   Chapter 12.6, Problem 1.3ACP

Chapter
Section
Textbook Problem

The lithium unit cell is a cube with sides of 351 pm. Use this information, and a knowledge of unit cells, to calculate the density of lithium metal.

Interpretation Introduction

Interpretation:

The density of the lithium metal has to be calculated.

Concept introduction:

The density of the unit cell is calculated as follows,

Massvolume = density

The radius of the atom is calculated using following formula,

V=(a)3

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

Explanation

Cube with a side of lithium is 351 pm. The conversion of pm to 3.51 × 10-8

V=(a)3V=(3.51×108cm)3V=4.324×10-23cm

Molar mass of lithium is 6.941 g

Molar mass of lithium is 6.941Volume of the unit cell  =4.324×10-23cm3

Mass = number of moles × molar massNumber of moles = Number of atoms per unit cellAvogadro number Number of moles = 26

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