Basicity vs Nucleophilicity - Steric Hindrance 

Now i feel like i can be the god of organic chem

I guess Im randomly asking but does anybody know of a tool to log back into an Instagram account..? I somehow forgot my password. I love any help you can give me.

Yash Moharil easy way to remember thanks!

Yash Moharil for non polar ?

Thanks man !!

what the fuck does that mean

@@kiankelly6442 solvent types , polar protic solvent and polar aprotic solvent , google it to know better.

I agree.

bruH+

the way this is structured pains me

Are you taking o chem during summer? Brave

@@irynalebedyeva7900 Nope, I don't even know what that means😂 I'm giving my pre meds.

Yo bro !

@@sambhavmishra5423 yoo!

yes XD

NEET aspirants too.

Neet👍

NH2 stronger Nucleophile

Flourine is the smallest of the halides, so it will kinetically be the best nucleophile.. it will be small and able to get in to tight spots (also it's the most electronegative of the halides - so that helps out reactivity wise). The problem is when you have protic solvents, you have the possibility (and likelihood) of the fluorine ion becoming protonated to form HF (which a weak acid - this is a situation where the electronegativity of fluorine sort of undermines itself). With protic solvents, Iodide is the best nucleophile because its the weakest base. It's not going to donate a pair of electrons (lewis definition of a base) to the partially positive protic hydrogen on the solvent. -OR- it's not going to receive a proton from the solvent (brownstead lowry definition of a base... same difference) This would result in HI forming. Hydroiodic acid is a very strong acid, so in terms of acid-base reactions this is not favorable, mostly likely HI would be a WAY stronger acid then the solvent. So in the circumstance of polar protic solvents, the big bulky iodide ion (which normally is not a good nucleophile kinetic-wise) becomes a better nucleophile then fluoride, because at least iodide will BE ABLE to act as a nucleophile, it will still exist as an ion... fluoride won't be an ion anymore, it will be tied up as HF (a weak acid)

And HF is also stabilised by H-Bonds I presume?

c+ are overall not stable what re you trying to say?

Its because HBr is a stronger acid than a carbon conpound with bromine. When there is a loss of proton from carbon adjacent to Bromine, Bromine does backbonding and makes it a bit more stable but Br- is much more stable in solution. Well the reaction is feasible only if a weaker acid/base is formed in product. And carbon with Bromine is less acidic than HBr.

Mobark Alwahishi LG have high electronegativity or positive charge. LG is happy with electron.

Through the door.

@@dhawalarora7544 😂😂😂 why would you do that

Carbon is tetravalent. It can't have 5 bonds so when the nucleophile attaches, the tendency is for the carbon to kick out the atom that is relatively stable on its own -- a good leaving group (usually halide).

The stronger the acid, weaker it's conjugate base , More weaker the conjugate base , Better the leaving group is and vice versa