(Polar molecules, Non-polar molecules, etc.)
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As the post above states, it kind of looks like a seesaw. Two bonds are at the bottom forming a somewhat triangular shape, with two more bonds balancing on top (where if you "bounced" them they'd tilt like a seesaw). I guess you could also pretend the lone pair are kids on the seesaw as well? Though they aren't really in the right place for it, it might help with remembering there's one lone pair in a seesaw shape.
The seesaw shape refers to a molecule with five regions of e- density with four bonding regions and one lone pair. The seesaw shape has bond angles of <120 and <90. SF4 would be an example of a seesaw shape.
Hi! like other people have said above, in a seesaw shape, there is 5 regions of electron density with 4 bonding pairs and 1 lone pair. 5 regions of electron density would normally be a trigonal bipyramidal shape, but because lone pairs are not used to name the shape, we replace one of the atoms in the trigonal bipyramidal shape with the lone pair. It matters which position you place the lone pair in, so you would place it in the horizonal plane to limit lone pair-bonding pair interactions and this positioning of the lone pair results in the seesaw shape. Hope this helps!
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