Input interpretation
![tetradecanoyl chloride](../image_source/43759c3ce4c56481e736d51402125c01.png)
tetradecanoyl chloride
Chemical names and formulas
![formula | CH_3(CH_2)_12COCl Hill formula | C_14H_27ClO name | tetradecanoyl chloride alternate names | myristic acid chloride | myristoyl chloride | myristyl chloride | tetradecanoic acid chloride mass fractions | C (carbon) 68.1% | Cl (chlorine) 14.4% | H (hydrogen) 11% | O (oxygen) 6.48%](../image_source/544215d7187111d8181157a09c33d664.png)
formula | CH_3(CH_2)_12COCl Hill formula | C_14H_27ClO name | tetradecanoyl chloride alternate names | myristic acid chloride | myristoyl chloride | myristyl chloride | tetradecanoic acid chloride mass fractions | C (carbon) 68.1% | Cl (chlorine) 14.4% | H (hydrogen) 11% | O (oxygen) 6.48%
Lewis structure
![Draw the Lewis structure of tetradecanoyl chloride. 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), chlorine (n_Cl, val = 7), hydrogen (n_H, val = 1), and oxygen (n_O, val = 6) atoms: 14 n_C, val + n_Cl, val + 27 n_H, val + n_O, val = 96 Calculate the number of electrons needed to completely fill the valence shells for carbon (n_C, full = 8), chlorine (n_Cl, full = 8), hydrogen (n_H, full = 2), and oxygen (n_O, full = 8): 14 n_C, full + n_Cl, full + 27 n_H, full + n_O, full = 182 Subtracting these two numbers shows that 182 - 96 = 86 bonding electrons are needed. Each bond has two electrons, so in addition to the 42 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/e50e25414f11b3931f62486e0cd0f101.png)
Draw the Lewis structure of tetradecanoyl chloride. 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), chlorine (n_Cl, val = 7), hydrogen (n_H, val = 1), and oxygen (n_O, val = 6) atoms: 14 n_C, val + n_Cl, val + 27 n_H, val + n_O, val = 96 Calculate the number of electrons needed to completely fill the valence shells for carbon (n_C, full = 8), chlorine (n_Cl, full = 8), hydrogen (n_H, full = 2), and oxygen (n_O, full = 8): 14 n_C, full + n_Cl, full + 27 n_H, full + n_O, full = 182 Subtracting these two numbers shows that 182 - 96 = 86 bonding electrons are needed. Each bond has two electrons, so in addition to the 42 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/545012a82de54175d720504bb310a00c.png)
3D structure
Basic properties
![molar mass | 246.8 g/mol phase | liquid (at STP) melting point | -1 °C boiling point | 250 °C (measured at 13330 Pa) density | 0.908 g/cm^3 solubility in water | insoluble](../image_source/f1d42bea281fc8ed1664ed12c6089b67.png)
molar mass | 246.8 g/mol phase | liquid (at STP) melting point | -1 °C boiling point | 250 °C (measured at 13330 Pa) density | 0.908 g/cm^3 solubility in water | insoluble
Units
Liquid properties (at STP)
![density | 0.908 g/cm^3 vapor pressure | 0.0014 mmHg (at 25 °C) refractive index | 1.449](../image_source/f07f93caa3dc1c788ee032a12b7c1a17.png)
density | 0.908 g/cm^3 vapor pressure | 0.0014 mmHg (at 25 °C) refractive index | 1.449
Units
Thermodynamic properties
![molar heat of vaporization | 53.6 kJ/mol specific heat of vaporization | 0.217 kJ/g (at STP)](../image_source/e3326a4fa79deb0b98559ac38856f9ff.png)
molar heat of vaporization | 53.6 kJ/mol specific heat of vaporization | 0.217 kJ/g (at STP)