Chlorine Trifluoride or ClF3 is a highly reactive and toxic chemical compound used in rocket propellants, cleaning agents, and as an oxidizing agent in chemical reactions. It can cause severe burns and can ignite spontaneously on contact with organic materials.
| IUPAC Name | Chlorine Trifluoride |
| Molecular Formula | ClF3 |
| CAS Number | 7790-91-2 |
| Synonyms | Chlorine fluoride, Trifluorochlorine, Trichlorofluoride, Fluorochlorine, Chloryl fluoride, Fluorine chloride |
| InChI | InChI=1S/ClF3/c2-1(3)4 |
Chlorine Trifluoride formula
The chemical formula of Chlorine Trifluoride is ClF3, which represents the three fluorine atoms and one chlorine atom in the molecule. The formula can be used to calculate the molar mass, density, and other physical properties of Chlorine Trifluoride. The formula also indicates the types and number of atoms present in the compound, which is important in understanding its chemical properties and reactivity.
Chlorine Trifluoride molar mass
The molar mass of Chlorine Trifluoride (ClF3) is 92.45 g/mol. This value is calculated by adding the atomic weights of the constituent elements, which are 35.45 g/mol for chlorine and 37.996 g/mol for fluorine. The molar mass of Chlorine Trifluoride is important in chemical calculations and determining the amount of the compound in a given sample.
Chlorine Trifluoride boiling point
Chlorine Trifluoride has a boiling point of 11.75°C at standard pressure. This makes it a volatile and highly reactive compound that can easily vaporize and form toxic fumes. The low boiling point of Chlorine Trifluoride is attributed to the weak intermolecular forces between its molecules, which allows them to break apart and escape as a gas at relatively low temperatures.
Chlorine Trifluoride melting point
Chlorine Trifluoride has a melting point of -76.3°C (-105.3°F) at standard pressure. This makes it a solid at room temperature and pressure, but it can easily sublimate and form toxic fumes due to its high volatility. The low melting point of Chlorine Trifluoride is attributed to the weak intermolecular forces between its molecules, which allows them to break apart and become a gas at relatively low temperatures.
Chlorine Trifluoride density g/ml
The density of Chlorine Trifluoride is 1.77 g/mL at standard temperature and pressure (STP). This value is higher than that of air (1.29 g/mL), which makes Chlorine Trifluoride a denser gas than air. The high density of Chlorine Trifluoride is due to its molecular weight, which is higher than that of most gases in the atmosphere.
Chlorine Trifluoride molecular weight
The molecular weight of Chlorine Trifluoride is 92.45 g/mol. This value is calculated by adding the atomic weights of the constituent elements, which are 35.45 g/mol for chlorine and 37.996 g/mol for fluorine. The high molecular weight of Chlorine Trifluoride makes it a dense gas that is heavier than air.
Chlorine Trifluoride Structure
Chlorine Trifluoride has a trigonal bipyramidal molecular geometry, with a central chlorine atom bonded to three fluorine atoms in equatorial positions and two vacant sites in axial positions. This structure gives rise to a polar molecule, with the two axial positions having a partial positive charge and the three equatorial positions having a partial negative charge.
| Appearance | Colorless to pale yellow gas or yellow liquid |
| Specific Gravity | 1.77 |
| Color | Colorless to pale yellow |
| Odor | Pungent, suffocating odor |
| Molar Mass | 92.45 g/mol |
| Density | 1.77 g/mL at STP |
| Melting Point | -76.3°C (-105.3°F) |
| Boiling Point | 11.75 °C |
| Flash Point | Not applicable |
| Water Solubility | Reacts violently with water |
| Solubility | Soluble in sulfuric acid, nitric acid, and other oxidizing agents |
| Vapour Pressure | 1.73 atm at 20°C |
| Vapour Density | 3.2 (air = 1) |
| PKa | Not applicable |
| pH | Not applicable |
Chlorine Trifluoride Safety and Hazards
Chlorine Trifluoride is a highly reactive and hazardous compound. It poses serious health and safety risks, and must be handled with extreme caution. It can cause severe burns, corrosion, and irritation upon contact with skin, eyes, and mucous membranes. Inhalation of its fumes can cause respiratory distress, coughing, and chest pain. Chlorine Trifluoride can also ignite and react violently with organic materials, metals, and water, leading to explosions and fires. Specialized protective equipment, such as chemical-resistant suits and respirators, must be worn when handling Chlorine Trifluoride, and it should only be used in a well-ventilated and controlled environment by trained professionals.
