Ionic Crystals

Ionic Crystal : 

Ionic Crystal

Ionic Crystals : 

Ionic Crystals Ionic crystals have at least two atoms in their base which are ionized. Charge neutrality demands that the total charge in the base must be zero; so we always need ions with opposing charge. The binding between the ions is mostly electrostatic and rather strong (binding energies around 1000 kJ/mol); it has no directionality.

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Ionic crystals thus can be described as an ensemble of hard spheres which try to occupy a minimum volume while minimizing electrostatic energy at the same time (i.e. having charge neutrality in small volumes, too). There are no free electrons, ionic crystals are insulators.

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Ionic crystals come in simple and more complicated lattice types; the latter is true in particular for oxides which are often counted among ionic crystals. Some prominent lattice types follow

The NaCl Structure : 

The NaCl Structure The lattice is face centered cubic (fcc), with two atoms in the base: one at (0, 0, 0), the other one at (½, 0, 0)

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Many salts and oxides have this structure, e.g. KCl, AgBr, KBr, PbS, ...orMgO, FeO, ...

The CsCl Structure : 

The CsCl Structure The lattice is cubic primitive with two atoms in the base at (0,0,0) and (½, ½, ½). It is a common error to mistake it for a bcc lattice.

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Intermetallic compounds (not necessarily ionic crystals), but also common salts assume this structure; e.g. CsCl, TlJ, ..., or AlNi, CuZn,

The ZnS (or Diamond, or Sphalerite) Structure : 

The ZnS (or Diamond, or Sphalerite) Structure The "zinc blende" lattice is face centered cubic (fcc) with two atoms in the base at (0,0,0) and (¼, ¼, ¼).

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It is not only an important lattice for other ionic crystals like ZnS, which gave it its name, but also the typical lattice of covalently bonded group IV semiconductors (C (diamond form), Si, Ge) or III-V compounds semiconductors (GaAs, GaP, InSb, InP, ..) The ZnS lattice is easily confused with the ZrO2 lattice below.

The CaF2 or ZrO2 Structure : 

The CaF2 or ZrO2 Structure The lattice is face centered cubic (fcc) with three atoms in the base, one kind (the cations) at (0,0,0), and the other two (anions of the same kind) at (¼, ¼, ¼), and (¼, ¾, ¼).

Perovskite Structure : 

Perovskite Structure The lattice is essentially cubic primitive, but may be distorted to some extent and then becomes orthorhombic or worse. It is also known as the BaTiO3 or CaTiO3 lattice and has three different atoms in the base. In the example it would be Ba at (0,0,0), O at (½, ½, ,0) and Ti at (½, ½, ½).

Spinel Structure : 

Spinel Structure The spinel structure (sometimes called garnet structure) is named after the mineral spinel (MgAl2O4); the general composition is AB2O4. It is essentially cubic, with the O - ions forming a fcc lattice. The cations (usually metals) occupy 1/8 of the tetrahedral sites and 1/2 of the octahedral sites and there are 32 O-ions in the unit cell.

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This sounds complicated, but it is not as bad as it could be; look at the drawing. We "simply" have two types of cubic building units inside a big fcc O-ion lattice, filling all 8 octants.

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The spinel structure is very flexible with respect to the cations it can incorporate; there are over 100 known compounds. In particular, the A and B cations can mix! In other words, the composition with respect to one unit cell can be (A8) (B16)O32, or A8 (B8A8)O32 = A(AB)O4 in regular chemical spelling, or (A8/3B16/3) (A16/3B32/3)O32 and so on, with the atoms in the brackets occupying the respective site at random.

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A few examples (in regular chemical symbols) Magnetite; Fe3+( Fe2+ Fe3+)O4 Spinel; Mg2+( Al23+)O4 Chromite; Fe3+(Cr23+)O4 Jacobsite; Fe3+( Mn2+ Fe3+)O4

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The spinel structure is also interesting because it may contain vacancies as regular part of the crystal. For example, if magnetite is slowly oxidized by lying around a couple of billion years, or when rocks cool, Fe2+ will turn into Fe3+ (oxidation, in chemical terms, means you take electrons away).

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If all Fe2+ is converted into Fe3+, charge balance requires a net formula of Fe21,67O32 per unit cell and this means that 2,33 sites must be vacant - we have what is called a defect spinel. In a way, the composition is now Fe21,67Vac2,33O3; having lots of vacancies as an integral part of the structure.

Octahedral Sites : 

Octahedral Sites An octahedral position for an (interstitial) atom is the space in the interstices between 6 regular atoms that form an octahedra. Four regular atoms are positioned in a plane, the other two are in a symmetrical position just above or below. All spheres can be considered to be hard and touching each other.

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The six spheres define a regular octahedra, in its interior there is a defined space for an interstitial atom, bordered by six spheres. Octahedral sites exists in fcc and bcc crystals. The other prominent geometric environment for interstitials is the tetrahedral site.

Tetrahedral Sites : 

Tetrahedral Sites In a tetrahedral site the interstitial is in the center of a tetrahedra forms by four lattice atoms. Three atoms, touching each other, are in plane; the fourth atom sits in the symmetrical position on top. Again, the tetrahedral site has a defined geometry and offers space for an interstitial atom.

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Aidin Nejadsalim Student of Ceramic Engineering Email: eng.a.nejadsalim@gmail.com