The Periodic Table

hBy2Py

00:44

So, homework is still to be used? @Jan

chemistry.stackexchange.com/revisions/61000/3

@Loong Is there also an implication that equal volumes were transferred to each tube?

@Jan Why is technician/technician not MacGuyver?

Jan

01:03

@hBy2Py Whyever should homework not be used for questions that are clearly homework?

Jan

01:18

@hBy2Py Is it Chuck Norris? (I’m bad at recognising people.)

If it is, Chuck Norris >>>>>>>>>>>>>>>>>>>>>>>>>>>>>>>>>>>>>>> MacGyver.

hBy2Py

02:20

@Jan Oh, there was some discussion at some point about homework being a purely meta tag, and therefore should be discarded.

And yep, that's Chuck Norris. :-)

Aaron Abraham

04:14

Anyone into Inorganic chem. ?

DHMO

@AaronAbraham do you have a question?

Aaron Abraham

Yep.

DHMO

@AaronAbraham just ask

"inorganic chem" is quite broad

no idea which branch you refer to

Aaron Abraham

Well, if I've got this correct, the greater the stability of an ion, the higher its Ionization enthalpy, right?

DHMO

@AaronAbraham i think so

Aaron Abraham

04:17

Good, now that would imply that the tripositive ions of Gd and Lu in the f-block ought to be fairly high right?

DHMO

Gd: 3rd: 1990 kJ/mol
Lu: 3rd: 2022.3 kJ/mol

@AaronAbraham

Aaron Abraham

It looks high to me..

DHMO

Eu: 3rd: 2404 kJ/mol

[Xe] 4f7 6s2

Aaron Abraham

But my textbook says those values are abnormally low

@DHMO Ah...

I see..

DHMO

@AaronAbraham then why?

Aaron Abraham

04:24

But Gd and Lu tripositive ions have half and fully filled f-orbitals respectively....so shouldn't that symmetry make them extra stable? So shouldn't their third I.E be higher than the rest of the Lanthanides?

Melanie Shebel

Should I clean this up for the umm... posterity... of the site or leave it? chemistry.stackexchange.com/questions/38607/…

It's a hot mess.

Aaron Abraham

@Mel By all means.

@DHMO ?

DHMO

@AaronAbraham thinking

Aaron Abraham

Ah, sorry.

DHMO

@AaronAbraham if the ion is stable and the ionization enthalpy is low, that means the atom is stable as well?

because ionization energy cannot be more relative

Aaron Abraham

04:28

Whaaa...

DHMO

just a guess

Aaron Abraham

Wait, a low I.E value would imply that the electron's going to be easier to remove; so we'd be looking at an unstable/ less stable electronic configuration, right?

DHMO

yes

Aaron Abraham

So should the tripositive Gd and Lu have a higher IE value?

My textbook an even the data you provided (thank you) seem to contradict that...

DHMO

in fact ie3 is just the potential energy of 5d right

Aaron Abraham

04:32

4f?

DHMO

and ie3 of Eu is 4f

no

5d for Gd

Aaron Abraham

I thought IE2 pulls out the last electron from 5d for Gd?

DHMO

but Gd is [Xe] 4f7 5d1 6s2

Aaron Abraham

Give me a sec...

dipositive Gd is 4f7 5d1 6s0 Right? Ah okay....

DHMO

yes

Aaron Abraham

04:40

Alright, I see I wasn't thinking straight....my bad. Thanks @DHMO

I'm clear with this now.

DHMO

ok

Aaron Abraham

I'll be off now, Danke ;)

user228700

Hi everyone :-)

user228700

Quick question; is the Xenon atom in $XeO_3$ $sp^3$ hybridized?

user228700

It seems like that from my calculations, but it doesn't make any sense :/

user228700

04:51

(Only 'cause $Xe$ is one of the noble gases)

user228700

Hang on, let me show its lewis dot structure:

user228700

DHMO

sp2

user228700

Can u tell me how?

user228700

The only other possible lewis structure is this:

DHMO

04:55

3 steric regions?

user228700

@DHMO No, there are 4; there's a lp too.

DHMO

yes, sp3 then

user228700

How come? (I mean, how does it work in the orbitals thing?)

DHMO

what do you mean?

user228700

05:03

OK, let me draw...

user228700

Hang on, $\pi$ bonds can't even be made using a hybridized orbital, correct?

user228700

So how does $sp^3$ make any sense?

user228700

U there?

