Welding TIPS in WELDING HANDBOOK
An alloy is essentially a mixture of two or more elements, the principal component being a metallic element (the ‘parent metal’ or ’solvent’), so that the resultant mixture exhibits metallic properties. A wide variety of mechanical and physical properties may be obtained by alloying, so that alloys, rather than pure metals, are of the greatest importance for engineering.
If the constituent metallic atoms are chemically similar to one another, they will crystallise as a single set of crystals, since all the atoms will behave as if they belonged to the same species. A single-phase solid solution is then said to form, and its microstructure is often indistinguishable from that of a pure metal.
However, there may be a tendency for the elements to crystallise separately to form distinct and different crystals joined at mutual grain boundaries. Such a structure is an example of a phase mixture, which can usually be distinguished from a single-phase solid by metallographic examination.
Note that this could include the formation of an intermetallic compound. These compounds are in themselves of little practical value, since they tend to be hard and brittle, but they can be important as constituents of alloy systems.
1.3 Solid Solutions
Initially when a solid solution is formed the crystal structure is the same as that of the parent metal - the atoms of the solute or alloying element are distributed throughout each crystal, and a range of composition is possible. The solution may be formed in two ways:
(a) In substitutional solid solutions the atoms share a single common array of atomic sites (Fig 4a).
In some systems the parent metal will dissolve any proportion of the solute and retain its original crystal structure. However, in many cases there is a limited solubility and in order to accommodate a larger proportion of the added alloying element a change in the initial crystal structure becomes necessary to form a different solid solution, that is, another phase. In this way two solid solutions may exist together over a range of composition.
(b) In interstitial solid solutions the atoms of the solute element are small enough to fit into the spaces between the parent metal atoms, as illustrated (Fig 4b).
7
(a) substitutional
(b) interstitial
Fig 4 The formation of solid solutions
Because of the atom size limitation, interstitial solid solutions are less common than substitutional solutions, although Carbon atoms can dissolve in iron crystals in this way in steel. Similarly Nitrogen can dissolve in steel and this is the basis of the Nitriding surface hardening process. The very small atoms of Hydrogen will dissolve interstitially in ferrous alloys, usually producing brittleness.
1.4 Phase Mixtures
A phase, present in an alloy as a separate entity, can be pure metal, a solid solution or an intermetallic compound. Any mixtures of two or more of these can occur. In binary systems, that is those of two elements, generally not more than two phases can exist together.
8
2. EQUILIBRIUM DIAGRAMS
Thermal equilibrium (also known as Phase or Constitutional) diagrams are of great importance in metallurgy for with their aid it is possible to determine exactly the structure of a particular alloy at any given temperature, provided the alloy has been allowed to reach a state of equilibrium. Thus the phases present, their quantities and the chemical composition of each phase can be shown with precision. The diagrams are constructed principally by thermal analysis but also with microscopic studies, the examination of volume changes, X-ray diffraction and other techniques.
Equilibrium can be considered as a state of balance ultimately arrived at by the components at the temperature of the system concerned. However, in some cases such a state would take a very long time to be reached while in others it may never be reached at the temperature in question. For example, if an alloy is rapidly cooled by quenching to room temperature, chemical and physical changes may be suppressed such that they will never take place unless the alloy is reheated to allow them to occur. Very slow cooling must then follow.
2.1 Iron-Carbon Equilibrium Diagram (Fig 5)
Steel may be defined as an alloy of Iron and Carbon (up to about 1.7%C). Here it may be helpful to recall the allotropic nature of iron and that up to 910°C it has a body centred cubic crystalline form known as alpha α Iron, from 910°C-1400°C a face centred cubic structure, gamma γ Iron, reverting to body centred cubic delta δ. Iron above that temperature. These terms are modified in steel to Ferrite, Austenite and δ Ferrite. Other phases in the equilibrium structure are Cementite the inter-metallic compound Fe3C, and, Pearlite a phase mixture known as a Eutectoid consisting in this case of alternate layers of Cementite and Ferrite. Pearlite contains about 0.83%C.
Ferrite and δ Ferrite, the body centred cubic structures dissolve only very small amounts of carbon: less than 0.01% at room temperature. The face centred cubic Austenite however, is capable of dissolving up to nearly 2%C at 1150°C although this structure will change on reaching the Lower Critical Temperature 723°C below which the Eutectoid reaction will be complete. (Fig 6)
9
Fig 5 The Iron-Carbon phase diagram
10
Fig 6 Part of the Iron-Carbon Thermal-equilibrium diagram
Note that the Lower Critical Temperature 723°C below which all Austenite has been converted to Ferrite and Cementite is commonly known as the A1 temperature. The temperature above which the structure will be wholly Austenite, the Upper Critical Temperature, is known as the A3 temperature. Also the temperature above which the steel reverts to a wholly body centred cubic δ ferrite is known as the A4 temperature.
2.2 Slowly Cooled Structures
The most important reaction in steel is the decomposition of austenite on cooling. Consider the slow cooling of a steel of 0.83%C content (i.e. of the eutectoid composition) (Fig 7a); at 723°C the structure will transform to an eutectoid mixture consisting of alternate lamellae or plates of ferrite and cementite.
A steel of higher carbon content (known as a ‘hyper-eutectoid’ steel) (Fig 7b), 1.20%C, will remain austenitic down to the temperature around, say, 870°C at which the solvus line is crossed, so that Fe3C will start to be precipitated at the austenite grain boundaries.
Continued cooling and precipitation of cementite Fe3C will reduce the carbon content of the austenite until it reaches that of the eutectoid 0.83%C. When the temperature falls to below 723°C, this residual austenite will transform to pearlite, and the final microstructure will be cementite plus pearlite.
11
A lower carbon steel (i.e. a ‘hypoeutectoid steel) of 0.4%C (Fig 7c) will begin to transform when the temperature falls below the solvus line by the precipitation of ferrite at the austenite grain boundaries.
Continued cooling and precipitation of ferrite will increase the carbon content of the austenite until it reaches that of the eutectoid 0.83%C. At 723°C this remaining austenite will transform to pearlite resulting in a final structure of ferrite plus pearlite.
2.3 Quenched Structures
The previous microstructures form in plain carbon steels which have been moderately slowly cooled (e.g. by cooling in air) from temperatures within the austenitic phase field, say from 50°C above the lower boundary line CED. This is called a ‘normalising’ heat treatment, but medium and high-carbon steels are very commonly subjected to more complex treatments in order fully to exploit their properties. These treatments involve, first, heating the alloy into the austenite phase field, as before, but then quenching it in water or brine which suppresses diffusion and thus the formation of ferrite and cementite. Under these conditions the austenite transforms by a process not involving diffusion into a metastable distorted form of body-centred iron known as ‘Martensite’ (Fig 7d). This process is extremely rapid and the transformation may be completed in a few microseconds.
All the carbon originally dissolved in the Austenite at high temperature remains after quenching in interstitial solution in the Martensite crystals. This has the effect of distorting the lattice from cubic to tetragonal symmetry. This lattice distortion by the dissolved carbon has the effect of hardening the structure and the resulting steels will not only be hard but brittle, for which there is little practical application. A second heat treatment called tempering is therefore required and this will reduce hardness and brittleness. If Martensitic steel is reheated to the temperature range 200-600°C (below the Austenite forming temperature) it rapidly decomposes to form body centred cubic ferrite and particles of Cementite.
This structure is on an extremely fine scale, the size of the carbide particles being dependent on the time and temperature of the treatment. The higher the temperature and the longer the time, the softer and less brittle the product.





This is default description text on Padangan Themes, of course you can change this text via you profile administration.