Magnesium Fluoride: Formula, Uses & Properties

Magnesium fluoride, represented by the chemical formula MgF₂, is an inorganic compound with diverse applications and unique properties. The crystal structure of magnesium fluoride, similar to that studied using X-ray diffraction techniques at institutions like the National Institute of Standards and Technology (NIST), contributes significantly to its functionality. Opticians often utilize MgF₂ as an optical coating to enhance the transmission of ultraviolet and infrared light in lenses. Understanding the composition of this compound is fundamental, leading many to ask: what is the formula for magnesium fluoride, and how does this formula relate to its observed characteristics and applications in fields like metallurgy?

Magnesium Fluoride, represented by the chemical formula MgF₂, is an inorganic compound composed of magnesium and fluorine. At room temperature, it appears as a white, crystalline solid, often found in powder or crystal form. This seemingly simple composition belies its remarkable versatility and importance across various scientific and technological domains.

The Significance of Magnesium Fluoride

MgF₂ stands out due to its unique combination of optical, chemical, and physical properties, rendering it indispensable in applications ranging from advanced optics to protective coatings. Its ability to transmit a broad spectrum of electromagnetic radiation, coupled with its chemical inertness and mechanical robustness, positions it as a critical material in contemporary technology.

Wide-Ranging Applications

The applications of Magnesium Fluoride are remarkably diverse. In the realm of optics, it serves as a crucial component in lenses, prisms, and windows, particularly in ultraviolet (UV) and infrared (IR) optical systems.

Its high transparency across a broad spectral range makes it ideal for these demanding applications.

Beyond optics, MgF₂ finds extensive use as a thin-film coating material, enhancing the durability and performance of various surfaces.

It is used in anti-reflection coatings on lenses and other optical elements to minimize light loss.

Unique Properties: UV Transparency

One of the most defining characteristics of Magnesium Fluoride is its exceptional transparency to ultraviolet (UV) radiation. Unlike many other materials that absorb UV light, MgF₂ allows it to pass through with minimal attenuation.

This property makes it invaluable in UV spectroscopy, UV lasers, and other UV-based technologies.

The UV transparency of MgF₂ opens doors to applications where UV light manipulation is paramount. This single property significantly elevates its value in the broader scientific and industrial landscape.

Unveiling the Composition and Structure of MgF₂

Magnesium Fluoride, represented by the chemical formula MgF₂, is an inorganic compound composed of magnesium and fluorine. At room temperature, it appears as a white, crystalline solid, often found in powder or crystal form. This seemingly simple composition belies its remarkable versatility and importance across various scientific and technological applications, warranting a deeper investigation into its fundamental structure and composition.

Constituent Elements and Their Roles

MgF₂ is formed through the interaction of two key elements: magnesium (Mg) and fluorine (F). Each element contributes unique properties to the resulting compound.

Magnesium (Mg)

Magnesium is an alkaline earth metal, possessing a silvery-white appearance. Its atomic number is 12, and it has a relatively low density. Magnesium's key property in the context of MgF₂ is its tendency to lose two electrons, forming a positively charged ion (cation). This oxidation is crucial for ionic bond formation.

Fluorine (F)

Fluorine, a halogen, is a pale yellow gas under normal conditions. It has an atomic number of 9 and is the most electronegative element on the periodic table. This extreme electronegativity drives fluorine to readily gain an electron, forming a negatively charged ion (anion). This reduction complements magnesium's oxidation, facilitating the formation of a stable ionic compound.

Chemical Formula and Stoichiometry

The chemical formula MgF₂ indicates the stoichiometric ratio of magnesium and fluorine atoms in the compound. For every magnesium atom, there are two fluorine atoms. This 1:2 ratio is essential for charge balance within the crystal lattice. One magnesium atom loses two electrons, and two fluorine atoms each gain one electron, resulting in a neutral compound.

Valency and Charge Distribution

Valency refers to the combining capacity of an element, which is determined by the number of electrons an atom can gain, lose, or share to achieve a stable electron configuration.

Magnesium exhibits a valency of +2. This means it tends to lose two electrons to achieve the stable electron configuration of the noble gas neon. Fluorine, on the other hand, has a valency of -1, readily gaining one electron to attain the stable electron configuration of neon. These valencies are critical in understanding the ionic bonding within MgF₂.

