A metallic element crystallizes in a face-centered cubic unit cell with an edge length of 344.68pm, what is the molar mass of this element if it has a density of 41.944 g/cm³ ? (enter your answer as the magnitude of the molar mass in units of g/mol, do not include the units in the text of your answer) 258.58 517.16 103.43 75.021 217.65E-03 216.86 2.12E-07 318

A metallic element crystallizes in a face-centered cubic unit cell with an edge length of 344.68pm, what is the molar mass of this element if it has a density of 41.944 g/cm³ ? (enter your answer as the magnitude of the molar mass in units of g/mol, do not include the units in the text of your answer) 258.58 517.16 103.43 75.021 217.65E-03 216.86 2.12E-07 318

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Many elements crystallize with a unit cell that is hexagonally shaped (6 sided). The calculations of the unit cell dimension are not significantly more complicated than those for cubic unit cells. A hexagonal unit cell is shown below. 3/3 a²c Volume 6 atoms per unit cell The cell dimension "a" is twice the radius (r) of the atom. 2r=a. For most elements the dimension "c" is approximately 1.633x"a". The element cerium (Ce) crystallizes with a Simple Hexagonal unit cell. The density of a cerium is 6.689 g/cm³. Use this information to calculate the metallic radius of cerium in picometers (pm). 1 pm = 1×10-12 meters. You can assume that the dimension c=1.633-a [Note: The theoretical value for the radius may be different from the experimentally determined value. Simply Googling the radius may not yield the correct result] Radius = pm
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Possibilities are 2, 0.33, 6, 7, 0.25, 0.5, 5, 4, 0, 1, 1/8, 3, 8
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