Indicate the electron pair geometry and the molecular...

Indicate the electron pair geometry and the molecular geometry for each of the six compounds. Compound Electron pair geometry Molecular geometry :O=S=O: :F-O-F: :O=C=O: :Cl-S-Cl: || :O: Answer Bank trigonal planar tetrahedral linear bent trigonal pyramidal

Transcript

00:01 So for this one, we're asked to find the electron pair geometry and molecular geometry for each of these compounds.

00:08 So for the first one, we have sulfur bonded to two oxygens.

00:12 So when we look at how many electron pairs we have, we look at how many lone pairs and how many bonds it has.

00:21 So we have a double bondably one, two, and three.

00:27 So we have three electron pairs, which means its geometry is going to be trigonal planar.

00:41 Now we look at those three and see how many are lone pairs.

00:46 We have one that are lone pairs.

00:49 So of the three electron pairs, we have two bonding, one lone pair.

00:53 Because of that one lone pair, its molecular geometry is going to be bent.

01:00 If instead sulfur was bonded to only three things, then it would stay trigonal planar because all of these angles would be the same.

01:13 However, because we have that lone pair on top, these electrons will repulse those bonds down.

01:26 And so these two angles will be larger than that angle.

01:30 And so we'll have a bent molecular geometry because of the lone pair versus a trigonal planar.

01:39 Next, we'll go to the oxygen bonded to two fluorines.

01:44 So when we look at the number of electron pairs, we have two lone pairs and then two bonds.

01:55 So we have four electron pairs, which gives it an electron pair geometry of tetrahed.

02:07 However, because we have two of those are lone pairs, the molecular geometry is going to be bent, right? and it's going to be just like above those lone pairs are going to repulse those bonds.

02:33 And so these two areas are going to have a greater angle than the two bonds to each other because those lone pairs need lots and lots of space...

Question

Indicate the electron pair geometry and the molecular geometry for each of the six compounds. Compound Electron pair geometry Molecular geometry :O=S=O: :F-O-F: :O=C=O: :Cl-S-Cl: || :O: Answer Bank trigonal planar tetrahedral linear bent trigonal pyramidal

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