Nh3 + H20 -> Nh4+ + Oh

[atlanta213]

Why ammonia is lewis base here?

NH3 + H20 -> NH4+ + OH

I see ammonia is accepting proton.

It should be bronsted lowery base.


correct me if i am wrong.

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[condoleezarice]

I believe it would be both. It is donating electrons to the H2O proton, thus a lewis base.

 

[doc3232]

Nah
That reaction won't happen.
OH- is a stronger base than NH3.
None of the common reagents we use can deprotonate water.
Only:
HC(triple bond)-
NH2-
LDA
Grignards
And a few more can deprotonate water

 

[alanan84]

Per Wikipedia:
A Lewis base is any molecule or ion that can form a new coordinate covalent bond, by donating a pair of electrons, named after the American chemist Gilbert Lewis. The term base is ambiguous. This is one interpretation. To put it another way, any molecule with an electron lone pair in a bonding orbital may act as a Lewis base, as it is capable of accepting an ion with a single positive charge.

So that would be why NH3 is a lewis base. It has a lone electron pair that forms the covalent bond with the proton to make NH4

 

[atlanta213]

Nah
That reaction won't happen.
OH- is a stronger base than NH3.
None of the common reagents we use can deprotonate water.
Only:
HC(triple bond)-
NH2-
LDA
Grignards
And a few more can deprotonate water

it is one of kaplan question.

 

[atlanta213]

This is confusing. According to kaplan, NH3 accpets a proton from water to become NH4+ while H2O gives up this proton to become OH-.

By their way, ammonia should be bronsted lowery base.

 

[alanan84]

Nah
That reaction won't happen.
OH- is a stronger base than NH3.
None of the common reagents we use can deprotonate water.
Only:
HC(triple bond)-
NH2-
LDA
Grignards
And a few more can deprotonate water

Regardless of whether the reaction would "actually" happen, it is a common reaction to illustrate acid base chemistry and could certainly show up on the DAT.

Is one of the answer choices a bronsted lowery base?

 

[PooyaH]

This is confusing. According to kaplan, NH3 accpets a proton from water to become NH4+ while H2O gives up this proton to become OH-.

By their way, ammonia should be bronsted lowery base.

NH3 is a LB and a BB! It's accepting a proton (H)

 

[atlanta213]

Regardless of whether the reaction would "actually" happen, it is a common reaction to illustrate acid base chemistry and could certainly show up on the DAT.

Is one of the answer choices a bronsted lowery base?

nah.. not on the choices.

 

[doc3232]

Regardless of whether the reaction would "actually" happen, it is a common reaction to illustrate acid base chemistry and could certainly show up on the DAT.

Is one of the answer choices a bronsted lowery base?

You can use it as an example here for the sake of learning but it wouldn't be fair to be put on the DAT.
It just can't happen.

 

[alanan84]

NH3 is a LB and a BB! It's accepting a proton (H)

Yeah it's definitely both. I guess the confusing part is by the equation, the bronsted lowery is much more evident. I guess since that wasn't one of the answer choices then you would choose the lewis base but their expanation doesn't correlate with the answer if it talks about a transfer of protons.

 

[PooyaH]

Yeah it's definitely both. I guess the confusing part is by the equation, the bronsted lowery is much more evident. I guess since that wasn't one of the answer choices then you would choose the lewis base but their expanation doesn't correlate with the answer if it talks about a transfer of protons.

Most compounds or atoms that receive or donate electrons are LB and LA respectively...whenever a proton (H) is involved makes them also BB and BA

 

[yakuza]

If you search lewis base, ammonia is usually the main basic example they give

 

[appleonius]

Most compounds or atoms that receive or donate electrons are LB and LA respectively...

that's backwards.

 

[condoleezarice]

If you look at this from an organic chemistry perspective. You would be drawing an arrow from the lone pair on NH3 to the proton on H20. The NH3 is donating electrons, the definition of a lewis base. It's as simple as that.

 

[doc toothache]

Nah
That reaction won't happen.
OH- is a stronger base than NH3.
None of the common reagents we use can deprotonate water.
Only:
HC(triple bond)-
NH2-
LDA
Grignards
And a few more can deprotonate water

http://scifun.chem.wisc.edu/chemweek/pdf/Ammonia.pdf

 

[BAdriano]

I believe it would be both. It is donating electrons to the H2O proton, thus a lewis base.

If you see, the both of compounds have pair of electron... so why do NH3 donate them instead of water?

 

[FeralisExtremum]

If you see, the both of compounds have pair of electron... so why do NH3 donate them instead of water?

One way to look at it...whichever atom donates its electron pair is going to end up with a positive charge on it. In terms of stability, you want the positive charge on the less electronegative atom - in this case N rather than O.

 

[DAT Destroyer]

Why ammonia is lewis base here?

NH3 + H20 -> NH4+ + OH

I see ammonia is accepting proton.

It should be bronsted lowery base.




correct me if i am wrong.

First draw in the lone electron pair on the Nitrogen atom in NH3.......draw an arrow from these electrons to the Hydrogen on water. If done correctly, you will note that NH3 donates electrons.....and is a Lewis base......The Hydrogen atom accepts the electrons,,,,,and is the Lewis acid. NH3 is also Bronsted Base.....since it is accepting a proton !

Hope this helps.

Dr. Romano