Match each equation with the acid-base definition that best describes how the reaction can be viewed as involving acids and bases 1. BrF2 (s) + KF (s) 2. BrF4 (n BrF3 soln) + K+ (in BcF3 soln) Choose: 1. Na2O (s) + SiO2 (s) 2. Na2SiO3 (s) Choose: 1. PtCl4 (soln) + APH3 (soln) 2. [PA(PH3)2]+ (soln) Choose: 1. 2Na (s) + H2O (l) 2. 2Na+ (aq) + 2OH- (aq) + H2 (g) Choose:
The Correct Answer and Explanation is:
Here’s the breakdown of how these reactions can be viewed from the acid-base perspective, focusing on different acid-base theories such as Lewis, Brønsted-Lowry, and others:
1. BrF2 (s) + KF (s)
Theory: Lewis Acid-Base
Explanation: In this reaction, BrF2 can be considered a Lewis acid because it can accept a pair of electrons from the fluoride ion (F-) in KF, which acts as a Lewis base. The fluoride ion donates its lone pair to form a bond, making this a Lewis acid-base interaction.
2. BrF4 (in BrF3 solution) + K+ (in BcF3 solution)
Theory: Lewis Acid-Base
Explanation: BrF4 is a Lewis acid because it can accept electrons from the fluoride ion in BrF3, which is a Lewis base. Similarly, K+ is a Lewis acid because it can accept electron pairs from the solvent molecules or other electron donors. This reaction showcases electron pair donation and acceptance.
3. Na2O (s) + SiO2 (s)
Theory: Lewis Acid-Base
Explanation: This reaction involves the formation of Na2SiO3, where Na2O (which acts as a Lewis base) donates electron pairs to SiO2 (which acts as a Lewis acid). The SiO2 molecule has a central silicon atom that can accept electron pairs, thus forming a bond with the oxygen from Na2O.
4. Na2SiO3 (s)
Theory: Lewis Acid-Base
Explanation: Na2SiO3, or sodium metasilicate, contains the SiO3²⁻ ion, which can act as a Lewis base, donating electron pairs. In reactions, it can act as a Lewis base when interacting with other Lewis acids.
5. PtCl4 (solution) + APH3 (solution)
Theory: Lewis Acid-Base
Explanation: In this reaction, PtCl4 is a Lewis acid because the platinum (Pt) ion can accept electron pairs from the phosphorus in APH3 (where APH3 is a Lewis base). The phosphorus atom donates a lone pair of electrons to the platinum ion, facilitating the formation of a new complex.
6. [PA(PH3)2]+ (solution)
Theory: Lewis Acid-Base
Explanation: The complex [PA(PH3)2]+ contains the PA ion (phosphorus atom), which can act as a Lewis acid because it accepts electron pairs from the PH3 ligands, which are acting as Lewis bases.
7. 2Na (s) + H2O (l)
Theory: Brønsted-Lowry Acid-Base
Explanation: In this reaction, sodium metal (Na) reacts with water to form sodium hydroxide (NaOH) and hydrogen gas. Sodium metal donates an electron (acting as a Brønsted-Lowry base) to the hydrogen ion (H+) in water, which acts as a Brønsted-Lowry acid. The hydroxide ion (OH-) is formed in the process.
8. 2Na+ (aq) + 2OH- (aq) + H2 (g)
Theory: Brønsted-Lowry Acid-Base
Explanation: In this reaction, Na+ and OH- are the products from the reaction of Na with water. The Na+ ions can accept a lone pair from water molecules, and the OH- ion can act as a Brønsted-Lowry base by accepting a proton (H+). The resulting hydrogen gas (H2) shows the production of a Brønsted-Lowry acid (H+ from H2O) and base (OH-).
In summary, these reactions primarily illustrate interactions between acids and bases from the Lewis acid-base and Brønsted-Lowry acid-base perspectives. Lewis acid-base theory focuses on electron pair donation and acceptance, while Brønsted-Lowry theory emphasizes proton transfer.
