name of arsenic(V) sulfide

arsenic(V) sulfide

formula | As_2S_5 name | arsenic(V) sulfide mass fractions | As (arsenic) 48.3% | S (sulfur) 51.7%

Draw the Lewis structure of arsenic(V) sulfide. Start by drawing the overall structure of the molecule, ignoring potential double and triple bonds: Count the total valence electrons of the arsenic (n_As, val = 5) and sulfur (n_S, val = 6) atoms: 2 n_As, val + 5 n_S, val = 40 Calculate the number of electrons needed to completely fill the valence shells for arsenic (n_As, full = 8) and sulfur (n_S, full = 8): 2 n_As, 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 2.18 (arsenic) and 2.58 (sulfur). Because the electronegativity of arsenic is smaller than the electronegativity of sulfur and the electronegativity of {} is smaller than the electronegativity of {}, expand the valence shell of arsenic 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 | 310.1 g/mol phase | solid (at STP) melting point | 300 °C

CAS number | 1303-34-0 PubChem CID number | 3371533 PubChem SID number | 24874060 SMILES identifier | S=[As](=S)S[As](=S)=S InChI identifier | InChI=1/As2S5/c3-1(4)7-2(5)6 MDL number | MFCD00049840