Skip to main content
Ch.16 - Acid-Base Equilibria
Brown - Chemistry: The Central Science 14th Edition
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Non è quello che usi tu?Cambia libro di testo
Tutti i libri di testoBrown 14th EditionCh.16 - Acid-Base EquilibriaProblema 95
Capitolo 16, Problema 95

Identify the Lewis acid and Lewis base among the reactants in each of the following reactions:
(a) Fe(ClO4)3(s) + 6 H2O(l) ⇌ [Fe(H2O)6]3+(aq) + 3 ClO4-(aq)
(b) CN-(aq) + H2O(l) ⇌ HCN(aq) + OH-(aq)
(c) (CH3)3N(g) + BF3(g) ⇌ (CH3)NBF3(s)
(d) HIO(lq) + NH2-(lq) ⇌ NH3(lq) + IO-(lq) (lq denotes liquid ammonia as solvent)

Guida verificata passo dopo passo
1
Identify the Lewis acid and Lewis base by understanding their definitions: A Lewis acid is an electron pair acceptor, and a Lewis base is an electron pair donor.
Examine the reactants: HIO and NH2-. Consider which species can donate an electron pair and which can accept an electron pair.
Recognize that NH2- has a lone pair of electrons that it can donate, making it a potential Lewis base.
Consider HIO, which can accept an electron pair to form a bond, making it a potential Lewis acid.
Conclude that in the reaction, NH2- acts as the Lewis base (electron pair donor) and HIO acts as the Lewis acid (electron pair acceptor).

Risposta video verificata per un problema simile:

Questa soluzione video è stata consigliata dai nostri tutor come utile per risolvere questo problema.
Durata del video:
2m

Concetti chiave

Ecco i concetti essenziali che devi comprendere per rispondere correttamente alla domanda.

Lewis Acids and Bases

Lewis acids are substances that can accept an electron pair, while Lewis bases are those that can donate an electron pair. This definition expands the concept of acids and bases beyond protons (H+) to include electron pair interactions, making it applicable to a wider range of chemical reactions.
Video consigliato:
Percorso guidato
05:04
Lewis Acids and Bases

Electron Pair Donation and Acceptance

In a Lewis acid-base reaction, the Lewis base donates an electron pair to the Lewis acid, forming a coordinate covalent bond. Understanding this interaction is crucial for identifying which reactant acts as the acid and which as the base in a given reaction.
Video consigliato:
Percorso guidato
00:47
Valence Shell Electron Pair Repulsion Theory

Solvent Effects

The solvent can influence the behavior of acids and bases in a reaction. In this case, liquid ammonia serves as a solvent, which can stabilize certain ions and affect the reactivity of the reactants, thereby impacting the identification of Lewis acids and bases in the reaction.
Video consigliato:
Percorso guidato
02:31
Photoelectric Effect
Pratica correlata
Domanda del libro di testo
The fluoride ion reacts with water to produce HF. (c) Is fluoride acting as a Lewis acid or as a Lewis base when reacting with water?
562
views
Domanda del libro di testo

Indicate whether each of the following statements is true or false. For each statement that is false, correct the statement to make it true. (a) Acid strength in a series of H¬A molecules increases with increasing size of A. (b) For acids of the same general structure but differing electronegativities of the central atoms, acid strength decreases with increasing electronegativity of the central atom. (c) The strongest acid known is HF because fluorine is the most electronegative element.

633
views
Domanda del libro di testo

Identify the Lewis acid and Lewis base in each of the following reactions:

(a) HNO2(aq) + OH-(aq) ⇌ NO2-(aq) + H2O(l)

(b) FeBr3(s) + Br-(aq) ⇌ FeBr4-(aq)

(c) Zn2+(aq) + 4 NH3(aq) ⇌ Zn(NH3)42+(aq)

(d) SO2(g) + H2O(l) ⇌ H2SO3(aq)

1152
views
Domanda del libro di testo

Which member of each pair produces the more acidic aqueous solution: (a) ZnBr2 or CdCl2 (b) CuCl or Cu(NO3)2 (c) Ca(NO3)2 or NiBr2

472
views