18 of 30 >The unit cell of a compound containing potassium, aluminum,and fluorine is shown here.II Review I Constants I Periodic TablePart A3.55 Å3.55 ÅWhat type of lattice does this crystal possess(all three lattice vectors are mutually perpendicular)?O monoclinicO orthorhombicO hexagonalO cubicO tetragonal6.18 ÅO thombohedralO triclinicSubmitRequest AnswerPart BWhat is the empirical formula?Express your answer as a chemical formula.Π-ΑΣφP PearsonShow AllCh. 2- Chemistr.pdfCh. 2 Note Outlin..pdfMacBook AirDIIDD80888F12F7F10F6F4FSF3F2&@#3$dele-78234{WERYJKSFMCVcommandoptioncommandww.. .-

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What type of lattice does this crystal possess(all three lattice vectors are mutually perpendicular)? O monoclinic O orthorhombic O hexagonal O cubic O tetragonal O rhombohedral O triclinic Submit Request Answer Part B What is the empirical formula? Express your answer as a chemical formula. 0 ΑΣφ ?

What type of lattice does this crystal possess(all three lattice vectors are mutually perpendicular)? O monoclinic O orthorhombic O hexagonal O cubic O tetragonal O rhombohedral O triclinic Submit Request Answer Part B What is the empirical formula? Express your answer as a chemical formula. 0 ΑΣφ ?

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter10: Liquids And Solids

Section: Chapter Questions

Problem 87E: Materials containing the elements Y, Ba, Cu, and O that are superconductors (electrical resistance...

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Materials containing the elements Y, Ba, Cu, and O that are superconductors (electrical resistance equals zero) at temperatures above that of liquid nitrogen were recently discovered. The structures of these materials are based on the perovskite structure. Were they to have the ideal perovskite structure, the superconductor would have the structure shown in pant (a) of the following figure. a. What is the formula of this ideal perovskite material? b. How is this structure related to the perovskite structure shown in Exercise 85? These materials, however, do not act as superconductors unless they are deficient in oxygen. The structure of the actual superconducting phase appears to be that shown in pan (b) of the figure. c. What is the formula of this material?
A crystal has a cubic unit cell of 4.2 Å. Using a wavelength of 1.54 Å at which 2θ value would you expect tomeasure the (111) peak?
The atomic radius of an atom that is present in a BCC unit cell having a lattice parameter of 4.5 A is 1.12 A 1.59 A 2.25 A 1.95 A Show handwritten solution pls
2-the lattice parameter of FCC strontium is 6.0849A. if one atom is missing for each 1500 strontium atoms, calculate (a) the density of strontium and (b) the number of vacancies per gram. 3-calculate the planar atomic densities of planes (-110), (-110), and(01-1) in BCC unit cell and apply your result for iron(BCC form).
Show complete and detailed solution: 1. An element crystallizes in a body centered cubic unit cell. The radius of this element is 2.2 x 10-10 m, and the density is 0.991 g/cm3. How many moles of atoms are within one unit cell? 2. Nickel has a FCC crystal structure, an atomic radius of 0.125 nm, and an atomic weight of 58.68 g/mol. Compute and compare its theoretical density with the experimental value of 8.90 g/cm3.
onlyroundoffat 2decimalplaces in final answer tyIron has an atomic weight of 55.85 g/mol and a density of 7.86 g/cm3. It crystallizes in a cubic unit cell with an edge length of 0.46 nm. How many atoms are in the cell?
2)The cubic unit cell parameter (a) of polonium (α-Po) is 335 pm. Use the Goldschmidt correction (Table 1) to calculate a metallic radius for this element.
The element Fe has bcc packing with a body-centered cubic unit cell. The density of iron is 7.86 g/cm3 and the cell volume is 2.354 x 10-23 cm3. Calculate the value of Avogadro's number to three significant figures based on these data.
Calculate the volume of a unit cell of Nickel in nm3. The volume of unit cell of Nickel is 4.3142×10-29 m3. Note that Nickel has a Face Centred Cubic Lattice Structure. The atomic mass of nickel is 58.11 g/mole. Find the density of Nickel in Mg/m3. (Here, Mg is defined as Mega-gram) Use the value of Avogedro Number NA=6.023×1023 Use the below mentioned formulae to calculate the density (ρ) ρ=(n×A)/(NA×Vc ), Here, A = the atomic mass of Nickel, Vc=Volume of unit cell of nickel, n=number of atoms in an unit cell of Nickel.
Please help me answer this problem. It will be great help, thank you! Express the answer to the nearest fourth decimal place. *A hypothetical alloy has a face-centered cubic unit cell. Its density is 10, 470 kg/m3 and its atomic weight is 106. 8 g/mole. a) What is the atomic radius of the alloy in cm? b) What is the volume of the single atom in cm3?
An element has bcc packing with a body-centered cubic unit cell. Its density is 19300 kg/m3 and the unit cell volume is 3.17 x 10-26 L. Calculate the molar mass (g/mol) of the element to three significant figures.
(ii) Prove that the volume of an FCC unit cell, VC is; ?? = 16?3√2