Question

Acids and bases: definitions ut of Consider the following reactions: (a) Ca(OH)2 + 2 HCI - CaCl + 2 H2O (b) CaH2 + 2 H2O + Ca(OH)2 + 2 H2 (c) BF3 + F - BF4 Match with the definitions that apply for the substances indicated. Note: In a given reaction, the same definition must apply for both the acid and base for it to hold true, Ca(OH)2 in reaction (a) Arrhenius, Bransted-Lowry, and Lewis base HCI Arrhenius, Bransted-Lowry, and Lewis acid CaH2 Arrhenius, Brønsted-Lowry, and Lewis base H2O in reaction (b) Choose... BF3 Arrhenius, Bransted-Lowry, and Lewis acid Arrhenius, Brønsted-Lowry, and Lewis base

Answer 1

H2O IN reaction (b)--Ionic Bonding: no distribution of electron wave function

- Bronsted Basic because they will react with proton

- Lewis Basic because they can be ligands

CaH2 + 2H2O -> 2H2 + Ca(OH)2

1.***********a Lewis acid is an electron-pair acceptor. A Lewis base is any substance, such as the OH^- ion, that can donate a pair of nonbonding electrons. ... In the Lewis theory, an acid is any ion or molecule that can accept a pair of nonbonding valence electrons.

2. that acids are substances that dissociate in water to yield electrically charged atoms or molecules, called ions, one of which is a hydrogen ion (H⁺), and that bases ionize in water to yield hydroxide ions (OH⁻)

3. Brønsted-Lowry acid is any substance (molecule or ion) that can donate a hydrogen ion (H+).A Brønsted-Lowry base is any species that can accept a hydrogen ion (H+).
Ca(OH)2 Her H₂o BE – Arrhenius base - Awhenius aid and Bronsted acid - Lewis base - Lewis freid due to accepter of lone pair - Lewis base donar of et pair f k you very much PAGE 1