Trimethylamine, (CH3)3 N:, reacts readily with diborane, B2 H6. The diborane dissociates to two

step 1 Question is trimethylamine react readily with the diborate and diborate dissociate into 2 BS3 fr

Trimethylamine, (CH3)3 N:, reacts readily with diborane, B2...

Trimethylamine, $\left(\mathrm{CH}_{3}\right)_{3} \mathrm{~N}:$, reacts readily with diborane, $\mathrm{B}_{2} \mathrm{H}_{6}$. The diborane dissociates to two $\mathrm{BH}_{3}$ fragments, each of which can react with trimethylamine to form a complex, $\left(\mathrm{CH}_{3}\right)_{3} \mathrm{~N}: \mathrm{B} \mathrm{H}_{3}$. Write an equation for this reaction and interpret it in terms of Lewis acid-base theory.

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Key Concepts

Electron Deficiency and Adduct Formation

Certain molecules, particularly those with elements like boron, are electron deficient and act as Lewis acids. Their ability to accept electron pairs makes them prone to forming adducts with electron-rich species. The formation of these adducts, also known as complexes, is driven by the stabilization achieved when the electron-deficient center is saturated by donated electrons.

Coordinate (Dative) Covalent Bond Formation

Coordinate covalent bond formation involves one atom (typically a Lewis base) donating an electron pair to an electron-deficient atom (typically a Lewis acid) to form a bonding interaction. This bond is initially formed by the complete donation of an electron pair from the donor to the acceptor, stabilizing both species in a complex.

Lewis Acid?Base Theory

Lewis acid?base theory is a fundamental concept in chemistry where a Lewis acid is defined as an electron pair acceptor, and a Lewis base is an electron pair donor. This theory broadens the notion of acids and bases beyond proton transfer to include any species that can accept or donate an electron pair, forming a coordinate covalent bond.

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