Input interpretation
![carbonic acid](../image_source/cb182c80ebed08945567737ec968f87d.png)
carbonic acid
Chemical names and formulas
![formula | H_2CO_3 Hill formula | CH_2O_3 name | carbonic acid mass fractions | C (carbon) 19.4% | H (hydrogen) 3.25% | O (oxygen) 77.4%](../image_source/6f0c86d9932a7ade24c55f8b635d4e4a.png)
formula | H_2CO_3 Hill formula | CH_2O_3 name | carbonic acid mass fractions | C (carbon) 19.4% | H (hydrogen) 3.25% | O (oxygen) 77.4%
Lewis structure
![Draw the Lewis structure of carbonic acid. Start by drawing the overall structure of the molecule, ignoring potential double and triple bonds: Count the total valence electrons of the carbon (n_C, val = 4), hydrogen (n_H, val = 1), and oxygen (n_O, val = 6) atoms: n_C, val + 2 n_H, val + 3 n_O, val = 24 Calculate the number of electrons needed to completely fill the valence shells for carbon (n_C, full = 8), hydrogen (n_H, full = 2), and oxygen (n_O, full = 8): n_C, full + 2 n_H, full + 3 n_O, full = 36 Subtracting these two numbers shows that 36 - 24 = 12 bonding electrons are needed. Each bond has two electrons, so in addition to the 5 bonds already present in the diagram add 1 bond. To minimize formal charge oxygen wants 2 bonds and carbon wants 4 bonds. Identify the atoms that want additional bonds and the number of electrons remaining on each atom: Fill in the 1 bond by pairing electrons between adjacent highlighted atoms: Answer: | |](../image_source/02ab46564b25725b73982f72e446875d.png)
Draw the Lewis structure of carbonic acid. Start by drawing the overall structure of the molecule, ignoring potential double and triple bonds: Count the total valence electrons of the carbon (n_C, val = 4), hydrogen (n_H, val = 1), and oxygen (n_O, val = 6) atoms: n_C, val + 2 n_H, val + 3 n_O, val = 24 Calculate the number of electrons needed to completely fill the valence shells for carbon (n_C, full = 8), hydrogen (n_H, full = 2), and oxygen (n_O, full = 8): n_C, full + 2 n_H, full + 3 n_O, full = 36 Subtracting these two numbers shows that 36 - 24 = 12 bonding electrons are needed. Each bond has two electrons, so in addition to the 5 bonds already present in the diagram add 1 bond. To minimize formal charge oxygen wants 2 bonds and carbon wants 4 bonds. Identify the atoms that want additional bonds and the number of electrons remaining on each atom: Fill in the 1 bond by pairing electrons between adjacent highlighted atoms: Answer: | |
3D structure
![3D structure](../image_source/2eebdd7204429a20040637d74cd52679.png)
3D structure
Basic properties
![molar mass | 62.024 g/mol](../image_source/8d38c428a79bf28556cdeb95dda49fdf.png)
molar mass | 62.024 g/mol
Units
Chemical identifiers
![PubChem CID number | 767 SMILES identifier | C(=O)(O)O InChI identifier | InChI=1S/CH2O3/c2-1(3)4/h(H2, 2, 3, 4)](../image_source/537dcac8f854f2e14b4fe46bdb50d93a.png)
PubChem CID number | 767 SMILES identifier | C(=O)(O)O InChI identifier | InChI=1S/CH2O3/c2-1(3)4/h(H2, 2, 3, 4)