{"id":80,"date":"2021-09-16T19:28:28","date_gmt":"2021-09-16T19:28:28","guid":{"rendered":"https:\/\/pressbooks.ccconline.org\/physicalgeology\/chapter\/2-4-silicate-minerals-physical-geology-2nd-edition\/"},"modified":"2021-09-16T19:42:58","modified_gmt":"2021-09-16T19:42:58","slug":"2-4-silicate-minerals-physical-geology-2nd-edition","status":"publish","type":"chapter","link":"https:\/\/pressbooks.ccconline.org\/physicalgeology\/chapter\/2-4-silicate-minerals-physical-geology-2nd-edition\/","title":{"raw":"2.4 Silicate Minerals -- Physical Geology – 2nd Edition","rendered":"2.4 Silicate Minerals — Physical Geology – 2nd Edition"},"content":{"raw":"\n\n
[1]<\/sup><\/a>). Because of this size similarity, and because they are both divalent cations (both can have a charge of +2), iron and magnesium can readily substitute for each other in olivine and in many other minerals.<\/p>\n
Table 2.6 Silicate mineral configurations. The triangles represent silica tetrahedra.<\/caption>
[Skip Table]<\/a><\/td> <\/tr>
Tetrahedron Configuration Picture<\/th> Tetrahedron Configuration Name<\/th> Example Minerals<\/th> <\/tr> <\/thead>
 \"One<\/a><\/td> Isolated (nesosilicates)<\/td> Olivine, garnet, zircon, kyanite<\/td> <\/tr>
\"Two<\/a><\/td> Pairs (sorosilicates)<\/td> Epidote, zoisite<\/td> <\/tr>
 \"Six<\/a><\/td> Rings (cyclosilicates)<\/td> Tourmaline<\/td> <\/tr>
\"Five<\/a><\/td> Single chains (inosilicates)<\/td> Pyroxenes, wollastonite<\/td> <\/tr>
 \"Two<\/a><\/td> Double chains (inosilicates)<\/td> Amphiboles<\/td> <\/tr>
 \"Multiple<\/a><\/td> Sheets (phyllosilicates)<\/td> Micas, clay minerals, serpentine, chlorite<\/td> <\/tr>
3-dimensional structure<\/td> Framework (tectosilicates)<\/td> Feldspars, quartz, zeolite<\/td> <\/tr> <\/tbody> <\/table>\n
\n
\n
\n

\n \"\"\n <\/p>\n

Cut around the outside of the shape (solid lines and dotted lines), and then fold along the solid lines to form a tetrahedron. If you have glue or tape, secure the tabs to the tetrahedron to hold it together. If you don\u2019t have glue or tape, make a slice along the thin grey line and insert the pointed tab into the slit.<\/p>\n

If you are doing this in a classroom, try joining your tetrahedron with others into pairs, rings, single and double chains, sheets, and even three-dimensional frameworks.<\/p>\n

See Appendix 3 for Exercise 2.3 answers<\/a>.<\/p>\n <\/div>\n <\/div>\n

In olivine, unlike most other silicate minerals, the silica tetrahedra are not bonded to each other. Instead they are bonded to the iron and\/or magnesium ions, in the configuration shown on Figure 2.4.1.<\/p>\n

\n \"\"\n
Figure 2.4.1 A depiction of the structure of olivine as seen from above. The formula for this particular olivine, which has three Fe ions for each Mg ion, could be written: Mg0.5<\/sub>Fe1.5<\/sub>SiO4<\/sub>.<\/div>\n <\/div>\n

As already noted, the 2 ions of iron and magnesium are similar in size (although not quite the same). This allows them to substitute for each other in some silicate minerals. In fact, the ions that are common in silicate minerals have a wide range of sizes, as depicted in Figure 2.4.2. All of the ions shown are cations, except for oxygen. Note that iron can exist as both a +2 ion (if it loses two electrons during ionization) or a +3 ion (if it loses three). Fe2+ <\/sup> is known as ferrous<\/span><\/strong> iron. Fe3+ <\/sup> is known as ferric<\/span><\/strong> iron. Ionic radii are critical to the composition of silicate minerals, so we\u2019ll be referring to this diagram again.<\/a><\/p>\n

\n \"\"\n
Figure 2.4.2 The ionic radii (effective sizes) in angstroms, of some of the common ions in silicate minerals. [Image Description]<\/a><\/div>\n <\/div>\n

