Vanadium (V) crystallises in a bcc structure and has an atomic radius of 131 pm. Determine the density if the edge length of the bcc unit cell is 4r/v3 and the atomic mass is 50.94 g/mol. (NA = 6.022×1023 mol-1) A. 3.06 g/cm³ B. 6.11 g/cm³ C. 2.77 g/cm³ D. 12.2 g/cm3 F. 8.46 a/cm³

Vanadium (V) crystallises in a bcc structure and has an atomic radius of 131 pm. Determine the density if the edge length of the bcc unit cell is 4r/v3 and the atomic mass is 50.94 g/mol. (NA = 6.022×1023 mol-1) A. 3.06 g/cm³ B. 6.11 g/cm³ C. 2.77 g/cm³ D. 12.2 g/cm3 F. 8.46 a/cm³

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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Concept explainers

Crystal Lattices and Unit Cell

Consider a crystal. The regular and repeating pattern of constituent particles is the most distinguishing feature of crystalline solids. A crystal lattice is formed when these particles are replaced with representative points. The three-dimensional arrangement of constituent particles is known as a crystal lattice. Unit cell is that the smallest portion of a space lattice which when repeated in several directions, generate the whole lattice. Unit cell is a building block of a lattice. It is the smallest unit of cell.

Question

Vanadium (V) crystallises in a bCC
structure and has an atomic radius of 131 pm. Determine
the density if the edge length of the bcc unit cell is 4r/V3 and
the atomic mass is 50.94 g/mol. (N = 6.022x1023 mol-1)
A. 3.06 g/cm³
B. 6.11 g/cm3
C. 2.77 g/cm3
D. 12.2 g/cm3
F. 8.46 a/cm3

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