size of octahedral hole a =0.414r
r= redius of metal
a=88pm =radius of boron
min. radius of metal r=212.56pm
There is a simple relation between octahedral void and radius of the atom that is,
The radius of atom = 0.732 X radius of octahedral void
So, Radius of octahedral void required = 88 / 0.732 = 120.22 ppm
Nickel has an atomic radius of 124 pm and forms a solid with a cubic closest packed structure. Calculate the density of solid nickel in g/cm3.
An interstitial alloy contains hydrogen in half of the tetrahedral holes of a closest packed metal, M. What is the formula of this alloy? Group of answer choices MH2 MH M2H MH4 M4H
If the atomic radius of a metal that has the face-centered cubic crystal structure is 0.137nm, calculate the volume of its unit cell.
Identify the packing in the figure shown below. body-centered cubic cubic closest packed (face-centered cubic) hexagonal closest packed simple cubic
For a crystalline salt, the anions, X, are cubic close packed; the cations, M, are found in all of the octahedral holes. What is the coordination number of the cation, M? Enter your answer as an integer.
The ideal perovskite (ABO3) structure consists of AOs closest packed layers (ordered Am cations and O2-anions) with B cations in ¼ of the octahedral holes. What pairs of charges are possible for A and B (there is more than one combination of charges)? For each pair, say which cation will likely sit in the closest packed layers and which will likely sit in the holes. Without specific examples of ions (e.g., Ca, Ti+), base your answer around the fact that...
Given Values Atomic Radius (nm) = 0.18 FCC Metal = Silver BCC Metal: = Sodium Temperature (c) = 1127 Metal A = Zinc Equilibrium Number of Vacancies (m^-3) = 7.42E + 23 Temperature for Metal A = 247 Metal B = Calcium If the atomic radius of a metal is the value shown above and it has the face-centered cubic crystal structure, calculate the volume of its unit cell in nm^3 Your Answer = What is the atomic packing factor...
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.
Elemental magnesium crystallizes in a cubic close packed arrangement. The density of magnesium is 1.1 g/cm. What is the atomic radius of Mg in pm? Report your answer to 1 decimal place. 1 pm = 10 cm Answer:
Elemental magnesium crystallizes in a cubic close packed arrangement. The density of magnesium is 6.4 g/cm . What is the atomic radius of Mg in pm? Report your answer to 1 decimal place. 1 pm = 10 cm Answer: