Unit Cell and Crystal CharacteristicThe volume of sphere is 4/3 (1) ³ and the radius of each atom is 1.0 cm. Assume that all thesolids are aluminum (MM=26.98 g/mol). Calculate the following: number of atoms(spheres)inside the unit cell, total volume of spheres inside the unit cell, volume of the unit cell and the% of space occupied in the unit cell using the equation:Density (g/cc)VspheresV cel% occupiedCubic(express tono. of atomscm3cm3scientificUnit(round-off to two | (round-off to two | (round-off to two | notation; round-decimal places) | decimal places)(whole no.)Celldecimal places)off to twodecimal places)SCX10-24FCCX10-24ВсС|x10-24Based on the calculated density, what is the most probable lattice type of aluminum metal?Body Centered Cubic (BCC) Structure, Simple Cubic (SB) Structure, or Face-Centered Cubic(FCC) Structure?--Please explain how do you get the answersbecause I can't understand my prof. Thank you!--

Radius of each atom r = 1.00 cm Molar mass of Al = 26.98 g/mol We need to find density for SC, FCC,…

Unit Cell and Crystal Characteristic The volume of sphere is 4/3 (7) r³ and the radius of each atom is 1.0 cm. Assume that all the solids are aluminum (MM=26.98 g/mol). Calculate the following: number of atoms(spheres) inside the unit cell, total volume of spheres inside the unit cell, volume of the unit cell and the % of space occupied in the unit cell using the equation: Density (g/cc) Vspheres Vcel % occupied Cubic (express to no. of atoms cm3 cm3 scientific Unit (whole no.) notation; round- (round-off to two | (round-off to two decimal places) Cell (round-off to two decimal places) decimal places) off to two decimal places) SC x10-24 FCC x10-24 ВСС x10-24 Based on the calculated density, what is the most probable lattice type of aluminum metal? Body Centered Cubic (BCC) Structure, Simple Cubic (SB) Structure, or Face-Centered Cubic (FCC) Structure?

Unit Cell and Crystal Characteristic The volume of sphere is 4/3 (7) r³ and the radius of each atom is 1.0 cm. Assume that all the solids are aluminum (MM=26.98 g/mol). Calculate the following: number of atoms(spheres) inside the unit cell, total volume of spheres inside the unit cell, volume of the unit cell and the % of space occupied in the unit cell using the equation: Density (g/cc) Vspheres Vcel % occupied Cubic (express to no. of atoms cm3 cm3 scientific Unit (whole no.) notation; round- (round-off to two | (round-off to two decimal places) Cell (round-off to two decimal places) decimal places) off to two decimal places) SC x10-24 FCC x10-24 ВСС x10-24 Based on the calculated density, what is the most probable lattice type of aluminum metal? Body Centered Cubic (BCC) Structure, Simple Cubic (SB) Structure, or Face-Centered Cubic (FCC) Structure?

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter9: Liquids, Solids, And Materials

Section: Chapter Questions

Problem 115QRT

See similar textbooks

Similar questions

Outline a two-dimensional unit cell for the pattern shown here. If the black squares are labeled A and the white squares are B, what is the simplest formula for a compound based on this pattern?
Consider the three types of cubic units cells. (a) Assuming that the spherical atoms or ions in a primitive cubic unit cell just touch along the cubes edges, calculate the percentage of occupied space within the unit cell. (Recall that the volume of a sphere is (4/3)r3, where r is the radius of the sphere.) (b) Compare the percentage of occupied space in the primitive cell (pc) with the bcc and fcc unit cells. Based on this, will a metal in these three forms have the same or different densities? If different, in which is it most dense? In which is it least dense?
Aluminum metal crystallizes with a face-centered cubic unit cell. The volume of the cell is 0.0662 nm3. (a) What is the atomic radius of aluminum in cm? (b) What is the volume of a single aluminum atom? (c) What is the density of a single aluminum atom? (d) In face-centered cubic cell packing, the fraction of empty space is 26.0%. When this is factored in, what is the calculated density of aluminum?
The free space in a metal may be found by subtracting the volume of the atoms in a unit cell from the volume of the cell. Calculate the percentage of free space in each of the three cubic lattices if all atoms in each are of equal size and touch their nearest neighbors. Which of these structures represents the most efficient packing? That is, which packs with the least amount of unused space?
Which solid phase that is, which allotrope of carbon is more stable, graphite or diamond? You should consult some of the tables in the thermodynamics section of this text.. Both solid phases exist under normal conditions of pressure and temperature. Explain why this is so, given that one solid phase is more thermodynamically stable than the other. Do their unit cells provide any suggestion for their relative stabilities?
Lithium hydride (LiH) has the sodium chloride structure, and the length of the edge of the unit cell is 4.086 108 cm. Calculate the density of this solid.
Explain in words how Avogadros number could be obtained from the unit-cell edge length of a cubic crystal. What other data are required?
In the LiCl structure shown in Figure 9.21, the chloride ions form a face-centered cubic unit cell 0.513 nm on an edge. The ionic radius of Cl- is 0.181 nm. (a) Along a cell edge, how much space is between the Cl- ions? (b) Would an Na+ ion (r=0.095nm) fit into this space? a K+ ion (r=0.133nm)?
The structures of another class of ceramic, high-temperature superconductors are shown in figures a-d. a. Determine the formula of each of these four superconductors. b. One of the structural features that appears to be essential for high-temperature superconductivity is the presence of planar sheets of copper and oxygen atoms. As the number of sheets in each unit cell increases, the temperature for the onset of superconductivity increases. Order the four structures from lowest to the highest superconducting temperature. c. Assign oxidation states to Cu in each structure assuming Tl exists as Tl3+. The oxidation states of Ca, Ba, and O are assumed to be + 2, + 2, and 2, respectively. d. It also appears that copper must display a mixture of oxidation states for a material to exhibit superconductivity. Explain how this occurs in these materi.als as well as in the superconductor in Exercise 87.
The memory metal, nitinol, is an alloy of nickel and titanium. It is called a memory metal because after being deformed, a piece of nitinol wire will return to its original shape. The structure of nitinol consists of a simple cubic array of Ni atoms and an inner penetrating simple cubic array of Ti atoms. In the extended lattice, a Ti atom is found at the center of a cube of Ni atoms; the reverse is also true. a. Describe the unit cell for nitinol. b. What is the empirical formula of nitinol? c. What are the coordination numbers (number of nearest neighbors) of Ni and Ti in nitinol?
A diamond unit cell is shown here. Unit cell of diamond (a) How many carbon atoms are in one unit cell? (b) The unit cell can be considered as a cubic unit cell of C atoms with other C atoms in holes in the lattice. What type of unit cell is this (pc, bcc, fcc)? In what holes are other C atoms located, octahedral or tetrahedral holes?
Outline a two-dimensional unit cell for the pattern shown here. If the black squares are labeled A and the white squares are B, what is the simplest formula for a compound based on this pattern?