metaphosphoric acid

metaphosphoric acid

formula | HPO_3 Hill formula | HO_3P name | metaphosphoric acid IUPAC name | phosphenic acid alternate names | hydridohydroxidodioxidophosphate(1-) | phosphenic acid mass fractions | H (hydrogen) 1.26% | O (oxygen) 60% | P (phosphorus) 38.7%

Draw the Lewis structure of metaphosphoric 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: n_H, val + 3 n_O, val + n_P, val = 24 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): n_H, full + 3 n_O, full + n_P, full = 34 Subtracting these two numbers shows that 34 - 24 = 10 bonding electrons are needed. Each bond has two electrons, so in addition to the 4 bonds already present in the diagram add 1 bond. To minimize formal charge oxygen wants 2 bonds. Identify the atoms that want additional bonds and the number of electrons remaining on each atom: To fully fill its valence shell, phosphorus will donate one of its electrons, allowing it to form four bonds (the maximum number an element on period 2 can form). Fill in the 1 bond by pairing electrons between adjacent highlighted atoms, noting the formal charges of the atoms. Double bonding phosphorus to the other highlighted oxygen atom would result in an equivalent molecule: Answer: | |

molar mass | 79.979 g/mol phase | liquid (at STP) melting point | 21 °C boiling point | 260 °C density | 2.4 g/cm^3 solubility in water | soluble

density | 2.4 g/cm^3 vapor pressure | 0.03 mmHg

specific heat of formation Δ_fH° | solid | -11.86 kJ/g molar heat of formation Δ_fH° | solid | -948.5 kJ/mol (at STP)

CAS number | 37267-86-0 PubChem CID number | 3084658 SMILES identifier | O[P+](=O)[O-] InChI identifier | InChI=1/HO3P/c1-4(2)3/h(H, 1, 2, 3)/f/h1H EU number | 253-433-4 Gmelin number | 1616