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Dichloromethane, a chlorinated solvent, is a common ingredient in many industrial applications. It is used to strip paint, as a degreasing agent and as a cleaning solvent in metal processing. It has been linked to a number of health hazards, including respiratory tract irritation, drowsiness, dizziness, headaches and nausea.
It is also a probable human carcinogen (Group B2). The US Environmental Protection Agency has banned its use in consumer products, but this does not go far enough to protect the public from these risks.
In the laboratory, dichloromethane is often used as an extractant in chemical reactions. This is particularly so in the case of organic compounds.
However, it is important to understand the chemical behavior of dichloromethane. It is a volatile liquid that can be flammable.
This property is attributed to the attractive forces that are formed between molecules or atoms in pure substances. The melting point and boiling point of pure substances reflect these attractions.
They can be influenced by a variety of factors, such as molecular size and shape. Larger molecules have more electrons and nuclei that generate van der Waals attractions, which give them higher boiling points than similar compounds made up of smaller molecules.
These boiling points are often used to identify and distinguish one substance from another. This is because they are a good indicator of the intermolecular attraction between the two components.