Sections 12.1 – 12.2 Types of Solids Metallic Solids.

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Presentation transcript:

Sections 12.1 – 12.2 Types of Solids Metallic Solids

Types of Solids and Metallic Solids In these sections… a.Types of Solids b.Unit Cells c.Cubic Unit Cells d.X-Ray Diffraction

Types of Solids: Ionic Molecular Network: crystalline amorphous Metallic Close-packed

More Network Solids diamond Quartz: SiO 2

Counting Atoms in Unit Cells: Inside: 1 Face:½ Edge:¼ Corner:1/8

Unit Cells, Dimensions and Measurements: What percentage of a simple cubic unit cell is filled with atoms?

Unit Cells, Dimensions and Measurements: Ca metal: Face centered cubic unit cell Density = 1.54 g/cm 3 What is the radius of a Ca atom?

Unit Cells, Dimensions and Measurements: U metal: Body centered cubic unit cell Unit cell edge = 343 pm What is the radius of a U atom?

What fraction of a simple cubic unit cell is filled with atoms? What fraction of a face-centered cubic unit cell is filled with atoms?

Determining Crystal Structures: X-Ray Diffraction

X-Ray Diffraction: Determining the distance between planes of atoms X-rays and atoms Orders of diffraction Bragg’s Law

Using X-Ray Diffraction: Bragg’s Law Platinum metal crystallizes in a face-centered cubic lattice with one atom per lattice point. Monochromatic X-radiation from a Mo target has a wavelength of pm. If this radiation is used in a diffraction experiment with a platinum crystal, a second order diffracted beam is observed at a theta value of 10.43°. If the spacing between these planes corresponds to the unit cell length (d = a), what is the d-spacing between the planes that gave rise to this reflection?