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Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074

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BuyFindarrow_forward

Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074
Textbook Problem

Using the dimensions of the unit cell (Figure 2) and the molar mass of tin, calculate the density of white tin (in g/cm3).

images

Figure 2 A tetragonal unit cell of white tin (β-tin). The tetragonal unit cod has 90° angles at each corner. Two of the three sides are equal in length (583 pm) while the third side is shorter (318 pm) (Note that the lines connecting atoms are not bonds They are meant only to show the spatial relationship of the atoms.)

Interpretation Introduction

Interpretation:

The density of the white tin has to be identified.

Concept introduction:

The density of the unit cell is calculated as follows,

Massvolume = density

Mass = number of moles × molar massNumber of moles = Number of atoms per unit cellAvogadro number 

Explanation

Cube with a two side of white tin is 583 pm, and one side with 318 pm. The conversion of pm to cm is 5.83 × 10-8cm and 3.18 × 10-8cm

  V=(a)3Cube with a two side of white tin is583 pm, and one side 318pmV=(5.83×108cm)2(3.18×10-8cm)V=1.081×10-22cm

  Molar mass of tin is 118.7 gVolume of the unit cell  =1.081×10-22cm3

  Mass = number of moles × molar massNumber of moles = Number of atoms per unit cellAvogadro number Number of moles = 46

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