bioex_lect13

bioex_lect13 - MIT OpenCourseWare http:/ocw.mit.edu 5.111...

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MIT OpenCourseWare http://ocw.mit.edu 5.111 Principles of Chemical Science Fall 2008 For information about citing these materials or our Terms of Use, visit: http://ocw.mit.edu/terms .
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non-polar polar Polar Covalent Bonds/Polar Molecules See lecture 13 for an discussion of polar covalent bonds and polar versus non-polar molecules. A polar covalent bond is an unequal sharing of electrons between two atoms with different electronegativities ( χ ). In general, a bond between two atoms with an χ difference of 0.4 to 1.7 (on the Pauling scale) is considered polar covalent. Polar molecules have a non-zero net dipole moment. Both CO 2 and H 2 O have two polar bonds. However the dipoles in the linear CO 2 molecule cancel each other out, meaning that the CO 2 molecule is non-polar. The polar bonds in the bent H 2 O molecule result in a net dipole moment, so H 2 O is polar. In large organic molecules, such as drugs and vitamins, and in biomolecules, such as proteins, we often consider the number of polar groups within the molecule to determine
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This note was uploaded on 03/02/2012 for the course CHEM 5111 taught by Professor Vogel during the Fall '08 term at MIT.

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bioex_lect13 - MIT OpenCourseWare http:/ocw.mit.edu 5.111...

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