9. Show that Mgo has the sodium chloride crystal structure and calculate the density of Mgo....
Calculate the theoretical density of Mns, given that it has the rock salt crystal structure. You may want to use the table below. The atomic weights for Mn and S are 54.94 g/mol and 32.06 g/mol, respectively. Cation Fe2+ Ni2+ Mg2+ Ionic Radius (nm) Anion Ionic Radius (nm) 0.077 0.140 0.069 S2- 0.184 0.072 0.067 Mn2+ p= g/cm3 the tolerance is +/-2%
NaCl has a rock salt crystal structure with a unit cell edge length of 0.56 nm. The atomic weights of the Na and Cl are 23 and 35.5 g/mol, respectively, and the Avogadro's number is 6.022 x 10“ formula units/mol. (a) Draw a unit cell to show the crystal structure of the NaCl. (b) What is the coordination number of the atoms in this structure? (c) How many Na atoms and Cl atoms in one unit-cell of such a structure?...
13. (13 pts.) Calculated the th below. (Assuming ro-2=0.140 nm. Calculated the theoretical density of Mgo which has a NaCl structure shown ning to 0.140 nm, I'Mg2+ =0.072 nm, Ame=24.305 g/mol, A.-16 g/mol). Show all calculations steps to receive full credit. 1.56x102 hardnes s n=6 1.50 Santa n (Eute) - v NA 2 Mg2+
Material science 2. Barium (Ba) has a BCC crystal structure, a measured density of 3.51 g/cm3, and a lattice parameter of 0.502 nm. If the atomic mass of Ba is 137.33 g/mol calculate (a) the fraction of attice points that contain vacancies, and (b) the total number of vacancies in a cubic meter of Ba.
as soon as possible uestion 2: (16 points) agnesium oxide (Mg0) has the rock salt crystal structure and a ensity of 3.58 g/cm2. The atomic weights of magnesium doxygen are 24.31 g/mol and 16.00 g/mol, respectively. Using the information above, determine the unit cell edge length. etermine the unit cell edge length from the radii in the table below assuming that ns just touch each other along the edges. Ionic Radius (nm) Ionic Radius (nm) Anion Cation Mg2 Fe2 Na...
Calculate the theoretical density, in g/cm3, of an AX compound given the following information. It has a cesium chloride structure (CN=8), the ionic radii of the cation and anion are 0.130 and 0.157 nm, respectively, and the atomic weights of A and X are 74.65 and 16.00 g/mol, respectively.
3.8 Calculate the radius of an iridium atom, given that Ir has an FCC crystal structure, a density of 22.4 g/cm3 , 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.
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.
Consider a face-centered cubic crystal structure that has one atom at each lattice point. The atomic radius, ? is 0.152 nm and the atomic weight, ? is 68.4 g/mol. Assuming the atoms to be hard spheres and touch each other with their nearest neighbor, calculate the mass density.