Input interpretation
![acetonitrile-1-13 C](../image_source/38cfacab980e85dec34ce137dec8d551.png)
acetonitrile-1-13 C
Chemical names and formulas
![formula | CH_3^13CN Hill formula | C(13C)H_3N name | acetonitrile-1-13 C IUPAC name | acetonitrile alternate names | ethanenitrile | methyl cyanide-13C mass fractions | N (nitrogen) 0.333% | C (carbon) 0.595% | H (hydrogen) 0.0719%](../image_source/011085f40ab826fee93718176411a6e8.png)
formula | CH_3^13CN Hill formula | C(13C)H_3N name | acetonitrile-1-13 C IUPAC name | acetonitrile alternate names | ethanenitrile | methyl cyanide-13C mass fractions | N (nitrogen) 0.333% | C (carbon) 0.595% | H (hydrogen) 0.0719%
Lewis structure
![Draw the Lewis structure of acetonitrile-1-13 C. 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 nitrogen (n_N, val = 5) atoms: 2 n_C, val + 3 n_H, val + n_N, val = 16 Calculate the number of electrons needed to completely fill the valence shells for carbon (n_C, full = 8), hydrogen (n_H, full = 2), and nitrogen (n_N, full = 8): 2 n_C, full + 3 n_H, full + n_N, full = 30 Subtracting these two numbers shows that 30 - 16 = 14 bonding electrons are needed. Each bond has two electrons, so in addition to the 5 bonds already present in the diagram add 2 bonds. To minimize formal charge nitrogen wants 3 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 2 bonds by pairing electrons between adjacent highlighted atoms: Answer: | |](../image_source/f0c5a9cca2c73dc2f2350f27d22237d2.png)
Draw the Lewis structure of acetonitrile-1-13 C. 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 nitrogen (n_N, val = 5) atoms: 2 n_C, val + 3 n_H, val + n_N, val = 16 Calculate the number of electrons needed to completely fill the valence shells for carbon (n_C, full = 8), hydrogen (n_H, full = 2), and nitrogen (n_N, full = 8): 2 n_C, full + 3 n_H, full + n_N, full = 30 Subtracting these two numbers shows that 30 - 16 = 14 bonding electrons are needed. Each bond has two electrons, so in addition to the 5 bonds already present in the diagram add 2 bonds. To minimize formal charge nitrogen wants 3 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 2 bonds by pairing electrons between adjacent highlighted atoms: Answer: | |
Basic properties
![molar mass | 42.045 g/mol phase | liquid (at STP) melting point | -48 °C boiling point | 81.5 °C density | 0.805 g/cm^3](../image_source/21e3709141ad64d2bf8d6dd4da7741b4.png)
molar mass | 42.045 g/mol phase | liquid (at STP) melting point | -48 °C boiling point | 81.5 °C density | 0.805 g/cm^3
Units
Liquid properties (at STP)
![density | 0.805 g/cm^3 refractive index | 1.344](../image_source/fdc5ae712477c7b94713010f184731e7.png)
density | 0.805 g/cm^3 refractive index | 1.344
Units
Non-standard atom properties
![C-13 | 1](../image_source/416406a0b6b1c2028d022f2c753686fc.png)
C-13 | 1
Chemical identifiers
![CAS number | 31432-55-0 PubChem CID number | 10866249 PubChem SID number | 24872032 SMILES identifier | CC#N InChI identifier | InChI=1/C2H3N/c1-2-3/h1H3/i1+1 MDL number | MFCD00001879](../image_source/a7662b0cf511afaba3ada44473d3200f.png)
CAS number | 31432-55-0 PubChem CID number | 10866249 PubChem SID number | 24872032 SMILES identifier | CC#N InChI identifier | InChI=1/C2H3N/c1-2-3/h1H3/i1+1 MDL number | MFCD00001879
Safety properties
![flash point | 5.556 °C](../image_source/9f7d48ce90e165a257839ad77feab3ba.png)
flash point | 5.556 °C