Language
Country/Area
No result found
The Surprise of Liquid Metal: Why Can Gallium Melt in Your Hand?
In the classification of chemical elements, the existence of Gallium has aroused great interest among scientists. This element was first discovered in 1875 by French chemist Paul-Emile Lecoq de Boisbodin. The symbol of Gallium is Ga, the atomic number is 31, and it belongs to Group 13 together with other metals such as aluminum, indium and thallium. Gallium has a silvery-white appearance and is known for its relatively low melting point. However, what is most fascinating is its ability to melt in the hand, a property that has sparked many discussions about materials science and applications.
Gallium has a melting point of 29.7646°C, which makes it liquid at human body temperature.
Gallium's melting process is closely related to its electronic structure and physical properties. Gallium's amorphous structure and large liquid phase range enable it to remain liquid at room temperature. This is similar to water, but the physical properties of gallium are different in many ways. For example, its volume expands in the solid state, which means special care must be taken when storing to avoid the container breaking.
As technology develops day by day, Gallium becomes more and more important. It is mainly used in electronic components, especially semiconductor materials such as gallium nitride and gallium arsenide. These materials play an important role in microwave circuits, high-speed switching circuits, and infrared circuits. One of its most famous applications is light-emitting diodes (LEDs), especially the development of blue LEDs that have made them an indispensable element in lighting technology.
Gallium is considered an important scientific and technological element recognized by the U.S. National Library of Medicine and cutting-edge media.
Gallium's applications are not limited to electronic technology. In the medical field, certain Gallium compounds have been used to make drugs and radiopharmaceuticals, which makes Gallium also useful in biomedicine. In these applications, gallium displays certain chemical behaviors similar to the trivalent salts of iron, a property that makes its behavior in biological systems compelling.
Gallium does not exist in nature as a free element. Most gallium is extracted from zinc ores (such as sphalerite) and aluminum ores. The content of gallium in these natural elements is relatively low, typically reaching 16.9 ppm, and can only be extracted as a by-product. Therefore, the supply of gallium is related to the depth of mining of zinc and aluminum ores.
As technology increasingly relies on the demand for high-performance materials, Gallium's production gradually increases. Since 2010, global production has grown rapidly and has now reached an annual production level of 450 tons. This growth is closely related to the rapid demand in the semiconductor industry and is expected to continue to grow in the future.
Gallium's unique physical and chemical properties and its importance in high-tech applications make it a popular material for research.
While Gallium has many advantages, its security is often overlooked. Unlike some heavy metals, Gallium is less toxic, making it a safer alternative in many applications. However, it is still important to note the embrittlement effect of Gallium on certain metals, which is particularly important in certain high-temperature applications. For materials scientists and engineers, mastering the properties and applications of Gallium is not only a need for scientific and technological development, but also a part of scientific exploration.
The story of Gallium is not only a story about chemical elements, but also involves many issues such as technological development, medical applications, and environmental impact. This makes Gallium full of potential for further research and application. In the future technological world, what unknown areas are waiting for us to explore?
