Classify the solid state of the following substances as ionic crystals, covalent crystals, molecular crystals, or metallic crystals. Ionic: Covalent: Molecular: Metallic: CO2 CO2 O CO2 CO2 I2 I2 I2 I2 Sg S8 S8 S8 KBr KBr KBr KBr Mg Mg Mg Mg SiO2 SiO2 SiO2 SiO2 LICI LİCI LICI LİCI Cr Cr Cr Cr O O O O 0 O 0 0 0 0 0 O 0 0 0

Classify the solid state of the following substances as ionic crystals, covalent crystals, molecular crystals, or metallic crystals. Ionic: Covalent: Molecular: Metallic: CO2 CO2 O CO2 CO2 I2 I2 I2 I2 Sg S8 S8 S8 KBr KBr KBr KBr Mg Mg Mg Mg SiO2 SiO2 SiO2 SiO2 LICI LİCI LICI LİCI Cr Cr Cr Cr O O O O 0 O 0 0 0 0 0 O 0 0 0

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter9: Liquids And Solids

Section: Chapter Questions

Problem 4RQ

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Similar questions

MnO has either the NaCI type structure or the CsCI type structure (see Exercise 69). The edge length of the MnO unit cell is 4.47 10-8 cm and the density of MnO is 5.28 g/cm3. a. Does MnO crystallize in the NaCl or the CsCl type structure? b. Assuming that the ionic radius of oxygen is 140. pm, estimate the ionic radius of manganese.
Classify each of the following by the type of solid it forms: a F2; b BaCl2; c BCl3; d CCl4; e CaO.
The structures of some common crystalline substances are shown below. Show that the net composition of each unit cell corresponds to the correct formula of each substance.
The 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.
Spinel is a mineral that contains 37.9% aluminum, 17.1% magnesium, and 45.0% oxygen, by mass, and has a density of 3.57 g/cm3.The edge of the cubic unit cell measures 809 pm. How many of each type of ion are present in the unit cell?
Barium crystallizes in a body-centered cubic unit cell with an edge length of 3.025 (a) What is the atomic radius of barium in this structure? (b) Calculate the density of barium.
At very low temperatures oxygen, O2, freezes and forms a crystalline solid. Which best describes these crystals? (a) ionic (b) covalent network (c) metallic (d) amorphous (e) molecular crystals
Mn crystallizes in the same type of cubic unit cell as Cu. Assuming that the radius of Mn is 5.6% larger than the radius of Cu and the density of copper is 8.96 g/cm3, calculate the density of Mn.
How 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.
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.
A metal burns in air at 600c under high pressure to form an oxide with formula MO2. This compound is 23.72% oxygen by mass. The distance between the centers of touching atoms in a cubic closest packed crystal of this metal is 269.0 pm. What is this metal? What is its density?
What is a lattice? What is a unit cell? Describe a simple cubic unit cell. How many net atoms are contained in a simple cubic unit cell? How is the radius of the atom related to the cube edge length for a simple cubic unit cell? Answer the same questions for the body-centered cubic unit cell and for the face-centered unit cell.

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