DHMO

@Kaumudi let me think

user228700

05:13

Alright.

DHMO

@Kaumudi just treat them as dative bonds

Aaron Abraham

Org Chem anyone?

DHMO

@AaronAbraham Guten Tag

Aaron Abraham

1

Q: How's the IUPAC name of basketane determined?

A book of mine mentions a certain molecule, basketane, and provides its corresponding structure: Now, I appreciate the book went on to mention this particular compound (I didn't know that organic molecules could be shaped like...well...a basket, so I find this interesting) but the problem is, ...

Mornin' to ya too

DHMO

@AaronAbraham duplicate

Aaron Abraham

05:17

@DHMO

Where??/

DHMO

7

A: How to name tricyclo carbon compounds?

The main ring of a polycyclic hydrocarbon ring system is selected so as to include as many skeletal atoms of the structure as possible. The main bridge is the bridge that includes as many of the atoms as possible that are not included in the main ring. Bridges other than the main bridge are calle...

Aaron Abraham

That was..fast

Oh, and hello to you too @Kaumudi :/

@DHMO Let me read up on it first..

DHMO

11

Q: Cubane systematic name

Why is cubane called $pentacyclo[4.2.0.0^{2,5}.0^{3,8}.0^{4,7}]octane$? I am especially intrigued by the pentacyclo part.

organic-chemistry nomenclature

user228700

@DHMO But we can't have $\pi$ bonds using hybridized orbitals.

DHMO

@Kaumudi then there is no $\pi$ bond

user228700

05:19

@AaronAbraham: Why the ":/"? Morning :-)

DHMO

@Kaumudi because i just suggested two duplicates to his question

Aaron Abraham

How efficient

-_- ^

user228700

OK, it turns out that that's not even the correct structure:

DHMO

@AaronAbraham because earlier I thought about making a self-question about polycyclic compound nomenclature

Aaron Abraham

Pardon?

@DHMO I see.

DHMO

05:21

@AaronAbraham she's talking to me

Aaron Abraham

Oh you've been around for a little over a month @DHMO

She?

DHMO

@AaronAbraham Kaumudi

Aaron Abraham

?

DHMO

?

What did you mean by "Pardon"?

user228700

27 mins ago, by Kaumudi

Aaron Abraham

05:22

I joined a while before you though ^_^

Chuck the 'Pardon'...

user228700

^This is the correct structure

Aaron Abraham

So it is...so it is...

user228700

But this still doesn't make sense.

Aaron Abraham

You're DHMO

DHMO

@Kaumudi what doesn't?

Aaron Abraham

05:23

^

user228700

The orbital thing for this structure either.

user228700

Look:

user228700

DHMO

@Kaumudi No chemistry in high school makes sense

when drawing Lewis structure, treat it as 3 double bonds

when doing hybridization, treat it as 3 dative bonds.

user228700

@DHMO That's a cop out.

DHMO

05:25

yesterday, by DHMO

@Kaumudi complete bullshit

user228700

Yes, well, I don't agree. @orthocresol: Can u help me with this?

user228700

What about you @AaronAbraham? Do u know..?

Aaron Abraham

Well auf wiedersehen wasser

@DHMO

DHMO

@Kaumudi I already told you the answer

@AaronAbraham auf wiedersehen

Aaron Abraham

He already did @Kaumudi

DHMO

05:26

> when drawing Lewis structure, treat it as 3 double bonds
when doing hybridization, treat it as 3 dative bonds.

user228700

@DHMO It doesn't make sense.

DHMO

@Kaumudi 3 dative bonds is more accurate

Lewis structure likes expanded octet

user228700

Well, I mean...it does, but I just want to make sure that that's correct.

DHMO

look, no diagram is accurate

the reality is closer to 3 dative bonds

but Lewis thinks it should be explained by expanded octet

Lewis didn't have quantum machines

user228700

Alright. I just wanna make sure. Also, $S$ in $SO_3$ is $sp^2$ hybridized.

DHMO

05:29

yes

user228700

But u said that it's $sp^3d^2$ yesterday o.O

DHMO

sp3d2 if it has expanded octet

like

if you want to use expanded octet to explain it, then you use sp3d2

if you want to use dative to explain it, then you use sp2

user228700

Uhh. OK...

user228700

06:26

@orthocresol: Hi :-) Do ping me back when u're free...I've got a small question.

DHMO

08:25

@Martin-マーチン You said sp3 is not s x 1 + p x 3?

