2E1 - Molecules with bent geometry

[nicolely2F]

Exercise 2E.1 displays one bent molecule and one linear molecule. The answer key says that the linear molecule "may have" (not necessarily has) lone pairs of electrons on the central atom. I have a theory for why this is possible (since the textbook didn't mention this, at least not in 2E); is it when the central atom has more than 1 lone pair (in addition to e.g. 2 bound atoms) and these lone pairs cancel each other out, allowing for a linear geometry? I'd also appreciate examples!

[Qilan Li 4I]

I think a good example would be XeF2 where it has 2 bound atoms and 3 lone pairs. Another example would be I3.

[chrisleung-2J]

Yes, although most molecules in which the central atom has lone pairs of electrons have a dipole moment, there are some exceptions in which the dipole moments caused by the lone pairs of electrons cancel out. One example of this is the configuration AX2E3, which is linear due to the three lone pairs of electrons around the central atom having diploe moments which cancel out, thereby resulting in a linear configuration.

[Ashley Tran 2I]

For this problem, I found it useful to look at the bond angles. The first example, bent, has angles 120 degrees and we know that for a bent electron arrangement, there must be 2 bonding pairs and 1 or 2 lone pairs. Therefore, in the diagram, when only 2 bonding pairs are shown, we know we must have at least one more lone pair. On the other hand, the second example shows a molecule with a bond angle of 180 degrees. We know this must is a linear molecular shape and therefore there are 2 bonding pairs and 0 lone pairs. However, the electron arrangement with 2 bonding pairs and 3 lone pairs is also linear, therefore, in this example, there may be lone pairs, but it is not required like the first one.

[005384106]

Do lone pair electrons have a stronger force of repulsion of atoms compared to the strength of atoms repelling against each other?

[Emily Chirila 2E]

Do lone pair electrons have a stronger force of repulsion of atoms compared to the strength of atoms repelling against each other?

These are the relative strengths of repulsion:
lone-lone pair repulsion > lone-bonding pair repulsion > bonding-bonding pair repulsion

[Julia Mazzucato 4D]

Do lone pair electrons have a stronger force of repulsion of atoms compared to the strength of atoms repelling against each other?

These are the relative strengths of repulsion:
lone-lone pair repulsion > lone-bonding pair repulsion > bonding-bonding pair repulsion

I've heard from a past student knowledge of this hierarchy is important in a test question at some point, either on the second exam or final.

[005384106]

What is the difference between lone-lone pair repulsion, lone-bonding pair repulsion, and bonding- bonding pair repulsion? I thought there was only repulsion differences of 2 types such as a lone pair electron pair and an atom.