Chloroform is attracted to itself because of London Dispersion Forces and Dipole-Dipole Forces. The Cl of the first molecule (circled in red) is negative and the H of the second molecule (also circled in red) is positive. The negative end of the first molecule is attracted to the positive end of the second molecule. The orange line between the two atoms represents the dipole-dipole attraction. London dispersion forces also act upon this bond. London dispersion forces are present in every bond, creating a temporary dipole between the two molecules. This is due to the quick movement of the electrons around the atoms.
Intermolecular Forces:
ReplyDeleteBrooke did a nice job showing the intermolecular forces in the picture. She correctly identified the forces and drew a nice picture to show the forces.
Brooke's blog is very appealing. The multiple images and soothing backgorund make this blog very welcoming. She includes multiple pictures of the molecule which are all correct. the picture above that she has drawn is a correct dash model of chloroform.There are dispersion forces which she has identified as well as dipole-dipole attraction. The molecule is correctly named polar. The ad is very persuasive. The way so lists all the different uses for chloroform show that there are benefits to purchasing it. The 30% off makes the offer even more intriguing.
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