Ionic Bonding in Magnesium Fluoride

Magnesium fluoride is a quintessential example of an ionic compound. Ionic bonding arises from the electrostatic attraction between oppositely charged ions. In the case of MgF₂, this attraction occurs between magnesium cations (Mg²⁺) and fluorine anions (F⁻).

Formation of Magnesium Cations (Mg²⁺)

Magnesium atoms achieve a stable electron configuration by losing their two outermost valence electrons. This process results in the formation of a magnesium cation with a +2 charge (Mg²⁺). This positively charged ion is significantly smaller than the neutral magnesium atom due to the increased effective nuclear charge experienced by the remaining electrons.

Formation of Fluorine Anions (F⁻)

Fluorine atoms, with their high electronegativity, readily accept one electron to complete their octet and achieve a stable electron configuration. This results in the formation of a fluorine anion with a -1 charge (F⁻). The resulting fluoride ion is larger than the neutral fluorine atom because the increased electron-electron repulsion expands the electron cloud.

Exploring the Key Properties of Magnesium Fluoride

The practical utility of Magnesium Fluoride (MgF₂) stems directly from its distinctive array of physical and chemical properties. These characteristics dictate its suitability for various applications, ranging from advanced optical systems to specialized industrial coatings. Understanding these properties is crucial to leveraging MgF₂ effectively in diverse technological domains.

Physical Properties of MgF₂

The physical attributes of magnesium fluoride are particularly noteworthy. They are central to its performance in many of its crucial applications.

Rutile Crystal Structure

Magnesium fluoride adopts a rutile crystal structure, a tetragonal arrangement where each magnesium ion (Mg²⁺) is coordinated by six fluoride ions (F⁻), and each fluoride ion is coordinated by three magnesium ions. This specific arrangement contributes to its stability and influences its optical characteristics.

The rutile structure dictates many of its anisotropic properties, meaning its properties differ depending on the direction in which they are measured. This structural element is a fundamental aspect of its behavior in optical systems.

Molar Mass and its Significance

The molar mass of MgF₂ is approximately 62.30 g/mol. This value is derived from the atomic masses of magnesium and fluorine, as found on the periodic table, and is crucial for stoichiometric calculations in chemical reactions and material preparation.

A precise understanding of the molar mass is essential for accurately controlling the synthesis and processing of MgF₂ in both research and industrial settings. In particular, it is paramount when creating thin films where precise mass-based deposition rate and thickness is necessary.

Refractive Index in Optical Applications

Magnesium fluoride possesses a relatively low refractive index, typically around 1.38 at a wavelength of 589 nm. This low refractive index is a critical factor in its application as an anti-reflective coating on lenses and other optical components.

By applying a thin film of MgF₂ to a lens surface, the amount of light reflected is reduced, thereby increasing the transmission and clarity of the optical system. This is particularly important in high-precision optical instruments.

Transparency to UV and IR Radiation

One of the most valuable physical properties of MgF₂ is its exceptional transparency across a broad spectrum of electromagnetic radiation, ranging from the ultraviolet (UV) to the infrared (IR) regions.

This transparency makes it an ideal material for windows, lenses, and prisms in UV and IR spectroscopic instruments. It ensures minimal signal loss or distortion in these applications.

MgF₂'s ability to transmit UV light is particularly significant, as many common optical materials are opaque in this region. This transparency enables its use in specialized applications such as UV lithography and excimer laser optics.

Chemical Properties of MgF₂

While its physical properties are key to its optical applications, the chemical properties of MgF₂ determine its stability and compatibility in various environments.

Reactivity with Acids and Bases

Magnesium fluoride is generally inert under normal conditions. However, it can react with strong acids to form hydrofluoric acid (HF), which is a highly corrosive substance. The reaction with acids typically requires elevated temperatures.

MgF₂ is more resistant to reactions with bases, but prolonged exposure to strong bases can lead to the formation of magnesium hydroxide and fluoride salts. The stability of MgF₂ in different chemical environments is a critical consideration for its use in industrial applications.

Chemical Reactions Involving MgF₂

The primary chemical reaction involving MgF₂ is its formation from magnesium and fluorine. The reaction is highly exothermic, releasing a significant amount of energy.

MgF₂ can also decompose at very high temperatures, releasing fluorine gas, which is highly reactive and toxic. Understanding these chemical reactions is important for handling MgF₂ safely and effectively.

