Input interpretation
phosphorus(V) dichloride trifluoride
Chemical names and formulas
formula | PCl_2F_3 Hill formula | Cl_2F_3P_1 name | phosphorus(V) dichloride trifluoride mass fractions | Cl (chlorine) 44.6% | F (fluorine) 35.9% | P (phosphorus) 19.5%
Lewis structure
Draw the Lewis structure of phosphorus(V) dichloride trifluoride. Start by drawing the overall structure of the molecule: Count the total valence electrons of the chlorine (n_Cl, val = 7), fluorine (n_F, val = 7), and phosphorus (n_P, val = 5) atoms: 2 n_Cl, val + 3 n_F, val + n_P, val = 40 Calculate the number of electrons needed to completely fill the valence shells for chlorine (n_Cl, full = 8), fluorine (n_F, full = 8), and phosphorus (n_P, full = 8): 2 n_Cl, full + 3 n_F, full + n_P, full = 48 Subtracting these two numbers shows that 48 - 40 = 8 bonding electrons are needed, which are already accounted for in the structure. Note that the valence shell of phosphorus has been expanded to 5 bonds. After accounting for the expanded valence, there are 5 bonds and hence 10 bonding electrons in the diagram. Lastly, fill in the remaining unbonded electrons on each atom. In total, there remain 40 - 10 = 30 electrons left to draw: Answer: | |
Basic properties
molar mass | 158.9 g/mol melting point | -125 °C boiling point | 7.1 °C
Units
Chemical identifiers
CAS number | 13454-99-4 SMILES identifier | ClP(Cl)(F)(F)F