Chemistry by OpenStax (2015-05-04)
1st Edition
ISBN: 9781938168390
Author: Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher: OpenStax
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Textbook Question
Chapter 10, Problem 79E
Cobalt metal crystallizes in a hexagonal closest packed structure. What is the coordination number of a cobalt atom?
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Chapter 10 Solutions
Chemistry by OpenStax (2015-05-04)
Ch. 10 - In terms of their bulk properties, how do liquids...Ch. 10 - In terms of the kinetic molecular theory, in what...Ch. 10 - In terms of the kinetic molecular theory, in what...Ch. 10 - Explain why liquids assume the shape of any...Ch. 10 - What is the evidence that all neutral atoms and...Ch. 10 - Open the PhET States of Matter Simulation...Ch. 10 - Define the following and give an example of each:...Ch. 10 - The types of intermolecular forces in a substance...Ch. 10 - Why do the boiling points of the noble gases...Ch. 10 - Neon and HF have approximately the same molecular...
Ch. 10 - Arrange each of the following sets of compounds in...Ch. 10 - The molecular mass of butanol, C4H9OH, is 74.14;...Ch. 10 - On the basis of intermolecular attractions,...Ch. 10 - On the basis of dipole moments and/or hydrogen...Ch. 10 - The melting point of H2O(s) is O C. Would you...Ch. 10 - Silane SiH4, phosphine (PH3), and hydrogen sulfide...Ch. 10 - Explain why a hydrogen bond between two water...Ch. 10 - Under certain conditions, molecules of acetic...Ch. 10 - Proteins are chains of amino acids that can form...Ch. 10 - The density of liquid NH3 is 0.64 g/mL; the...Ch. 10 - Identify the intermolecular forces present in the...Ch. 10 - The test tubes shown here contain equal amounts of...Ch. 10 - Although steel is denser than water, a steel...Ch. 10 - The surface tension and viscosity values for...Ch. 10 - You may have heard someone use the figure of...Ch. 10 - It is often recommended that you let your car...Ch. 10 - The surface tension and viscosity of water at...Ch. 10 - At 25 C, how high will water rise in a glass...Ch. 10 - Water rises in a glass capillary tube to a height...Ch. 10 - Heat is added to boiling water. Explain why the...Ch. 10 - Heat is added to ice at 0 C. Explain why the...Ch. 10 - What feature characterizes the dynamic equilibrium...Ch. 10 - Identify two common observations indicating some...Ch. 10 - Identify two common observations indicating some...Ch. 10 - What is the relationship between the...Ch. 10 - What is the relationship between the...Ch. 10 - Why does spilled gasoline evaporate more rapidly...Ch. 10 - Carbon tetrachloride, CCl4, was once used as a dry...Ch. 10 - When is the boiling point of a liquid equal to its...Ch. 10 - How does the boiling of a liquid differ from its...Ch. 10 - Use the information in Figure 10.24 to estimate...Ch. 10 - A syringe at a temperature of 20 C is filled with...Ch. 10 - Explain the following observations: (a) It takes...Ch. 10 - The enthalpy of vaporization of water is larger...Ch. 10 - Explain why the molar enthalpies of vaporization...Ch. 10 - Explain why the enthalpies of vaporization of the...Ch. 10 - The enthalpy of vaporization of CO2(l) is 9.8...Ch. 10 - The hydrogen fluoride molecule, HF, is more polar...Ch. 10 - Ethyl chloride (boiling point, 13 C) is used as a...Ch. 10 - Which contains the compounds listed correctly in...Ch. 10 - How much heat is required to convert 422 g of...Ch. 10 - Evaporation of sweat requires energy and thus take...Ch. 10 - Titanium tetrachloride, TiCl4, has a melting point...Ch. 10 - From the phase diagram for water (Figure 10.31),...Ch. 10 - What phase changes will take place when water is...Ch. 10 - Pressure cookers allow food to cook faster because...Ch. 10 - From the phase diagram for carbon dioxide in...Ch. 10 - Determine the phase changes that carbon dioxide...Ch. 10 - Consider a cylinder containing a mixture of liquid...Ch. 10 - Dry ice, CO2(s) , does not melt at atmospheric...Ch. 10 - If a severe storm results in the loss of...Ch. 10 - Is it possible to liquefy nitrogen at room...Ch. 10 - Elemental carbon has one gas phase, one liquid...Ch. 10 - What types of liquids typically form amorphous...Ch. 10 - At very low temperatures oxygen, O2, freezes and...Ch. 10 - As it cools, olive oil slowly solidifies and forms...Ch. 10 - Explain why ice, which is a crystalline solid, has...Ch. 10 - Identify the type of crystalline solid (metallic,...Ch. 10 - Identify the type of crystalline solid (metallic,...Ch. 10 - Classify each substance in the table as either a...Ch. 