2) Draw unit cell for face-centered cubic crystal structures (FCC). a) Show number of atoms per unit cell and coordination number, Derive the relationships between unit cell edge length and atomic radius, Calculate atomic packing factor (APF). b) As compared with body centered cubic crystal structure, why is plastic deformation of metals easy for face centered cubic crystal structure?

2) Draw unit cell for face-centered cubic crystal structures (FCC). a) Show number of atoms per unit cell and coordination number, Derive the relationships between unit cell edge length and atomic radius, Calculate atomic packing factor (APF). b) As compared with body centered cubic crystal structure, why is plastic deformation of metals easy for face centered cubic crystal structure?

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter21: Structure And Bonding In Solids

Section: Chapter Questions

Problem 24P

See similar textbooks

Similar questions

What is the coordination number in the cesium chloride cubic structure?
What is the coordination number of an aluminum atom in the facecentered cubic structure of aluminum?
Aluminum (atomic radius = 1.43 ) crystallizes in a cubic closely packed structure. Calculate the edge length of the face—centered cubic unit cell and the density of aluminum.
8.13 What is the coordination number of atoms in the diamond structure?
Which of the following statements regarding the cubic dense stacking of metals is false? a) Two tetrahedral spaces per atom. b) One octahedral space falls per atom. c) Stacking type is A-B-A-B…. d) The unit cell of the cubic dense stacking is the face-centered cubic structure. e) The coordination number of metal is 12.
Draw unit cell for face-centered cubic crystal structures (FCC). Show number of atoms per unit cell and coordination number, Derive the relationships between unit cell edge length and atomic radius, Calculate atomic packing factor (APF).
Five grams of vinegar solution was given to you to analyze for the percent acetic acid present in the vinegar. After the titration, 0.0036 moles of NaOH was used to For a face-centered cubic (FCC) crystal structure, a total of whole atoms can be found inside an FCC unit cell.
Use the References to access important values if needed for this question. Metallic tantalum crystallizes in a body-centered cubic lattice, with one Ta atom per lattice point. If the edge length of the unit cell is found to be 328 pm, what is the metallic radius of Ta in pm? H pm Submit Answer Retry Entire Group No more group attempts remain
Figure below shows the first four peaks of the x-ray diffraction pattern for copper, which has a face centered cubic crystal structure; monochromatic x-radiation having a wavelength of 0.1542 nm was used. Reflection indices are presented in the table below. The whole number of wavelengths equals one. (a) Index (i.e., give h, k, and I indices) for each of these peaks. (b) Determine the interplanar spacing for each of the peaks. (c) For each peak, determine the atomic radius for Cu. 40.0 50.0 60.0 70.0 80.0 90.0 Diffraction angle 20 Reflection Indices for First Six Planes Reflections Present (h + k + ) even Crystal Structure 110, 200, 211, 220, 310, 222 ВСС h, k, and I either all odd or all even 111, 200, 220, 311, 222, 400 FCC 100, 110, 111, 200, 210, 211 Simple cubic All Intensity (relative)
Explain face centered cubic unit cell in the simplest way possible and create an overview about it and its objective to impart on students.
Ni3Al is used in the turbines of aircraft engines because of its strength and low density. Nickel metal has a cubic close-packed structure with a face-centered cubic unit cell, whereas Ni3Alhas the ordered cubic structure shown in the figure below. The length of the cubic unit cell edge is 3.53 Å for nickel and 3.56 Å for Ni3Al. Use these data to calculate and compare the densities of these two materials. a). Give the calculated density of pure nickel (FCC with an edge length of 3.53 Å). Express the density in grams per cubic centimeter to three significant digits b). Give the calculated density of the Ni3Al alloy (ordered structure shown in the image with an edge length of 3.56 Å). Express the density in grams per cubic centimeter to three significant digits.