Interpretation:
The term crystalline solid should be explained. The kind of microscopic structure do such solids have must be explained. How is this microscopic structure reflected in macroscopic structure must also be explained.
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.
Trending nowThis is a popular solution!
Chapter 14 Solutions
Introductory Chemistry: A Foundation
- The amount of heat required to melt 2 lbs of ice is twice the amount of heat required to melt 1 lb of ice. Is this observation a macroscopic or microscopic description of chemical behavior? Explain your answer.arrow_forwardExplain what is meant by the 'structure of a liquid'.arrow_forwardWhy does the structure of molecules behaves as an independent unit?arrow_forward
- What is the difference between a chemical and physical change? What is the difference between an intermolecular force and an intramolecular force? Explain why it takes more energy to break an intramolecular force than it does an intermolecular force. Define viscosity. Describe what surface tension is and how you know that water has a higher surface tension than alcohol. If a substance has a high viscosity, then it has strong intermolecular forces. For example, in the investigation we did, we found that room-temperature corn syrup had stronger intermolecular forces/higher viscosity than the hot corn syrup because it took longer for it to pour out of the beaker. Describe cohesion and adhesion and how they relate to your everyday life. Substances with high boiling, melting, and freezing points have stronger intermolecular forces. Four types of intermolecular forces: dispersion forces, hydrogen bonds (H-O, H-F, H-N), ion-dipole, dipole-dipole Which intermolecular force exists…arrow_forwardIn a solid, any two adjacent molecules remain adjacent to one another for a a long time (minutes or longer). A molecular-scale snapshot of the position of molecules in the liquid phase would look more like a snapshot of an amorphous solid than a snapshot of a crystalline solid. At higher temperatures, a higher fraction of molecules in a liquid have enough energy to overcome the attractive forces between the molecules. In a liquid near room temperature, a given molecule spends a long time (minutes or longer) next to the same adjacent molecule before they slip away from one another. Also..! I think I know this next one already. But i Just wanted to check what you thought? If you agree? For most compounds, which is the proper order of density for highest to lowest? O liquid, solid, gas gas, liquid, solid solid, liquid, gas gas, solid, liquidarrow_forward4. Water is less dense as a solid than as a liquid. A. Why can solid ice float on liquid water? B. When a lake freezes, how does the density of water prevent all of the living organisms in the lake from freezing as well? OEL r TE OT 1arrow_forward
- a. This substance can be liquified by compression at room temperature. b. At any point on the curve represented by the section ABC, the substance will exist in two phases. c. The intermolecular force of attraction observed at point E is greater than that at point D. d. Point D to C describes a process whereby the substance is completely vaporized.arrow_forwardA student left a sealed jar of water outside her home. Water can be a solid, liquid, or gas. When she put it outside, the water was a solid. Twelve hours later, the water had changed phase and was a liquid. What happened to the water molecules?arrow_forwardConsider the melting points of the substances below (see figures for two compounds). Explain the trend in melting point using your knowledge of intermolecular forces. (In the structures below, carbon is black, hydrogen is white, and oxygen is red.) Substance Melting Point (°C) Molar Mass (g/mol) Cl2 −102 71 Ethyl formate (CH3CH2OCHO) −80 74 Propionic acid (CH3CH2COOH) −20 74 Br2 −7.2 160arrow_forward
- What are solid substances?arrow_forwarda. Water is good solvent. Relate this property to issues of pollution. b.Water has a high specific heat. Relate this property to changing climate and the capacity of bodies of water to act as temperature buffer. c. The boiling point of water is unusually high. Relate this property to questions on small water bodies drying up.arrow_forwardConstant Pressure Transitions 1. Suppose you had the following phase diagram for a simple pure substance: a. What physical state would the substance be in under the conditions at point 1? b. Suppose the temperature was then increased on this substance at constant pressure. What state(s) would the substance be in at each of points 2 to 5? c. Suppose the constant pressure was 1 atmosphere. What useful information can you get from the diagram about the simple physical properties of the substance? d. Suppose at a much lower pressure, the substance was under the conditions at point 6. Describe what happens to the substance as you increase the temperature from point 6 to point 8.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 by OpenStax (2015-05-04)ChemistryISBN:9781938168390Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark BlaserPublisher:OpenStax
- Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage LearningChemistry for Today: General, Organic, and Bioche...ChemistryISBN:9781305960060Author:Spencer L. Seager, Michael R. Slabaugh, Maren S. HansenPublisher:Cengage Learning