The structure of the single-chain silicate pyroxene is shown on Figures 2.4.3 and 2.4.4. In pyroxene<\/span><\/strong>, silica tetrahedra are linked together in a single chain, where one oxygen ion from each tetrahedron is shared with the adjacent tetrahedron, hence there are fewer oxygens in the structure. The result is that the oxygen-to-silicon ratio is lower than in olivine (3:1 instead of 4:1), and the net charge per silicon atom is less (\u22122 instead of \u22124).  Therefore, fewer cations are necessary to balance that charge. Pyroxene compositions are of the type MgSiO3<\/sub>, FeSiO3<\/sub>, and CaSiO3<\/sub>, or some combination of these. Pyroxene can also be written as (Mg,Fe,Ca)SiO3<\/sub>, where the elements in the brackets can be present in any proportion. In other words, pyroxene has one cation for each silica tetrahedron (e.g., MgSiO3<\/sub>) while olivine has two (e.g., Mg2<\/sub>SiO4<\/sub>). Because each silicon ion is +4 and each oxygen ion is \u22122, the three oxygens (\u22126) and the one silicon (+4) give a net charge of \u22122 for the single chain of silica tetrahedra. In pyroxene, the one divalent cation (2) per tetrahedron balances that \u22122 charge. In olivine, it takes two divalent cations to balance the \u22124 charge of an isolated tetrahedron.The structure of pyroxene is more \u201cpermissive\u201d than that of olivine\u2014meaning that cations with a wider range of ionic radii can fit into it. That\u2019s why pyroxenes can have iron (radius 0.63 \u00c5) or magnesium (radius 0.72 \u00c5) or calcium (radius 1.00 \u00c5) cations (see Figure 2.4.2 above).<\/p>\n

\n \n \"Three\n <\/a>\n
Figure 2.4.3 A depiction of the structure of pyroxene. The tetrahedral chains continue to left and right and each is interspersed with a series of divalent cations. If these are Mg ions, then the formula is MgSiO3<\/sub>.<\/div>\n <\/div>\n
\n \n \"""\"\n <\/a>\n
Figure 2.4.4 A single silica tetrahedron (left) with four oxygen ions per silicon ion (SiO4<\/sub>). Part of a single chain of tetrahedra (right), where the oxygen atoms at the adjoining corners are shared between two tetrahedra (arrows). For a very long chain the resulting ratio of silicon to oxygen is 1 to 3 (SiO3<\/sub>).<\/div>\n <\/div>\n <\/div>\n
\n
\n

The diagram below represents a single chain in a silicate mineral. Count the number of tetrahedra versus the number of oxygen ions (yellow spheres). Each tetrahedron has one silicon ion so this should give you the ratio of Si to O in single-chain silicates (e.g., pyroxene).<\/p>\n

\n \n \"A\n <\/a>\n <\/p>\n

The diagram below represents a double chain in a silicate mineral. Again, count the number of tetrahedra versus the number of oxygen ions. This should give you the ratio of Si to O in double-chain silicates (e.g., amphibole).<\/p>\n

\n \n \"A\n <\/a>\n <\/p>\n

See Appendix 3 for Exercise 2.4 answers<\/a>.<\/p>\n <\/div>\n <\/div>\n

\n

In amphibole<\/span><\/strong> structures, the silica tetrahedra are linked in a double chain that has an oxygen-to-silicon ratio lower than that of pyroxene, and hence still fewer cations are necessary to balance the charge. Amphibole is even more permissive than pyroxene and its compositions can be very complex. Hornblende, for example, can include sodium, potassium, calcium, magnesium, iron, aluminum, silicon, oxygen, fluorine, and the hydroxyl ion (OH\u2212<\/sup>).<\/p>\n <\/div>\n

In mica<\/span><\/strong> structures, the silica tetrahedra are arranged in continuous sheets, where each tetrahedron shares three oxygen anions with adjacent tetrahedra. There is even more sharing of oxygens between adjacent tetrahedra and hence fewer cations are needed to balance the charge of the silica-tetrahedra structure in sheet silicate minerals. Bonding between sheets is relatively weak, and this accounts for the well-developed one-directional cleavage in micas (Figure 2.4.5). Biotite<\/span><\/strong> mica can have iron and\/or magnesium in it and that makes it a ferromagnesian<\/span><\/strong> silicate mineral (like olivine, pyroxene, and amphibole). Chlorite<\/span><\/strong> is another similar mineral that commonly includes magnesium. In muscovite<\/span><\/strong> mica, the only cations present are aluminum and potassium; hence it is a non-ferromagnesian silicate mineral.<\/p>\n

