CHEM 281 Lecture Notes - Lecture 2: Van Der Waals Surface, Van Der Waals Force, Carbon Tetrachloride
12 Jun 2017
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Example: the hcl molecule: the more electronegative chlorine draws electron density away from the hydrogen, the more electronegative chlorine develops a partial negative charge. Module 2: physical properties and molecular structure (including polarity) v note that hcl has a permanent dipole, it is a polar molecule. Not all molecules with polar bonds though are polar. Sometimes the polar bonds with a molecule cancel each other out in terms of dipole moments though and the overall molecule is not polar: the dipole moment of a molecule can be measured experimentally. In a diatomic molecule, a dipole exists if the two atoms are of different electronegativity. In carbon tetrachloride, the bond dipoles cancel and the overall molecular dipole is 0 debye (fig. 3) the c-h bonds have only small dipoles but the c-cl bond has a large dipole and the molecular is quite polar.
