Chapter_7 Oct_08 Lecture_21.pptx

# Because all four electron domains are bonds the

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Because all four electron domains are bonds, the molecular geometry of this part of the molecule is also tetrahedral. The electron-domain geometry of the middle C is trigonal planar. Again, because all the domains are bonds, the molecular geometry is also trigonal planar. The electron-domain geometry of the O atom is tetrahedral. Because two of the domains are lone pairs, the molecular geometry about the O atom is bent.

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Solution (cont.) Bond angles are determined using electron-domain geometry. Therefore, the approximate bond angles about the leftmost C are 109.5°C, those about the middle C are 120°, and those about the O are 109.5°. The angle between the two single bonds on the middle carbon will be less than 120° because the double bond repels the single bonds more strongly than they repel each other. Likewise, the bond angle between the two bonds on the O will be less than 109.5° because the lone pairs on O repel the single bonds more strongly than they repel each other and push the two bonding pairs closer together. The angles are labeled as follows: Worked Example
Molecular Geometry and Polarity Molecular polarity affects boiling point, melting point, solubility, etc. -- E.g. polar molecules attract each other, high boiling point Bonds in a molecule can be polar, but molecule can be nonpolar -- depends on arrangement of polar bonds -- polar molecules often have lone pair(s) on central atom -- polar molecules often have asymmetric arrangement of terminal atoms A diatomic molecule is polar when the electronegativities of the two atoms are different.
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• Fall '16
• hawk
• Atom, Molecule, trigonal bipyramidal, Molecular Geometry and Polarity

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