Martin - マーチン

09:43

A hybrid orbital is a linear combination of atomic orbitals at the same orbital. It is a mathematical description; nothing more nothing less. Hence a sp3 orbital consists of one part s and three parts p. It does not mean that you will always have four sp3 orbitals when you mix one s and three p orbitals. It is very much dependent on the geometry of the molecule you are looking at.

DHMO

@Martin-マーチン I never said you always get 4 sp3 orbitals when you mix one s and three p orbitals

Martin - マーチン

See for example this question about Brent's rule: chemistry.stackexchange.com/q/15671/4945

@DHMO you kind of did

> sp3 means that 1 s orbital mixes with 3 p orbitals to create 4 hybrid orbitals known as sp3 orbitals.

DHMO

@Martin-マーチン Yes, I said what sp3 means is that one s orbital mixes with three p orbitals to create four sp3 orbitals

Martin - マーチン

And that is not correct

DHMO

why?

Martin - マーチン

09:46

because you can have different types of hybrid orbitals at the same atom

DHMO

@Martin-マーチン for example?

Martin - マーチン

I don't have the time to go into it now

DHMO

In that case you shouldn't be using sp3 sp2 sp at all...

Martin - マーチン

this might help though:

6

Q: Difference between oxygens in a carboxylic acid?

I've been reading about MO theory and am wondering if the traditional model of carboxylic acids is correct. Usually, how it's presented is that the carbonyl carbon is doubly bonded to one oxygen and singly bonded to a hydroxyl group. This would mean that one oxygen is $sp^3$ hybridization and the...

organic-chemistry molecular-orbital-theory hybridization

DHMO

I view sp3/sp2/sp to be a simplification, different from what is used in your answer

Martin - マーチン

09:49

I'm not a big fan of hybridisation, because it is often overused in a wrong way. It is not predicting anything, it's just a tool to analyse a given bonding situation

DHMO

@Martin-マーチン looks like there are two meanings of hybridization

not that the simple version is overused

Martin - マーチン

yes, one is absolutely false, the other one only incorrect

DHMO

a simplification has its advantages and disadvantages

@Martin-マーチン how is "false" different from "incorrect"?

Martin - マーチン

incorrect as in at least incomplete hence not correct, but not necessarily wrong if used in the limits of its approximation

DHMO

@Martin-マーチン and the question is asking for sp3/sp2/sp, which clearly points to the false version

Martin - マーチン

09:52

please stop pinging me for every thing. I'm right in front of the monitor, I see what you type

You cleared that question up quite nicely, i was just pointing out that the last part is only true for tetrahedral molecules like methane

DHMO

Sorry that's a habit

Martin - マーチン

for example in $\ce{CHClBrF}$ you have four different hybrid orbitals

DHMO

And in the sp3/sp2/sp model it is explained by, you know, sp3 orbitals.

Martin - マーチン

sp3 orbital can only exist in the symmetric description which is suitable

yes, but that would lead to a wrong description of the molecule

DHMO

no description is accurate

some are just more accurate

Martin - マーチン

09:58

but some are plain wrong

DHMO

...

@Martin-マーチン which means, when a molecule has sp3, it also has 4 sp3 orbitals?

Martin - マーチン

nope

see this one:

21

Q: Are the lone pairs in water equivalent?

It sounds like a dumb question based on the way we draw water, but supposedly water is $sp^3$ hybridized, so one of those lone pairs should be in an $sp^3$ orbital and the other should be in a pure p atomic orbital. First, am I correct about the lone pairs being non-equivalent? Second, if so, d...

water hybridization vsepr-theory

DHMO

but it is rare for sp3 to happen

so water does not have sp3

Martin - マーチン

5. The terminology we use for hybridisation actually is just an abbreviation:
$$\mathrm{sp}^{x} = \mathrm{s}^{\frac{1}{x+1}}\mathrm{p}^{\frac{x}{x+1}}$$
In theory $x$ can have any value; since it is just a [unitary transformation](https://en.wikipedia.org/wiki/Unitary_matrix) the representation does not change, hence
\begin{align}
1\times\mathrm{s}, 3\times\mathrm{p}
&\leadsto 4\times\mathrm{sp}^3 \\
&\leadsto 3\times\mathrm{sp}^2, 1\times\mathrm{p} \\
&\leadsto 2\times\mathrm{sp}, 2\times\mathrm{p} \\

DHMO

water does not have sp3 right

Martin - マーチン

10:04

yeah, it's closer to 2*sp4, p, sp(2/3)

DHMO

exactly

now, what i said is that sp3 means s*1 + p*3

so you haven't exactly disproved this

Martin - マーチン

i never said it wouldn't be

DHMO

well you said i am wrong?

