Input interpretation
![carbonic acid](../image_source/eb62c7403d06feaae53c1c20364420ed.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/3b2f1cec76ea61f40b828ffd2d5716e2.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/a4150b7b1a3e6306d2fb3257567d966a.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/0c20eeed027c9663abfb2695d6557a89.png)
3D structure
Basic properties
![molar mass | 62.024 g/mol](../image_source/48710aa4d3522c9cdbe81925910ada91.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/8391609590fd216722faeaa5ebb0d670.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)