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By the Bransted-Lowry definition, acids are proton donors and bases are proton acceptors. By the Lewis definition, acids are electron-pair acceptors, and bases are electron-pair donors. For bases, the two definitions are equivalent such that all Lewis bases are Brensted- Lowry bases and vice versa. However, it is possible to have a Lewis acid that is not a Bronsted-Lowry acid. This is because Lewis acids include molecules and cations that have a vacant valence orbital, regardless of whether they have a proton to donate Common examples of Lewis acids (that are not Bransted-Lowry acids) are metal ions, such as AP and Cu²+ The following is an example of a Lewis acid-base reaction: Cu²+ +4NH3-Cu(NH₂), NH, donates the electron pair to Cu²+. Therefore, NH, is a Lewis base, and Cu²+ is a Lewis acid. Identify the Lewis acid in the following reaction: View Available Hint(s) Co²+ NH₁ Co(NH3)2+ Submit Part B Co*+(aq) +6NHs(aq) == Co[NH,)**(aq) Classify each of the following as a Lewis acid or a Lewis base. Drag the appropriate items to their respective bins. View Available Hint(s) OH NO₂ (CH₂)N SICU F M² Reset Help 18

By the Bransted-Lowry definition, acids are proton donors and bases are proton acceptors. By the Lewis definition, acids are electron-pair acceptors, and bases are electron-pair donors. For bases, the two definitions are equivalent such that all Lewis bases are Brensted- Lowry bases and vice versa. However, it is possible to have a Lewis acid that is not a Bronsted-Lowry acid. This is because Lewis acids include molecules and cations that have a vacant valence orbital, regardless of whether they have a proton to donate Common examples of Lewis acids (that are not Bransted-Lowry acids) are metal ions, such as AP and Cu²+ The following is an example of a Lewis acid-base reaction: Cu²+ +4NH3-Cu(NH₂), NH, donates the electron pair to Cu²+. Therefore, NH, is a Lewis base, and Cu²+ is a Lewis acid. Identify the Lewis acid in the following reaction: View Available Hint(s) Co²+ NH₁ Co(NH3)2+ Submit Part B Co*+(aq) +6NHs(aq) == Co[NH,)**(aq) Classify each of the following as a Lewis acid or a Lewis base. Drag the appropriate items to their respective bins. View Available Hint(s) OH NO₂ (CH₂)N SICU F M² Reset Help 18

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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By the Bransted-Lowry definition, acids are proton donors and bases are proton acceptors. By the Lewis definition, acids are electron-pair acceptors, and bases are electron-pair donors. For bases, the two definitions are equivalent such that all Lewis bases are Brensted- Lowry bases and vice versa. However, it is possible to have a Lewis acid that is not a Bronsted-Lowry acid. This is because Lewis acids include molecules and cations that have a vacant valence orbital, regardless of whether they have a proton to donate. Common examples of Lewis acids (that are not Bransted-Lowry acids) are metal ions, such as AP and Cu The following is an example of a Lewis acid-base reaction: Cu²+ +4NH, Cu(NH₂), NH, donates the electron pair to Cu²+, Therefore, NH, is a Lewis base, and Cu²+ is a Lewis acid. Identify the Lewis acid in the following reaction: View Available Hint(s) Co²+ NH₂ Co(NH3)²+ Submit Part B Classify each of the following as a Lewis acid or a Lewis base. Drag the appropriate items to their respective bins. View Available Hint(s) OH NO₂ (CH₂) N Co2+ (aq) +6NH, (aq) = Co(NH3)²(aq) SICU F Mu Reset Help 8 CO =
Transcribed Image Text:By the Bransted-Lowry definition, acids are proton donors and bases are proton acceptors. By the Lewis definition, acids are electron-pair acceptors, and bases are electron-pair donors. For bases, the two definitions are equivalent such that all Lewis bases are Brensted- Lowry bases and vice versa. However, it is possible to have a Lewis acid that is not a Bronsted-Lowry acid. This is because Lewis acids include molecules and cations that have a vacant valence orbital, regardless of whether they have a proton to donate. Common examples of Lewis acids (that are not Bransted-Lowry acids) are metal ions, such as AP and Cu The following is an example of a Lewis acid-base reaction: Cu²+ +4NH, Cu(NH₂), NH, donates the electron pair to Cu²+, Therefore, NH, is a Lewis base, and Cu²+ is a Lewis acid. Identify the Lewis acid in the following reaction: View Available Hint(s) Co²+ NH₂ Co(NH3)²+ Submit Part B Classify each of the following as a Lewis acid or a Lewis base. Drag the appropriate items to their respective bins. View Available Hint(s) OH NO₂ (CH₂) N Co2+ (aq) +6NH, (aq) = Co(NH3)²(aq) SICU F Mu Reset Help 8 CO =
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