(Polar molecules, Non-polar molecules, etc.)
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Trigonal planar molecules have 4 electron pairs, 1 lone PR and 3 bonding pairs (with 3 atoms). T-shaped molecules have 5 electron pairs, 2 lone pairs and 3 bonding pairs (with 3 atoms). Both of these have 3 bonding pairs with 3 separate atoms, but the amount of lone pairs differs.
Trigonal Planar has uniform bond angles of 120°. It has three regions of electron density: three bound atoms and no lone pairs.
T-shaped looks like a T; it doesn't have uniform bond angles, they're 90°, 180°. It has five regions of electron density: three bound atoms and two lone pairs.
(tshape, but with the lone pairs drawn as the yellow portions)
they have different amounts of electron dense areas - trigonal planar has 3 electron dense (paired) areas while t-shaped has 5 electron dense areas while 2 are lone pairs (aka there should be a different amount of electrons on the molecule that will help you tell)
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