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11.2 VSEPR Theory: The Five Basic Shapes
Determine the geometry of NO 3.
Determine the number of valence electrons in the NO 3 by NO 3.
The Lewis counts the number of electron groups around the structure.
Draw a Lewis structure for NO 3.
There are three equivalent bonds in the hybrid structure.
There are two single bonds and one double bond in the nitrogen atom.
The geometry that reduces the repulsions between three electron groups is called trigonal planar.
The three bonds exert the same repulsion on the other two and the molecule has three equal bond angles.
Determine the geometry of CCl4.
In the examples that follow, we see that the lone pairs repel other electron groups.
The bonding pairs are influenced by the lone pair.
Lone pair electrons exert more repulsions than bonding electrons.
A lone electron pair is more spread out in space than a bonding electron pair because a lone pair is attracted to only one nucleus.
The lone pair electrons exert H sion.
There are five electron groups in the central sulfur atom.
If you notice, the lone pair could occupy either an equatorial position or an axial position within the trigonal bipyramidal electron geometry.
As we have just seen, lone pair-bonding pair repulsions are greater than bonding pair-bonding pair repulsions.
The lone pair occupies a position that reduces its interaction with the bonding pairs.
The lone pair would have three 90deg interactions with bonding pairs.
There are only two 90deg interactions in an equatorial posi.
A lone pair-lone pair 90deg repulsion is avoided by F.
In XeF2, when three of the five electron groups around the central atom are lone pairs, the lone pairs occupy all three of the equatorial positions.
The Lewis structure is shown here.
There are six electron groups in the central bromine atom.
The six electron groups make up the electron geometry.
The lone pair can be found in any of the six positions.
The central atom has only electron groups.
Each of the following is considered a single electron group.
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