A body-centered cubic unit cell has a volume of 2.17×10−23 cm3 . Find the radius of the atom in pm.
Determine the edge length of the unit cell:
[cube root of] 2.583 x 10¯23 cm3 = 2.789 x 10¯8 cm
We wish to determine the value of 4r, from which we will obtain r, the radius of the atom. Using the Pythagorean Theorem, we can find:
d2 + (d√2)2 = (4r)2
3d2 = (4r)2
3(2.789 x 10¯8 cm)2 = 16r2
r = 1.207 x 10¯8 cm
Radius of the atom = 120.777 pm
A body-centered cubic unit cell has a volume of 2.17×10−23 cm3 . Find the radius of...
A body-centered unit cell has a volume of 4.32×10−23 cm3 .Find the radius of the atom in pm. (1m = 1 x 102 cm = 10 12 pm)
1)Molybdenum crystallizes with a body-centered unit cell. The radius of a molybdenum atom is 136 pm . Part A Calculate the edge length of the unit cell of molybdenum . Part B Calculate the density of molybdenum . 2)An atom has a radius of 135 pm and crystallizes in the body-centered cubic unit cell. Part A What is the volume of the unit cell in cm3?
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).
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.
Iron crystallizes with a body-centered cubic unit cell. The radius of a iron atom is 126 pm. Calculate the density of solid crystalline iron in grams per cubic centimeter.
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.
Strontium has density of 2.64 g/cm3 and crystallizes with the face-centered cubic unit cell. Calculate the radius of a strontium atom in units of picometers. Enter your answer numerically, to three significant figures, and in terms of pm.
Chromium crystallizes with a body-centered cubic unit cell. The radius of a chromium atom is 125 pm . Calculate the density of solid crystalline chromium in grams per cubic centimeter. Express the density in grams per cubic centimeter to three significant figures.
Aluminum crystallizes with a face-centered-cubic unit cell. The radius of an Al atom is 143 pm. Calculate the density of solid crystalline Al in g/cm3.
A metal (FW 307.1 g/mol) crystallises into a body-centered cubic unit cell and has a radius of 2.40 Angstrom. What is the density of this metal in g/cm3? Enter to 2 decimal places.