1 Structures and Properties of Orthodontic Materials

1 Structures and Properties of Orthodontic Materials

William A. Brantley

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Schematic illustration of an edge dislocation in a crystalline material

Introduction

Interatomic Bonding and Atomic Arrangement

Modes of Interatomic Bonding

Atomic Arrangements for Metallic Materials

Atomic Arrangements for Ceramic Materials

Atomic Arrangements for Polymeric Materials

Properties of Orthodontic Materials

Property Areas of Importance for Orthodontic Materials

Mechanical Property Concepts for Orthodontic Materials

Surface Property Concepts for Orthodontic Materials

Structures of Orthodontic Materials

Metallic Materials

Ceramic Materials

Polymeric Materials

References

Introduction

Knowledge of fundamental principles governing the relationships between compositions, structures and properties is central to an understanding of orthodontic materials. Because wide arrays of metallic, ceramic, and polymeric materials are used in the profession, and new materials are continuously being introduced, it is essential that the scientific basis for the selection and proper use of materials for clinical practice be thoroughly understood.

The general plan of this chapter is to develop these concepts following the standard basic approach that has historically been used in engineering materials science. First, the different modes of interatomic bonding will be described, followed by a description of how these modes of bonding lead to the atomic arrangements found in the metallic, ceramic, and polymeric materials. Second, terminology will be presented to describe the clinically relevant properties of these orthodontic materials. After these foundations have been acquired, the linkages between the structures and properties of these materials can readily be understood.

It is expected that graduate students in orthodontic programs, as well as practicing orthodontists, will already have been exposed to many of these concepts in an introductory biomaterials course or a series of lectures that are found in the predoctoral dental school curriculum. Because of the very wide scope of the subject matter involved, it is not possible in a single chapter to fully develop all of the topics germane to the structure-property relationships of orthodontic materials. The reader is referred to the excellent textbooks on dental materials science and engineering materials science listed at the end of this chapter for further information.

Interatomic Bonding and Atomic Arrangement

Modes of Interatomic Bonding

Traditionally, textbooks on dental materials science have subdivided the modes of interatomic bonding into two major categories: chemical bonding and physical bonding. Chemical bonding involves the valence electrons of atoms that participate in chemical reactions and includes the three modes of covalent, ionic, and metallic bonding. Physical bonding, also known as ver der Waals bonding, occurs between atoms or molecules with closed electronic shells.

Covalent bonding involves the sharing of valence electrons, such as that which occurs for carbon-carbon bonding in polymer chains. Another example is the sharing of valence electrons between silicon and oxygen to form SiO2. In both of these examples, after the sharing of valence electrons the atoms have the closed shell or noble gas electron configurations. The strongest covalent bonding occurs with the carbon atoms in diamond, where each of the four valence electrons (two 2s and two 2p) for a given carbon atom is shared with a valence electron of an adjacent carbon atom in a hybridized sp3 arrangement. Covalent bonding is highly directional, and materials dominated by covalent bonding typically have relatively open structures and low densities, and also lack the ability to undergo permanent deformation except at high temperatures.

Ionic bonding involves a transfer of valence electrons, such as that which occurs between sodium and chlorine atoms to form the NaCl molecule. The sodium atom has a single 3s electron in the M shell and the chlorine atom has a single 3p vacancy in the M shell (Table 1.1). Transfer of the valence electron from the sodium to the chlorine atom allows both atom species to have the closed shell noble gas configuration, and the bonding arises from the strong electrostatic attraction between the resulting positive and negative ions. Because of the symmetric electron charge distributions around the ions, ionic bonding is not directional. Materials dominated by ionic bonding tend to have higher densities than materials dominated by covalent bonding.

Generally, materials that are dominated by covalent or ionic bonding should be considered to have a mixture of both modes of interatomic bonding. Pauling developed an empirical concept, in which the fractional ionic bonding character for simple materials consisting of two different atomic species is related to the difference in electronegativity of the two atoms. The electronegativity for a given atom is approximately proportional to the sum of the ionization potential and the electron affinity. For example, from a plot of the electro-negativities for the different atoms, it can be estimated that the fractional ionic character is 0.52 and 0.63 for SiO2 and Al2O3, respectively.

