Which is the stronger base in each pair?
a. Ammonia or ethylamine
b.Triethylamine or pyridine

Question

Which is the stronger base in each pair?

a. Ammonia or ethylamine

b.Triethylamine or pyridine

Accepted Answer

Welcome everybody. Our next problem says, identify the stronger base among the pairs of compounds given below. And there's Roman number one ana line or Trolamine and Roman Emeril too, but amine or ammonia. And then we have four different answer choices A through D with different combinations of these two. So we'll look at each of them once we look at our compounds and figure out which is the stronger base. So when we're talking about a means which is what we have here, there's a way to figure out which is the stronger base. Recall that amines are a base because the lone pair on the nitrogen can bond with a proton. So depending on what's bonded to that nitrogen in our amine, it affects how likely those electrons are to be shared. So there's a, an order of baity to am means. So the most basic amines are non aromatic. So it means with an alkyl chain to a added to them, these are more basic. So I'm gonna put a little greater than sign than ammonia. So NH three, which is more basic than aromatic means. And that's due to that stabilization of the lone pair with the aromatic ring that's attached. So with that in mind, let's look at our compounds. So for number one, the first one is annale and anneline is a benzene ring with an NH two group as a substituent. So we'll just try that. So this is obviously an aromatic, I mean, and then our second compound is trolamine. The tri tells us we have three substituents on our nitrogen. It's a tertiary amine and it's symmetrical because they all it's three of the same thing and it's propol. So three carbons on those substituents. So we have a nitrogen molecule or nitrogen atom, excuse me with 33 carbon chains attached to it. So 123, one, 23, 123. And then of course, it still has a lone pair remaining on it that allows it to act as a base. But this is a non aromatic amine. So the tropy lamine would be the more basic of the two because anneline has a benzene ring on it. So this is a non aromatic, I mean, so that has to do with number one. So we can actually look at our answer choices and perhaps eliminate some choice. A says that anneline is the more basic. So we can eliminate that since that's not the case choice. B says that for number one tropy amine is more basic choice. C says that for number one annale is more basic. So we can eliminate that and choice D says that for number one, tropy lamine is more basic. So let's look at number two, it says butty amine or ammonia. Well, we know that ammonia is in the middle here. So we just have to look at Butty amine. So that beta would tell us it's a four carbon chain attached to our nitrogen, just one chain. So it's a primary mean with NH two and then just four carbons attached to it. So let's draw that four carbon chain 1234. So this is a non aromatic amine. So it is therefore more basic than ammonia. So butty amine is our answer for number two. So that gives brings us to choice B as our answer which has bet amine for number two and not choice D which has ammonia for number two. So once again, the stronger base among pairs of the compounds below is choice B. Number one tropy lamine and number two, butty amine. See you in the next video.

Which is the stronger base in each pair?
a. Ammonia or ethylamine
b.Triethylamine or pyridine

Verified video answer for a similar problem:

Key Concepts

Basicity

Amine Structure

Resonance and Electron Delocalization

Which is the stronger base in each pair?a. Ammonia or ethylamineb.Triethylamine or pyridine

Verified video answer for a similar problem:

Key Concepts

Basicity

Amine Structure

Resonance and Electron Delocalization

Which is the stronger base in each pair?
a. Ammonia or ethylamine
b.Triethylamine or pyridine