Molecules with Electrons Oriented in Five Directions

Five pairs of electrons will orient themselves with three pairs 120 degrees apart in a plane and the two additional pairs at right angles to the plane.  If there are lone pairs, they exert an influence but are not seen in the molecular geometry.  Click on the image and drag to rotate the molecules.

What do you think happens to the bond angles between adjacent atoms when lone pairs are present?

Any lone pairs arrange themselves in the plane of the three electron pairs.

Phosphorus pentachloride   PCl5 Sulfur tetrafluoride  SF4 Iodine trichloride    ICl3
trigonal bipyramidal see-saw T-shaped

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