Chapter 12.6, Problem 1.3ACP

### Chemistry & Chemical Reactivity

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

Chapter
Section

### Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074
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 351Â pm. The conversion of pm to 3.51Â Ã—Â 10-8

Â Â Vâ€‰=â€‰(a)3V=â€‰(3.51Ã—10âˆ’8cm)3V=â€‰4.324â€‰Ã—â€‰10-23â€‰cm

Molar mass of lithium is 6.941 g

Â Â MolarÂ massÂ ofÂ lithiumÂ isÂ 6.941VolumeÂ ofÂ theÂ unitÂ cellÂ Â =â€‹â€‰4.324â€‰Ã—â€‰10-23â€‰cm3

Â Â MassÂ =Â numberÂ ofÂ molesÂ Ã—Â molarÂ massNumberÂ ofÂ molesÂ =Â NumberÂ ofÂ atomsÂ perÂ unitÂ cellAvogadroÂ numberÂ NumberÂ ofÂ molesÂ =Â 26

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