Which is the stronger base, \(\left(\mathrm{CH}_{3}\right)_{3} \mathrm{N}\) or \(\mathrm{H}_{2} \mathrm{BO}_{3}^{-} ?\)

Basicity is a fundamental concept in acid-base chemistry, representing a substance's propensity to accept protons (H+ ions). Imagine a molecule eagerly waiting to grab a passing H+; that eagerness is its basicity. The more willing it is to snap up a proton, the stronger a base it is considered. A molecule's basicity can depend on various factors, such as charge, surrounding atoms, and the structure of the molecule itself.

For instance, bases that carry a negative charge are generally stronger than their neutral counterparts. This is because the negative charge indicates a surplus of electrons that are readily available to form a bond with the incoming proton. Structural aspects like the size of the molecule and the presence of electron-donating groups also impact how readily a base will accept a proton.

Delving into the Brønsted-Lowry theory, we shift our focus to a more dynamic view of acids and bases. This theory presents a base as not merely a substance sitting idly by but as an active participant in the dance of proton exchange. In this framework, an acid is a proton donor and a base is a proton acceptor. They come together, exchange partners, and part ways, now transformed as conjugate pairs.

What's interesting is that the Brønsted-Lowry theory extends the definition of acids and bases beyond just those substances which dissolve in water to encompass a broader range of chemical species, including molecules that accept protons in non-aqueous environments. This emphasizes not just the features of the molecule but also the importance of context in acid-base reactions.

In the intricate ballet of acid-base reactions, every base has a partner called a conjugate acid, and likewise, every acid has a corresponding conjugate base. After an acid donates its proton, what remains is the conjugate base. It's like the aftermath of a grand event; the acid has given away something precious, and the remaining part, the conjugate base, reflects that change.

Conjugate bases are interesting because their strength is inversely related to their corresponding acid's strength. Strong acids leave behind weak conjugate bases, while weak acids tend to have stronger conjugate bases. This inverse relationship is crucial when predicting the outcomes of chemical reactions and helps in understanding various chemical equilibria.

Electronegativity is like the measure of how much atoms hanker for electrons. It's a concept that helps us understand a variety of chemical properties, including basicity. Atoms with higher electronegativity are more adept at holding onto their electrons and are less inclined to be generous with them in forming new bonds.

When it comes to basicity, the higher the electronegativity of the atom holding the charge in a base, the lower the basicity tends to be. An atom that isn't so keen on sharing its electrons won't be as good at welcoming a proton. As such, in the competition for protons, bases composed of less electronegative atoms often have the upper hand.

Amines are compounds that feature nitrogen atoms which possess a lone pair of electrons, making them prime candidates for forming bonds with protons. The basicity of amines can be quite the conundrum as it is influenced by a host of factors such as the electronic properties of substituents attached to the nitrogen.

Substituents like the methyl groups in trimethylamine help to push electrons towards the nitrogen, making it more of a base. It's akin to giving someone a pair of boxing gloves; they become better fighters. The basicity increases because the nitrogen becomes more ready and willing to bond with a proton. However, every amine's story is unique, and predicting their basicity requires considering their molecular context in detail.