Chapter 11, Problem 11.12A

Interpretation Introduction

Interpretation:

Calculate the atomic mass of the metal as well as identify the metal. Given that the density of a sample of metal was measured to be $22.67g/c{m}^3$ and an X-ray diffraction experiment measures the edge of a face-centered cubic cell as $383.3pm$.

Concept Introduction: Density of crystalline solid is given by the formula

  $Density=\frac{z\times M}{V\times N_A}$

  Where, z = number of atoms per unit cell

    M = Molar mass of the substance
    V = Volume of the substance

    $N_A$ = Avogadro’s Number = $\text{6}\text{.022 }\times {\text{ 10}}^{23}$