/*! 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 12 Place the following oxides in or... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 21: Problem 12

Place the following oxides in order of increasing basicity: \(\mathrm{Na}_{2} \mathrm{O}, \mathrm{Al}_{2} \mathrm{O}_{3}, \mathrm{SiO}_{2}, \mathrm{SO}_{3}\).

Short Answer

Expert verified
Order of increasing basicity: \(\mathrm{SO}_3, \mathrm{SiO}_2, \mathrm{Al}_2\mathrm{O}_3, \mathrm{Na}_2\mathrm{O}\).

Step by step solution

01

Understand Basicity in Oxides

Basicity in oxides generally refers to the ability of the oxide to react with acids to form salts and water. Basic oxides usually form from metals, while acidic oxides tend to form from non-metals.
02

Identify Types of Oxides

Determine if each oxide is basic, acidic, or amphoteric. \(\mathrm{Na}_2\mathrm{O}\) is a basic oxide, \(\mathrm{Al}_2\mathrm{O}_3\) is amphoteric, \(\mathrm{SiO}_2\) is acidic, and \(\mathrm{SO}_3\) is acidic.
03

Arrange Oxides by Basicity

Place the oxides in order of increasing basicity. Since \(\mathrm{SiO}_2\) and \(\mathrm{SO}_3\) are both acidic, they should be first. \(\mathrm{Al}_2\mathrm{O}_3\) is amphoteric, having some basic characteristics but less than \(\mathrm{Na}_2\mathrm{O}\), which is fully basic.

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.

Acidic Oxides
Acidic oxides are oxides that can react with water to form acids or with bases to form salts. These oxides are typically formed from nonmetals. When they dissolve in water, they contribute to the acidity of the solution. For example, sulfur trioxide (\(\mathrm{SO}_3\)), a non-metal oxide, reacts with water to form sulfuric acid (\(\mathrm{H}_2\mathrm{SO}_4\)). Another example is silicon dioxide (\(\mathrm{SiO}_2\)), which, although not reacting readily with water, can still react with strong bases to form silicates. Such properties define these oxides as acidic.
  • Non-metal oxides: Typically show acidic properties.
  • Reactions: Form acids when combined with water or form salts when reacting with bases.
  • Examples: \(\mathrm{SO}_3\) and \(\mathrm{SiO}_2\).
Understanding the nature of acidic oxides helps in predicting their reactions and their role in chemical processes.
Amphoteric Oxides
Amphoteric oxides are unique as they exhibit both acidic and basic properties. This dual nature allows them to react with both acids and bases to form salts. A classic example is aluminum oxide (\(\mathrm{Al}_2\mathrm{O}_3\)), which can react with hydrochloric acid (\(\mathrm{HCl}\)) to form aluminum chloride (\(\mathrm{AlCl}_3\)) and with sodium hydroxide (\(\mathrm{NaOH}\)) to form sodium aluminate (\(\mathrm{NaAlO}_2\)).
  • Dual Reactivity: Reacts with both acids and bases.
  • Salts Formation: Produces different types of salts depending on the reactant.
  • Example: \(\mathrm{Al}_2\mathrm{O}_3\) is a typical amphoteric oxide.
This dual characteristic is important in industrial processes where balance between acids and bases may be necessary.
Metal vs Non-metal Oxides
Oxides can be categorized based on the element they originate from鈥攎etals or non-metals. Metal oxides typically have basic characteristics, whereas non-metal oxides are mostly acidic. Metal oxides, such as sodium oxide (\(\mathrm{Na}_2\mathrm{O}\)), react with water to form hydroxides which are basic in nature.
  • Metal Oxides: Often basic, metal oxides form hydroxides.
  • Non-metal Oxides: Usually acidic, they react with water to form acids.
Understanding whether an element forms a metal or non-metal oxide helps predict its behavior in chemical reactions. This distinction clarifies the order of basicity: metals generally increase basicity, while non-metals tend towards acidity.

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

Place the following oxides in order of increasing basicity: \(\mathbf{C O}_{2}, \mathrm{SiO}_{2}, \mathrm{SnO}_{2}\).

What current must be used in a Downs cell operating at \(7.0 \mathrm{V}\) to produce 1.00 metric ton (exactly \(1000 \mathrm{kg}\) ) of sodium per day? Assume \(100 \%\) efficiency.

You are given a stoppered flask that contains hydrogen, nitrogen, or oxygen. Suggest an experiment you could do to identify the gas.

When magnesium burns in air, it forms both an oxide and a nitride. Write balanced equations for the formation of both compounds.

Unlike carbon, which can form extended chains of atoms, nitrogen can form chains of very limited length. Draw the Lewis electron dot structure of the azide ion, \(\mathrm{N}_{3}^{-} .\) Is the ion linear or bent?
See all solutions

Recommended explanations on Chemistry Textbooks

Kinetics

Read Explanation

Organic Chemistry

Read Explanation

The Earths Atmosphere

Read Explanation

Making Measurements

Read Explanation

Chemical Analysis

Read Explanation

Nuclear 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.