Chemistry 1027A/B Chapter Notes - Chapter 2.2: Chlorine Pentafluoride, Chlorine Trifluoride, Xenon Difluoride

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ochrebee715

30 Apr 2012

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Pairs of electrons, both bonding and non-bonding, occupy the valence shell of a central atom. These electron pairs, or regions of electron density, repel each other and spatially position themselves to maximize the separation of the pairs. Lone pairs exert greater repulsive forces than bonding pairs. Multiple bonds are treated as single regions of electron density. M" is the number of atoms x" bonded on the central atom, a". N" is the number of lone electron pairs e" on the central atom a". M+n = the total number of regions of electron density around the central atom. *indicates a non-polar molecule if the dipoles cancel out. Line represents a bond in the plane of the paper. Dotted line represents a bond directed behind the plane of the paper. Wedged line represents a bond directed in front of the plane of the paper. A molecule is polar if it has a net dipole movement.

Related Questions

Predict the molecular shape of using VSEPR theory.

Draw for yourself the best Lewis structure.
Count the number of electron groups (bond pairs and lone pairs, with multiple counting as one effective electron group) around the central atom, Answer

To establish the electron-group arrangement, Answer. From the electron-group arrangement, you can determine the hybridization of the central atom to be Answer

The electron-group arrangement is not (necessarily) the same as the molecular shape, which is named on the basis of the arrangement of atoms. The molecular shape is Answer
The ideal bond angles around the central atom are Answer. By analyzing repulsive forces between electron pairs (both lone pairs and bond pairs) and realizing that only bond angles subtended by atoms (not lone pairs) can actually be observed, you can predict if any deviations will occur; the experimental bond angles around the central atom will be Answer the ideal bond angles.
Taking the vector sum of bond dipoles, you can evaluate the net dipole moment and predict that the molecule will be Answer