Table 1.1 Electronic configurations for some atoms
    Element Atomic Number Electronic Configuration
    C 6 1s22s22p2
    O 8 1s22s22p4
    Na 11 1s22s22p63s1
    Al 13 1s22s22p63s23p1
    Si 14 1s22s22p63s23p2
    Cl 17 1s22s22p63s23p5
    Ti 22 1s22s22p63s23p63d24s2
    Cr 24 1s22s22p63s23p63d54s1
    Fe 26 1s22s22p63s23p63d64s2
    Co 27 1s22s22p63s23p63d74s2
    Ni 28 1s22s22p63s23p63d84s2
    Cu 29 1s22s22p63s23p63d104s1
    Ag 47 1s22s22p63s23p63d104s24p64d105s1

    Au

79

1s22s22p63s23p63d104s24p64d104f145s25p65d106s1

In metals the valence electrons are loosely bound and can be considered to form a gas that permeates the atomic arrangement of the resulting ionic cores, in contrast to the localization of valence electrons around parent atoms for covalent and ionic bonding. Metallic bonding is nondirectional on the atomic scale, and the metallic atoms form arrangements leading to materials of high density. Table 1.1 shows the electronic configurations for the atoms of some metals that are found in orthodontic and restorative alloys. The valence electrons that are lost in forming the cations from these metals are obvious. Many of the metals listed in Table 1.1 are transition elements, in which the outermost subshells (4s, 5s, 6s or 7s) are filled before the interior subshells. Transition metals frequently have multiple valences and are important for orthodontic and restorative alloys.

Physical interatomic bonding occurs with symmetric atoms (noble gas atoms) or molecules, such as methane (CH4), where weak dispersive forces arise from fluctuations in the electronic charge distribution. This bonding mode can have significance for the adhesion between different materials where a polymeric material is involved. The other type of physical bonding occurs with asymmetric molecules having permanent dipole moments, such as water (H2O), where strong electrostatic forces exist between the positive and negative centers of charge.

Atomic Arrangements for Metallic Materials

In general, materials can be subdivided into two categories according to their atomic arrangements. In crystalline materials there is a three-dimensional periodic pattern of the atoms, whereas no such long-range periodicity is present in noncrystalline materials, which possess only short-range atomic order.

It is appropriate to first consider the pure metals, which have the simplest compositions (a single element) and atomic arrangements. Except for extraordinary conditions of preparation (solidification from the liquid state or condensation from the vapor state under extremely rapid conditions) that are not applicable to dental alloys, metals always have crystalline structures. There are seven crystal systems (cubic, tetragonal, orthorhombic, rhombohedral [trigonal], hexagonal, monoclinic, and triclinic), with lattice parameters as summarized in Table 1.2. The corresponding fourteen space lattices (Bravais lattices) are listed in Table 1.3. Inherently, a space lattice is a geometric construct wherin each point has identical surroundings. Crystal structures of real materials are based upon space lattices, where there is a single atom or a group of atoms at each space lattice point.

Table 1.2 The seven crystal systems
    System Axial Lengths Axial Angles
    Cubic a = b = c α = β = γ = 90°
    Tetragonal a = b ≠ c α = β = γ = 90°
    Orthorhombic a ≠ b ≠ c α = β = γ = 90°
    Rhombohedral a = b = c α = β = γ ≠ 90°
    Hexagonal a1 = a2 = a3 ≠ c α1 = α2 = α3 = 120°; γ = 90°
    Monoclinic a ≠ b ≠ c α = γ = 90° ≠ β

    Triclinic

a ≠ b ≠ c

α ≠ β ≠ γ ≠ 90°

The axial lengths (a, b and c) are the atomic repeat distances or lattice parameters along the three crystallographic axes, except for the hexagonal system where the axial lengths (a1, a2 and a3) in the basal plane are used.

For crystal systems other than hexagonal, the axial angle α is the angle between the b and c axes, and the β and γ angles have analogous definitions. In some textbooks the rhombohedral system is referred to as the trigonal system.

