Many minerals do not melt uniformly. Instead they decompose as they melt. One example is potassium feldspar (KAlSi3O8) which decomposes on melting to leucite (KAlSi2O6) plus liquid. Another is forsterite (Mg2SiO4), which decomposes to enstatite (MgSiO3) plus liquid.
Both forsterite and leucite are chemically incompatible with quartz. They would react with quartz as follows:
However, this doesn't mean that potassium feldspar (KAlSi3O8) decomposes on melting to leucite (KAlSi2O6) plus quartz liquid. What actually happens is that most of the potassium feldspar melts but the rest converts to leucite. The melt actually contains appreciable potassium feldspar.
This page assumes you are reasonably familiar with the behavior of simple eutectic systems.
|Let's consider the system forsterite-enstatite-quartz. We
|Let's read the fields as they are now. We can identify four possibilities, labeled by A-D.|
|Sketching in the liquidus curves, we can infer they look pretty much as at left. Things like actual melting points and the location of the quartz-enstatite eutectic, of course, have to be determined experimentally. The one major remaining question is what happens between the Fo+Liq and the En+Liq fields?|
|Figuring out the rest works best if we start from the bottom. If we melt a mixture of enstatite plus a little quartz (at the bottom of zone B), we will get enstatite plus liquid. The solid enstatite will coexist with the liquid until we reach the conversion temperature, at which point it should convert to forsterite plus liquid. Thus we expect a boundary along the conversion temperature of enstatite as shown. Above that line there can be no enstatite.|
|We can divide this diagram into four zones as shown. The history of a melt in each is different.|
|In Zone A we go from melt to melt + forsterite to solid
enstatite plus forsterite. This is pretty similar to a eutectic with one twist.
Note that as the liquid cools, it can actually become more silica rich than enstatite itself. Once it does, it is actually chemically incompatible with forsterite and when the melt reaches the solidification temperature of enstatite, forsterite reacts with the melt to form enstatite. This actually happens in real igneous rocks and is why Bowen's Series is called Bowen's Reaction Series. Many rocks show signs that early-formed crystals dissolved in their own magma.
We can verify that forsterite actually decreases from the diagram. Assume we begin with 100 grams of melt. When the melt and solid reach d, we can see that about 2/3 of the melt has solidified (67 grams). But when the solid entirely solidifies (equals the original system composition), we see that the system is about 50 per cent each. Thus the final system has 50 grams of forsterite, a loss of 17 grams. We might conjecture (correctly, it turns out) that if the system has the compostion of pure enstatite, the forsterite will disappear entirely.
|This zone has the most complex history of all. We go from melt
to forsterite plus melt to enstatite plus melt to solid enstatite plus quartz. Therefore
we must form forsterite, then lose it completely.
But that's not the end of the story. The solid has not reached the initial system composition yet and there must still be some melt present (about 20% judging from the diagram). Between f and the original system composition (open square d), both adjacent fields contain liquid. Therefore the system cannot completely solidify by moving directly right from f. The only way the system can solidify completely is to move down to a field where everything is solid: the enstatite + quartz field.
The only solid that can form now is enstatite. The solid composition moves down the vertical enstatite line, and the melt moves down the liquidus to the eutectic, where quartz begins to form. The history is like that of Zone C, shown below.
In reality this is a quite narrow zone out in the middle of the diagram, thus this sequence of evolution is uncommon. Also it lies far from both forsterite and quartz in composition, so the amounts of quartz and forsterite that can form are fairly small. It may happen that the olivine doesn't react completely with the melt before being rimmed by enstatite. When that happens the forsterite is isolated from the melt and may persist when the rock solidifies. Thus on rare occasions we do find rocks with both olivine and quartz, but they are not in direct physical contact.
In extreme cases of magmatic segregation, we could start with a very mafic magma (Zone A), and form a great deal of forsterite which sinks to the bottom of the magma chamber. That would have the effect of resetting the system composition equal to that of the melt, because the segregated olivine is effectively removed from the system. The system could now be in zone B. Thus we could easily (and do) end up with a layered igneous complex with olivine-bearing rocks at the base and quartz-bearing rocks at the top.
|Zone C is simple; it is just a binary eutectic.
Although part of the solid composition path lies in Zone B, that has no effect on the evolution of the melt.
| Zone D is simple; it is also just a binary eutectic.
This is a familiar system but few people really know what goes on. It's the system water - NaCl
On the left side, we see the familiar fact that salt lowers the melting point of water, so that a solution of 23% salt melts at -21 C. This is why you put salt in ice to make homemade ice cream and why you do not put salt in ice for first aid. It's the familiar example of a eutectic.
However, what crystallizes out of a saturated salt water solution at low temperatures isn't salt. It's a hydrate of NaCl called hydrohalite and is a recognized mineral in places like the lakes in the dry valleys of Antarctica, where conditions are suitable for it to form. Hydrohalite is 61% NaCl and 39% water.
When we heat hydrohalite ("heat" being a relative term because we only get to near zero C) it doesn't melt. Instead, it breaks down to brine plus halite. The water "sweats" out of the hydrohalite, or the solid hydrohalite turns to a mush of saturated brine plus NaCl. The process here is just what happens with enstatite melting to liquid plus olivine, just at a much lower temperature.
If the thought of salt melting at 0C bothers you, consider this. Despite the name, hydrohalite has two molecular units of water for every one of NaCl. It has a low density (1.61) and a pseudohexagonal crystal structure (actually monoclinic). Rather than regard it as a hydrate of sodium chloride, it is just as accurate to regard it as ice with incorporated NaCl (although actually its structure is distinct from both. Once we regard it as salty ice, the mystery of it breaking down at 0 C ceases to be a mystery.
Created November 18, 1999, Last Update November 18,, 1999
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