Martin - マーチン

i said you are wrong that sp3 necessarily means four of them

DHMO

alright

Martin - マーチン

10:07

like 1s + 3p = 4 sp3

that's only true for methane

okidoke... need to go now.

DHMO

bye

Martin - マーチン

your answer was good, my comment was only a slight correction of a very popular misconception...

have a great rest-sunday ;)

DHMO

thanks

@Martin-マーチン Could you help me to see if this question is a duplicate before I copy one of the answers from the other questions?

3

Q: How's the IUPAC name of basketane determined?

A book of mine mentions a certain molecule, basketane, and provides its corresponding structure: Now, I appreciate the book went on to mention this particular compound (I didn't know that organic molecules could be shaped like...well...a basket, so I find this interesting) but the problem is, ...

organic-chemistry nomenclature

Martin - マーチン

Questions are only duplicates when they ask the same thing. Only look at the question, not at the answer. They might be related, and one answer probably fits the other, but to be duplicates they need to ask the same thing.

DHMO

but they are essentially asking about the nomenclature of polycyclic compounds

orthocresol

10:16

@Kaumudi ?

Martin - マーチン

yeah, but different compounds

DHMO

@orthocresol She's trying to asking about the (traditionally-assigned) hybridization of Xe in XeO3

She's trying to pass an exam so stop that kind of "sp3 is wrong" thing

orthocresol

Aren't you the one who's saying it's complete bs?

DHMO

but I'm still trying to help people pass their exams

@orthocresol no, I was talking about a paragraph in a textbook

which states that electrons are excited before they form hybrid orbitals

orthocresol

So, by saying that, you are helping her pass her exams?

Right.

DHMO

10:19

@orthocresol why not?

DHMO

10:29

@orthocresol so, could we continue?

What is the hybridization of Xe in XeO3?

orthocresol

10:40

Hmm, seems that S in SO3 is sp2 as well, so I was wrong. @Kaumudi

orthocresol

11:13

This oxidation states guy is irritating. Nothing seems to be enough.

Almost like he wants to use oxidation states to design a new anti-cancer drug and save the world.

Henning Makholm

11:49

No, I just want a conclusion that's not of the form "this is what happens to the oxidation states in that reaction".

And one or more examples of rules that go FROM a premise about oxidation states TO a conclusion that's not about oxidation states.

@orthocresol Would you like to try to enlighten me here instead of in a confused comment thread?

orthocresol

12:18

@HenningMakholm Sure. I think everybody misunderstands what you are asking

Which is why you are getting answers that aren't what you are looking for.

user228700

@orthocresol Yes. $XeO_3$.

user228700

Can u help me out?

orthocresol

Oxidation states are not a physically measurable quantity. From what I've read of your comments, they would be what you call a "pseudo-random number". Yes, the rules that we use to assign oxidation states are arbitrary.

Think of it as a paradigm, if you wish.

One that works.

Did some of the examples not satisfy what you were looking for?

user228700

@orthocresol Yeah, I figured that out today!

orthocresol

e.g. mine about KMnO4, and what Ivan said about reactivity of a certain compound.

What he said was essentially: if an atom is in an unusually high or low oxidation state, then it tends to be reactive.

What I said was essentially: look at oxidation state -> determine electronic configuration -> determine certain properties of compound.

user228700

12:22

@orthocresol: Shall I wait, or will u busy..?

orthocresol

There are more examples of such links between oxidation state -> electronic configuration -> properties, but I figured that if you do not have a chemistry background then it would be Greek to you anyway. Lots of spectroscopy and magnetism of transition metal complexes, for example.

@Kaumudi XeO3 is sp3. It turns out that those pi bonds that you were talking about do not exist.

user228700

@orthocresol OK..? How so?

orthocresol

The Lewis structure is inaccurate.

Sorry for telling you this, but I figured it was the best way to reconcile the two.

Henning Makholm

@orthocresol Indeed. It seems I have somehow gotten it worded in a way that comes across as combative ...

user228700

@orthocresol U're sorry for telling me what..?

orthocresol

12:25

@Kaumudi That the Lewis structure is incorrect.

user228700

@orthocresol I'm learning something every time I'm wrong so don't worry about that :-)

orthocresol

If we talk about SO3 first, you might get an idea of what I mean.

user228700

Alright. Do go on...

orthocresol

So, in SO3, S is sp2 hybridised, and the three sp2 orbitals form three sigma bonds with the oxygens.