\n \"\"\n
Figure 2.4.5 Biotite mica (left) and muscovite mica (right). Both are sheet silicates and split easily into thin layers along planes parallel to the sheets. Biotite is dark like the other iron- and\/or magnesium-bearing silicates (e.g., olivine, pyroxene, and amphibole), while muscovite is light coloured. (Each sample is about 3 cm across.)<\/div>\n <\/div>\n

Apart from muscovite, biotite, and chlorite, there are many other sheet silicates<\/span><\/strong> (a.k.a. phyllosilicates<\/span><\/strong>), many of which exist as clay-sized fragments (i.e., less than 0.004 millimetres). These include the clay minerals kaolinite<\/span><\/strong>, illite<\/span><\/strong>, and smectite<\/span><\/strong>, and although they are difficult to study because of their very small size, they are extremely important components of rocks and especially of soils.<\/p>\n

All of the sheet silicate minerals also have water molecules within their structure.<\/p>\n

Silica tetrahedra are bonded in three-dimensional frameworks in both the feldspars<\/span><\/strong> and quartz<\/span><\/strong>. These are non-ferromagnesian minerals<\/span><\/strong>\u2014they don\u2019t contain any iron or magnesium. In addition to silica tetrahedra, feldspars include the cations aluminum, potassium, sodium, and calcium in various combinations. Quartz contains only silica tetrahedra.<\/p>\n

The three main feldspar<\/span><\/strong> minerals are potassium feldspar<\/span><\/strong>, (a.k.a. K-feldspar or K-spar) and two types of plagioclase feldspar: albite<\/span><\/strong> (sodium only) and anorthite<\/span><\/strong> (calcium only). As is the case for iron and magnesium in olivine, there is a continuous range of compositions (solid solution series) between albite and anorthite in plagioclase. Because the calcium and sodium ions are almost identical in size (1.00 \u00c5 versus 0.99 \u00c5) any intermediate compositions between CaAl2<\/sub>Si3<\/sub>O8<\/sub> and NaAlSi3<\/sub>O8<\/sub> can exist (Figure 2.4.6). This is a little bit surprising because, although they are very similar in size, calcium and sodium ions don\u2019t have the same charge (Ca2+<\/sup> versus Na+<\/sup> ). This problem is accounted for by the corresponding substitution of Al+3 <\/sup> for Si+4 <\/sup>. Therefore, albite is NaAlSi3<\/sub>O8<\/sub> (1 Al and 3 Si) while anorthite is CaAl2<\/sub>Si2<\/sub>O8<\/sub> (2 Al and 2 Si), and plagioclase feldspars of intermediate composition have intermediate proportions of Al and Si. This is called a \u201ccoupled-substitution.\u201d<\/p>\n

The intermediate-composition plagioclase feldspars are oligoclase (10% to 30% Ca), andesine (30% to 50% Ca), labradorite (50% to 70% Ca), and bytownite (70% to 90% Ca). K-feldspar <\/span><\/strong>(KAlSi3<\/sub>O8<\/sub>) has a slightly different structure than that of plagioclase, owing to the larger size of the potassium ion (1.37 \u00c5) and because of this large size, potassium and sodium do not readily substitute for each other, except at high temperatures. These high-temperature feldspars are likely to be found only in volcanic rocks because intrusive igneous rocks cool slowly enough to low temperatures for the feldspars to change into one of the lower-temperature forms.<\/p>\n

\n \"\"\n
Figure 2.4.6 Compositions of the feldspar minerals.<\/div>\n <\/div>\n

In quartz <\/span><\/strong>(SiO2<\/sub>),<\/strong> the silica tetrahedra are bonded in a \u201cperfect\u201d three-dimensional framework. Each tetrahedron is bonded to four other tetrahedra (with an oxygen shared at every corner of each tetrahedron), and as a result, the ratio of silicon to oxygen is 1:2. Since the one silicon cation has a +4 charge and the two oxygen anions each have a \u22122 charge, the charge is balanced. There is no need for aluminum or any of the other cations such as sodium or potassium. The hardness and lack of cleavage in quartz result from the strong covalent\/ionic bonds characteristic of the silica tetrahedron.<\/p>\n