The three identical axial angles in the basal plane of the hexagonal system are designated α1, α2, and α3. γ is the angle between each of the three axes in the basal plane and the axis in the c-direction

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Fig. 1.1 Unit cells for the simple cubic (A), body-centered cubic (B), face-centered cubic (C), and hexagonal close-packed (D) structures. (Adapted from Anusavice, 1996)

It is most convenient to visualize the crystal structures of metals in terms of their unit cells, where a unit cell is the smallest portion that can be repeated in three dimensions to produce the crystal structure. Figure 1.1 shows the unit cells of the important body-centered cubic (bcc), face-centered cubic (fcc), and hexagonal close-packed (hcp) structures for metals in dentistry. For comparison, the unit cell for the simple cubic structure is also shown. The hcp structure can be considered as formed from two interpenetrating simple hexagonal structures. Important pure metals found in orthodontic alloys for archwires (Chapter 4) and brackets (Chapter 7) that have these crystal structures are as follows:

    fcc Fe (above ~ 910 °C), Ni
    bcc Fe (below ~ 910 °C and above ~ 1400 °C), Cr, Ti (above ~ 880 °C)
    hcp Co, Ti (below ~ 880 °C).

It can be seen that, while nickel and chromium have the fcc and bcc structures, respectively, at all temperatures below their melting points, iron and titanium have crystal structures that depend upon temperature. For example, titanium has the hcp α structure from room temperature up to ~ 880 °C, where there is a transformation to the bcc β structure. At room temperature iron has the bcc α structure and transforms to the fcc γ structure at ~ 910 °C. The different crystal structures of a given metal (or other crystalline material) are termed polymorphic or allotropic forms. Cobalt ordinarily has the hcp α structure but can also exist in an fcc β polymorphic form.

Table 1.3 The fourteen space (Bravais) lattices
    Crystal System Space Lattice

    Cubic

Simple cubic

Body-centered cubic

Face-centered cubic

    Tetragonal

Simple tetragonal

Body-centered tetragonal

    Orthorhombic

Simple orthorhombic

Body-centered orthorhombic

Face-centered orthorhombic

Base-centered orthorhombic

    Rhombohedral (Trigonal)

Simple rhombohedral

    Hexagonal

Simple hexagonal

    Monoclinic

Simple monoclinic

Base-centered monoclinic

    Triclinic

Simple triclinic

In textbooks on crystallography, the term simple is by the term primitive

Atomic Arrangements for Ceramic Materials

Ceramics, which consist of more than one atomic species, can have crystalline or noncrystalline structures, depending upon the material and sometimes the mode of preparation. Important ceramics for orthodontic applications are aluminum oxide (alumina) and zirconium oxide (zirconia), which are used as bracket materials (Chapter 7). Other ceramics are found in the powder portions of cements (Chapter 11). Silicon dioxide (silica) is an important filler in composite restorative resins.

The crystal structure of aluminum oxide is illustrative of the principles involved with ceramics having substantial ionic bonding character. The crystal structure consists of a nearly hcp arrangement of the larger oxygen anions (O2−), with the smaller aluminum cations (Al3+) located in two-thirds of the octahedral interstitial sites in the hcp structure (Fig. 1.2). The layers in the structure provide the maximum separation of the Al3+ ions. These octahedral sites have six-fold coordination, i.e., each aluminum ion is surrounded by six oxygen ions. The crystal structure is determined by the ratio of the radii of the aluminum and oxygen ions and the requirement of an electrically neutral unit cell. The crystal structure of zirconia at room temperature consists of a distorted simple cubic (monoclinic) arrangement of the oxygen ions, with the zirconium cations (Zr4+) located in half of the available sites (eightfold coordination), similar to Figure 1.3.

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Fig. 1.2 Structure of alumina.
(From Kingery et al, 1976)

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Fig. 1.3 Structure of calcium fluorite (CaF2), which is similar to the structure of zirconia. (From Kingery et al, 1976)

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Fig. 1.4 Structure of cristobalite. (From Greener et al, 1972)

Silica is principally found in dental materials (investments, composite resins, and elastomeric impression materials) in the crystalline quartz or cristobalite polymorphic forms or as the glassy form of vitreous silica. Moreover, both cristobalite and quartz have high-temperature (the more stable form) and low-temperature polymorphic forms. The basic unit in the structure of SiO2 is the SiO4 tetrahedron, where the small Si4+ cation is bonded to four much larger O2− anions in a tetrahedral arrangement. The high-temperature form of cristobalite (Fig. 1.4) has a diamond cubic (the structure for the diamond form of carbon) arrangement of the SiO4 tetrahedra. The high-temperature form of quartz has a complex structure consisting of connected chains of SiO4 tetrahedra. A schematic illustration of the structure of crystalline SiO2 in two dimensions in provided in Figure 1.5.

