Consider a hypothetical metal that has a density of 7.25 g/cm3, an atomic weight of 72.72 g/mol, and an atomic radius of 0.140 nm. Compute the atomic packing factor if the unit cell has tetragonal symmetry, values for the a and c lattice parameters are 0.416 and 0.385, respectively
Consider a hypothetical metal that has a density of 7.25 g/cm3, an atomic weight of 72.72...
The unit cell for tin has tetragonal symmetry, with a and b lattice parameters of 0.583 and 0.318 nm, respectively. If its density, atomic weight, and atomic radiusare 7.30 g/cm3, 118.69 g/mol, and 0.151 nm, respectively, compute the atomic packing factor.
A metal having a cubic structure has a density of 2.6 g/cm3, an atomic weight of 87.62 g/mol, and a lattice parameter of 6.0849 Å. How many atoms are present in the unit cell?
5 The atomic weight and atomic radius for a hypothetical BCC metal are 43.1 g/mol and 0.122 nm respectively. Determine its density. 6 Calculate the radius of a iridium atom, given that Ir has a FCC crystal structure, a density of 22.4 g/cm^3, and an atomic weight of 192.2 g/mol.
6) A hypothetical metal has the simple cubic crystal structure. If its atomic weight is 70.6 g/mol and the atomic radius is 0.128 nm, compute its theoretical density. (N=6.022 * 1023 atoms/mol) (Theoretical density-mass of atoms in unit cell/total volume of unit cell) 7) Write down the names of each crystal structure given below.
Chapter 03, Reserve Problem 09: Cubic unit cell Some metal is known to have a cubic unit cell with an edge length of 0.475 nm. In addition, it has a density of 3.82 g/cm3 and an atomic weight of 61.61 g/mol. Indicate the letter of the metal listed in the following table that has these characteristics. Atomic Radius (nm) 0.206 0.336 0.168 0.136 MetalCrystal Structure BCC FCC FCC HCP Chapter 03, Reserve Problem 09: Cubic unit cell Some metal is...
The unit cell for Cr2O3 has hexagonal symmetry with lattice parameters a = 0.4961 nm and c = 1.360 nm. If the density of this material is 5.22 g/cm3, calculate itsatomic packing factor. For this computation, assume ionic radii of 0.062 nm and 0.140 nm, respectively, for Cr3+ and O2-.
A hypothetical metal has the simple cubic crystal structure shown in Figure 3.3. If its atomic weight is 86.6 g/mol and the atomic radius is 0.169 nm, compute its density.
1. Compute the percent ionic character of the interatomic bonds for each of the following compounds: TiO2, ZnTe, Csci, InSb, and MgCl2. Calculate the number of vacancies per cubic meter in iron at 850°C. The energy for vacancy formation is 1.08 eV/atom. The density and atomic weight for Fe are 7.65 g/cm3 and 55.85 g/mol, respectively 3. Molybdenum forms a substitutional solid solution with tungsten. Compute the weight percent of molybdenum that must be added to tungsten to yield an...
7. The atomic weight and atomic radius for a hypothetical BCC alloy are 43.1 g/mol and 0.122 nm respectively. Determine its density.
fig 3.3 Problem 3.11 A hypothetical metal has the simple cubkc crystal structure shown in Egure 3.3. If its atomic weight is 73. 8 g/mol and the atomic radius is 0.147 nm, compute its density 9/cm the tolerance is +/-6% rfi : Figure 3.3 : For the simple cubic crystal : structure, (a) a hard-sphere : unit cell and (b) a reduced i sphere unit cell