![]() Electronegative ligands such as F will always go to the axial sites. Figure 8.6 The hypothetical overlap of two of the 2 p orbitals on an oxygen atom (red) with the 1 s orbitals of two hydrogen atoms (blue) would produce a bond angle of 90. First well look at an MO diagram for water, because its pretty simple and water is very important. The prediction of the valence bond theory model does not match the real-world observations of a water molecule a different model is needed. ![]() To understand why this is the case, we need to take a look at electron. The water molecule contains two hydrogen atoms bound to oxygen not at a 90 angle, but at an angle of 104.5. Whilst the atoms in carbon dioxide are held in a straight line, water is a bent molecule. In general, by this reasoning, lone pairs and electropositive ligands such as CH 3 will always prefer the equatorial sites in the trigonal bipyramidal geometry. Here we wont really explain these methods, just show some results. For an atom such as oxygen, we know that the 2s orbital is spherical, and that the 2p x, 2p y, and 2p z orbitals are dumbell-shaped and point along the Cartesian axes. = 0.867 \:bond (formal \: charge = -0.122)\)īecause fluorine is more electronegative than a lone pair, it prefers the axial site where it will have more negative formal charge.
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