| Hazard Symbols | Corrosive, Oxidizer |
| Safety Description | Keep away from heat, sparks, open flames, hot surfaces, and sources of ignition. Wear protective clothing and equipment. Avoid contact with skin, eyes, and clothing. Do not inhale fumes or vapors. Do not ingest. Use only in a well-ventilated area. |
| UN Ids | UN 1749 |
| HS Code | 281211 |
| Hazard Class | 8 |
| Packing Group | I |
| Toxicity | Highly toxic |
Chlorine Trifluoride Synthesis Methods
Direct fluorination of chlorine gas can synthesize chlorine trifluoride. Hydrogen fluoride and chlorine gas can react to synthesize chlorine trifluoride.
A mixture of chlorine gas and fluorine gas reacts over a bed of activated charcoal or other inert material at high temperatures to produce Chlorine Trifluoride in the direct fluorination method.
Another method involves the reaction between hydrogen fluoride and chlorine gas. In this method, the two gases are passed over a catalyst, such as activated alumina or platinum, at high temperatures. The reaction between the two gases produces Chlorine Trifluoride and hydrogen chloride as byproducts.
Sulfur tetrafluoride and chlorine gas react in the presence of a catalyst, such as iron or nickel, at high temperatures to synthesize Chlorine Trifluoride and produce sulfur dioxide as a byproduct.
Specialized equipment and careful handling are required for each of these methods due to the hazardous nature of Chlorine Trifluoride. Personnel and the environment must be ensured safety during the synthesis process through proper safety measures such as chemical-resistant suits and ventilation systems.
Chlorine Trifluoride Uses
Chlorine Trifluoride (ClF3) has several industrial applications due to its highly reactive nature and strong oxidizing properties.
- ClF3 cleans and etches semiconductor materials such as silicon and germanium by removing unwanted contaminants and impurities from their surfaces.
- ClF3 converts uranium oxide into uranium hexafluoride for nuclear fuel production. Uranium hexafluoride is enriched for use in nuclear reactors.
- ClF3 increases combustion efficiency and generates greater thrust when used in combination with other oxidizing agents such as hydrazine or hydrogen in rocket propellants and high-energy oxidizers for fuel systems.
- ClF3 bleaches textiles and paper products.
- ClF3 produces certain chemicals such as fluorine gas and fluorocarbons.
Due to its hazardous nature, Chlorine Trifluoride must be handled with extreme caution in all of its applications, and only by trained professionals with proper safety equipment and protocols.
Questions:
Q: Is chlorine trifluoride polar or nonpolar?
A: Chlorine Trifluoride is a polar molecule due to the difference in electronegativity between chlorine and fluorine atoms.
Q: How to put out chlorine trifluoride?
A: Chlorine Trifluoride can be extinguished using dry sand, graphite, or sodium chloride. Water should never be used to extinguish a Chlorine Trifluoride fire, as it can react violently and release toxic gases.
Q: Chlorine trifluoride lewis structure?
A: The Lewis structure of ClF3 consists of a central chlorine atom surrounded by three fluorine atoms. The chlorine atom is bonded to each of the three fluorine atoms through a single bond, and there is one lone pair of electrons on the chlorine atom.
Q: What is the formal charge of the chlorine atom in the chlorine trifluoride molecule?
A: The formal charge of the chlorine atom in Chlorine Trifluoride is zero. The chlorine atom has seven valence electrons and is bonded to three fluorine atoms, which have a higher electronegativity than chlorine. The lone pair of electrons on the chlorine atom is not involved in any bonding and is thus not considered when determining the formal charge.
Q: Chlorine trifluoride fire?
A: Chlorine Trifluoride is a highly reactive and flammable substance that can ignite spontaneously in contact with organic materials or even with air. In the case of a Chlorine Trifluoride fire, dry sand, graphite, or sodium chloride should be used to extinguish the fire, and water should never be used as it can cause a violent reaction. Evacuation of the area and seek immediate medical attention for any exposure is also crucial in case of a Chlorine Trifluoride fire.