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\n

Silicate minerals are classified as being either ferromagnesian or non-ferromagnesian depending on whether or not they have iron (Fe) and\/or magnesium (Mg) in their formula. A number of minerals and their formulas are listed below. For each one, indicate whether or not it is a ferromagnesian silicate<\/em>.<\/p>\n
Mineral<\/strong><\/td> Formula<\/strong><\/td> Ferromagnesian silicate?<\/strong><\/td> <\/tr>
olivine<\/td> (Mg,Fe)2<\/sub>SiO4<\/sub><\/td> .<\/td> <\/tr>
pyrite<\/td> FeS2<\/sub><\/td> .<\/td> <\/tr>
plagioclase feldspar<\/td> CaAl2<\/sub>Si2<\/sub>O8<\/sub><\/td> .<\/td> <\/tr>
pyroxene<\/td> MgSiO3<\/sub><\/td> .<\/td> <\/tr>
hematite<\/td> Fe2<\/sub>O3<\/sub><\/td> .<\/td> <\/tr>
orthoclase feldspar<\/td> KAlSi3<\/sub>O8<\/sub><\/td> .<\/td> <\/tr>
quartz<\/td> SiO2<\/sub><\/td> .<\/td> <\/tr>
amphibole<\/td> Fe7<\/sub>Si8<\/sub>O22<\/sub>(OH)2<\/sub><\/td> .<\/td> <\/tr>
muscovite<\/td> K2<\/sub>Al4<\/sub>Si6<\/sub>Al2<\/sub>O20<\/sub>(OH)4<\/sub><\/td> .<\/td> <\/tr>
magnetite<\/td> Fe3<\/sub>O4<\/sub><\/td> .<\/td> <\/tr>
biotite<\/td> K2<\/sub>Fe4<\/sub>Al2<\/sub>Si6<\/sub>Al4<\/sub>O20<\/sub>(OH)4<\/sub><\/td> .<\/td> <\/tr>
dolomite<\/td> (Ca,Mg)CO3<\/sub><\/td> .<\/td> <\/tr>
garnet<\/td> Fe2<\/sub>Al2<\/sub>Si3<\/sub>O12<\/sub><\/td> .<\/td> <\/tr>
serpentine<\/td> Mg3<\/sub>Si2<\/sub>O5<\/sub>(OH)4<\/sub><\/td> .<\/td> <\/tr> <\/tbody> <\/table>\n


See Appendix 3 for Exercise 2.5 answers<\/a>.*Some of the formulas, especially the more complicated ones, have been simplified.<\/p>\n <\/div>\n <\/div>\n

Image Descriptions<\/h3>\n
Figure 2.4.2 image description: The ionic radii of elements in angstroms and their charges.<\/a><\/caption>
Element<\/th> Ionic Radii (in angstroms)<\/th> Charge<\/th> <\/tr> <\/thead>
Oxygen<\/td> 1.4<\/td> \u22122 (Anion)<\/td> <\/tr>
Potassium<\/td> 1.37<\/td> 1 (Cation)<\/td> <\/tr>
Calcium<\/td> 1.00<\/td> 2 (Cation)<\/td> <\/tr>
Sodium<\/td> 0.99<\/td> 1 (Cation)<\/td> <\/tr>
Magnesium<\/td> 0.72<\/td> 2 (Cation)<\/td> <\/tr>
Iron<\/td> 0.63<\/td> 2 (Cation)<\/td> <\/tr>
0.49<\/td> 3 (Cation)<\/td> <\/tr>
Aluminum<\/td> 0.39<\/td> 3 (Cation)<\/td> <\/tr>
Silicon<\/td> 0.26<\/td> 4 (Cation)<\/td> <\/tr>
Carbon<\/td> 0.15<\/td> 4 (Cation)<\/td> <\/tr> <\/tbody> <\/table>\n

