Concept explainers
Interpretation:
The three types of crystalline solids must be explained with example.
Concept Introduction:
Solids are generally two types namely crystalline solid and amorphous solid. Crystalline solids are common among them. They have definite shape, they are rigid and non-compressible in nature. The faces of such solids are flats and they generally have geometric shapes. The example are diamond, metals and salt etc.
To identify the type of crystals, the structure should be identified first. In crystalline solids, the arrangement of particles is in orderly fashion. The atoms have very less space between them due to strong intermolecular forces. The crystals so formed have high melting and boiling point.
Compared to crystalline solids, amorphous are randomly arranged. They do not have any geometry or shape. There is a range of temperature over which amorphous solids will melt but there is not definite temperature for this. They have short order arrangement and there is variety of arrangement present in it.
Want to see the full answer?
Check out a sample textbook solutionChapter 14 Solutions
Introductory Chemistry: A Foundation
- An amorphous solid can sometimes be converted to a crystalline solid by a process called annealing. Annealing consists of heating the substance to a temperature just below the melting point of the crystalline form and then cooling it slowly. Explain why this process helps produce a crystalline solid.arrow_forwardHow do ionic solids differ in structure from molecular solids? What are the fundamental panicles in each? Give two examples of each type of solid and indicate the individual particles that make up the solids in each of your examples.arrow_forwardWhat types of liquids typically form amorphous solids?arrow_forward
- Silicon carbide, SiC, is a very hard, high-melting solid. What kind of crystal forces account for these properties?arrow_forwardThe CsCl structure is a simple cubic array of chloride ions with a cesium ion at the center of each cubic array (see Exercise 69). Given that the density of cesium chloride is 3.97 g/cm3, and assuming that the chloride and cesium ions touch along the body diagonal of the cubic unit cell, calculate the distance between the centers of adjacent Cs+ and Cl ions in the solid. Compare this value with the expected distance based on the sizes of the ions. The ionic radius of Cs+ is 169 pm, and the ionic radius of Cl is 181 pm.arrow_forward
- World of Chemistry, 3rd editionChemistryISBN:9781133109655Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCostePublisher:Brooks / Cole / Cengage LearningIntroductory Chemistry: A FoundationChemistryISBN:9781337399425Author:Steven S. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistry: Matter and ChangeChemistryISBN:9780078746376Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl WistromPublisher:Glencoe/McGraw-Hill School Pub Co
- Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage LearningIntroductory Chemistry: An Active Learning Approa...ChemistryISBN:9781305079250Author:Mark S. Cracolice, Ed PetersPublisher:Cengage LearningChemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning