Decide whether each of the following substances should be...

Decide whether each of the following substances should be classified as a Lewis acid or a Lewis base. (a) $\mathrm{BCl}_{3}$ (Hint: Draw the electron dot structure.) (b) $\mathrm{H}_{2} \mathrm{NNH}_{2}$, hydrazine (Hint: Draw the electron dot structure.) (c) the reactants in $\mathrm{Ag}^{+}+2 \mathrm{NH}_{3} \rightleftharpoons\left[\mathrm{Ag}\left(\mathrm{NH}_{3}\right)_{2}\right]^{+}$

Decide whether each of the following substances should be classified as a Lewis acid or a Lewis base.
(a) $\mathrm{BCl}_{3}$ (Hint: Draw the electron dot structure.)
(b) $\mathrm{H}_{2} \mathrm{NNH}_{2}$, hydrazine (Hint: Draw the electron dot structure.)
(c) the reactants in $\mathrm{Ag}^{+}+2 \mathrm{NH}_{3} \rightleftharpoons\left[\mathrm{Ag}\left(\mathrm{NH}_{3}\right)_{2}\right]^{+}$

Key Concepts

Coordinate Covalent Bonding

Coordinate covalent bonding, also known as dative bonding, occurs when both electrons in a shared pair come from the same atom. This type of bond is a fundamental part of many Lewis acid-base reactions where an electron-rich species (Lewis base) donates an electron pair to an electron-deficient species (Lewis acid), forming a stable complex.

Electron Dot Structure

The electron dot structure is a diagrammatic method used to represent the valence electrons of atoms within a molecule. This representation is crucial for identifying sites of electron deficiency or surplus, which in turn helps in determining the potential of a substance to act as either a Lewis acid or a Lewis base.

Lewis Base

A Lewis base is defined as a chemical species that can donate an electron pair to form a covalent bond with an electron pair acceptor. Unlike the proton-accepting definition present in Bronsted–Lowry theory, this definition is centered on the availability of electrons and includes many molecules with lone pairs that can be donated to electrophilic centers.

Lewis Acid

A Lewis acid is a chemical species that can accept an electron pair in order to form a new chemical bond. This concept goes beyond the proton-donating definition found in Bronsted–Lowry theory, and includes many compounds, such as electron-deficient molecules or metal ions, that are capable of accepting electron pairs from donors.

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