So far, so good?

user228700

Yes...

orthocresol

12:27

That leaves one p orbital on sulfur, as well as p orbitals on oxygen.

user228700

Yes.

orthocresol

Now, the Lewis structure says that somehow, sulfur forms pi bonds to all three oxygens.

Henning Makholm

@orthocresol How is that not circular? The explanation I could find says that to define the oxidation states you start by the electronic structure, assign electrons to neighboring atoms via certain rules, and finally get some numbers.

user228700

@orthocresol All three? Just one, no..?

orthocresol

@Kaumudi What's your Lewis structure like? Mine has three S=O double bonds.

@HenningMakholm Going straight from electronic structure -> properties is not always so easy.

Henning Makholm

12:29

But that's already half of your oxidation states -> electronic structure -> properties, isn't it?

user228700

@orthocresol Mine has only one. DHMO posted it earlier...hang on, I'll go look.

orthocresol

@HenningMakholm No, electronic configuration is not the same as electronic structure.

user228700

(Too lazy to draw and then upload lol :-P)

orthocresol

@Kaumudi Don't bother.

Let's assume for now that we're talking about three S=O bonds.

Henning Makholm

@orthocresol Was that not to me?

user228700

12:31

Wait, no, I'll look. Just one second.

orthocresol

@HenningMakholm Oops, sorry. Yes.

Oxidation state is determined by cleaving all bonds heterolytically and assigning the electrons to the more electronegative element.

The electronic structure of a molecule describes the distribution of electron density between the different atoms.

user228700

orthocresol

By assuming that the electron density is completely localised on the more electronegative atom, you arrive at the oxidation state.

Henning Makholm

Yes but -- please bear with me for a moment with a silly thought experiment.

Okay?

orthocresol

Go on.

@Kaumudi That's incorrect, mainly because there are no formal charges. That monovalent oxygen is not happy.

user228700

12:33

@orthocresol Right. OK. 3 $\pi$ bonds. Go on...

orthocresol

The truth is that there is only one pi bond stretching throughout the entire molecule.

So two of those "three pi bonds" don't exist.

As you were told.

But the conventional Lewis structure of SO3 still depicts them as existing.

user228700

Can u please elaborate..?

orthocresol

I could, but that would require MO theory.

Henning Makholm

Suppose we define a different number by, for example, drawing a Lewis structure and assign all bonding electrons to the atom with lowest atomic number instead of by electronegativity. Call it the "kablam number". Now, I'm assuming that kablam numbers are not as useful as oxidation states, because all the world's chemists are not uniformly stupid.

But the reason why kablam numbers are less useful than oxidation numbers must be that there are predictive rules that oxidation numbers satisfy but kablam numbers don't. And I'm trying to get to see one or more of those rules, because they never seem to be stated, or at least not in the places I look.

user228700

I think I could handle MOT. I have that in my syllabus...haven't revised it in awhile, but sure, I guess I 'll understand...

orthocresol

12:36

@Kaumudi Ok, put very simply, in the MO diagram of SO3, there are four bonding orbitals. Three of those four bonding orbitals lead to S-O sigma-type bonding, and the fourth is a pi-type bond between all four atoms.

user228700

@orthocresol Oh, I see...

orthocresol

@HenningMakholm Let me think about it.

user228700

Damn. This "between all four atoms" is weird :/

orthocresol

Indeed. So, the MO description of SO3 does not correspond to the hypervalent Lewis structure with three S=O double bonds.

Which is why I say that two of the three pi bonds don't exist.

user228700

OK...

orthocresol

12:38

Likewise, in XeO3, those pi bonds don't really exist either. So there is no need to try to form them with sp3 orbitals.

You are right, sp3 orbitals do not have the correct geometry to form pi-type bonds.

But they don't exist, so there's no real need to form them.

user228700

So wait, how the heck do I handle these cases w/o knowing all this?

user228700

@orthocresol Yes, I think I get this...

orthocresol

Follow your steric rule and all will be well. :)

XeO3 has four steric regions, as you were saying. Which corresponds to sp3.

Three bonds and one lone pair.

user228700

Yep.

user228700

Alright, I will do this. And I will remember u every time the damned thing doesn't work :-P

user228700

12:41

Also...