\n [Return to Figure 2.4.2]<\/a>\n <\/p>\n

\n
\n
    \n
  1. An angstrom is the unit commonly used for the expression of atomic-scale dimensions. One angstrom is 10\u221210<\/sup> metres or 0.0000000001 metres. The symbol for an angstrom is \u00c5. \u21b5<\/a>
    <\/li>\n <\/ol>\n <\/div>\n <!-- pb_fixme -->\n<\/div>\n<\/div>
    \n <!-- pb_fixme -->\n <!-- pb_fixme -->\n<\/div>\n<\/div>\n","rendered":"
    \n
    [1]<\/sup>). Because of this size similarity, and because they are both divalent cations (both can have a charge of +2), iron and magnesium can readily substitute for each other in olivine and in many other minerals.<\/p>\n\n\n\n\n\n\n\n\n\n\n\n\n
    Table 2.6 Silicate mineral configurations. The triangles represent silica tetrahedra.<\/caption>\n
    [Skip Table]<\/a><\/td>\n<\/tr>\n
    Tetrahedron Configuration Picture<\/th>\nTetrahedron Configuration Name<\/th>\nExample Minerals<\/th>\n<\/tr>\n<\/thead>\n
     \"One<\/a><\/td>\nIsolated (nesosilicates)<\/td>\nOlivine, garnet, zircon, kyanite<\/td>\n<\/tr>\n
    \"Two<\/a><\/td>\nPairs (sorosilicates)<\/td>\nEpidote, zoisite<\/td>\n<\/tr>\n
     \"Six<\/a><\/td>\nRings (cyclosilicates)<\/td>\nTourmaline<\/td>\n<\/tr>\n
    \"Five<\/a><\/td>\nSingle chains (inosilicates)<\/td>\nPyroxenes, wollastonite<\/td>\n<\/tr>\n
     \"Two<\/a><\/td>\nDouble chains (inosilicates)<\/td>\nAmphiboles<\/td>\n<\/tr>\n
     \"Multiple<\/a><\/td>\nSheets (phyllosilicates)<\/td>\nMicas, clay minerals, serpentine, chlorite<\/td>\n<\/tr>\n
    3-dimensional structure<\/td>\nFramework (tectosilicates)<\/td>\nFeldspars, quartz, zeolite<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n
    \n
    \n
    \n

    \n \"\"\n <\/p>\n

    Cut around the outside of the shape (solid lines and dotted lines), and then fold along the solid lines to form a tetrahedron. If you have glue or tape, secure the tabs to the tetrahedron to hold it together. If you don\u2019t have glue or tape, make a slice along the thin grey line and insert the pointed tab into the slit.<\/p>\n

    If you are doing this in a classroom, try joining your tetrahedron with others into pairs, rings, single and double chains, sheets, and even three-dimensional frameworks.<\/p>\n

    See Appendix 3 for Exercise 2.3 answers<\/a>.<\/p>\n<\/p><\/div>\n<\/p><\/div>\n

    In olivine, unlike most other silicate minerals, the silica tetrahedra are not bonded to each other. Instead they are bonded to the iron and\/or magnesium ions, in the configuration shown on Figure 2.4.1.<\/p>\n

    \n \"\"<\/p>\n
    Figure 2.4.1 A depiction of the structure of olivine as seen from above. The formula for this particular olivine, which has three Fe ions for each Mg ion, could be written: Mg0.5<\/sub>Fe1.5<\/sub>SiO4<\/sub>.<\/div>\n<\/p><\/div>\n

    As already noted, the 2 ions of iron and magnesium are similar in size (although not quite the same). This allows them to substitute for each other in some silicate minerals. In fact, the ions that are common in silicate minerals have a wide range of sizes, as depicted in Figure 2.4.2. All of the ions shown are cations, except for oxygen. Note that iron can exist as both a +2 ion (if it loses two electrons during ionization) or a +3 ion (if it loses three). Fe2+ <\/sup> is known as ferrous<\/span><\/strong> iron. Fe3+ <\/sup> is known as ferric<\/span><\/strong> iron. Ionic radii are critical to the composition of silicate minerals, so we\u2019ll be referring to this diagram again.<\/a><\/p>\n

    \n \"\"<\/p>\n
    Figure 2.4.2 The ionic radii (effective sizes) in angstroms, of some of the common ions in silicate minerals. [Image Description]<\/a><\/div>\n<\/p><\/div>\n

