Input interpretation
![1, 2-difluorobenzene](../image_source/7f141d18ae7583127819f6b660b48905.png)
1, 2-difluorobenzene
Chemical names and formulas
![formula | C_6H_4F_2 name | 1, 2-difluorobenzene alternate names | benzene, 1, 2-difluoro- | benzene, o-difluoro- | o-difluorobenzene | ortho-difluorobenzene mass fractions | C (carbon) 63.2% | F (fluorine) 33.3% | H (hydrogen) 3.53%](../image_source/11df0b0d58e50571d00875db36270b77.png)
formula | C_6H_4F_2 name | 1, 2-difluorobenzene alternate names | benzene, 1, 2-difluoro- | benzene, o-difluoro- | o-difluorobenzene | ortho-difluorobenzene mass fractions | C (carbon) 63.2% | F (fluorine) 33.3% | H (hydrogen) 3.53%
Lewis structure
![Draw the Lewis structure of 1, 2-difluorobenzene. Start by drawing the overall structure of the molecule, ignoring potential double and triple bonds: Count the total valence electrons of the carbon (n_C, val = 4), fluorine (n_F, val = 7), and hydrogen (n_H, val = 1) atoms: 6 n_C, val + 2 n_F, val + 4 n_H, val = 42 Calculate the number of electrons needed to completely fill the valence shells for carbon (n_C, full = 8), fluorine (n_F, full = 8), and hydrogen (n_H, full = 2): 6 n_C, full + 2 n_F, full + 4 n_H, full = 72 Subtracting these two numbers shows that 72 - 42 = 30 bonding electrons are needed. Each bond has two electrons, so in addition to the 12 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/b194544f14c3564f1bdb099ee4e1a3f5.png)
Draw the Lewis structure of 1, 2-difluorobenzene. Start by drawing the overall structure of the molecule, ignoring potential double and triple bonds: Count the total valence electrons of the carbon (n_C, val = 4), fluorine (n_F, val = 7), and hydrogen (n_H, val = 1) atoms: 6 n_C, val + 2 n_F, val + 4 n_H, val = 42 Calculate the number of electrons needed to completely fill the valence shells for carbon (n_C, full = 8), fluorine (n_F, full = 8), and hydrogen (n_H, full = 2): 6 n_C, full + 2 n_F, full + 4 n_H, full = 72 Subtracting these two numbers shows that 72 - 42 = 30 bonding electrons are needed. Each bond has two electrons, so in addition to the 12 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/551e5444699a3bdd015c3baf0abd9763.png)
3D structure
Basic properties
![molar mass | 114.09 g/mol phase | liquid (at STP) melting point | -34 °C boiling point | 92 °C density | 1.158 g/cm^3 solubility in water | slightly soluble](../image_source/d0d5e6c42f65dfa8cea357817e1c5bc7.png)
molar mass | 114.09 g/mol phase | liquid (at STP) melting point | -34 °C boiling point | 92 °C density | 1.158 g/cm^3 solubility in water | slightly soluble
Units
Liquid properties (at STP)
![density | 1.158 g/cm^3 vapor pressure | 57 mmHg (at 25 °C) refractive index | 1.443](../image_source/56688050c59365b9382308d828b9230b.png)
density | 1.158 g/cm^3 vapor pressure | 57 mmHg (at 25 °C) refractive index | 1.443
Units
Thermodynamic properties
![specific heat capacity c_p | liquid | 1.394 J/(g K) molar heat capacity c_p | liquid | 159 J/(mol K) specific heat of formation Δ_fH° | gas | -2.575 kJ/g | liquid | -2.892 kJ/g molar heat of formation Δ_fH° | gas | -293.8 kJ/mol | liquid | -330 kJ/mol specific entropy S° | liquid | 1.951 J/(g K) molar entropy S° | liquid | 222.6 J/(mol K) molar heat of vaporization | 32.2 kJ/mol | specific heat of vaporization | 0.282 kJ/g | molar heat of fusion | 11.05 kJ/mol | specific heat of fusion | 0.0968 kJ/g | critical temperature | 566 K | (at STP)](../image_source/faa743ea1fe0e3a836f5b55c529e3c12.png)
specific heat capacity c_p | liquid | 1.394 J/(g K) molar heat capacity c_p | liquid | 159 J/(mol K) specific heat of formation Δ_fH° | gas | -2.575 kJ/g | liquid | -2.892 kJ/g molar heat of formation Δ_fH° | gas | -293.8 kJ/mol | liquid | -330 kJ/mol specific entropy S° | liquid | 1.951 J/(g K) molar entropy S° | liquid | 222.6 J/(mol K) molar heat of vaporization | 32.2 kJ/mol | specific heat of vaporization | 0.282 kJ/g | molar heat of fusion | 11.05 kJ/mol | specific heat of fusion | 0.0968 kJ/g | critical temperature | 566 K | (at STP)
Chemical identifiers
![CAS number | 367-11-3 Beilstein number | 1905113 PubChem CID number | 9706 PubChem SID number | 24847704 SMILES identifier | C1=CC=C(C(=C1)F)F InChI identifier | InChI=1/C6H4F2/c7-5-3-1-2-4-6(5)8/h1-4H RTECS number | CZ5655000 MDL number | MFCD00000284](../image_source/00f32b63b1f7e75cc126d896c441b735.png)
CAS number | 367-11-3 Beilstein number | 1905113 PubChem CID number | 9706 PubChem SID number | 24847704 SMILES identifier | C1=CC=C(C(=C1)F)F InChI identifier | InChI=1/C6H4F2/c7-5-3-1-2-4-6(5)8/h1-4H RTECS number | CZ5655000 MDL number | MFCD00000284
NFPA label
![NFPA label](../image_source/6b97009a45d340f04f0ef538c64cd054.png)
NFPA label
![NFPA health rating | 1 NFPA fire rating | 3 NFPA reactivity rating | 0](../image_source/1d88095ce1fce6294cbacbb7c9180379.png)
NFPA health rating | 1 NFPA fire rating | 3 NFPA reactivity rating | 0
Safety properties
![flash point | 2.222 °C](../image_source/2068f9ac5b192800cf9d60bb4fae804b.png)
flash point | 2.222 °C
![DOT hazard class | 3 DOT numbers | 1993](../image_source/34d5cd01f5415755b3341e8932444a91.png)
DOT hazard class | 3 DOT numbers | 1993
Toxicity properties
![RTECS classes | other](../image_source/f01e9500676f683c9757e8106a194276.png)
RTECS classes | other