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Okay and for that you're gonna get 3.8 four times tend to be negative a power. You're actually gonna have to um the vital in by one times 10 to the 10th power. So in order to convert to pick commoners you're actually going to have to two centimeters. Well we can also solve it using the commoners but it's going to be way harder to do so. Now we are going to have to convert from commoners um two centimeters in order to solve this problem. The problem is 22.42 g per centimeter tube. And also the density of Iranian given to us. That was found by x ray diffraction to be um 300 83.9 the commoners. Problem #16: Aluminum crystallizes in a face-centered cubic unit cell and has an atomic radius of 143 pm.So in this problem we are given that radium Madame crystallizes in a face centered um cubic structure and the edge line of the units. Given that the density of NiO is 6.67 g/cm 3, calculate the length of the edge of its unit cell (in pm). Problem #15: NiO adopts the face-centered-cubic arrangement. The length of the unit cell of NiO is 4.20 Å. Problem #14: Nickel oxide (NiO) crystallizes in the NaCl type of crystal structure. If the radius of the metal atom is 138 pm, what is the most probable identity of the metal. Problem #13: A metal crystallizes in a face-centered cubic structure and has a density of 11.9 g cm -3. Use this length (and the fact that Pt has a face-centered unit cell) to calculate the density of platinum metal in kg/m 3 (Hint: you will need the atomic mass of platinum and Avogadro's number). Problem #12: The unit cell of platinum has a length of 392.0 pm along each side. What is the atomic radius of platinum? (1 Å = 10 -8 cm.) Problem #11: Platinum has a density of 21.45 g/cm 3 and a unit cell side length 'd' of 3.93 Ångstroms. Use these data to calculate a value for Avogadro's Number. Problem #10: Iridium has a face centered cubic unit cell with an edge length of 383.3 pm. What is the center-to-center distance between nearest silver atoms? Problem #9: Metallic silver crystallizes in a face-centered cubic lattice with L as the length of one edge of the unit cube. Problem #8: The density of an unknown metal is 2.64 g/cm 3 and its atomic radius is 0.215 nm. The density of the element is 1.54 g/cm 3. Problem #7: A metal crystallizes in a face-centered cubic lattice. Find the gram-atomic weight of this metal and tentatively identify it. An X-ray diffraction experiment measures the edge of the face-centered cubic unit cell as 4.06 x 10 -10 m. You find the density of the metal to be 11.5 g/cm 3. Problem #6: You are given a small bar of an unknown metal. (a) What is the density of solid krypton? (b) What is the atomic radius of krypton? (c) What is the volume of one krypton atom? Problem #5: Krypton crystallizes with a face-centered cubic unit cell of edge 559 pm. Assuming that calcium has an atomic radius of 197 pm, calculate the density of solid calcium. Problem #4: Calcium has a cubic closest packed structure as a solid. Problem #3: Nickel has a face-centered cubic structure with an edge length of 352.4 picometers. If the density of the metal is 8.908 g/cm 3, what is the unit cell edge length in pm?
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Problem #2: Nickel crystallizes in a face-centered cubic lattice. Calculate the atomic radius of palladium. Problem #1: Palladium crystallizes in a face-centered cubic unit cell. Face-centered cubic problem list Face-centered cubic problem list