   Chapter 21, Problem 5PS

Chapter
Section
Textbook Problem

Give examples of two basic oxides. Write equations illustrating the formation of each oxide from its component elements. Write another chemical equation that illustrates the basic character of each oxide.

Interpretation Introduction

Interpretation: Examples for two basic oxides has to be given. Equations illustrating the formation of each oxide from its component elements should be written.

Concept introduction: Oxides are formed by reaction of metal with oxygen. If metal belongs to group 2A of periodic table, then the general reaction of formation of oxide is:

M(s)+O2(g)MO(s)

Here, metal has +2 oxidation number and oxide ion has 2 oxidation number.

A basic oxide is an oxide that shows basic properties in solution. Basic oxides on reaction with water form a base. This is a characteristic property of basic oxides and thus illustrates its basic behavior. Basic oxides are mostly oxides of group 1A and 2A elements. Thus, basic oxides are generally oxides of metals and they react with water to form alkaline solutions of metal hydroxides. The general reaction of a metal oxide with water is as follows:

MO(s)+H2O(l)M(OH)2(aq)

Explanation

Basic oxides are generally oxides of metals of group 1A and 2A metals. The two examples of basic oxide are CaO and MgO. Both calcium and magnesium belongs to group 2A of periodic table and have  highest oxidation number of +2. Oxide ion has oxidation number of 2. Thus, the formula of the product is CaO and MgO respectively.

Thus, the balanced chemical equation is:

• 2Ca(s)+O2(g)2CaO(s)
• 2Mg(s)+O2(g)2MgO(s)

The stoichiometric coefficients are multiplied with the compounds in the chemical equation to have equal number of atoms on both sides of the equation. Since oxygen is present as O2 in the reaction, hence the stoichiometric coefficient of metal oxide is 2 due to which metal also has a stoichiometric coefficient of 2

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