Name: crystalline and amorphous solid patterns
Uploaded: 2020-09-24T15:06:49.000Z
Duration: 2 min 22 s
Channel: JoVE

K12 Standards

Pennsylvania State Academic Standards

9-12

Physical Science

Structure and Properties of Matter

3.2.9-12.B

Structures of Solids

Solids are classified as either amorphous or crystalline on the basis of their three-dimensional internal structure.
Amorphous solids like fused silica glass lack an ordered internal arrangement of their constituent particles, whereas crystalline solids like quartz have their constituent particles arranged in a repeating three-dimensional pattern throughout the solid. 
The structure of a crystalline solid is represented by a unit cell, which is the smallest repeating unit of the crystalline structure that retains the symmetry of the structure.
The overall three-dimensional pattern is known as a crystal lattice, which is composed of lattice points and lattice vectors. The lattice vectors delineate the edges of the unit cell, and the lattice points may be at the corners, on the faces, or at the center of the unit cell.
Lattice systems are defined by the dimensions of the unit cell. There are 7 types of lattice systems: cubic, tetragonal, orthorhombic, rhombohedral, monoclinic, triclinic, and hexagonal.
The positions of the atoms in a unit cell are not necessarily the same as those of the lattice points. The pattern of atoms in the unit cell, or motif, is often defined in terms of the

structures of solids

Solids in which the atoms, ions, or molecules are arranged in a definite repeating pattern are known as crystalline solids. Metals and ionic compounds typically form ordered, crystalline solids. A crystalline solid has a precise melting temperature because each atom or molecule of the same type is held in place with the same forces or energy. Amorphous solids or non-crystalline solids (or, sometimes, glasses) which lack an ordered internal structure and are randomly arranged. Substances that consist of large molecules, or a mixture of molecules whose movements are more restricted, often form amorphous solids. Amorphous material undergoes gradual softening, over a range of temperatures, due to the structural non-equivalence of the molecules. When an amorphous material is heated, the weakest intermolecular attractions break first. As the temperature is increased further, the stronger attractions are broken.
Unit Cell
The structure of a crystalline solid is best described by its simplest repeating unit, referred to as its unit cell. The unit cell consists of lattice points that represent the locations of atoms or ions. The entire structure then consists of this unit cell repeating in three dimensions, as illustrated in Figure 1.
<img alt="Crystallography diagram showing atomic lattice structure, illustrating cubic crystal arrangement." src="/files/ftp_upload/11353/11353_Image1.png" style="text-align: center; height: 275px;" data-altupdatedat="1761830439000" data-alt="Image1" />
Figure 1. Unit cell and crystal lattice with lattice points indicated in red.
In general, a unit cell is defined by the lengths of three axes (a, b, and c) and the angles (&#945;, &#946;, and &#947;) between them as shown in Figure 2. The axes are defined as being the lengths between points in the space lattice.
<img alt="Hexagonal crystal structure diagram, angles &#945;, &#946;, and &#947;; lattice arrangement concept." src="/files/ftp_upload/11353/11353_Image_2.png" style="text-align: center; height: 175px;" data-altupdatedat="1761830439000" data-alt="Image2" />
Figure 2. Unit cell is defined by its axes (a, b, and c), and angles (&#945;, &#946;, and &#947;)
There are seven different lattice systems, some of which have more than one type of lattice, for a total of fourteen different unit cells.
<table style="margin-left: auto; margin-right: auto;">
	<tbody>
		<tr>
			<td style="color: black; border: 1px solid black; text-align: center;">Systems</td>
			<td style="color: black; border: 1px solid black; text-align: center;">Angles</td>
			<td style="color: black; border: 1px solid black; text-align: center;">Axes</td>
		</tr>
		<tr>
			<td style="color: black; border: 1px solid black; text-align: center;">Cubic</td>
			<td style="color: black; border: 1px solid black; text-align: center;">&#945; = &#946; = &#947; = 90&#176;</td>
			<td style="color: black; border: 1px solid black; text-align: center;"> a = b = c </td>
		</tr>
		<tr>
			<td style="color: black; border: 1px solid black; text-align: center;">Tetragonal</td>
			<td style="color: black; border: 1px solid black; text-align: center;">&#945; = &#946; = &#947; = 90&#176;</td>
			<td style="color: black; border: 1px solid black; text-align: center;">a = b &#8800; c</td>
		</tr>
		<tr>
			<td style="color: black; border: 1px solid black; text-align: center;"> Orthorhombic </td>
			<td style="color: black; border: 1px solid black; text-align: center;">&#945;= &#946; = &#947; = 90&#176;</td>
			<td style="color: black; border: 1px solid black; text-align: center;">a &#8800; b &#8800; c</td>
		</tr>
		<tr>
			<td style="color: black; border: 1px solid black; text-align: center;">Monoclinic</td>
			<td style="color: black; border: 1px solid black; text-align: center;"> &#945; = &#947; = 90&#176;; &#946; &#8800; 90&#176; </td>
			<td style="color: black; border: 1px solid black; text-align: center;">a &#8800; b &#8800; c</td>
		</tr>
		<tr>
			<td style="color: black; border: 1px solid black; text-align: center;">Triclinic</td>
			<td style="color: black; border: 1px solid black; text-align: center;">&#945; &#8800; &#946; &#8800; &#947; &#8800; 90&#176;</td>
			<td style="color: black; border: 1px solid black; text-align: center;">a &#8800; b &#8800; c</td>
		</tr>
	</tbody>
</table>

