Logout Open In App
Open In App
Warning: foreach() argument must be of type array|object, bool given in /var/www/html/web/app/themes/studypress-core-theme/template-parts/header/mobile-offcanvas.php on line 20

Chapter 7: Problem 96

Predict the products of the following oxides with water: \(\mathrm{Na}_{2} \mathrm{O}, \mathrm{BaO}, \mathrm{CO}_{2}, \mathrm{~N}_{2} \mathrm{O}_{5}, \mathrm{P}_{4} \mathrm{O}_{10}, \mathrm{SO}_{3} .\) Write an equation for each of the reactions. Specify whether the oxides are acidic, basic, or amphoteric.

Short Answer

Expert verified
Na2O and BaO are basic, forming NaOH and Ba(OH)2. CO2, N2O5, P4O10, and SO3 are acidic, forming acids (H2CO3, HNO3, H3PO4, H2SO4).

Step by step solution

Achieve better grades quicker with Premium

  • Unlimited AI interaction
  • Study offline
  • Say goodbye to ads
  • Export flashcards
Start your free trial Skip

Over 22 million students worldwide already upgrade their learning with Vaia!

01

Understanding Types of Oxides

Oxides can be classified as acidic, basic, or amphoteric based on their behavior with water. Acidic oxides react with water to form acids, basic oxides react with water to form bases, and amphoteric oxides can form either acids or bases depending on the conditions.
02

Predicting Products for Sodium Oxide (\(\mathrm{Na}_2\mathrm{O}\))

\(\mathrm{Na}_2\mathrm{O}\) is a basic oxide as it is an oxide of an alkali metal. When it reacts with water, it forms sodium hydroxide (a base):\[\mathrm{Na}_2\mathrm{O} + \mathrm{H}_2\mathrm{O} \rightarrow 2\mathrm{NaOH}\]
03

Predicting Products for Barium Oxide (\(\mathrm{BaO}\))

\(\mathrm{BaO}\) is also a basic oxide due to it being an oxide of an alkaline earth metal. It reacts with water to form barium hydroxide:\[\mathrm{BaO} + \mathrm{H}_2\mathrm{O} \rightarrow \mathrm{Ba(OH)}_2\]
04

Predicting Products for Carbon Dioxide (\(\mathrm{CO}_2\))

\(\mathrm{CO}_2\) is an acidic oxide. It reacts with water to form carbonic acid:\[\mathrm{CO}_2 + \mathrm{H}_2\mathrm{O} \rightarrow \mathrm{H}_2\mathrm{CO}_3\]
05

Predicting Products for Dinitrogen Pentoxide (\(\mathrm{N}_2\mathrm{O}_5\))

\(\mathrm{N}_2\mathrm{O}_5\) is an acidic oxide and reacts with water to produce nitric acid:\[\mathrm{N}_2\mathrm{O}_5 + \mathrm{H}_2\mathrm{O} \rightarrow 2\mathrm{HNO}_3\]
06

Predicting Products for Tetraphosphorus Decaoxide (\(\mathrm{P}_4\mathrm{O}_{10}\))

\(\mathrm{P}_4\mathrm{O}_{10}\) is acidic and reacts with water to form phosphoric acid:\[\mathrm{P}_4\mathrm{O}_{10} + 6\mathrm{H}_2\mathrm{O} \rightarrow 4\mathrm{H}_3\mathrm{PO}_4\]
07

Predicting Products for Sulfur Trioxide (\(\mathrm{SO}_3\))

\(\mathrm{SO}_3\) is another acidic oxide that combines with water to yield sulfuric acid:\[\mathrm{SO}_3 + \mathrm{H}_2\mathrm{O} \rightarrow \mathrm{H}_2\mathrm{SO}_4\]
08

Classifying Each Oxide

\(\mathrm{Na}_2\mathrm{O}\) and \(\mathrm{BaO}\) are basic oxides. \(\mathrm{CO}_2\), \(\mathrm{N}_2\mathrm{O}_5\), \(\mathrm{P}_4\mathrm{O}_{10}\), and \(\mathrm{SO}_3\) are acidic oxides.

Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Acidic Oxides
Acidic oxides are chemical compounds formed when nonmetals react with oxygen. These oxides show a unique characteristic – they react with water to produce acids. This behavior is typical because the nonmetals involved generally have a high electronegativity, which results in the oxide exhibiting acidic properties.

When an acidic oxide such as carbon dioxide (\(\mathrm{CO}_2\)in)comes into contact with water, it forms carbonic acid:\[\mathrm{CO}_2 + \mathrm{H}_2\mathrm{O} \rightarrow \mathrm{H}_2\mathrm{CO}_3\]

Similarly, sulfur trioxide (\(\mathrm{SO}_3\)in)reacts to form sulfuric acid:\[\mathrm{SO}_3 + \mathrm{H}_2\mathrm{O} \rightarrow \mathrm{H}_2\mathrm{SO}_4\]

Here are some examples of acidic oxides and their corresponding acids after reacting with water:
  • Carbon dioxide (\(\mathrm{CO}_2\)in) -> Carbonic acid
  • Sulfur trioxide (\(\mathrm{SO}_3\)in) -> Sulfuric acid
  • Dinitrogen pentoxide (\(\mathrm{N}_2\mathrm{O}_5\)in) -> Nitric acid
  • Tetraphosphorus decaoxide (\(\mathrm{P}_4\mathrm{O}_{10}\)in) -> Phosphoric acid
This behavior makes acidic oxides important in understanding chemical reactions in environmental science, such as acid rain formation.
Basic Oxides
Basic oxides are typically formed from metals, especially those from the alkali and alkaline earth metal groups. These oxides are noted for their ability to react with water to form bases, specifically hydroxides, which are substances that can accept hydrogen ions. This makes basic oxides fundamental in various chemical processes, particularly those involving neutralization reactions.