    The structure of the single-chain silicate pyroxene is shown on Figures 2.4.3 and 2.4.4. In pyroxene<\/span><\/strong>, silica tetrahedra are linked together in a single chain, where one oxygen ion from each tetrahedron is shared with the adjacent tetrahedron, hence there are fewer oxygens in the structure. The result is that the oxygen-to-silicon ratio is lower than in olivine (3:1 instead of 4:1), and the net charge per silicon atom is less (\u22122 instead of \u22124).  Therefore, fewer cations are necessary to balance that charge. Pyroxene compositions are of the type MgSiO3<\/sub>, FeSiO3<\/sub>, and CaSiO3<\/sub>, or some combination of these. Pyroxene can also be written as (Mg,Fe,Ca)SiO3<\/sub>, where the elements in the brackets can be present in any proportion. In other words, pyroxene has one cation for each silica tetrahedron (e.g., MgSiO3<\/sub>) while olivine has two (e.g., Mg2<\/sub>SiO4<\/sub>). Because each silicon ion is +4 and each oxygen ion is \u22122, the three oxygens (\u22126) and the one silicon (+4) give a net charge of \u22122 for the single chain of silica tetrahedra. In pyroxene, the one divalent cation (2) per tetrahedron balances that \u22122 charge. In olivine, it takes two divalent cations to balance the \u22124 charge of an isolated tetrahedron.The structure of pyroxene is more \u201cpermissive\u201d than that of olivine\u2014meaning that cations with a wider range of ionic radii can fit into it. That\u2019s why pyroxenes can have iron (radius 0.63 \u00c5) or magnesium (radius 0.72 \u00c5) or calcium (radius 1.00 \u00c5) cations (see Figure 2.4.2 above).<\/p>\n

    \n
    \n \"Three
    \n <\/a><\/p>\n
    Figure 2.4.3 A depiction of the structure of pyroxene. The tetrahedral chains continue to left and right and each is interspersed with a series of divalent cations. If these are Mg ions, then the formula is MgSiO3<\/sub>.<\/div>\n<\/p><\/div>\n
    \n
    \n \"""\"
    \n <\/a><\/p>\n
    Figure 2.4.4 A single silica tetrahedron (left) with four oxygen ions per silicon ion (SiO4<\/sub>). Part of a single chain of tetrahedra (right), where the oxygen atoms at the adjoining corners are shared between two tetrahedra (arrows). For a very long chain the resulting ratio of silicon to oxygen is 1 to 3 (SiO3<\/sub>).<\/div>\n<\/p><\/div>\n<\/p><\/div>\n
    \n
    \n

    The diagram below represents a single chain in a silicate mineral. Count the number of tetrahedra versus the number of oxygen ions (yellow spheres). Each tetrahedron has one silicon ion so this should give you the ratio of Si to O in single-chain silicates (e.g., pyroxene).<\/p>\n

    \n
    \n \"A
    \n <\/a>\n <\/p>\n

    The diagram below represents a double chain in a silicate mineral. Again, count the number of tetrahedra versus the number of oxygen ions. This should give you the ratio of Si to O in double-chain silicates (e.g., amphibole).<\/p>\n

    \n
    \n \"A
    \n <\/a>\n <\/p>\n

    See Appendix 3 for Exercise 2.4 answers<\/a>.<\/p>\n<\/p><\/div>\n<\/p><\/div>\n

    \n

    In amphibole<\/span><\/strong> structures, the silica tetrahedra are linked in a double chain that has an oxygen-to-silicon ratio lower than that of pyroxene, and hence still fewer cations are necessary to balance the charge. Amphibole is even more permissive than pyroxene and its compositions can be very complex. Hornblende, for example, can include sodium, potassium, calcium, magnesium, iron, aluminum, silicon, oxygen, fluorine, and the hydroxyl ion (OH\u2212<\/sup>).<\/p>\n<\/p><\/div>\n

    In mica<\/span><\/strong> structures, the silica tetrahedra are arranged in continuous sheets, where each tetrahedron shares three oxygen anions with adjacent tetrahedra. There is even more sharing of oxygens between adjacent tetrahedra and hence fewer cations are needed to balance the charge of the silica-tetrahedra structure in sheet silicate minerals. Bonding between sheets is relatively weak, and this accounts for the well-developed one-directional cleavage in micas (Figure 2.4.5). Biotite<\/span><\/strong> mica can have iron and\/or magnesium in it and that makes it a ferromagnesian<\/span><\/strong> silicate mineral (like olivine, pyroxene, and amphibole). Chlorite<\/span><\/strong> is another similar mineral that commonly includes magnesium. In muscovite<\/span><\/strong> mica, the only cations present are aluminum and potassium; hence it is a non-ferromagnesian silicate mineral.<\/p>\n

