4. Calculate the atomic radius (in Å) of the following element: tantalum, body-centered cubic, density is...
Tantalum (Ta) crystalizes in a body centered cubic unit cell and has a density of 16.68 g/cm3 . Calculate the edge length and radius (in pm).
A certain element exists in a face-centered cubic structure. The atomic radius of an atom of this element is 155 pm. Calculate the density of this element in g/cm3. (Assume the element has a molar mass of 55.8 g/mol.) g/cm3
A certain element exists in a face-centered cubic structure. The atomic radius of an atom of this element is 121 pm. Calculate the density of this element in g/cm3. (Assume the element has a molar mass of 64.2 g/mol.) g/cm3
A certain element exists in a face-centered cubic structure. The atomic radius of an atom of this element is 143 pm. Calculate the density of this element in g/cm3. (Assume the element has a molar mass of 62.6 g/mol.) ________ g/cm3
A certain element exists in a face-centered cubic structure. The atomic radius of an atom of this element is 121 pm. Calculate the density of this element in g/cm3. (Assume the element has a molar mass of 59.3 g/mol.)
The element W has bcc packing with a body-centered cubic unit cell. The density of tungsten is 19.3 g/cm3 and the cell volume is 3.170 x 10-23 mL. Calculate the value of Avogadro's number to three significant figures based on these data. The element xenon has ccp packing with a face-centered cubic unit cell. The density of Xe is 3.78 g/cm3. Calculate the volume (m3) of the unit cell of xenon.
Sodium crystallizes in the body-centered cubic structure with a = 4.24 Å. Calculate the theoretical density of Na.
Metals with body‑centered cubic (bcc) structures, such as tantalum, are not closely packed. If they were to change to a cubic close‑packed (ccp) structure (under pressure, for instance), their densities would be greater. What would the density of tantalum be if its structure were ccp rather than bcc? Its actual density is 16.7 g⋅cm−316.7 g⋅cm−3 .
An element forms a body-centered cubic crystalline substance. The edge length of the unit cell is 287 pm and the density of the crystal is 7.92 g/cm3. Calculate the atomic weight of the substance. A. 63.5 amu O B. 48.0 amu C.56.4 amu OD. 45.0 amu
9. Hypothesize why a compound would adopt a body-centered cubic unit cell when it crystallizes versus a face-centered cubic. 10. Calculate the edge length of a simple cubic unit cell composed of polonium atoms. The atomic radius of polonium is 167 pm. 11. Calculate the density in g/cm3 of platinum if the atomic radius is 139 pm and it forms a face- centered unit cell.