Identify the Lewis acid and the Lewis base in each reaction. (a) I2( s)+I^-(aq) →I3^-(aq) (b) SO

step 1 Let's identify the lewis acid and base in each reaction. For A, we have I2 plus I minus to form

Identify the Lewis acid and the Lewis base in each reaction....

Identify the Lewis acid and the Lewis base in each reaction. (a) $\mathrm{I}_{2}(\mathrm{~s})+\mathrm{I}^{-}(\mathrm{aq}) \rightarrow \mathrm{I}_{3}^{-}(\mathrm{aq})$ (b) $\mathrm{SO}_{2}(\mathrm{~g})+\mathrm{BF}_{3}(\mathrm{~g}) \rightarrow \mathrm{O}_{2} \mathrm{SBF}_{3}(\mathrm{~s})$ (c) $\mathrm{Au}^{+}(\mathrm{aq})+2 \mathrm{CN}^{-}(\mathrm{aq}) \rightarrow\left[\mathrm{Au}(\mathrm{CN})_{2}\right]^{-}(\mathrm{aq})$ (d) $\mathrm{CO}_{2}(\mathrm{~g})+\mathrm{H}_{2} \mathrm{O}(\ell) \rightarrow \mathrm{H}_{2} \mathrm{CO}_{3}($ aq $)$

Identify the Lewis acid and the Lewis base in each reaction.
(a) $\mathrm{I}_{2}(\mathrm{~s})+\mathrm{I}^{-}(\mathrm{aq}) \rightarrow \mathrm{I}_{3}^{-}(\mathrm{aq})$
(b) $\mathrm{SO}_{2}(\mathrm{~g})+\mathrm{BF}_{3}(\mathrm{~g}) \rightarrow \mathrm{O}_{2} \mathrm{SBF}_{3}(\mathrm{~s})$
(c) $\mathrm{Au}^{+}(\mathrm{aq})+2 \mathrm{CN}^{-}(\mathrm{aq}) \rightarrow\left[\mathrm{Au}(\mathrm{CN})_{2}\right]^{-}(\mathrm{aq})$
(d) $\mathrm{CO}_{2}(\mathrm{~g})+\mathrm{H}_{2} \mathrm{O}(\ell) \rightarrow \mathrm{H}_{2} \mathrm{CO}_{3}($ aq $)$

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Key Concepts

Coordination Chemistry

In many reactions involving Lewis acids and bases, complex species are formed through the coordination of electron pair donors (ligands) to an electron-deficient central atom. This process is a key aspect of coordination chemistry, which deals with the structures and bonding of such complexes.

Electron Pair Donation and Acceptance

Central to Lewis acid–base theory is the transfer of an electron pair from the base to the acid. This concept highlights the mechanism by which bonds are formed in Lewis acid-base reactions, where the Lewis base donates electrons to the Lewis acid, establishing a new chemical bond.

Lewis Acid

A Lewis acid is a chemical species that accepts an electron pair during a reaction. This characteristic makes it electron deficient, and these species typically have vacant orbitals ready to accommodate electron pairs donated by a Lewis base.

Lewis Base

A Lewis base is a chemical species that donates an electron pair to form a chemical bond. Such species contain lone pairs of electrons, making them electron rich, and are capable of interacting with electron-deficient species to form coordinate covalent bonds.

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