Solubility, Degree, and Affecting Factors

Magnesium fluoride is sparingly soluble in water, with a solubility product (Ksp) value of approximately 6.4 x 10⁻⁹ at 25°C. This low solubility means that MgF₂ remains largely undissolved in aqueous solutions under normal conditions.

The solubility of MgF₂ can be affected by factors such as temperature, pH, and the presence of other ions in the solution. For example, increasing the temperature generally increases its solubility, while changes in pH can affect the equilibrium of its dissolution.

The low solubility of MgF₂ contributes to its stability in many applications, particularly in coatings and thin films where resistance to dissolution is essential.

Synthesis and Production of Magnesium Fluoride

Exploring the Key Properties of Magnesium Fluoride, the practical utility of Magnesium Fluoride (MgF₂) stems directly from its distinctive array of physical and chemical properties. These characteristics dictate its suitability for various applications, ranging from advanced optical systems to specialized industrial coatings. Understanding these properties sets the stage for a critical examination of how MgF₂ is synthesized and produced, both in laboratory settings and on an industrial scale. The synthesis methods influence the purity, morphology, and ultimately, the performance of MgF₂ in its diverse applications.

Chemical Synthesis Methods

Chemical synthesis of MgF₂ involves several established methods, each with its own advantages and limitations in terms of cost, yield, and product quality. These methods often rely on controlled chemical reactions in aqueous or solid-state environments to achieve the desired product.

Precipitation Method

The precipitation method is a widely used technique for synthesizing MgF₂ due to its relative simplicity and cost-effectiveness. This process typically involves reacting a soluble magnesium salt, such as magnesium chloride (MgCl₂) or magnesium nitrate (Mg(NO₃)₂), with a fluoride source, like sodium fluoride (NaF) or hydrofluoric acid (HF).

The reaction is conducted in an aqueous solution, leading to the precipitation of MgF₂ as a solid product. The stoichiometry of the reaction is critical, as deviations from the ideal ratio can lead to impurities or incomplete conversion.

The general reaction can be represented as follows:

MgCl₂ (aq) + 2 NaF (aq) → MgF₂ (s) + 2 NaCl (aq)

Or,

Mg(NO₃)₂ (aq) + 2 HF (aq) → MgF₂ (s) + 2 HNO₃ (aq)

After precipitation, the MgF₂ precipitate is filtered, washed to remove residual reactants and byproducts, and then dried. The drying process is crucial to prevent agglomeration of the particles and to remove any remaining moisture. The resulting MgF₂ powder can then be further processed, such as by annealing at elevated temperatures, to improve its crystallinity and purity.

Sol-Gel Method

The sol-gel method offers a more sophisticated approach to synthesizing MgF₂, allowing for better control over particle size, morphology, and composition. This method involves the formation of a sol (a stable dispersion of colloidal particles) followed by gelation to create a solid network.

Magnesium alkoxides, such as magnesium ethoxide (Mg(OC₂H₅)₂), are commonly used as precursors in the sol-gel process. These alkoxides are hydrolyzed in a controlled environment, leading to the formation of magnesium hydroxide [Mg(OH)₂] species in the sol.

A fluoride source, such as hydrofluoric acid (HF) or ammonium fluoride (NH₄F), is then added to the sol, promoting the formation of MgF₂ within the gel matrix. The gel is subsequently dried and calcined at high temperatures to remove organic components and consolidate the MgF₂ structure.

The sol-gel method allows for the incorporation of dopants or other additives into the MgF₂ matrix, providing a means to tailor its properties for specific applications. This level of control is particularly valuable for producing high-performance optical materials.

Hydrothermal Method

The hydrothermal method involves the synthesis of MgF₂ under high-temperature and high-pressure conditions in an aqueous solution. This method is particularly effective for producing crystalline MgF₂ with controlled morphology and high purity.

In a typical hydrothermal synthesis, magnesium salts and a fluoride source are sealed in a hydrothermal autoclave. The autoclave is then heated to a specific temperature, typically between 100°C and 300°C, and maintained at a high pressure, ranging from several bars to hundreds of bars.

Under these conditions, the solubility of the reactants increases, and the reaction kinetics are enhanced, leading to the formation of well-defined MgF₂ crystals. The size and morphology of the crystals can be controlled by adjusting the reaction time, temperature, pressure, and the concentrations of the reactants.

