/*! This file is auto-generated */ .wp-block-button__link{color:#fff;background-color:#32373c;border-radius:9999px;box-shadow:none;text-decoration:none;padding:calc(.667em + 2px) calc(1.333em + 2px);font-size:1.125em}.wp-block-file__button{background:#32373c;color:#fff;text-decoration:none} Problem 89 Acidic oxides are those that rea... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 8: Problem 89

Acidic oxides are those that react with water to produce acid solutions, whereas the reactions of basic oxides with water produce basic solutions. Nonmetallic oxides are usually acidic, whereas those of metals are basic. Predict the products of the reactions of these 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.

Short Answer

Expert verified
Metal oxides form NaOH and Ba(OH)鈧�; nonmetal oxides form H鈧侰O鈧�, HNO鈧�, H鈧働O鈧�, and H鈧係O鈧�.

Step by step solution

01

Identify Metal Oxides

Metallic oxides, such as those formed by alkali and alkaline earth metals, tend to be basic. In this exercise, we identify the metal oxides: Sodium oxide (\(\mathrm{Na}_2\mathrm{O}\)) and Barium oxide (\(\mathrm{BaO}\)).
02

Reaction of Metallic Oxides with Water

When metallic oxides react with water, they form basic solutions or hydroxides. Here are the reactions for the identified metal oxides:- \(\mathrm{Na}_2\mathrm{O} + \mathrm{H}_2\mathrm{O} \rightarrow 2\mathrm{NaOH}\)- \(\mathrm{BaO} + \mathrm{H}_2\mathrm{O} \rightarrow \mathrm{Ba(OH)_2}\)
03

Identify Nonmetal Oxides

Nonmetallic oxides are typically acidic. In this problem, the nonmetal oxides are: Carbon dioxide (\(\mathrm{CO}_2\)), Dinitrogen pentoxide (\(\mathrm{N}_2\mathrm{O}_5\)), Diphosphorus pentoxide (\(\mathrm{P}_4\mathrm{O}_{10}\)), and Sulfur trioxide (\(\mathrm{SO}_3\)).
04

Reaction of Nonmetal Oxides with Water

Nonmetallic oxides react with water to form acidic solutions. Here are their respective reactions:- \(\mathrm{CO}_2 + \mathrm{H}_2\mathrm{O} \rightarrow \mathrm{H}_2\mathrm{CO}_3\) (carbonic acid)- \(\mathrm{N}_2\mathrm{O}_5 + \mathrm{H}_2\mathrm{O} \rightarrow 2\mathrm{HNO}_3\) (nitric acid)- \(\mathrm{P}_4\mathrm{O}_{10} + 6\mathrm{H}_2\mathrm{O} \rightarrow 4\mathrm{H}_3\mathrm{PO}_4\) (phosphoric acid)- \(\mathrm{SO}_3 + \mathrm{H}_2\mathrm{O} \rightarrow \mathrm{H}_2\mathrm{SO}_4\) (sulfuric acid)

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Over 30 million students worldwide already upgrade their learning with 91影视!

Key Concepts

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

Metallic Oxides
Metallic oxides are compounds that typically consist of oxygen and a metal. These oxides are basic in nature, meaning they can react with water to produce basic or alkaline solutions. When dissolved in water, metallic oxides tend to form metal hydroxides, which are strong bases.
  • Sodium oxide (\(\mathrm{Na}_2\mathrm{O}\)) and Barium oxide (\(\mathrm{BaO}\)) are examples of metallic oxides.

  • When reacted with water, they form the following hydroxides:

    • Sodium oxide reacts with water to form sodium hydroxide: \[\mathrm{Na}_2\mathrm{O} + \mathrm{H}_2\mathrm{O} \rightarrow 2\mathrm{NaOH}\]
    • Barium oxide reacts with water to produce barium hydroxide: \[\mathrm{BaO} + \mathrm{H}_2\mathrm{O} \rightarrow \mathrm{Ba(OH)_2}\]

These reactions result in solutions that are characteristically basic, raising the pH of the solution. This behavior is significant in many chemical processes, such as neutralization reactions and industrial applications involving bases.
Nonmetallic Oxides
Nonmetallic oxides are compounds formed from oxygen and nonmetals. They generally exhibit acidic characteristics when dissolved in water, forming acidic solutions. This tendency to produce acids upon hydration is why nonmetallic oxides are commonly referred to as acidic oxides.
  • Some common nonmetallic oxides include Carbon dioxide (\(\mathrm{CO}_2\)), Dinitrogen pentoxide (\(\mathrm{N}_2\mathrm{O}_5\)), Diphosphorus pentoxide (\(\mathrm{P}_4\mathrm{O}_{10}\)), and Sulfur trioxide (\(\mathrm{SO}_3\)).

