Input interpretation
sulfur hexafluoride
Chemical names and formulas
formula | SF_6 Hill formula | F_6S name | sulfur hexafluoride alternate names | contrast agent bR1 | elegas | sulfur fluoride | sulphur hexafluoride mass fractions | F (fluorine) 78% | S (sulfur) 22%
Lewis structure
Draw the Lewis structure of sulfur hexafluoride. Start by drawing the overall structure of the molecule: Count the total valence electrons of the fluorine (n_F, val = 7) and sulfur (n_S, val = 6) atoms: 6 n_F, val + n_S, val = 48 Calculate the number of electrons needed to completely fill the valence shells for fluorine (n_F, full = 8) and sulfur (n_S, full = 8): 6 n_F, full + n_S, full = 56 Subtracting these two numbers shows that 56 - 48 = 8 bonding electrons are needed, which are already accounted for in the structure. Note that the valence shell of sulfur has been expanded to 6 bonds. After accounting for the expanded valence, there are 6 bonds and hence 12 bonding electrons in the diagram. Lastly, fill in the remaining unbonded electrons on each atom. In total, there remain 48 - 12 = 36 electrons left to draw: Answer: | |
Basic properties
molar mass | 146.05 g/mol phase | gas (at STP) melting point | -49.596 °C boiling point | -63.8 °C density | 0.00597 g/cm^3 (at 50 °C) dielectric constant | 1.002
Gas properties (at STP)
density | 0.00597 g/cm^3 (at 50 °C) vapor density | 5.11 (relative to air) molar volume | 24460 cm^3/mol dynamic viscosity | 3.7204×10^-5 Pa s (at 627 °C)
Units
Thermodynamic properties
specific free energy of formation Δ_fG° | gas | -7.645 kJ/g molar free energy of formation Δ_fG° | gas | -1117 kJ/mol specific heat of formation Δ_fH° | gas | -8.357 kJ/g molar heat of formation Δ_fH° | gas | -1221 kJ/mol specific entropy S° | gas | 1.999 J/(g K) molar entropy S° | gas | 292 J/(mol K) molar heat of fusion | 5.02 kJ/mol | specific heat of fusion | 0.03437 kJ/g | thermal conductivity | 0.01262 W/(m K) | critical temperature | 319 K | critical pressure | 3.77 MPa | (at STP)
Phase diagram
Phase diagram
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