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Why is chloroform a non-polar solvent?
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+ Physical chemistry
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+ Chloroform
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+ Organic chemistry
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Mark Cox
Why is chloroform a non-polar solvent?
Polarity can be defined by many different parameters. On a broad sense, solvents which are miscible with water are considered polar, while immiscible solvents are considered non-polar. In this case, chloroform is considered non-polar.
If one wants a more quantitative description, usually the dielectric constant is used: in this case polarity is not defined as a dichotomic characteristic, but every solvent will lie somewhere on a continuum that goes from "extremely polar" to "extremely non polar". In this case chloroform would be considered somewhere mid-scale, being less polar than the short chain alcohols but definitely more than the alkanes.
Update: as underlined by Yagna, the values previously listed for the dipole moment were wrong
Polarity can be defined by many different parameters. On a broad sense, solvents which are miscible with water are considered polar, while immiscible solvents are considered non-polar. In this case, chloroform is considered non-polar.
If one wants a more quantitative description, usually the dielectric constant is used: in this case polarity is not defined as a dichotomic characteristic, but every solvent will lie somewhere on a continuum that goes from "extremely polar" to "extremely non polar". In this case chloroform would be considered somewhere mid-scale, being less polar than the short chain alcohols but definitely more than the alkanes.
Update: as underlined by Yagna, the values previously listed for the dipole moment were wrong
chloroform has two types of dipoles C-H and three C-Cl they are polarized in opposite direction (delta plus) on the H and (delta) minus on the C in C-H and (delta plus) on the C and (delta) minus on the Cl. Due to the tetrahedral geometry of the CHCl3 molecule, the C-Cl dipoles are partially canceled out but still the whole molecule has noticeable dipole moment rendering chloroform polar molecule/solvent. However, the degree of polarity (absolute value of the dipole moment) is not great as compared to CH3-CN, one of the most polar organic solvents, or H2O, very polar inorganic solvent. To understand this issue, learn about electronegativity of the elements, polarization of covalent bonds and geometry of organic molecules.
chloroform has two types of dipoles C-H and three C-Cl they are polarized in opposite direction (delta plus) on the H and (delta) minus on the C in C-H and (delta plus) on the C and (delta) minus on the Cl. Due to the tetrahedral geometry of the CHCl3 molecule, the C-Cl dipoles are partially canceled out but still the whole molecule has noticeable dipole moment rendering chloroform polar molecule/solvent. However, the degree of polarity (absolute value of the dipole moment) is not great as compared to CH3-CN, one of the most polar organic solvents, or H2O, very polar inorganic solvent. To understand this issue, learn about electronegativity of the elements, polarization of covalent bonds and geometry of organic molecules.
Polarity can be defined by many different parameters. On a broad sense, solvents which are miscible with water are considered polar, while immiscible solvents are considered non-polar. In this case, chloroform is considered non-polar.
If one wants a more quantitative description, usually the dielectric constant is used: in this case polarity is not defined as a dichotomic characteristic, but every solvent will lie somewhere on a continuum that goes from "extremely polar" to "extremely non polar". In this case chloroform would be considered somewhere mid-scale, being less polar than the short chain alcohols but definitely more than the alkanes.
Update: as underlined by Yagna, the values previously listed for the dipole moment were wrong
Polarity can be defined by many different parameters. On a broad sense, solvents which are miscible with water are considered polar, while immiscible solvents are considered non-polar. In this case, chloroform is considered non-polar.
If one wants a more quantitative description, usually the dielectric constant is used: in this case polarity is not defined as a dichotomic characteristic, but every solvent will lie somewhere on a continuum that goes from "extremely polar" to "extremely non polar". In this case chloroform would be considered somewhere mid-scale, being less polar than the short chain alcohols but definitely more than the alkanes.
Update: as underlined by Yagna, the values previously listed for the dipole moment were wrong
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chloroform has two types of dipoles C-H and three C-Cl they are polarized in opposite direction (delta plus) on the H and (delta) minus on the C in C-H and (delta plus) on the C and (delta) minus on the Cl. Due to the tetrahedral geometry of the CHCl3 molecule, the C-Cl dipoles are partially canceled out but still the whole molecule has noticeable dipole moment rendering chloroform polar molecule/solvent. However, the degree of polarity (absolute value of the dipole moment) is not great as compared to CH3-CN, one of the most polar organic solvents, or H2O, very polar inorganic solvent. To understand this issue, learn about electronegativity of the elements, polarization of covalent bonds and geometry of organic molecules.
chloroform has two types of dipoles C-H and three C-Cl they are polarized in opposite direction (delta plus) on the H and (delta) minus on the C in C-H and (delta plus) on the C and (delta) minus on the Cl. Due to the tetrahedral geometry of the CHCl3 molecule, the C-Cl dipoles are partially canceled out but still the whole molecule has noticeable dipole moment rendering chloroform polar molecule/solvent. However, the degree of polarity (absolute value of the dipole moment) is not great as compared to CH3-CN, one of the most polar organic solvents, or H2O, very polar inorganic solvent. To understand this issue, learn about electronegativity of the elements, polarization of covalent bonds and geometry of organic molecules.
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