Concept explainers
Interpretation:
The reason as to why ionic crystals are brittle on the basis of an atomic-level is to be stated.
Concept introduction:
A substance that is hard but easy to break is known as a brittle substance. Ionic crystal is composed of positively charge ion, cations and negatively charged ion, anions. Crystal lattice is
Answer to Problem 21.1E
Due to the strong interactions between the ions, the ionic crystal is hard, but once distortion occurs in the crystal, the repulsion of ions take place which results in the destabilization of the crystal. This destabilization causes crystal to break.
Explanation of Solution
Ionic crystals are composed of cations and anions. The negatively and positively charged ions in the native state are placed by each other. The attraction between these ions is strong and due to the strong interactions between the ions, the ionic crystal is hard.
The normal lattice becomes distorted once a crystal is stressed. Due to this distortion, the same charge ions come close together. Hence, they repel each other and causes destabilization of the crystal. Thus, due to destabilization, ionic crystal is easy to break.
Due to the strong interactions between the ions, the ionic crystal is hard, but once distortion occurs in the crystal, the repulsion of ions take place which results in the destabilization of the crystal. This destabilization causes crystal to break.
Want to see more full solutions like this?
Chapter 21 Solutions
EBK PHYSICAL CHEMISTRY
- What is the difference between sulfuric acid and hydrosulfuric acid?arrow_forwardWrite chemical formulas for the following compounds. a. Sodium sulfide b. Sodium sulfate c. Sodium carbonate d. Sodium hydrogen carbonatearrow_forwardsilver nitrate + sodium chloride → silver chloride + sodium nitrate List two physical / chemical properties for each compoundarrow_forward
- Write the chemical formula for cadmium hydrogen sulfatearrow_forwardDifferentiate between Oxides and Oxyacids of Nitrogen?arrow_forwardSome salts make hydrates when there is moisture around. Some hydrate samples can absorb lights in visible legion. Therefore, they show some colors. Thus, hydrates can be used to detect the moisture in the environment. Let's say you are working in a laboratory with a group and you are the only student who has taken chemistry courses. Your laboratory received a sample of cobalt(iI) chloride which has the formula CoCl2xH20. Let's say your boss asked you to find the formula of this hydrate salt sample since you are the only chemist there. From your laboratory experience, simply explain the experimental procedure you would follow to find the formula of this unknown sample. Then, use the given data for the calculation part. Mass of crucible: 32.27g Mass of crucible + unknown hydrate: 33.92 g Color of unknown hydrate: purple Mass of crucible + anhydrous form of hydrate: 33.41 g Color of anhydrous form: sky bluearrow_forward
- What is the chemical formula for the compound formed between manganese(IV) and chlorine? chemical formula: What is the chemical formula for the compound formed between manganese(IV) and sulfur? chemical formula:arrow_forwardAssume that you are given samples of two white crystalline compounds, one of them ionic and the other one covalent. Describe how you might tell which is which.arrow_forwardMetals can be rolled into sheets and stamped into various forms. In contrast, diamond is very hard and brittle. Which explanation for these different properties is correct? Metals have semi-ionic bonds, whereas diamond has covalent bonds. The electrons of a metal are held more tightly to the parent atom than the electrons of carbon. Hence, the bonds in a metal are stronger than the bonds in diamond. Metals are made of metal atoms, whereas diamond is made of non-metal carbon atoms. The electrons that surround a metal atom are free to move through the metal. The bonding electron pairs in a diamond are held tightly between two carbon atoms in an overall tetrahedral pattern. Diamond has strong double bonds between carbon atoms. Metal bonds are normally single covalent bonds, which bend easily.arrow_forward
- Chemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningChemistry: 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
- Chemistry: Matter and ChangeChemistryISBN:9780078746376Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl WistromPublisher:Glencoe/McGraw-Hill School Pub CoGeneral, Organic, and Biological ChemistryChemistryISBN:9781285853918Author:H. Stephen StokerPublisher:Cengage LearningChemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage Learning