Input interpretation
![sulfuryl chloride fluoride](../image_source/e2d808acab504886972e1f4bde6a4c22.png)
sulfuryl chloride fluoride
Chemical names and formulas
![formula | SO_2ClF Hill formula | ClFO_2S name | sulfuryl chloride fluoride alternate names | chlorosulfonyl fluoride | fluorosulfonyl chloride | sulfonyl chloride fluoride | sulfuryl chlorofluoride | sulfuryl fluorochloride mass fractions | Cl (chlorine) 29.9% | F (fluorine) 16% | O (oxygen) 27% | S (sulfur) 27.1%](../image_source/c70d0f168a864473dbd0be85d6b7467f.png)
formula | SO_2ClF Hill formula | ClFO_2S name | sulfuryl chloride fluoride alternate names | chlorosulfonyl fluoride | fluorosulfonyl chloride | sulfonyl chloride fluoride | sulfuryl chlorofluoride | sulfuryl fluorochloride mass fractions | Cl (chlorine) 29.9% | F (fluorine) 16% | O (oxygen) 27% | S (sulfur) 27.1%
Lewis structure
![Draw the Lewis structure of sulfuryl chloride fluoride. Start by drawing the overall structure of the molecule, ignoring potential double and triple bonds: Count the total valence electrons of the chlorine (n_Cl, val = 7), fluorine (n_F, val = 7), oxygen (n_O, val = 6), and sulfur (n_S, val = 6) atoms: n_Cl, val + n_F, val + 2 n_O, val + n_S, val = 32 Calculate the number of electrons needed to completely fill the valence shells for chlorine (n_Cl, full = 8), fluorine (n_F, full = 8), oxygen (n_O, full = 8), and sulfur (n_S, full = 8): n_Cl, full + n_F, full + 2 n_O, full + n_S, full = 40 Subtracting these two numbers shows that 40 - 32 = 8 bonding electrons are needed. Each bond has two electrons, so we expect that the above diagram has all the necessary bonds. However, to minimize formal charge oxygen wants 2 bonds. Identify the atoms that want additional bonds and the number of electrons remaining on each atom: In order to minimize their formal charge, atoms with large electronegativities can force atoms with smaller electronegativities on period 3 or higher to expand their valence shells. The electronegativities of the atoms are 2.58 (sulfur), 3.16 (chlorine), 3.44 (oxygen), and 3.98 (fluorine). Because the electronegativity of sulfur is smaller than the electronegativity of oxygen, expand the valence shell of sulfur to 6 bonds. Therefore we add a total of 2 bonds to the diagram: Answer: | |](../image_source/d8060f99841afd149824420e2310b8f5.png)
Draw the Lewis structure of sulfuryl chloride fluoride. Start by drawing the overall structure of the molecule, ignoring potential double and triple bonds: Count the total valence electrons of the chlorine (n_Cl, val = 7), fluorine (n_F, val = 7), oxygen (n_O, val = 6), and sulfur (n_S, val = 6) atoms: n_Cl, val + n_F, val + 2 n_O, val + n_S, val = 32 Calculate the number of electrons needed to completely fill the valence shells for chlorine (n_Cl, full = 8), fluorine (n_F, full = 8), oxygen (n_O, full = 8), and sulfur (n_S, full = 8): n_Cl, full + n_F, full + 2 n_O, full + n_S, full = 40 Subtracting these two numbers shows that 40 - 32 = 8 bonding electrons are needed. Each bond has two electrons, so we expect that the above diagram has all the necessary bonds. However, to minimize formal charge oxygen wants 2 bonds. Identify the atoms that want additional bonds and the number of electrons remaining on each atom: In order to minimize their formal charge, atoms with large electronegativities can force atoms with smaller electronegativities on period 3 or higher to expand their valence shells. The electronegativities of the atoms are 2.58 (sulfur), 3.16 (chlorine), 3.44 (oxygen), and 3.98 (fluorine). Because the electronegativity of sulfur is smaller than the electronegativity of oxygen, expand the valence shell of sulfur to 6 bonds. Therefore we add a total of 2 bonds to the diagram: Answer: | |
3D structure
![3D structure](../image_source/e2305c0a5894911bdb694209c4bc35ea.png)
3D structure
Basic properties
![molar mass | 118.5 g/mol phase | gas (at STP) melting point | -125 °C boiling point | 7 °C density | 1.623 g/cm^3 (at 25 °C) solubility in water | soluble](../image_source/5933922f3ba6101cf6e1acf5a79d70d4.png)
molar mass | 118.5 g/mol phase | gas (at STP) melting point | -125 °C boiling point | 7 °C density | 1.623 g/cm^3 (at 25 °C) solubility in water | soluble
Units
Gas properties (at STP)
![density | 1.623 g/cm^3 (at 25 °C) vapor density | 4.08 (relative to air) molar volume | 73 cm^3/mol](../image_source/2d4cbd9752fb36c88fad318fa7917e48.png)
density | 1.623 g/cm^3 (at 25 °C) vapor density | 4.08 (relative to air) molar volume | 73 cm^3/mol
Units
Thermodynamic properties
![molar heat of vaporization | 26.5 kJ/mol specific heat of vaporization | 0.224 kJ/g (at STP)](../image_source/4a683541ec43410a5430f28c9ed29a9e.png)
molar heat of vaporization | 26.5 kJ/mol specific heat of vaporization | 0.224 kJ/g (at STP)
Chemical identifiers
![CAS number | 13637-84-8 PubChem CID number | 26159 PubChem SID number | 24867414 SMILES identifier | O=S(=O)(F)Cl InChI identifier | InChI=1/ClFO2S/c1-5(2, 3)4 RTECS number | WT4900000 MDL number | MFCD00011607](../image_source/e25cfa802ac41866a5c5c8858a8da1aa.png)
CAS number | 13637-84-8 PubChem CID number | 26159 PubChem SID number | 24867414 SMILES identifier | O=S(=O)(F)Cl InChI identifier | InChI=1/ClFO2S/c1-5(2, 3)4 RTECS number | WT4900000 MDL number | MFCD00011607
NFPA label
![NFPA label](../image_source/12fdc1119a54e29be1c07a98ac5b03d6.png)
NFPA label
![NFPA health rating | 3 NFPA fire rating | 1 NFPA reactivity rating | 2](../image_source/44d7de100cecdd06e3addee3653bc3d8.png)
NFPA health rating | 3 NFPA fire rating | 1 NFPA reactivity rating | 2
Safety properties
![flash point | 109 °C](../image_source/11ff4b8bc15665574660617565db6a57.png)
flash point | 109 °C
![DOT hazard class | 8 DOT numbers | 1760](../image_source/b7c4e3f8550320966ba3c88d31338a25.png)
DOT hazard class | 8 DOT numbers | 1760
Toxicity properties
![RTECS classes | other](../image_source/7324023031d3218e349fcca58b8d1603.png)
RTECS classes | other