*blocks your path*

*blocks your path*

Other urls found in this thread:

en.wikipedia.org/wiki/T-shaped_molecular_geometry
twitter.com/SFWRedditGifs

is it officially the most violent oxidizer known?

*protonates you*

*Protonates you harder*

*electrophilically donates an oxygen atom*

Does it arrange the F atoms in that particular way because of the two electronpairs above Cl?

Sorry to randomly throwing in a question, but i'm still learning chemistry

*decides it's just not worth it to go down that path*

yes. See NH3 vs CH4

yes
en.wikipedia.org/wiki/T-shaped_molecular_geometry

the T shape isn't the only option though, you could have a planar AX3 with both nonbonding pairs aligned on the z axis

>antimony
barely even a real element

*leaches through your rubber gloves and kills you a month later*

*makes you evacuate the lab after spill*

*blocks everyone's path*

triphenylamine has a lone pair but the nitrogen and the three carbons its bound to all lie in a plane

but that's not the case with PPh3, why is this?

The bulky phenyl groups in NPh3 would experience significant back strain if they were forced to assume a trigonal pyramidal geometry, since nitrogen is a small atom. The larger phosphorus atom is more accommodating. The low pKa value of triphenylamine compared to saturated trialkylamines also suggest delocatization of the nitrogen's lone pair within the phenyl groups, which is more efficient when the compound assumes a planar geometry. The lone pair of phosphorus is too high in energy to overlap efficiently with the phenyl groups.

*resists synthesis*

thanks for the explanation user

primarily because of double bond rule

*carbon sheet*
> enough to block alpha

chemistry is cool

*explodes*

You are like little baby
Watch this

>tfw putting this molecule on VSPER quizzes
Its fun molecule in all sorts of ways

>oxidizer
>doesn't have oxygen
take a look at this brainlet over here

*ruins your can of soup*

Fuck you, I didn't want to can any garlic.

Just a random chemistry question, but why does pH affect the solubility of heavy metals?

>what is redox chemistry
>what is fluorine
>what is ammonia

The question is not the question you should be asking. pH changes the solubility of lots of different things, not only heavy metals, and the presence of some ions in a solution can help other ions enter solution, or inversely prevent them dissolving. pH simply measures the balance of H3O+ and OH ions in a solution. If you want a general answer as to why heavy metals are often affected by pH in particular, that's beyond my understanding. Note that metals often form complexes with other ions in the right environment, and these complexes may be more or less soluble than their constituents, so changing the environment may indirectly change how many of these metal ions are in solution.

*allows life*

>Oxidizer
>huurrr durrr it not have oxygen

>Note that metals often form complexes with other ions in the right environment, and these complexes may be more or less soluble than their constituents
that's basically the answer, metals are generally less soluble in higher pH (>9) because they form metal hydroxides like Fe(OH)2-3 for example which are not very soluble

*protonates your hydrocarbons*

Is this the "hypergolic with wood, cloth and test engineers" fucker that was considered as a rocket fuel?

Best post all thread

>doesn't know F2 to O2 endothermic reaction

Why would that block the path?

>In a Veeky Forums thread
>Doesn't realise that an oxidising agent is just an electron acceptor and doesn't have to contain oxygen
Congratulations brainlet, you played yourself

this has to be b8

neopentane is sterically really bulky. think of the tert-butyl group only slightly more so.
it's not as enthusiastically explosive as the other shit posted in this thread though, yeah.

You all got baited