Input interpretation
![1, 2-dibromoethylene](../image_source/75055f424afe5c172c5b99ba8ee47e99.png)
1, 2-dibromoethylene
Chemical names and formulas
![formula | BrCH=CHBr Hill formula | C_2H_2Br_2 name | 1, 2-dibromoethylene IUPAC name | (E)-1, 2-dibromoethylene alternate names | 1, 2-dibromoethene | acetylene dibromide | (E)-1, 2-dibromoethene | (E)-1, 2-dibromoethylene | ethylene, 1, 2-dibromo | ethylene, 1, 2-dibromo- | sym-dibromoethylene mass fractions | Br (bromine) 86% | C (carbon) 12.9% | H (hydrogen) 1.08%](../image_source/5d984a6f40ece28d02d6d30d7c4db0bb.png)
formula | BrCH=CHBr Hill formula | C_2H_2Br_2 name | 1, 2-dibromoethylene IUPAC name | (E)-1, 2-dibromoethylene alternate names | 1, 2-dibromoethene | acetylene dibromide | (E)-1, 2-dibromoethene | (E)-1, 2-dibromoethylene | ethylene, 1, 2-dibromo | ethylene, 1, 2-dibromo- | sym-dibromoethylene mass fractions | Br (bromine) 86% | C (carbon) 12.9% | H (hydrogen) 1.08%
Lewis structure
![Draw the Lewis structure of 1, 2-dibromoethylene. 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: 2 n_Br, val + 2 n_C, val + 2 n_H, val = 24 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): 2 n_Br, full + 2 n_C, full + 2 n_H, full = 36 Subtracting these two numbers shows that 36 - 24 = 12 bonding electrons are needed. Each bond has two electrons, so in addition to the 5 bonds already present in the diagram add 1 bond. 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 1 bond by pairing electrons between adjacent highlighted atoms: Answer: | |](../image_source/91c5c8ea34451a2322717317c1b6f1f7.png)
Draw the Lewis structure of 1, 2-dibromoethylene. 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: 2 n_Br, val + 2 n_C, val + 2 n_H, val = 24 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): 2 n_Br, full + 2 n_C, full + 2 n_H, full = 36 Subtracting these two numbers shows that 36 - 24 = 12 bonding electrons are needed. Each bond has two electrons, so in addition to the 5 bonds already present in the diagram add 1 bond. 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 1 bond by pairing electrons between adjacent highlighted atoms: Answer: | |
3D structure
![3D structure](../image_source/ce72587b96f6c9b743926148aad5bfef.png)
3D structure
Basic properties
![molar mass | 185.85 g/mol phase | liquid (at STP) melting point | -53 °C boiling point | 110 °C (measured at 100508 Pa) density | 2.246 g/cm^3 solubility in water | insoluble](../image_source/bc2ee0b0e98d73cd4ad471e07e766ec5.png)
molar mass | 185.85 g/mol phase | liquid (at STP) melting point | -53 °C boiling point | 110 °C (measured at 100508 Pa) density | 2.246 g/cm^3 solubility in water | insoluble
Units
Liquid properties (at STP)
![density | 2.246 g/cm^3 vapor pressure | 31 mmHg (at 25 °C) refractive index | 1.541](../image_source/6f283923cdad6110e2863d01670c4a50.png)
density | 2.246 g/cm^3 vapor pressure | 31 mmHg (at 25 °C) refractive index | 1.541
Units
Thermodynamic properties
![specific heat capacity c_p | gas | 0.3783 J/(g K) molar heat capacity c_p | gas | 70.3 J/(mol K) molar heat of vaporization | 33.3 kJ/mol | specific heat of vaporization | 0.179 kJ/g | (at STP)](../image_source/3a37fc0bdf6b01cd3f463657e846d0fc.png)
specific heat capacity c_p | gas | 0.3783 J/(g K) molar heat capacity c_p | gas | 70.3 J/(mol K) molar heat of vaporization | 33.3 kJ/mol | specific heat of vaporization | 0.179 kJ/g | (at STP)
Chemical identifiers
![CAS number | 540-49-8 Beilstein number | 1719351 PubChem CID number | 637929 PubChem SID number | 24893814 SMILES identifier | C(=CBr)Br InChI identifier | InChI=1/C2H2Br2/c3-1-2-4/h1-2H/b2-1+ RTECS number | KV7700000 MDL number | MFCD00000184](../image_source/44f9d601a3bd020a8dc8ca70bfb8f9dc.png)
CAS number | 540-49-8 Beilstein number | 1719351 PubChem CID number | 637929 PubChem SID number | 24893814 SMILES identifier | C(=CBr)Br InChI identifier | InChI=1/C2H2Br2/c3-1-2-4/h1-2H/b2-1+ RTECS number | KV7700000 MDL number | MFCD00000184
NFPA label
![NFPA label](../image_source/f29d0f2fc19c475a0b94cfc1009059b6.png)
NFPA label
![NFPA health rating | 2 NFPA fire rating | 0 NFPA reactivity rating | 0](../image_source/a1a77cff44add2405183234d3a92a431.png)
NFPA health rating | 2 NFPA fire rating | 0 NFPA reactivity rating | 0
Safety properties
![flash point | -4 °C](../image_source/726f42a7f631a0d74e8481f6cbb3c014.png)
flash point | -4 °C
![DOT hazard class | 6.1 DOT numbers | 2810](../image_source/c96d7c98dd62ffa9901fd7981d32a225.png)
DOT hazard class | 6.1 DOT numbers | 2810
Toxicity properties
![RTECS classes | mutagen](../image_source/601182525c8c3004eff94ea625370333.png)
RTECS classes | mutagen