Input interpretation
![methyl carbonate](../image_source/d1cbc6d8c563c47efc42908b8079b1be.png)
methyl carbonate
Chemical names and formulas
![formula | (CH_3O)_2CO Hill formula | C_3H_6O_3 name | methyl carbonate IUPAC name | carbonic acid dimethyl ester alternate names | carbonic acid, dimethyl ester | carbonic acid dimethyl ester | dimethyl carbonate mass fractions | C (carbon) 40% | H (hydrogen) 6.71% | O (oxygen) 53.3%](../image_source/a0785421bf83956c6ed12bc1198bb832.png)
formula | (CH_3O)_2CO Hill formula | C_3H_6O_3 name | methyl carbonate IUPAC name | carbonic acid dimethyl ester alternate names | carbonic acid, dimethyl ester | carbonic acid dimethyl ester | dimethyl carbonate mass fractions | C (carbon) 40% | H (hydrogen) 6.71% | O (oxygen) 53.3%
Lewis structure
![Draw the Lewis structure of methyl carbonate. 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: 3 n_C, val + 6 n_H, val + 3 n_O, val = 36 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): 3 n_C, full + 6 n_H, full + 3 n_O, full = 60 Subtracting these two numbers shows that 60 - 36 = 24 bonding electrons are needed. Each bond has two electrons, so in addition to the 11 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/8917761583072af135d17e217e96ee4f.png)
Draw the Lewis structure of methyl carbonate. 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: 3 n_C, val + 6 n_H, val + 3 n_O, val = 36 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): 3 n_C, full + 6 n_H, full + 3 n_O, full = 60 Subtracting these two numbers shows that 60 - 36 = 24 bonding electrons are needed. Each bond has two electrons, so in addition to the 11 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/6bd780312ce1a3a87b031f24598d16e3.png)
3D structure
Basic properties
![molar mass | 90.08 g/mol phase | liquid (at STP) melting point | 3 °C boiling point | 90 °C density | 1.069 g/cm^3 solubility in water | insoluble](../image_source/614c2a3d5d4d7e7aa0f3e950c3c73cf4.png)
molar mass | 90.08 g/mol phase | liquid (at STP) melting point | 3 °C boiling point | 90 °C density | 1.069 g/cm^3 solubility in water | insoluble
Units
Liquid properties (at STP)
![density | 1.069 g/cm^3 vapor pressure | 18 mmHg dynamic viscosity | 5.781×10^-4 Pa s (at 25 °C) surface tension | 0.0319 N/m refractive index | 1.368](../image_source/28ac8574d397083640d2982aa128bc8a.png)
density | 1.069 g/cm^3 vapor pressure | 18 mmHg dynamic viscosity | 5.781×10^-4 Pa s (at 25 °C) surface tension | 0.0319 N/m refractive index | 1.368
Units
Thermodynamic properties
![molar heat of vaporization | 37.7 kJ/mol specific heat of vaporization | 0.419 kJ/g molar heat of combustion | 1429 kJ/mol specific heat of combustion | 15.86 kJ/g thermal conductivity | 0.1696 W/(m K) critical temperature | 557 K critical pressure | 4.8 MPa (at STP)](../image_source/31c56d4a05760b4f758abd01a805ca50.png)
molar heat of vaporization | 37.7 kJ/mol specific heat of vaporization | 0.419 kJ/g molar heat of combustion | 1429 kJ/mol specific heat of combustion | 15.86 kJ/g thermal conductivity | 0.1696 W/(m K) critical temperature | 557 K critical pressure | 4.8 MPa (at STP)
Chemical identifiers
![CAS number | 616-38-6 Beilstein number | 635821 PubChem CID number | 12021 PubChem SID number | 24873943 SMILES identifier | COC(=O)OC InChI identifier | InChI=1/C3H6O3/c1-5-3(4)6-2/h1-2H3 RTECS number | FG0450000 MDL number | MFCD00008420](../image_source/5c799673914bc2933ecac7129d8ac7df.png)
CAS number | 616-38-6 Beilstein number | 635821 PubChem CID number | 12021 PubChem SID number | 24873943 SMILES identifier | COC(=O)OC InChI identifier | InChI=1/C3H6O3/c1-5-3(4)6-2/h1-2H3 RTECS number | FG0450000 MDL number | MFCD00008420
NFPA label
![NFPA label](../image_source/acd748aa898675e108abc252441a6bde.png)
NFPA label
![NFPA health rating | 1 NFPA fire rating | 3 NFPA reactivity rating | 1](../image_source/183866fd7659187ec2532d1eb4a40962.png)
NFPA health rating | 1 NFPA fire rating | 3 NFPA reactivity rating | 1
Safety properties
![flash point | 18.33 °C autoignition point | 458 °C lower explosive limit | 4.22% (concentration in air) upper explosive limit | 12.87% (concentration in air)](../image_source/935a20419ea367a91591dfe4afd08abe.png)
flash point | 18.33 °C autoignition point | 458 °C lower explosive limit | 4.22% (concentration in air) upper explosive limit | 12.87% (concentration in air)
![DOT hazard class | 3 DOT numbers | 1161](../image_source/88fc2da08552f04de4bac347cbfcf32e.png)
DOT hazard class | 3 DOT numbers | 1161
Toxicity properties
![RTECS classes | other](../image_source/5ae803c8716a46d0a4324c480ba611d0.png)
RTECS classes | other