    \n \"\"<\/p>\n
    Figure 2.4.5 Biotite mica (left) and muscovite mica (right). Both are sheet silicates and split easily into thin layers along planes parallel to the sheets. Biotite is dark like the other iron- and\/or magnesium-bearing silicates (e.g., olivine, pyroxene, and amphibole), while muscovite is light coloured. (Each sample is about 3 cm across.)<\/div>\n<\/p><\/div>\n

    Apart from muscovite, biotite, and chlorite, there are many other sheet silicates<\/span><\/strong> (a.k.a. phyllosilicates<\/span><\/strong>), many of which exist as clay-sized fragments (i.e., less than 0.004 millimetres). These include the clay minerals kaolinite<\/span><\/strong>, illite<\/span><\/strong>, and smectite<\/span><\/strong>, and although they are difficult to study because of their very small size, they are extremely important components of rocks and especially of soils.<\/p>\n

    All of the sheet silicate minerals also have water molecules within their structure.<\/p>\n

    Silica tetrahedra are bonded in three-dimensional frameworks in both the feldspars<\/span><\/strong> and quartz<\/span><\/strong>. These are non-ferromagnesian minerals<\/span><\/strong>\u2014they don\u2019t contain any iron or magnesium. In addition to silica tetrahedra, feldspars include the cations aluminum, potassium, sodium, and calcium in various combinations. Quartz contains only silica tetrahedra.<\/p>\n

    The three main feldspar<\/span><\/strong> minerals are potassium feldspar<\/span><\/strong>, (a.k.a. K-feldspar or K-spar) and two types of plagioclase feldspar: albite<\/span><\/strong> (sodium only) and anorthite<\/span><\/strong> (calcium only). As is the case for iron and magnesium in olivine, there is a continuous range of compositions (solid solution series) between albite and anorthite in plagioclase. Because the calcium and sodium ions are almost identical in size (1.00 \u00c5 versus 0.99 \u00c5) any intermediate compositions between CaAl2<\/sub>Si3<\/sub>O8<\/sub> and NaAlSi3<\/sub>O8<\/sub> can exist (Figure 2.4.6). This is a little bit surprising because, although they are very similar in size, calcium and sodium ions don\u2019t have the same charge (Ca2+<\/sup> versus Na+<\/sup> ). This problem is accounted for by the corresponding substitution of Al+3 <\/sup> for Si+4 <\/sup>. Therefore, albite is NaAlSi3<\/sub>O8<\/sub> (1 Al and 3 Si) while anorthite is CaAl2<\/sub>Si2<\/sub>O8<\/sub> (2 Al and 2 Si), and plagioclase feldspars of intermediate composition have intermediate proportions of Al and Si. This is called a \u201ccoupled-substitution.\u201d<\/p>\n

    The intermediate-composition plagioclase feldspars are oligoclase (10% to 30% Ca), andesine (30% to 50% Ca), labradorite (50% to 70% Ca), and bytownite (70% to 90% Ca). K-feldspar <\/span><\/strong>(KAlSi3<\/sub>O8<\/sub>) has a slightly different structure than that of plagioclase, owing to the larger size of the potassium ion (1.37 \u00c5) and because of this large size, potassium and sodium do not readily substitute for each other, except at high temperatures. These high-temperature feldspars are likely to be found only in volcanic rocks because intrusive igneous rocks cool slowly enough to low temperatures for the feldspars to change into one of the lower-temperature forms.<\/p>\n

    \n \"\"<\/p>\n
    Figure 2.4.6 Compositions of the feldspar minerals.<\/div>\n<\/p><\/div>\n

    In quartz <\/span><\/strong>(SiO2<\/sub>),<\/strong> the silica tetrahedra are bonded in a \u201cperfect\u201d three-dimensional framework. Each tetrahedron is bonded to four other tetrahedra (with an oxygen shared at every corner of each tetrahedron), and as a result, the ratio of silicon to oxygen is 1:2. Since the one silicon cation has a +4 charge and the two oxygen anions each have a \u22122 charge, the charge is balanced. There is no need for aluminum or any of the other cations such as sodium or potassium. The hardness and lack of cleavage in quartz result from the strong covalent\/ionic bonds characteristic of the silica tetrahedron.<\/p>\n

