820275fcffb84321281abd98c19999dc.png)
CAS number | 103-63-9 Beilstein number | 507487 PubChem CID number | 7666 PubChem SID number | 24891921 SMILES identifier | C1=CC=C(C=C1)CCBr InChI identifier | InChI=1/C8H9Br/c9-7-6-8-4-2-1-3-5-8/h1-5H, 6-7H2 RTECS number | CY9032000 MDL number | MFCD00000240
NFPA label
![NFPA label](../image_source/c0603ec47c7bfa239e2fe04d28a48dc6.png)
NFPA label
![NFPA health rating | 1 NFPA fire rating | 2 NFPA reactivity rating | 0](../image_source/b28d4ce804b82ea2dd22c446ebbb47ab.png)
NFPA health rating | 1 NFPA fire rating | 2 NFPA reactivity rating | 0
Safety properties
![flash point | 89.44 °C](../image_source/0ce74f38b55f5209a31a340e1896d38b.png)
flash point | 89.44 °C
Toxicity properties
![RTECS classes | other](../image_source/f617384087516f9265dfd61c66aac8d9.png)
RTECS classes | other