DHMO

@orthocresol so XeO4 is sp3?

user228700

DHMO kept asking me to treat them as dative bonds when doing hybridization and as $\pi$ bonds while drawing the Lewis structure.

DHMO

@Kaumudi double bonds

user228700

Is this a good way to think about it?

DHMO

double bonds consist of one $\sigma$ bond + one $\pi$ bond

user228700

12:42

@DHMO Same difference.

DHMO

@Kaumudi Lewis is older.

user228700

@DHMO So?

DHMO

@Kaumudi so his theory is less accurate

so we use expanded octet

user228700

OK?

DHMO

is this good enough?

user228700

12:46

No. I don't even get what u're trying to say, sorry :-P @orthocresol: U still here?

orthocresol

I don't get it either.

DHMO

I thought she was asking for ways to memorize this

user228700

@orthocresol Ah, u're still here!

user228700

7 mins ago, by Kaumudi

DHMO kept asking me to treat them as dative bonds when doing hybridization and as $\pi$ bonds while drawing the Lewis structure.

orthocresol

@HenningMakholm Ok, let's start with this "rule": Cu(I) compounds lack colour. (Which is in general true.) So, for example, CuCN and CuI are both white, or close to white.

user228700

12:50

^That a good way to think about this?

user228700

@DHMO Uhh, no..? I was just asking about that ^

DHMO

@Kaumudi alright

@orthocresol and insoluble in water

Henning Makholm

Hmm, okay.

orthocresol

Your kablam number would assign -1 to Cu in CuCN, and +1 to Cu in CuI.

DHMO

what about non-transition elements?

Hippalectryon

12:52

-1

Q: Thermodynamics Word Problems (VERY URGENT *sad face*)

The neutralization of a hypothetical acid with NaOH has a ΔHrxn = -156.44 kJ/mol. When 20.0mL of the hypothetical acid was titrated with 80.0mL of a standard 0.900 M NaOH solution, the solution turns pink. The resulting solution requires 30.0mL of a 0.6M HCl solution to reach a colorless endpoint...

thermodynamics energy enthalpy entropy free-energy

Wonderful title ._.

orthocresol

Using the oxidation state, however, allows us to predict that such-and-such compound of Cu(I) would be white.

Henning Makholm

Yes, that's the kind of thing I'm looking for.

orthocresol

There is a chemical basis behind that - again has to do with electronic configurations, which one deduces from the oxidation state.

user228700

@Hippalectryon ROFL 😂

user228700

@orthocresol..?

orthocresol

12:56

@Kaumudi I don't know, I have no real opinion on the matter. I'd say, just do whatever works for you.

user228700

OK. Thanks a lot :-)

DHMO

@orthocresol what's the difference between Cl(VII) and Cl(VI)?

Henning Makholm

But I'm seeing explanations that seem to imply e.g. "coal burns because the carbon wants to get to a higher oxidation state, so it likes being in CO2 better than being just C" and I'm trying to figure out what the operative rule behind that is. Because everything is balanced, the carbons cannot gain oxidation states without something else losing them, so that would be a zero-sum game with no net improvement in atomic oxidation happiness.

orthocresol

@HenningMakholm That's because it's not really a great explanation.

Oxygen doesn't lose its oxidation state just because it wants to decrease the oxidation state.

It loses it because oxygen is particularly stable in the -2 oxidation state.

And that can't be rationalised solely by the magnitude of the number -2.

So there is more to it than simply "carbon wants to increase its oxidation number" and "oxygen wants to decrease its".

DHMO

@HenningMakholm For example, oxygen "wants" to become +2 to form OF2 with fluorine

Henning Makholm

13:04

@DHMO Hmm, if orthocresol's explanation means what I think it does, wouldn't OF2 be the oxygen taking one for the team because the fluorines wants to be at -1 even stronger?

DHMO

@HenningMakholm I think so

orthocresol

@HenningMakholm Yes, pretty much.

Henning Makholm

If something like that explanation ended up in an answer, I think I could accept it.

Marcel

13:37

Does anyone by any chance have some input on these questions?
https://chemistry.stackexchange.com/questions/61038/why-are-many-chemical-relationships-logarithmic
https://chemistry.stackexchange.com/questions/60201/reaction-mechanism-in-fluoride-adsorption-to-aluminum-oxide

Despite a few hours of searching around i cannot seem to find an explanation for these (deceptively?) simple questions

DHMO

@Marcel not simple.

Marcel

@DHMO As is often the case, simple on the surface, leagues of murky water below

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