   Chemical properties
In diamond crystals, carbon atoms are connected to each other in a tetrahedral bond to form an infinite three-dimensional skeleton, which is a typical atomic crystal. In the diamond crystal, the carbon atoms are in each SP 3 hybrid orbital and the other four carbon atoms form a covalent bond to form a regular tetrahedron. Since the CC bond in diamond is very strong, all valence electrons participate in the formation of covalent bonds, and there is no free electron, so diamond is not only hard, but also has a very high melting point and is not electrically conductive. In the industry, it is mainly used in the manufacture of probes and grinding tools for drilling. Shaped diamonds are also used in the manufacture of high-end decorations such as jewelry, which are very expensive.
Ornamental use
Due to its high degree of inflection, diamonds shine brightly under the light and become the favorite gem of women. The giant diamonds can be worthless. The price of diamonds with color is higher. At present, the most expensive colored diamonds are those with a blue-blue water blue diamond. Diamonds are divided into one type and two types, which are mainly based on whether it contains N elements: one type contains; type two does not. The blue diamond is a two-B type, which is a semiconductor.
Industrial applications
Due to the extremely high hardness of diamonds, scientists use high-temperature and high-pressure diamond particles to be used on sandpaper, drilling and grinding tools to cut and characterize other substances.
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