The reaction between a hydride ion and water, in terms of Bronsted acid–base theory is to be described and its classification as a redox reaction is to be verified alongwith the identification of reducing and oxidizing agents. Concept introduction: According to the Bronsted–Lowry theory, a substance with the ability to donate a proton, acts as an acid. The acid is named as a Bronsted Acid. A Bronsted base is a substance that accepts a proton and forms its conjugate acid. Redox reactions are those in which both oxidation and reduction of the species takes place, simultaneously. Loss of electrons leads to oxidation and gain of electrons leads to reduction An element or compound that donates an electron to another chemical species in a redox chemical reaction is known as reductant or reducing agent. Reducing agent is said to have been oxidized, since it is losing electrons. An oxidizing agent also known as oxidant, gains electrons and is reduced in a chemical reaction. Asoxidizing agentgain electrons and be reduced, it is normally in one of its higher possible oxidation states.
The reaction between a hydride ion and water, in terms of Bronsted acid–base theory is to be described and its classification as a redox reaction is to be verified alongwith the identification of reducing and oxidizing agents. Concept introduction: According to the Bronsted–Lowry theory, a substance with the ability to donate a proton, acts as an acid. The acid is named as a Bronsted Acid. A Bronsted base is a substance that accepts a proton and forms its conjugate acid. Redox reactions are those in which both oxidation and reduction of the species takes place, simultaneously. Loss of electrons leads to oxidation and gain of electrons leads to reduction An element or compound that donates an electron to another chemical species in a redox chemical reaction is known as reductant or reducing agent. Reducing agent is said to have been oxidized, since it is losing electrons. An oxidizing agent also known as oxidant, gains electrons and is reduced in a chemical reaction. Asoxidizing agentgain electrons and be reduced, it is normally in one of its higher possible oxidation states.
Solution Summary: The author describes the reaction between a hydride ion and water in terms of the Bronsted acid–base theory and the identification of reducing and oxidizing agents.
Definition Definition Chemical reactions involving both oxidation and reduction processes. During a redox reaction, electron transfer takes place in such a way that one chemical compound gets reduced and the other gets oxidized.
Chapter 16, Problem 139AP
Interpretation Introduction
Interpretation:
The reaction between a hydride ion and water, in terms of Bronsted acid–base theory is to be described and its classification as a redox reaction is to be verified alongwith the identification of reducing and oxidizing agents.
Concept introduction:
According to the Bronsted–Lowry theory, a substance with the ability to donate a proton, acts as an acid. The acid is named as a Bronsted Acid.
A Bronsted base is a substance that accepts a proton and forms its conjugate acid.
Redox reactions are those in which both oxidation and reduction of the species takes place, simultaneously.
Loss of electrons leads to oxidation and gain of electrons leads to reduction
An element or compound that donates an electron to another chemical species in a redox chemical reaction is known as reductant or reducing agent. Reducing agent is said to have been oxidized, since it is losing electrons.
An oxidizing agent also known as oxidant, gains electrons and is reduced in a chemical reaction. Asoxidizing agentgain electrons and be reduced, it is normally in one of its higher possible oxidation states.
(a) Write down an equation for the reaction of ammonia solution (NH3) and hydrogenbromide (HBr) and explain the reaction in terms of the Brønsted theory of acids andbases (b) Write down an equation for the reaction of aluminium chloride (AlCl3) and chlorideions (Cl-) in the absence of water and explain the reaction in terms of the Lewis theory of acids and bases
Identify each of the following oxides as an acid or baseanhydride. Write the chemical formula and give the nameof the acid or base formed upon reaction with water.(a) MgO (b) Cl2O
(c) SO3 (d) Cs2O
calculate the pH of the following solution;
(a)2.8 × 10–⁴M Ba (OH)2
(b) 5.2 × 10–⁴M HNO3·
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