    \n
    \n

    Silicate minerals are classified as being either ferromagnesian or non-ferromagnesian depending on whether or not they have iron (Fe) and\/or magnesium (Mg) in their formula. A number of minerals and their formulas are listed below. For each one, indicate whether or not it is a ferromagnesian silicate<\/em>.<\/p>\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n
    Mineral<\/strong><\/td>\nFormula<\/strong><\/td>\nFerromagnesian silicate?<\/strong><\/td>\n<\/tr>\n
    olivine<\/td>\n(Mg,Fe)2<\/sub>SiO4<\/sub><\/td>\n.<\/td>\n<\/tr>\n
    pyrite<\/td>\nFeS2<\/sub><\/td>\n.<\/td>\n<\/tr>\n
    plagioclase feldspar<\/td>\nCaAl2<\/sub>Si2<\/sub>O8<\/sub><\/td>\n.<\/td>\n<\/tr>\n
    pyroxene<\/td>\nMgSiO3<\/sub><\/td>\n.<\/td>\n<\/tr>\n
    hematite<\/td>\nFe2<\/sub>O3<\/sub><\/td>\n.<\/td>\n<\/tr>\n
    orthoclase feldspar<\/td>\nKAlSi3<\/sub>O8<\/sub><\/td>\n.<\/td>\n<\/tr>\n
    quartz<\/td>\nSiO2<\/sub><\/td>\n.<\/td>\n<\/tr>\n
    amphibole<\/td>\nFe7<\/sub>Si8<\/sub>O22<\/sub>(OH)2<\/sub><\/td>\n.<\/td>\n<\/tr>\n
    muscovite<\/td>\nK2<\/sub>Al4<\/sub>Si6<\/sub>Al2<\/sub>O20<\/sub>(OH)4<\/sub><\/td>\n.<\/td>\n<\/tr>\n
    magnetite<\/td>\nFe3<\/sub>O4<\/sub><\/td>\n.<\/td>\n<\/tr>\n
    biotite<\/td>\nK2<\/sub>Fe4<\/sub>Al2<\/sub>Si6<\/sub>Al4<\/sub>O20<\/sub>(OH)4<\/sub><\/td>\n.<\/td>\n<\/tr>\n
    dolomite<\/td>\n(Ca,Mg)CO3<\/sub><\/td>\n.<\/td>\n<\/tr>\n
    garnet<\/td>\nFe2<\/sub>Al2<\/sub>Si3<\/sub>O12<\/sub><\/td>\n.<\/td>\n<\/tr>\n
    serpentine<\/td>\nMg3<\/sub>Si2<\/sub>O5<\/sub>(OH)4<\/sub><\/td>\n.<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n

    See Appendix 3 for Exercise 2.5 answers<\/a>.*Some of the formulas, especially the more complicated ones, have been simplified.<\/p>\n<\/p><\/div>\n<\/p><\/div>\n

    Image Descriptions<\/h3>\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n
    Figure 2.4.2 image description: The ionic radii of elements in angstroms and their charges.<\/a><\/caption>\n
    Element<\/th>\nIonic Radii (in angstroms)<\/th>\nCharge<\/th>\n<\/tr>\n<\/thead>\n
    Oxygen<\/td>\n1.4<\/td>\n\u22122 (Anion)<\/td>\n<\/tr>\n
    Potassium<\/td>\n1.37<\/td>\n1 (Cation)<\/td>\n<\/tr>\n
    Calcium<\/td>\n1.00<\/td>\n2 (Cation)<\/td>\n<\/tr>\n
    Sodium<\/td>\n0.99<\/td>\n1 (Cation)<\/td>\n<\/tr>\n
    Magnesium<\/td>\n0.72<\/td>\n2 (Cation)<\/td>\n<\/tr>\n
    Iron<\/td>\n0.63<\/td>\n2 (Cation)<\/td>\n<\/tr>\n
    0.49<\/td>\n3 (Cation)<\/td>\n<\/tr>\n
    Aluminum<\/td>\n0.39<\/td>\n3 (Cation)<\/td>\n<\/tr>\n
    Silicon<\/td>\n0.26<\/td>\n4 (Cation)<\/td>\n<\/tr>\n
    Carbon<\/td>\n0.15<\/td>\n4 (Cation)<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n

    \n [Return to Figure 2.4.2]<\/a>\n <\/p>\n

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      \n
    1. An angstrom is the unit commonly used for the expression of atomic-scale dimensions. One angstrom is 10\u221210<\/sup> metres or 0.0000000001 metres. The symbol for an angstrom is \u00c5. \u21b5<\/a>
      <\/li>\n<\/ol><\/div>\n

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