= SbH3

stibine

formula | SbH_3 Hill formula | H_3Sb_1 name | stibine mass fractions | H (hydrogen) 2.42% | Sb (antimony) 97.6%

Draw the Lewis structure of stibine. Start by drawing the overall structure of the molecule: Count the total valence electrons of the hydrogen (n_H, val = 1) and antimony (n_Sb, val = 5) atoms: 3 n_H, val + n_Sb, val = 8 Calculate the number of electrons needed to completely fill the valence shells for hydrogen (n_H, full = 2) and antimony (n_Sb, full = 8): 3 n_H, full + n_Sb, full = 14 Subtracting these two numbers shows that 14 - 8 = 6 bonding electrons are needed. Each bond has two electrons, so the above diagram has all the necessary bonds. There are 3 bonds and hence 6 bonding electrons in the diagram. Lastly, fill in the remaining unbonded electrons on each atom. In total, there remain 8 - 6 = 2 electrons left to draw: Answer: | |

molar mass | 124.78 g/mol melting point | -88 °C boiling point | -17 °C solubility in water | slightly soluble

CAS number | 7803-52-3 SMILES identifier | [SbH3]