Input interpretation
![2-bromophenol](../image_source/bcf1e847ed999b0d6876a175a3e0a227.png)
2-bromophenol
Chemical names and formulas
![formula | BrC_6H_4OH Hill formula | C_6H_5BrO name | 2-bromophenol alternate names | phenol, 2-bromo- | phenol, o-bromo- mass fractions | Br (bromine) 46.2% | C (carbon) 41.7% | H (hydrogen) 2.91% | O (oxygen) 9.25%](../image_source/1c9fa03687c8fb4cdbee9da15b4c3b77.png)
formula | BrC_6H_4OH Hill formula | C_6H_5BrO name | 2-bromophenol alternate names | phenol, 2-bromo- | phenol, o-bromo- mass fractions | Br (bromine) 46.2% | C (carbon) 41.7% | H (hydrogen) 2.91% | O (oxygen) 9.25%
Lewis structure
![Draw the Lewis structure of 2-bromophenol. 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), hydrogen (n_H, val = 1), and oxygen (n_O, val = 6) atoms: n_Br, val + 6 n_C, val + 5 n_H, val + n_O, val = 42 Calculate the number of electrons needed to completely fill the valence shells for bromine (n_Br, full = 8), carbon (n_C, full = 8), hydrogen (n_H, full = 2), and oxygen (n_O, full = 8): n_Br, full + 6 n_C, full + 5 n_H, full + n_O, full = 74 Subtracting these two numbers shows that 74 - 42 = 32 bonding electrons are needed. Each bond has two electrons, so in addition to the 13 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/afcd33ec2962bfefc822f292a43d77c7.png)
Draw the Lewis structure of 2-bromophenol. 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), hydrogen (n_H, val = 1), and oxygen (n_O, val = 6) atoms: n_Br, val + 6 n_C, val + 5 n_H, val + n_O, val = 42 Calculate the number of electrons needed to completely fill the valence shells for bromine (n_Br, full = 8), carbon (n_C, full = 8), hydrogen (n_H, full = 2), and oxygen (n_O, full = 8): n_Br, full + 6 n_C, full + 5 n_H, full + n_O, full = 74 Subtracting these two numbers shows that 74 - 42 = 32 bonding electrons are needed. Each bond has two electrons, so in addition to the 13 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/73c20538829c5939c37e71fc2409e849.png)
3D structure
Basic properties
![molar mass | 173.01 g/mol phase | liquid (at STP) melting point | 5 °C boiling point | 195 °C density | 1.492 g/cm^3 solubility in water | soluble](../image_source/666c1e7ee63ebf843f5723110d40d674.png)
molar mass | 173.01 g/mol phase | liquid (at STP) melting point | 5 °C boiling point | 195 °C density | 1.492 g/cm^3 solubility in water | soluble
Units
Hydrophobicity and permeability properties
![predicted LogP hydrophobicity | 2.52 predicted LogS | -1.36](../image_source/795c82ef8d7e3b44561d380a751b1c28.png)
predicted LogP hydrophobicity | 2.52 predicted LogS | -1.36
Basic drug properties
![approval status | experimental | small molecule](../image_source/6022f07784cb5be226a79a0dd5b491f7.png)
approval status | experimental | small molecule
Liquid properties (at STP)
![density | 1.492 g/cm^3 vapor pressure | 0.32 mmHg (at 25 °C) refractive index | 1.589](../image_source/822b1aef4eddb4700707243c613220e6.png)
density | 1.492 g/cm^3 vapor pressure | 0.32 mmHg (at 25 °C) refractive index | 1.589
Units
Thermodynamic properties
![molar heat of vaporization | 44.8 kJ/mol specific heat of vaporization | 0.259 kJ/g (at STP)](../image_source/2577ac73f6ed873f75450f8dfb4cdc5e.png)
molar heat of vaporization | 44.8 kJ/mol specific heat of vaporization | 0.259 kJ/g (at STP)
Chemical identifiers
![CAS number | 95-56-7 Beilstein number | 1905115 PubChem CID number | 7244 PubChem SID number | 24847983 SMILES identifier | C1=CC=C(C(=C1)O)Br InChI identifier | InChI=1/C6H5BrO/c7-5-3-1-2-4-6(5)8/h1-4, 8H InChI key | VADKRMSMGWJZCF-UHFFFAOYAR RTECS number | SJ7875000 MDL number | MFCD00002146](../image_source/5e97d93d8018c8ce04555691aec0f2d4.png)
CAS number | 95-56-7 Beilstein number | 1905115 PubChem CID number | 7244 PubChem SID number | 24847983 SMILES identifier | C1=CC=C(C(=C1)O)Br InChI identifier | InChI=1/C6H5BrO/c7-5-3-1-2-4-6(5)8/h1-4, 8H InChI key | VADKRMSMGWJZCF-UHFFFAOYAR RTECS number | SJ7875000 MDL number | MFCD00002146
NFPA label
![NFPA label](../image_source/56860892b521b2557b8ed4063aa42abb.png)
NFPA label
![NFPA health rating | 1 NFPA fire rating | 2 NFPA reactivity rating | 0](../image_source/ddbf6e0027fc3f4e61aba864c7a38e46.png)
NFPA health rating | 1 NFPA fire rating | 2 NFPA reactivity rating | 0
Safety properties
![flash point | 42.22 °C](../image_source/17cffaf23ebd4b6ea19d98f6dfbd8bcd.png)
flash point | 42.22 °C
![DOT hazard class | 6.1 DOT numbers | 2810](../image_source/7751437c1f360720b508379262ad8b19.png)
DOT hazard class | 6.1 DOT numbers | 2810
Toxicity properties
![RTECS classes | other](../image_source/e246058d0e80da3dfa26c93332d848f2.png)
RTECS classes | other