This text is adapted from <a href="https://openstax.org/books/chemistry-2e/pages/10-5-the-solid-state-of-matter">Openstax, Chemistry 2e, Section 10.6: Lattice Structures in Crystalline Solids.</a>

Solids in which the atoms, ions, or molecules are arranged in a definite repeating pattern are known as crystalline solids. Metals and ionic compounds ...

Education

JoVE Core

Chemistry

Liquids, Solids, and Intermolecular Forces

KEY TERMS AND CONCEPTS

crystalline and amorphous solid patterns

Crystalline and amorphous solids differ in how their particles are arranged. In crystalline solids, atoms, ions, or molecules follow a definite repeating pattern. Metals and ionic compounds typically form these ordered solids. Because the same particles are held in place by the same forces or energy, crystalline solids have a precise melting temperature.

Amorphous solids, also called non-crystalline solids or glasses, do not have an ordered internal structure. Their particles are arranged randomly. These solids often form from large molecules or from mixtures of molecules whose movement is more limited. When heated, amorphous materials soften gradually over a range of temperatures. This happens because the molecules are not all the same, so the weakest intermolecular attractions break first and stronger attractions break as the temperature rises.

The structure of a crystalline solid is described by its smallest repeating unit, called a unit cell. A unit cell contains lattice points, which mark the locations of atoms or ions. The whole crystal is built by repeating this unit cell in three dimensions. The unit cell is defined by the lengths of three axes, a, b, and c, and by the angles between them, α, β, and γ.

There are seven lattice systems, and some have more than one lattice type. Together, these make fourteen different unit cells. The cubic system has α = β = γ = 90° and a = b = c. Tetragonal has α = β = γ = 90° and a = b ≠ c. Orthorhombic has α = β = γ = 90° and a ≠ b ≠ c. Monoclinic has α = γ = 90° but β ≠ 90°, with a ≠ b ≠ c. Triclinic has α ≠ β ≠ γ ≠ 90° and a ≠ b ≠ c.

Crystalline and Amorphous Solid Patterns

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Crystalline and amorphous solids differ in how their particles are arranged. In crystalline solids, atoms, ions, or molecules follow a definite repeating pattern. Metals and ionic compounds typically form these ordered solids. Because the same particles are held in place by the same forces or energy, crystalline solids have a precise melting temperature. Amorphous solids, also called non-crystalline solids or glasses, do not have an ordered internal structure. Their particles are arranged...

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Crystalline and Amorphous Solid Patterns | JoVE K12

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Atomic Structure

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3.2.9-12.A

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3.2.9-12.H

Students who demonstrate understanding can communicate scientific and technical information about why the molecular-level structure is important in the functioning of designed materials. Clarifying Statement: Emphasis is on the attractive and repulsive forces that determine the functioning of the material. Examples could include why electrically conductive materials are often made of metal, flexible but durable materials are made up of long chained molecules, and pharmaceuticals are designed to interact with specific receptors. Assessment Boundry: Assessment is limited to provided molecular structures of specific designed materials.

Crystalline and Amorphous Solid Patterns

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