Take sodium oxide (\(\mathrm{Na}_2\mathrm{O}\)in) for example. It reacts with water to form sodium hydroxide:\[\mathrm{Na}_2\mathrm{O} + \mathrm{H}_2\mathrm{O} \rightarrow 2\mathrm{NaOH}\]

Barium oxide (\(\mathrm{BaO}\)in) follows a similar pattern, reacting with water to yield barium hydroxide:\[\mathrm{BaO} + \mathrm{H}_2\mathrm{O} \rightarrow \mathrm{Ba(OH)}_2\]

Here are some examples of basic oxides:
  • Sodium oxide (\(\mathrm{Na}_2\mathrm{O}\)in) -> Sodium hydroxide
  • Barium oxide (\(\mathrm{BaO}\)in) -> Barium hydroxide
These compounds are crucial in many industrial applications, for instance, in the manufacture of household cleaning products and in industries for removing sulfur impurities from fuels.
Amphoteric Oxides
Amphoteric oxides possess unique dual characteristics, meaning they can act as either acids or bases, depending on the surrounding environment or the reaction partner. This versatile behavior is particularly due to their ability to react with both acids and bases. While there were no amphoteric oxides mentioned in the original exercise, understanding them is crucial for a comprehensive grasp of chemical reaction behaviors.

Zinc oxide (\(\mathrm{ZnO}\)in) is a classic example of an amphoteric oxide. It can react with hydrochloric acid to form zinc chloride:\[\mathrm{ZnO} + 2\mathrm{HCl} \rightarrow \mathrm{ZnCl}_2 + \mathrm{H}_2\mathrm{O}\]

Conversely, it reacts with sodium hydroxide to produce sodium zincate:\[\mathrm{ZnO} + 2\mathrm{NaOH} + \mathrm{H}_2\mathrm{O} \rightarrow \mathrm{Na}_2\mathrm{Zn(OH)}_4\]

Other examples of amphoteric oxides include:
  • Aluminum oxide (\(\mathrm{Al}_2\mathrm{O}_3\)in)
  • Lead(II) oxide (\(\mathrm{PbO}\)in)
  • Chromium(III) oxide (\(\mathrm{Cr}_2\mathrm{O}_3\)in)
These oxides are particularly important in materials science and metallurgy, where they are involved in corrosion resistance and refining processes.

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

In general, the first ionization energy increases from left to right across a given period. Aluminum, however, has a lower first ionization energy than magnesium. Explain.

Group the following electron configurations in pairs that would represent elements with similar chemical properties: (a) \(1 s^{2} 2 s^{2} 2 p^{5}\) (d) \(1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{5}\) (b) \(1 s^{2} 2 s^{1}\) (e) \(1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 4 s^{1}\) (c) \(1 s^{2} 2 s^{2} 2 p^{6}\) (f) \(1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 4 s^{2} 3 d^{10} 4 p^{6}\)

The air in a manned spacecraft or submarine needs to be purified of exhaled carbon dioxide. Write equations for the reactions between carbon dioxide and (a) lithium oxide \(\left(\mathrm{Li}_{2} \mathrm{O}\right),(\mathrm{b})\) sodium peroxide \(\left(\mathrm{Na}_{2} \mathrm{O}_{2}\right),\) and (c) potassium superoxide \(\left(\mathrm{KO}_{2}\right)\)

The ionization energies of sodium (in \(\mathrm{kJ} / \mathrm{mol}\) ), starting with the first and ending with the eleventh, are 496 , 4562,6910,9543,13,354,16,613,20,117,25,496 \(28,932,141,362,159,075 .\) Plot the log of ionization energy \((y\) axis \()\) versus the number of ionization \((x\) axis); for example, \(\log 496\) is plotted versus 1 (labeled \(I E_{1}\), the first ionization energy), \(\log 4562\) is plotted versus 2 (labeled \(I E_{2},\) the second ionization energy \(),\) and so on. (a) Label \(I E_{1}\) through \(I E_{11}\) with the electrons in orbitals such as \(1 s, 2 s, 2 p,\) and \(3 s\) (b) What can you deduce about electron shells from the breaks in the curve?

Indicate which one of the two species in each of the following pairs is smaller: (a) \(\mathrm{Cl}\) or \(\mathrm{Cl}^{-},\) (b) Na or \(\mathrm{Na}^{+}\), (c) \(\mathrm{O}^{2-}\) or \(\mathrm{S}^{2-}\). (d) \(\mathrm{Mg}^{2+}\) or \(\mathrm{Al}^{3+}\) (e) \(\mathrm{Au}^{+}\) or \(\mathrm{Au}^{3+}\)
See all solutions

Recommended explanations on Chemistry Textbooks

Chemistry Branches

Read Explanation

The Earths Atmosphere

Read Explanation

Ionic and Molecular Compounds

Read Explanation

Chemical Analysis

Read Explanation

Kinetics

Read Explanation

Organic Chemistry

Read Explanation
View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.

Sign-up for free