Solvents 101
Solvents comes in different forms. The basic categories are nonpolar, polar aprotic, and polar protic.
Polar vs nonpolar has to do with the overall dipole moment of the molecules that make up the solvent or material. Symmetries tend to cause internal dipole moments to cancel out overall.
Protic vs aprotic has to do with whether the solvent has a hydrogen atom bound to oxygen or nitrogen (forming either hydroxyl or amine groups). The hydrogen atom, if it is "labile", may be seen as a ready-to-donate proton for any reagents.
Remembering the types of solvents is easy; solvent may be polar or nonpolar due to symmetry or a lack thereof. Solvents may be protic or aprotic due to having labile protons to donate.
Many different parameters exist that describe the ways in which bonds are formed or affect each other and overall give a more complete picture of a solvent's properties.
Sometimes you are able to replace one solvent or solvent mixture with a different solvent or mixture by substituting the constituents based on the Hansen solubility parameters. Taking the weighted averages of the pure values allows one to approximate replacements.
Other physical properties that affect a solvent's uses include boiling point and density. Boiling point determines rate of evaporation. Density determines how layers will form such as when partitioning compounds in a separatory funnel.
Most organic solvents are flammable and sometimes mixtures of solvent vapors and air can actually explode. Solvent vapors are heavier than air and can travel large distances or remain undiluted for long periods of time.
A strange thing can happen with solvents that are ethers. They can form highly explosive organic peroxides when exposed to oxygen and light. To avoid this, ethers should be stored in airtight containers far from light. Low-volume users of ethers should acquire only small amounts to minimize risk of peroxide formation over long periods of time.
Many solvents are dangerous to inhale or be chronically exposed to. Risks include toxicity or cancer.
Polar vs nonpolar has to do with the overall dipole moment of the molecules that make up the solvent or material. Symmetries tend to cause internal dipole moments to cancel out overall.
Protic vs aprotic has to do with whether the solvent has a hydrogen atom bound to oxygen or nitrogen (forming either hydroxyl or amine groups). The hydrogen atom, if it is "labile", may be seen as a ready-to-donate proton for any reagents.
Remembering the types of solvents is easy; solvent may be polar or nonpolar due to symmetry or a lack thereof. Solvents may be protic or aprotic due to having labile protons to donate.
Many different parameters exist that describe the ways in which bonds are formed or affect each other and overall give a more complete picture of a solvent's properties.
Sometimes you are able to replace one solvent or solvent mixture with a different solvent or mixture by substituting the constituents based on the Hansen solubility parameters. Taking the weighted averages of the pure values allows one to approximate replacements.
Other physical properties that affect a solvent's uses include boiling point and density. Boiling point determines rate of evaporation. Density determines how layers will form such as when partitioning compounds in a separatory funnel.
Most organic solvents are flammable and sometimes mixtures of solvent vapors and air can actually explode. Solvent vapors are heavier than air and can travel large distances or remain undiluted for long periods of time.
A strange thing can happen with solvents that are ethers. They can form highly explosive organic peroxides when exposed to oxygen and light. To avoid this, ethers should be stored in airtight containers far from light. Low-volume users of ethers should acquire only small amounts to minimize risk of peroxide formation over long periods of time.
Many solvents are dangerous to inhale or be chronically exposed to. Risks include toxicity or cancer.
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