The structure of fused or vitreous silica has the short-range order of the silicon and oxygen ions shown in Figure 1.5 but lacks the long-range periodicity found in crystalline materials. For feldspathic dental porcelain, where glass-modifying or fluxing oxides such as Na2O, K2O, and CaO are added to SiO2, the Na+, K+, and Ca2+ ions disrupt the three-dimensional silicate framework structure. Nonbridging oxygen ions that do not connect Si4+ ions are created by these large cations, which are situated in open spaces in the structure (Fig. 1.6).

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Fig. 1.5 Two-dimensional illustration of the structure of quartz. (From Kingery et al, 1976)

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Fig. 1.6 Structure of feldspathic dental porcelain, showing typical locations of glass-modifying cations and nonbridging oxygen ions. (From Kingery et al, 1976)

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Fig. 1.7 General structure of a urethane group (OCONH) formed by the reaction of a diol and a diisocyanate. (From Anusavice, 1996)

Atomic Arrangements for Polymeric Materials

A variety of polymeric materials are used in orthodontics, such as elastomeric impression materials (Chapter 12) and polyurethane modules for tooth movement (Chapter 8), adhesive cements for bonding brackets to enamel (Chapter 10), and polycarbonate brackets (Chapter 7). All of these polymeric materials are based upon macromolecules with varying compositions, molecular weights, and degrees of cross-linking. The general structures of a polyurethane elastomer for tooth movement and an alginate impression material are shown in Figures 1.7 and 1.8, respectively. The polymers have predominantly noncrystalline structures without long-range periodicity. Illustrations of important structural components for adhesive resins will be shown in Chapter 10. Information on the structure of polymeric materials is presented in references listed at the end of this chapter.

The elastomeric materials are lightly cross-linked and undergo a glass transition below room temperature. Below the glass transition temperature, the elastomers are relatively rigid, whereas above the glass transition temperature these materials become highly flexible with thermal activation of the polymeric backbones and side chains. The elastomers also typically contain a second phase of polymer crystallites, which undergo melting at temperatures above the glass transition temperature. In contrast, the polycarbonate material used for brackets is highly cross-linked and relatively rigid, although these brackets are subject to problematic deformation under the clinical loading imposed by archwires.

Mechanisms for permanent deformation of polymeric materials include chain stretching, slippage between adjacent chains, and chain scission. There is no mechanism on the molecular level in the noncrystalline orthodontic polymers that is analogous to the dislocation motion or twinning that occur in crystalline metals. Consequently, the cross-linked adhesive resins and the polycarbonate brackets fail in a brittle manner, although slow, time-dependent creep deformation under static loads may be possible. Under normal loading conditions, these brittle polymers will fail by propagation of cracks from microstructural flaws, analogously to the situation for ceramics.

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Fig. 1.8 Schematic polymer structure of alginate impression material in which sodium alginate molecules have cross-linked to form calcium alginate (Chapter 12). (From Anusavice, 1996)

Properties of Orthodontic Materials

Property Areas of Importance for Orthodontic Materials

The clinically important property areas for orthodontic materials include mechanical and surface properties for a variety of materials, and the corrosion properties for archwire alloys. The purpose of this section is to introduce property terminology that will be germane to the subject matter presented in subsequent sections of this chapter and that will provide a background for understanding the properties of the different types of orthodontic materials discussed in Chapters 4 to 15.

While thermal and optical properties are highly important for restorative dental materials, these areas have been omitted from this section. Little work has been reported on the roles of thermal properties for orthodontic materials, and the importance of optical properties for the clinical performance of ceramic orthodontic brackets will be discussed in Chapter 7.

Mechanical Property Concepts for Orthodontic Materials

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Jan 1, 2015 | Posted by in Dental Materials | Comments Off on 1 Structures and Properties of Orthodontic Materials
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