After the reaction is complete, the autoclave is cooled, and the MgF₂ crystals are collected by filtration, washed, and dried. The hydrothermal method is advantageous for producing MgF₂ with high crystallinity and minimal impurities.

Industrial Production Processes

Industrial production of MgF₂ primarily relies on scaled-up versions of the chemical synthesis methods described above. However, these processes often involve additional considerations, such as cost-effectiveness, scalability, and environmental impact.

Large-Scale Precipitation

The precipitation method is the most commonly used approach for large-scale MgF₂ production due to its simplicity and relatively low cost. Industrial processes typically involve continuous reactors where magnesium salt solutions and fluoride solutions are mixed in a controlled manner.

The reaction conditions, such as temperature, pH, and mixing rate, are carefully optimized to maximize the yield and purity of the MgF₂ product. The resulting precipitate is then continuously filtered, washed, and dried using large-scale equipment.

To reduce production costs, industrial facilities often utilize waste fluoride streams from other industrial processes as a fluoride source. This approach not only lowers costs but also helps in environmental waste management. The purity of the final product depends on the quality of the starting materials and the efficiency of the purification steps.

High-Temperature Reaction

Another industrial method involves the direct reaction of magnesium oxide (MgO) with fluorine gas (F₂) or hydrofluoric acid (HF) at elevated temperatures. This method can produce high-purity MgF₂, but it requires specialized equipment and safety measures due to the hazardous nature of fluorine and hydrofluoric acid.

The reaction can be represented as follows:

MgO (s) + 2 HF (g) → MgF₂ (s) + H₂O (g)

Or,

MgO (s) + F₂ (g) → MgF₂ (s) + ½ O₂ (g)

The reaction is typically carried out in a high-temperature furnace, and the resulting MgF₂ is collected and purified. This method is particularly suitable for applications requiring extremely high purity and low levels of contaminants.

Considerations for Industrial Production

Several factors must be considered for industrial production of MgF₂. These include the cost of raw materials, energy consumption, waste disposal, and environmental regulations. Efficient production processes aim to minimize these factors while maintaining the desired product quality.

Furthermore, the particle size and morphology of the MgF₂ product can be controlled by adjusting the reaction conditions and adding surfactants or other additives during the synthesis. Tailoring these properties is essential for optimizing the performance of MgF₂ in specific applications, such as optical coatings and thin films.

In conclusion, the synthesis and production of magnesium fluoride involve a range of chemical and industrial methods, each with its own set of advantages and limitations. The choice of method depends on the desired purity, morphology, and cost-effectiveness for specific applications. Continuous advancements in synthesis techniques and industrial processes are aimed at improving the performance and sustainability of MgF₂ production.

Applications of MgF₂: A Wide Spectrum of Uses

Exploring the Key Properties of Magnesium Fluoride, the practical utility of Magnesium Fluoride (MgF₂) stems directly from its distinctive array of physical and chemical properties. These characteristics dictate its suitability for various applications, ranging from advanced optical systems to specialized coatings and beyond. Its unique transparency to a broad spectrum of electromagnetic radiation, coupled with its robust chemical inertness, positions MgF₂ as a critical component in numerous technological domains.

MgF₂ in Optics: A Foundational Material

Magnesium fluoride’s exceptional optical properties render it indispensable in the field of optics. Its high transmission rate across a wide range of wavelengths, from the ultraviolet (UV) to the infrared (IR), is unmatched by many other materials. This characteristic is fundamentally important for manufacturing lenses, prisms, and windows that operate in these spectral regions.

Its relatively low refractive index also makes it ideal for minimizing reflection losses.

Anti-Reflective Coatings: Enhancing Optical Performance

One of the most significant applications of MgF₂ is in the creation of anti-reflective (AR) coatings. When applied as a thin film on optical surfaces, MgF₂ reduces the amount of light reflected, thereby increasing the transmission and overall efficiency of optical devices.

This is particularly crucial in applications where light intensity is paramount, such as in cameras, telescopes, and sophisticated laser systems. AR coatings made from MgF₂ improve image clarity and reduce glare, contributing to enhanced performance.

Thin Films: Tailoring Optical Properties

The deposition of MgF₂ thin films is a sophisticated process that enables the precise control of optical properties. These films are fabricated using techniques such as vacuum deposition, sputtering, and chemical vapor deposition.

