Super-dipoles create chloroform’s super powers
Polar stacks facilitate dissolution by polarising
Super-dipoles uncovered in chloroform by chemists in the UK could explain the solvent’s powerful ability to dissolve a large range of substances at high concentrations.
Chloroform is one chemistry’s most extensively used forms of liquid reaction media. However, as a suspected carcinogen, chloroform’s role underscores scientists’ aspirations to understand the science behind its remarkable properties. Now, Christoph Salzmann, from University College London, and colleagues have used neutron diffraction to gain insight into the microscopic structure of liquid chloroform.
This article provides a link to coverage by Chemistry World
Thanks for using Education in Chemistry. You can view one Education in Chemistry article per month as a visitor.
Register for Teach Chemistry for free, unlimited access
Registration is open to all teachers and technicians at secondary schools, colleges and teacher training institutions in the UK and Ireland.
Get all this, plus much more:
- unlimited access to resources, core practical videos and Education in Chemistry articles
- teacher well-being toolkit, personal development resources and online assessments
- applications for funding to support your lessons
Already a Teach Chemistry member? Sign in now.
Not eligible for Teach Chemistry? Sign up for a personal account instead, or you can also access all our resources with Royal Society of Chemistry membership.