Linked Questions

6
votes
1answer
9k views

why do electron pairs not take axial positions in the VSEPR structure of ClF3? [duplicate]

when we make a Valence shell electron pair repulsion theory based structure for an molecule after calculating its hybridisation ; when we have to decide the positions of the ions we put them in such ...
5
votes
0answers
81 views

Why do some molecules form T shapes instead of trigonal planar shapes [duplicate]

Consider a molecule such as $\ce{ClF_3}$. Shouldn't the electron clouds (which are more negative than the Chlorine atom) want to repel each other and so the $\ce{ClF_3}$molecule should arrange into a ...
2
votes
0answers
63 views

Trigonal bipyramidal arrangement with 2 lone pairs [duplicate]

So basically according to university textbooks, it is said that the second lone pair in a trigonal bypyramidal arrangement would also reside on the trigonal plane, causing the two lone pairs to be ...
70
votes
2answers
24k views

What is Bent's rule?

I'm all bent out of shape trying to figure out what Bent's rule means. I have several formulations of it, and the most common formulation is also the hardest to understand. Atomic s character ...
52
votes
1answer
6k views

Why does F replace the axial bond in PCl5?

Why does $\ce{F}$ replace an axial bond in $\ce{PCl5}$? I realize that it would be more stable there than at equatorial bond, but what is the reason of its stability? Similarly in $\ce{AB4}$ type of ...
33
votes
2answers
3k views

Hypervalency and the octet rule

I realize that the octet rule is more a suggestion than a rule, and that it applies mainly to non-transition metal compounds. Still, compounds that don't have an octet, like $\ce{BH3}$, tend to ...
6
votes
2answers
7k views

How can Iodine bond with 5 Fluorines in Iodine Pentafluoride?

According to this lewis diagram, Iodine has 12 valence electrons? How is the possible? Only thing I can think of is that I'm mistaken in counting the covalent bonds as two valence electrons each. Do ...
0
votes
2answers
2k views

Structure of the bifluoride anion [duplicate]

I came across this structure of $\ce{HF2-}$ and realized that the bond shown between H and F is a hydrogen bond. $$\Large\ce{[F-H-F]-}$$ HF hydrogen bond are the strongest hydrogen bonds we know, ...
4
votes
2answers
3k views

Does fluorine ever form a double or triple bond?

Does fluorine ever form a double or triple bond? I wonder if seeming lack of such higher order bonds is related to the electronegativity of fluorine.
2
votes
1answer
499 views

How can chlorine have 10 electrons around it in chlorine trifluoride?

I'm relatively new to chemistry, and while doing some exercises about $\ce{ClF_3}$ I tried to draw where the electrons are. I checked Google and got this: How is this structure possible? From what I'...