  • When these oxides react with water, they generate acids such as:

    • Carbon dioxide forms carbonic acid: \[\mathrm{CO}_2 + \mathrm{H}_2\mathrm{O} \rightarrow \mathrm{H}_2\mathrm{CO}_3\]
    • Dinitrogen pentoxide produces nitric acid: \[\mathrm{N}_2\mathrm{O}_5 + \mathrm{H}_2\mathrm{O} \rightarrow 2\mathrm{HNO}_3\]
    • Diphosphorus pentoxide yields phosphoric acid: \[\mathrm{P}_4\mathrm{O}_{10} + 6\mathrm{H}_2\mathrm{O} \rightarrow 4\mathrm{H}_3\mathrm{PO}_4\]
    • Sulfur trioxide forms sulfuric acid: \[\mathrm{SO}_3 + \mathrm{H}_2\mathrm{O} \rightarrow \mathrm{H}_2\mathrm{SO}_4\]

The formation of these acids is crucial in various environmental and industrial processes, such as acid rain and chemical synthesis.
Reactions with Water
Both metallic and nonmetallic oxides exhibit distinct behaviors when they interact with water, leading to different types of solutions. Understanding these reactions helps us grasp how different chemicals influence water's properties.
  • Metallic Oxides:
    • These oxides combine with water to form hydroxides, which are typically basic in nature. \(\mathrm{Na}_2\mathrm{O}\) combines with water to make \(2\mathrm{NaOH}\), creating an alkaline solution.
    • Barium oxide forms barium hydroxide in water, also yielding a basic solution.
  • Nonmetallic Oxides:
    • These oxides react with water to create acids, leading to an acidic solution.
    • For instance, the reaction of \(\mathrm{CO}_2\) with water gives carbonic acid, contributing to the mild acidity of carbonated water.

These reactions are central to understanding natural phenomena and industrial processes alike. The difference in behavior when reacting with water highlights the unique properties of metallic and nonmetallic oxides and their impact on solution chemistry.

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

A technique called photoelectron spectroscopy is used to measure the ionization energy of atoms. A sample is irradiated with ultraviolet (UV) light, and electrons are ejected from the valence shell. The kinetic energies of the ejected electrons are measured. Because the energy of the UV photon and the kinetic energy of the ejected electron are known, we can write $$h v=\mathrm{IE}+\frac{1}{2} m u^{2}$$ in which \(\nu\) is the frequency of the UV light, and \(m\) and \(u\) are the mass and velocity of the electron, respectively. In one experiment the kinetic energy of the ejected electron from potassium is found to be \(5.34 \times 10^{-19} \mathrm{~J}\) using a UV source of wavelength \(162 \mathrm{nm}\). Calculate the ionization energy of potassium. How can you be sure that this ionization energy corresponds to the electron in the valence shell (that is, the most loosely held electron)?

With reference to the periodic table, name (a) a halogen element in the fourth period, (b) an element similar to phosphorus in chemical properties, (c) the most reactive metal in the fifth period, \((\) d) an element that has an atomic number smaller than 20 and is similar to strontium.

Write the formulas and names of the oxides of the second-period elements (Li to \(\mathrm{N}\) ). Identify the oxides as acidic, basic, or amphoteric.

What is the characteristic of the electron configuration of stable ions derived from representative elements?

When carbon dioxide is bubbled through a clear calcium hydroxide solution, the solution becomes
See all solutions

Recommended explanations on Chemistry Textbooks

Chemistry Branches

Read Explanation

The Earths Atmosphere

Read Explanation

Physical Chemistry

Read Explanation

Inorganic Chemistry

Read Explanation

Organic Chemistry

Read Explanation

Kinetics

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.