The resulting thin films are used in a variety of optical devices, including:

• Interference filters
• Beam splitters
• Protective coatings

The ability to tailor the thickness and structure of MgF₂ thin films allows for the creation of optical components with specific performance characteristics.

UV Spectroscopy: Accessing the Deep Ultraviolet

Magnesium fluoride's high transparency in the ultraviolet region makes it an essential material for UV spectroscopy. This analytical technique is used to study the electronic structure of molecules and materials by measuring their absorption and emission of UV light.

Because MgF₂ windows and lenses allow UV light to pass through with minimal attenuation, they are critical components in UV spectrometers and other UV-based analytical instruments.

IR Spectroscopy: Expanding the Infrared Window

Similar to its role in UV spectroscopy, MgF₂ is also valuable in IR spectroscopy due to its infrared transparency. It is utilized in manufacturing windows and lenses for IR spectrometers, enabling the analysis of molecular vibrations and rotational modes. This transparency facilitates the identification and quantification of various compounds based on their unique IR absorption patterns.

Beyond Optics: Diverse Applications

While primarily known for its optical applications, MgF₂ also finds use in other areas:

• Plasma Displays: As a protective layer.
• Catalysis: As a support material for catalysts.
• Thermal Barrier Coatings: In specialized applications requiring thermal resistance.

These applications highlight the versatility of MgF₂ and its ability to contribute to technological advancements across diverse fields. The ongoing research and development efforts continue to uncover new applications for this remarkable compound, solidifying its importance in modern technology.

Characterization Techniques for Magnesium Fluoride

[Applications of MgF₂: A Wide Spectrum of Uses Exploring the Key Properties of Magnesium Fluoride, the practical utility of Magnesium Fluoride (MgF₂) stems directly from its distinctive array of physical and chemical properties. These characteristics dictate its suitability for various applications, ranging from advanced optical systems to specialized coatings. Effective characterization of MgF₂ is therefore crucial for ensuring its quality and performance in these applications. This requires the application of sophisticated analytical techniques to probe its structural, optical, and compositional attributes.

Structural Characterization: X-ray Diffraction (XRD)

X-ray Diffraction (XRD) stands as a cornerstone technique for elucidating the crystalline structure of Magnesium Fluoride. By analyzing the diffraction patterns produced when X-rays interact with the material, detailed information about the arrangement of atoms within the crystal lattice can be obtained.

The principle relies on Bragg's Law, which correlates the angle of incidence of the X-ray beam with the interplanar spacing of the crystal lattice. When the condition for constructive interference is met, a diffraction peak is observed.

Understanding the Diffraction Pattern

The position and intensity of these diffraction peaks provide a unique fingerprint of the crystalline phase. Analysis of the peak positions allows for the determination of the lattice parameters. These parameters specify the size and shape of the unit cell, which is the basic building block of the crystal.

Furthermore, the intensities of the peaks are related to the arrangement of atoms within the unit cell. This information allows for the determination of the space group, which describes the symmetry of the crystal structure.

Applications of XRD in MgF₂ Analysis

XRD is invaluable for:

• Identifying the crystalline phase of MgF₂.
• Determining the crystallite size and strain.
• Assessing the degree of crystallinity.
• Detecting the presence of impurities or secondary phases.

This technique is particularly important in verifying the successful synthesis of MgF₂ and ensuring its structural integrity for demanding optical applications.

Optical Characterization: Spectroscopic Methods

Beyond its structural properties, the optical behavior of Magnesium Fluoride is paramount, especially given its widespread use in optical coatings and components. Various spectroscopic methods are employed to characterize its optical properties, each providing unique insights into its interaction with electromagnetic radiation.

UV-Vis Spectroscopy

UV-Vis spectroscopy measures the absorption and transmission of light in the ultraviolet and visible regions of the electromagnetic spectrum. This is critical for assessing the transparency of MgF₂ in these regions.

Magnesium Fluoride is highly transparent in the UV region. The absorption edge, which indicates the wavelength at which the material starts to absorb light significantly, is a key parameter determined by UV-Vis spectroscopy.

This technique also allows for the determination of the refractive index and extinction coefficient, which are crucial for designing anti-reflective coatings.

