Input interpretation
![silicon disulfide](../image_source/6cd4719c0399b000322806653ef02167.png)
silicon disulfide
Chemical names and formulas
![formula | S_2Si name | silicon disulfide IUPAC name | disulfanylidenesilane alternate names | silicon disulphide | silicone disulfide | silicon sulfide mass fractions | S (sulfur) 69.5% | Si (silicon) 30.5%](../image_source/de87a3db77c3938178f7f62bfca9c0fb.png)
formula | S_2Si name | silicon disulfide IUPAC name | disulfanylidenesilane alternate names | silicon disulphide | silicone disulfide | silicon sulfide mass fractions | S (sulfur) 69.5% | Si (silicon) 30.5%
Lewis structure
![Draw the Lewis structure of silicon disulfide. Start by drawing the overall structure of the molecule, ignoring potential double and triple bonds: Count the total valence electrons of the sulfur (n_S, val = 6) and silicon (n_Si, val = 4) atoms: 2 n_S, val + n_Si, val = 16 Calculate the number of electrons needed to completely fill the valence shells for sulfur (n_S, full = 8) and silicon (n_Si, full = 8): 2 n_S, full + n_Si, full = 24 Subtracting these two numbers shows that 24 - 16 = 8 bonding electrons are needed. Each bond has two electrons, so in addition to the 2 bonds already present in the diagram add 2 bonds. To minimize formal charge sulfur wants 2 bonds and silicon wants 4 bonds. Identify the atoms that want additional bonds and the number of electrons remaining on each atom: Fill in the 2 bonds by pairing electrons between adjacent highlighted atoms: Answer: | |](../image_source/2f953b7cf2b004e40bc3b19baa96d39b.png)
Draw the Lewis structure of silicon disulfide. Start by drawing the overall structure of the molecule, ignoring potential double and triple bonds: Count the total valence electrons of the sulfur (n_S, val = 6) and silicon (n_Si, val = 4) atoms: 2 n_S, val + n_Si, val = 16 Calculate the number of electrons needed to completely fill the valence shells for sulfur (n_S, full = 8) and silicon (n_Si, full = 8): 2 n_S, full + n_Si, full = 24 Subtracting these two numbers shows that 24 - 16 = 8 bonding electrons are needed. Each bond has two electrons, so in addition to the 2 bonds already present in the diagram add 2 bonds. To minimize formal charge sulfur wants 2 bonds and silicon wants 4 bonds. Identify the atoms that want additional bonds and the number of electrons remaining on each atom: Fill in the 2 bonds by pairing electrons between adjacent highlighted atoms: Answer: | |
3D structure
![3D structure](../image_source/93ca5f96c9afd1f2ee67a8564e7f22ab.png)
3D structure
Basic properties
![molar mass | 92.21 g/mol phase | solid (at STP) melting point | 1090 °C density | 2.02 g/cm^3](../image_source/64d96e544e69ecb44e093003b8a5d445.png)
molar mass | 92.21 g/mol phase | solid (at STP) melting point | 1090 °C density | 2.02 g/cm^3
Units
Solid properties (at STP)
![density | 2.02 g/cm^3](../image_source/11061b11d0b306239052380cd26f833e.png)
density | 2.02 g/cm^3
Units
Chemical identifiers
![CAS number | 13759-10-9 PubChem CID number | 83705 SMILES identifier | [Si](=S)=S InChI identifier | InChI=1/S2Si/c1-3-2 EU number | 237-344-8](../image_source/fee73c1eb4a523fa73bf7addc4b740bb.png)
CAS number | 13759-10-9 PubChem CID number | 83705 SMILES identifier | [Si](=S)=S InChI identifier | InChI=1/S2Si/c1-3-2 EU number | 237-344-8
NFPA label
![NFPA label](../image_source/eeb0ca129c31eabb93371ae55e0542ed.png)
NFPA label
![NFPA health rating | 2 NFPA fire rating | 2 NFPA reactivity rating | 3](../image_source/e02f4f60d3313b6ff738a3d19286b46b.png)
NFPA health rating | 2 NFPA fire rating | 2 NFPA reactivity rating | 3