name of phosphorus pentasulfide

phosphorus pentasulfide

formula | P_2S_5 name | phosphorus pentasulfide alternate names | phosphorus(V) sulfide mass fractions | P (phosphorus) 27.9% | S (sulfur) 72.1%

Draw the Lewis structure of phosphorus pentasulfide. Start by drawing the overall structure of the molecule, ignoring potential double and triple bonds: Count the total valence electrons of the phosphorus (n_P, val = 5) and sulfur (n_S, val = 6) atoms: 2 n_P, val + 5 n_S, val = 40 Calculate the number of electrons needed to completely fill the valence shells for phosphorus (n_P, full = 8) and sulfur (n_S, full = 8): 2 n_P, full + 5 n_S, full = 56 Subtracting these two numbers shows that 56 - 40 = 16 bonding electrons are needed. Each bond has two electrons, so in addition to the 6 bonds already present in the diagram we expect to add 2 bonds. To minimize formal charge sulfur wants 2 bonds. Identify the atoms that want additional bonds and the number of electrons remaining on each atom: Add 2 bonds by pairing electrons between adjacent highlighted atoms. Additionally, atoms with large electronegativities can minimize their formal charge by forcing atoms with smaller electronegativities on period 3 or higher to expand their valence shells. The electronegativities of the atoms are 2.19 (phosphorus) and 2.58 (sulfur). Because the electronegativity of phosphorus is smaller than the electronegativity of sulfur and the electronegativity of {} is smaller than the electronegativity of {}, expand the valence shell of phosphorus to 5 bonds in 2 places and expand the valence shell of {} to {} bonds. Therefore we add a total of 4 bonds to the diagram: Answer: | |

molar mass | 222.3 g/mol phase | solid (at STP) melting point | 282 °C density | 2.09 g/cm^3

density | 2.09 g/cm^3

molar heat of vaporization | 95 kJ/mol specific heat of vaporization | 0.4274 kJ/g (at STP)

CAS number | 1314-80-3 SMILES identifier | S=P(=S)SP(=S)=S RTECS number | TH4375000 MDL number | MFCD00011441