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Ch.12 - Solids and Modern Material
Tro - Chemistry: A Molecular Approach 4th Edition
Tro4th EditionChemistry: A Molecular ApproachISBN: 9780134112831Non è quello che usi tu?Cambia libro di testo
Tutti i libri di testoTro 4th EditionCh.12 - Solids and Modern MaterialProblema 83
Capitolo 12, Problema 83

An unknown metal is found to have a density of 7.8748 g/cm3 and to crystallize in a body-centered cubic lattice. The edge of the unit cell is 0.28664 nm. Calculate the atomic mass of the metal.

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Convert the edge length of the unit cell from nanometers to centimeters by using the conversion factor: 1 nm = 1 x 10^{-7} cm.
Calculate the volume of the unit cell using the formula for the volume of a cube: V = a^3, where 'a' is the edge length in centimeters.
Determine the mass of the unit cell by multiplying the volume of the unit cell by the density of the metal: mass = density x volume.
In a body-centered cubic (BCC) lattice, there are 2 atoms per unit cell. Use this information to find the mass of a single atom by dividing the mass of the unit cell by 2.
Calculate the atomic mass of the metal by converting the mass of a single atom from grams to atomic mass units (amu) using the conversion factor: 1 amu = 1.66053906660 x 10^{-24} g.

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Density and its Calculation

Density is defined as mass per unit volume, typically expressed in grams per cubic centimeter (g/cm³). To calculate the density of a substance, one can use the formula: density = mass/volume. In this context, knowing the density of the metal allows us to relate it to the atomic mass and the volume of the unit cell.
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Density Concepts

Body-Centered Cubic (BCC) Lattice

A body-centered cubic lattice is a type of crystal structure where atoms are located at each corner of a cube and one atom is positioned at the center of the cube. This arrangement affects the packing efficiency and the volume occupied by the atoms, which is crucial for calculating the atomic mass based on the unit cell dimensions.
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Body Centered Cubic Example

Unit Cell Volume and Atomic Mass Relationship

The volume of a unit cell can be calculated using the edge length of the cube, raised to the third power (V = a³). In a BCC structure, there are two atoms per unit cell, and the relationship between the mass of the atoms, the density, and the volume of the unit cell can be used to derive the atomic mass of the metal using the formula: atomic mass = (density × unit cell volume) / number of atoms per unit cell.
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Atomic Mass
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