name of phosphinic acid

phosphinic acid

formula | HPH_2O_2 Hill formula | H_3O_2P_1 name | phosphinic acid mass fractions | H (hydrogen) 4.58% | O (oxygen) 48.5% | P (phosphorus) 46.9%

Draw the Lewis structure of phosphinic acid. Start by drawing the overall structure of the molecule, ignoring potential double and triple bonds: Count the total valence electrons of the hydrogen (n_H, val = 1), oxygen (n_O, val = 6), and phosphorus (n_P, val = 5) atoms: 3 n_H, val + 2 n_O, val + n_P, val = 20 Calculate the number of electrons needed to completely fill the valence shells for hydrogen (n_H, full = 2), oxygen (n_O, full = 8), and phosphorus (n_P, full = 8): 3 n_H, full + 2 n_O, full + n_P, full = 30 Subtracting these two numbers shows that 30 - 20 = 10 bonding electrons are needed. Each bond has two electrons, so we expect that the above diagram has all the necessary bonds. However, to minimize formal charge oxygen wants 2 bonds. Identify the atom that wants additional bonds and the number of electrons remaining on each atom: In order to minimize their formal charge, atoms with large electronegativities can force atoms with smaller electronegativities on period 3 or higher to expand their valence shells. The electronegativities of the atoms are 2.19 (phosphorus), 2.20 (hydrogen), and 3.44 (oxygen). Because the electronegativity of phosphorus is smaller than the electronegativity of oxygen, expand the valence shell of phosphorus to 5 bonds. Therefore we add a total of 1 bond to the diagram: Answer: | |

molar mass | 65.996 g/mol melting point | 26.5 °C boiling point | 130 °C density | 1.49 g/cm^3

CAS number | 6303-21-5 SMILES identifier | O[PH2]=O