What is the chemical formula of Strontium (II) fluoride?

The chemical formula of strontium (II) fluoride is $SrF_ {2} $. The common valence of strontium ($Sr $) is $+ 2 $, while the common valence of fluorine ($F $) is $- 1 $. According to the principle that the sum of the valence algebra of each element in the compound is zero, in order to make the sum of the valence algebra zero, one strontium ion ($Sr ^ {2 +} $) needs to be combined with two fluorine ions ($F ^ {-} $), so that the total positive valence and the total negative valence can be offset, that is, $+ 2 + ( - 1) \ times2 = 0 $, so its chemical formula is written as $SrF_ {2} $. This chemical formula accurately characterizes the proportional relationship between the number of atoms of strontium and fluorine in strontium (II) fluoride, which is an important symbol for expressing the composition of this substance in chemical research and related applications.

What are the main uses of Strontium (II) fluoride?

Strontium (II) fluoride, also known as strontium fluoride ($SrF_ {2} $), has a wide range of main uses. In the field of optics, strontium fluoride is often used in the manufacture of optical glass due to its excellent optical properties. This glass has the characteristics of low dispersion and high transmittance. It is widely used in the production of lenses in various optical instruments, such as telescopes and microscopes, which can effectively improve the clarity and quality of imaging.

In the electronics industry, strontium fluoride also plays a key role. It can be used as a raw material for electronic components. For example, in the manufacture of some special semiconductor devices, strontium fluoride can optimize the performance of the device and help electronic devices to achieve more efficient and stable operation.

Furthermore, in the ceramic industry, strontium fluoride can be used as an additive for ceramic glazes. After addition, it can improve the sintering performance of ceramics, enhance the hardness and wear resistance of ceramic products, and also make the ceramic surface smoother and brighter, which greatly enhances the quality and aesthetics of ceramic products.

In addition, in the metallurgical industry, strontium fluoride also has its uses. It can be used as a flux to reduce the melting point of ores and promote easier separation of metals and impurities, thereby improving the smelting efficiency and purity of metals, which is of great significance for the optimization of metallurgical processes.

What are the physical properties of Strontium (II) fluoride?

Strontium (II) fluoride, also known as strontium fluoride ($SrF_ {2} $), has many physical properties. It is a white crystalline powder, like fine sand, uniform and fine.

Strontium fluoride has a high density, about 4.24 g/cm3, and feels heavy in the hand. This is due to the close arrangement of strontium and fluorine atoms with a large atomic weight, resulting in a heavy weight per unit volume.

Its melting point is very high, reaching 1473 ° C, and its boiling point is 2460 ° C. Such a high melting boiling point is due to the strong ionic bonding. At high temperatures, the ionic lattice requires a lot of energy to destroy, causing it to melt and gasify.

Strontium fluoride is insoluble in water, with a solubility of only 0.01 g/100 g of water at 20 ° C. Due to its large lattice energy, the hydration energy is not enough to overcome the lattice energy, so it is insoluble.

Strontium fluoride has good optical properties and high transmittance. It has high transmittance in ultraviolet, visible and infrared bands. It can be used as optical materials, such as infrared windows and lenses.

In addition, its hardness is relatively large, with a Mohs hardness of about 3.5. It can resist a certain degree of marking wear and has good chemical stability. It does not react with common acids, bases, oxidants and reducing agents at room temperature. It will only react under specific conditions, such as high temperature and strong acids.

What are the chemical properties of Strontium (II) fluoride?

Strontium (II) fluoride, that is, strontium fluoride ($SrF_ {2} $), is a common inorganic compound. Its chemical properties are quite characteristic, as follows:

First, the stability is quite high. Under normal temperature and pressure, strontium fluoride can exist stably and is not easy to decompose on its own. This is because strontium ions ($Sr ^ {2 +} $) and fluoride ions ($F ^ {-} $) are closely combined by ionic bonds to form a stable lattice structure. As the ancient book says: "If the structure is stable, it will survive for a long time." Its lattice energy is large, which gives the compound good stability.

Second, it has a certain solubility. The solubility of strontium fluoride in water is relatively small, and it is a slightly soluble substance in water. According to the principle of similarity and miscibility, its ionic structure has limited interaction with the polarity of water molecules. However, in some specific organic solvents, its solubility may vary. "Water and oil are difficult to melt, and each has its own characteristics." This is the common sense of differences in the solubility of substances.

Third, it can react with acids. Strontium fluoride reacts with strong acids, such as hydrochloric acid, sulfuric acid, etc. Take the reaction with hydrochloric acid as an example, the reaction equation is: $SrF_ {2} + 2HCl = SrCl_ {2} + 2HF $. This reaction occurs because strong acids can provide hydrogen ions, which combine with fluoride ions to form hydrofluoric acid, following the law of metathesis reaction, that is, "strong for weak, and new substances are formed".

Fourth, under high temperature conditions, strontium fluoride can exhibit some special properties. For example, physical changes such as lattice structure transformation can occur, or participate in some high-temperature chemical reactions. High temperature is like a "universe furnace", which can make substances exhibit different characteristics.

Strontium fluoride has important applications in many fields, such as optical materials, ceramic industry, etc., due to its unique chemical properties.

What are the methods for preparing Strontium (II) fluoride?

The method of fluoridation (II) is as follows.

First, the oxidized fluoric acid can be neutralized and reversed. The two meet, and the inversion is as follows: $Sr (OH) _2 + 2HF\ longrightarrow SrF_2 + 2H_2O $. Take the amount of oxidized solid, put it into a container containing fluoric acid, and use a glass rod to make the two fully connected. Because of the neutralization and inversion of the inversion, there is a lot of inversion, so the operation should be careful, and it needs to be carried out in good condition, because the fluoric acid is toxic and corrosive. In contrast, the resulting mixed liquid can be mixed, washed, and dried, and fluorinated solid can be obtained.

Second, it can be reversed with carbonated fluoric acid. The reverse principle is: $SrCO_3 + 2HF\ longrightarrow SrF_2 + H_2O + CO_2 ↑ $. First put the carbonated powder in the reactor, and then add the fluoric acid dropwise. In the reverse process, carbon dioxide can escape. When it is reversed, it is the same as the steps of washing, washing, and dryness to take fluoridation. The carbonated phase is easier to take and the cost is also low. This method is commonly used in industrial production.

Third, it is decomposed by soluble (such as chlorination) and soluble fluoride (such as fluorination). Reverse formula: $SrCl_2 + 2NaF\ longrightarrow SrF_2? + 2NaCl $. Divide the chlorinated solution and the fluorinated solution, mix the two, and immediately a fluorinated white sediment is generated. The solution is separated and washed away from the surface of the sediment. The most dryness is achieved, that is, the required fluorination is obtained. This method is easy to operate, and the degree of material is also easy to control. It is often used in a room.