10 - Classify each substance in the table as either a...Ch. 10 - Identify the following substances as ionic,...Ch. 10 - Substance A is shiny, conducts electricity well,...Ch. 10 - Substance B is hard, does not conduct electricity,...Ch. 10 - Describe the crystal structure of iron, which...Ch. 10 - Describe the crystal structure of Pt, which...Ch. 10 - What is the coordination number of a chromium atom...Ch. 10 - What is the coordination number of an aluminum...Ch. 10 - Cobalt metal crystallizes in a hexagonal closest...Ch. 10 - Nickel metal crystallizes in a cubic closest...Ch. 10 - Tungsten crystallizes in a body-centered cubic...Ch. 10 - Platinum (atomic radius =1.38) crystallizes in a...Ch. 10 - Barium crystallizes in a body-centered cubic unit...Ch. 10 - Aluminum (atomic radius = 1.43 ) crystallizes in a...Ch. 10 - The density of aluminum is 2.7 g/cm3; that of...Ch. 10 - The free space in a metal may be found by...Ch. 10 - Cadmium sulfide, sometimes used as a yellow...Ch. 10 - A compound of cadmium, tin, and phosphorus is used...Ch. 10 - What is the formula of the magnetic oxide of...Ch. 10 - A compound containing zinc, aluminum, and sulfur...Ch. 10 - A compound of thallium and iodine crystallizes in...Ch. 10 - Which of the following elements reacts with sulfur...Ch. 10 - What is the percent by mass of titanium in rutile,...Ch. 10 - Explain why the chemically similar alkali metal...Ch. 10 - As minerals were formed from the molten magma,...Ch. 10 - Rubidium iodide crystallizes with a cubic unit...Ch. 10 - One of the various manganese oxides crystallizes...Ch. 10 - NaH crystallizes with the same ciystal structure...Ch. 10 - Thallium(I) iodide crystallizes with the same...Ch. 10 - A cubic unit cell contains manganese ions at the...Ch. 10 - What is the spacing between crystal planes that...Ch. 10 - A diffracrometer using X-rays with a wavelength of...Ch. 10 - A metal with spacing between planes equal to...Ch. 10 - Gold crystallizes in a face-centered cubic unit...Ch. 10 - When an electron in an excited molybdenum atom...
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Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Similar questions
- The coordination number of uniformly sized spheres in a cubic closest-packing (FCC) array is 12. Give the coordination number of each atom in (a) a simple cubic lattice. (b) a body-centered cubic lattice.arrow_forward• describe the arrangement of atoms in the common cubic crystal lattices and calculate the packing efficiency for a lattice.arrow_forwardWhat is the coordination number in the cesium chloride cubic structure?arrow_forward
- 8.13 What is the coordination number of atoms in the diamond structure?arrow_forwardNickel metal crystallizes in a cubic closest packed structure. What is the coordination number of a nickel atom?arrow_forwardAn 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_forward
- Silicon carbide, SiC, is a very hard, high-melting solid. What kind of crystal forces account for these properties?arrow_forwardCobalt fluoride crystallizes in a closest packed array of fluoride ions with the cobalt ions filling one-half of the octahedral holes. What is the formula of this compound?arrow_forwardDescribe the unit cell of lithium (see Figure).arrow_forward
- (a) Determining an Atom Radius from Lattice Dimensions: Gold has a face-centered unit cell, and its density is 19.32 g/cm3. Calculate the radius of a gold atom. (b) The Structure of Solid Iron: Iron has a density of 7.8740 g/cm3, and the radius of an iron atom is 126 pm. Verify that solid iron has a body-centered cubic unit cell. (Be sure to note that the atoms in a body-centered cubic unit cell touch along the diagonal across the cell. They do not touch along the edges of the cell.) (Hint: The diagonal distance across the unit cell = edge 3.)arrow_forwardPhase diagrams for materials that have allotropes can be more complicated than those shown in the chapter. Use the phase diagram for carbon given here to answer the following questions. (a) How many triple points are present and what phases are in equilibrium for each? (b) Is there a single point where all four phases are in equilibrium? (c) Which is more stable at high pressures, diamond or graphite? (d) Which is the stable phase of carbon at room temperature and 1 atmosphere pressure?arrow_forwardPlatinum (atomic radius =1.38) crystallizes in a cubic closely packed structure. Calculate the edge length of the facecentered cubic unit cell and the density of platinum.arrow_forward
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