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3. Calculate the Packing Factor of the Zinc Blenda structure to know the degree of occupancy of the ions that make it up.
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- 2. Calculate the Packing Factor of the Sodium Chloride structure to know the degree of occupancy of the ions that make it up.4) in metallic crystals a. How many types of close packing are known? Explain all types in detail. b. How many types of holes are found in the close packing? Compare with cach other the number and size of that holes. c. Define the crystal packing of group 1A and group 2A metals. Which metals are close packed and which metals are non-close packed in those two groups? Başlık ekle... > Cadı1.) Compare the relative atomic radius of iron and carbon. Fe: С: 2.) At low temperatures, Fe has a Body Centered Cubic (BCC) crystal structure. This phase is ferrite, a. The carbon is added into the system in the empty spaces in your BCC model. The C in these spots is known as an interstitial point defect. Determine how many spots for C are there in the model you built. Sketch the unit cell below and indicate where the spots for C to add are. 3.) At high temperatures, Fe has a Face Centered Cubic (FCC) crystal structure. This phase is austenite, y. The carbon is added into the system in the empty spaces in your FCC model. The C in these spots is known as an interstitial point defect. Determine how many spots for C are there in the model you built. Sketch the unit cell below and indicate where the spots for C to add are. In the coming weeks, you will see that these C interstitial point "defects" play a critical role in making the steel mechanically strong.
- 7. It is not possible to pack spheres together without leaving some void spaces between the spheres. Packing efficiency is the fraction of space in a crystal that is actually occupied by atoms. Determine the packing efficiency of a face- centered cubic metal as shown in a figure below. 4r- - 45° 8. What determines which species in a solid solution is the solute and which is the solvent? Explain the 24-karat Gold preparation. Au Ag Substitutional alloy 14karat geld Interstitial alloy Sael 9. The unit cell of a binary compound of copper and oxygen is shown here. Given this image and the ionic radii (a) determine the empirical formula of this compound, Cu* = 0.74 Å and ro = 1.26 A (b) determine the coordination numbers of copper and oxygen, (c) estimate the length of the edge of the cubic unit cell, and (d) estimate the density of the compound.The unit cell of strontium titanate SrTiO3 is depicted on the left in the figure below showing the crystal structure as confirmed by X-ray diffraction experiments. The lattice constant is a - 3.9 × 10-¹0 m. A typical X-ray powder diffraction spectrum is displayed on the right. The wave length of the X-ray beam (Cu-Ka radiation) is λ = 1.54 × 10-¹⁰ m. Unit cell of SrTiO3; Sr atoms are shown in blue, Ti in black and the oxygen atoms are in red. Normalized intensity (a.u.) (001) 20 (011) 30 (III) 40 (200) (210) 50 (211) (220) (300) 60 20 (degrees) 70 (310) (311) >(222) (320) 80 90 (17) 100 X ray powder diffraction data for SrTiO3; the plot shows an overlay for two different SrTiO3 samples. [L. da Silva et al, J. Nanomat., doi:10.1155/2012/890397] a) Identify the Bravais lattice of SrTiO 3and specify the basis for the primitive unit cell shown in the figure. b) Explain how the Miller indices (hkl) describe a family of lattice planes. State a set of possible reciprocal lattice vectors. c)…11.Demonstrate the fraction of these sites in an FCC lattice that Fe2+ ions would need to occupy in order to maintain charge neutrality with the O2– ions sitting in FCC lattice positions of a unit cell. 12.Describe how the bonding and atomic arrangement in diamond differs from that in other allotropes of carbon such as graphite, graphene, and fullerenes (Buckyballs). 13.The silicate anion (SiO44-) “orthosilicate” is the basic building block of all silicate materials. Draw the Lewis Dot Structure for the (SiO44-) ion. Based on your Lewis dot structure, what is the predicted geometry for the (SiO44-) ion? What kind of bonds occur between Si and O in the (SiO44-) ion?
- 3. Compare and contrast the two types of close-packing in solids? 4. Why is there % error in part II? What could be the reason for such error? 5. By understanding the structure of crystals molecularly, what is its relation to the strength of materials? 6. Use the internet to search three (3) examples of metals which have HCP, FCC and BCC structures. Relate the structure to the characteristic properties of each metal. Please indicate the condition the given structures are observed.Find the planer density (Po) in (atom/mm) of (100) in a face centered cubic unit cell with lattice constant of 3.5 A, and determined the atomic radiusDescribe how the anatomy of an atom. What is the atomic number and atomic mass? What are the three different types of bonding and their physical characteristics? How does the type of bonding and arrangement of atoms in the mineral determine the physical characteristics of the mineral crystal (hardness, cleavage, crystal shape, etc.)?
- 1. Calculate the number of atoms in a hexagonal unit cell. Please show all work rather than grouping atoms together. (Recall that y = 120° and that all four angles in the base must sum to 360°). 2. What is the packing efficiency for each of the following unit cells in which all the atoms are identical? Give your answers to four significant figures. Hint: Determine the length of an edge for each cubic cell in terms of r, the atoms' atomic radii. (a) Simple cubic cell (b) Face-centered cubic2. Why does a transparent polymer turn opaque in the necked region when tested in tension.a) Draw rock salt unit cell of NaCl and give the coordinates (u,v,w) describing the positions of all the atoms in such a unit cell. b) Calculate the structure factor |F_hkl|^ 2 for such a unit cell for x-ray scattering from a given set of crystallographic planes (hkl). c) Which reflection peaks have the lowest and highest intensities and why
