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Chapter 15: Problem 105

The oxide ion, \(\mathrm{O}^{2-}\), present in sodium oxide \(\left(\mathrm{Na}_{2} \mathrm{O}\right)\) reacts violently with water to produce a highly basic solution. The hydride ion, \(\mathrm{H}^{-}\), in sodium hydride (NaH) does the same. (a) Write a balanced total ionic equation for the reaction of sodium oxide with water. (b) In terms of the Bronsted-Lowry definition, how are oxide and hydride similar? (c) What is it about the hydride and oxide ions that allow them to do what they do in water?

Short Answer

Expert verified
(a) The balanced total ionic equation for the reaction of sodium oxide with water is: \(O^{2-} + 2H^+ \rightarrow 2OH^-\) (b) Oxide and hydride ions are similar because they both act as Bronsted-Lowry bases, as they can accept protons (H+ ions). (c) Hydride and oxide ions are highly reactive with water due to their high electron density and the presence of lone pairs of electrons, which enable them to easily act as Lewis and Bronsted-Lowry bases, accepting H+ ions from water molecules and producing highly basic solutions.

Step by step solution

01

(a) Write a balanced total ionic equation for the reaction of sodium oxide with water.

First, we need to write the chemical reaction between sodium oxide (Na2O) and water (H2O): Na2O + H2O -> 2NaOH Now let's break this equation down into its ionic components: 2Na+ + O2- + 2H+ + 2OH- -> 2Na+ + 2OH- Finally, we can cancel out the spectator ions (2Na+) to get the balanced total ionic equation for the reaction of sodium oxide with water: O2- + 2H+ -> 2OH-
02

(b) In terms of the Bronsted-Lowry definition, how are oxide and hydride similar?

According to the Bronsted-Lowry definition, an acid is a substance that can donate a proton (H+), and a base is a substance that can accept a proton. Oxide ions (O2-) can accept two protons, as seen in the reaction of sodium oxide with water, where it accepts 2 H+ ions to form 2OH- ions. Similarly, hydride ions (H-) can accept a proton and form hydrogen gas, as seen in the reaction between sodium hydride and water: NaH + H2O -> Na+ + H2 + OH- In this reaction, the hydride ion (H-) accepts a proton (H+) from water: H- + H2O -> H2 + OH- So, oxide and hydride ions are similar in that they both act as Bronsted-Lowry bases because they can accept protons (H+ ions).
03

(c) What is it about the hydride and oxide ions that allow them to do what they do in water?

Hydride (H-) and oxide (O2-) ions are highly reactive with water because of their high electron density and the presence of lone pairs of electrons on their respective atoms. These lone pairs make it easy for them to act as Lewis bases, which in turn makes them good Bronsted-Lowry bases as they can easily accept H+ ions from the water molecules. Their high electron density also stabilizes the OH- ions that are produced in the reaction, making the solutions highly basic.

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