Infrared (IR) Spectroscopy

IR spectroscopy probes the vibrational modes of molecules within the material. By analyzing the absorption of infrared radiation at specific frequencies, information about the chemical bonds and composition of MgF₂ can be obtained.

This is particularly useful for detecting the presence of impurities, such as water or other contaminants, which can affect its optical performance.

IR spectroscopy can also reveal information about the crystal structure and the presence of defects.

Spectroscopic Ellipsometry

Spectroscopic Ellipsometry is a sensitive technique for characterizing the optical properties of thin films. It measures the change in polarization of light upon reflection from the sample surface.

This information is then used to determine the refractive index, extinction coefficient, and thickness of the film with high precision.

This technique is especially valuable for optimizing the performance of MgF₂ thin films in optical coatings.

Photoluminescence Spectroscopy

Photoluminescence (PL) spectroscopy involves exciting the material with light and analyzing the emitted light. PL can reveal information about the electronic structure, defects, and impurities in MgF₂.

This technique is useful for understanding the origin of luminescence in MgF₂ and for identifying defects that may affect its optical properties. It also assists to reveal any potential down conversion properties that could benefit various novel applications.

The combined use of these characterization techniques provides a comprehensive understanding of the structural and optical properties of Magnesium Fluoride, enabling its effective utilization in a wide range of advanced technological applications.

Safety and Handling of Magnesium Fluoride

[Characterization Techniques for Magnesium Fluoride [Applications of MgF₂: A Wide Spectrum of Uses Exploring the Key Properties of Magnesium Fluoride, the practical utility of Magnesium Fluoride (MgF₂) stems directly from its distinctive array of physical and chemical properties. These characteristics dictate its suitability for various applications...], responsible utilization necessitates a thorough understanding of its safety profile and the implementation of appropriate handling procedures. While generally considered to possess low toxicity, adherence to established safety protocols is paramount to mitigate potential risks.

Toxicity Assessment

Magnesium Fluoride (MgF₂) exhibits relatively low acute toxicity. However, chronic exposure or inhalation of MgF₂ dust may lead to adverse health effects.

The primary concern lies in its fluoride content. Prolonged exposure to fluoride compounds can result in fluorosis, a condition affecting the skeletal system and teeth.

Symptoms may include joint pain, stiffness, and dental enamel defects. Therefore, minimizing exposure through appropriate safety measures is crucial.

Necessary Safety Precautions

To ensure the safe handling of MgF₂, several precautions must be observed.

Personal Protective Equipment (PPE) is indispensable. This includes:

• Safety glasses with side shields to protect against dust and particulate matter.
• Gloves constructed from chemically resistant materials (e.g., nitrile or neoprene) to prevent skin contact.
• A lab coat or other protective clothing to minimize contamination of personal attire.
• Respiratory protection, such as a dust mask or respirator, should be used in situations where dust generation is unavoidable or ventilation is inadequate.

Ventilation is a critical control measure. Work involving MgF₂ should ideally be conducted in a well-ventilated area or under a fume hood to minimize inhalation of airborne particles.

Hygiene Practices are also important. Avoid eating, drinking, or smoking while handling MgF₂.

Wash hands thoroughly with soap and water after each use and before breaks.

Handling and Storage Guidelines

Proper handling and storage practices are essential to maintain the integrity of MgF₂ and minimize potential hazards.

Storage Conditions should be considered. MgF₂ should be stored in a tightly sealed container in a cool, dry, and well-ventilated area.

Avoid exposure to moisture, as this can promote hydrolysis and the release of hydrogen fluoride (HF), a highly corrosive and toxic gas.

Spill Management protocols must be established. In the event of a spill, contain the material immediately to prevent its spread.

Use appropriate PPE and carefully sweep or vacuum the spilled material into a suitable container for disposal. Avoid creating dust during cleanup.

Consult local regulations for proper disposal methods.

Material Compatibility must be ensured. MgF₂ is generally compatible with most common laboratory materials. However, avoid contact with strong acids, as they may react to form hydrogen fluoride.

Labeling is crucial for identification. All containers of MgF₂ should be clearly labeled with the chemical name, hazard warnings, and relevant safety information.

So, there you have it! Magnesium Fluoride, or MgF2, is a pretty fascinating compound with a surprising range of applications. Hopefully, this gave you a good overview of its properties and uses. Keep an eye out – you might just encounter it in unexpected places!