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Chlorine Trifluoride is an interhalogen compound with the chemical formula ClF3 which is a poisonous, corrosive, colourless, and extremely reactive gas with the sweet and suffocating pungent type of colour. It is also a severe irritant to the skin, eyes, and mucous membranes and Lung damage can be caused by exposure to this gas. A 30-minute exposure to 400 ppm was lethal to rats and the mechanism whereby metals resist the attack of elemental fluorine or chlorine trifluoride is not completely understood. If most combustible material comes in contact with chlorine trifluoride it ignites spontaneously as it is a powerful oxidizer. Some of the other names of Chlorine Trifluoride are Chlorine fluoride, trifluoro – λ3 – chlorane
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Key Takeaways: Chlorine Trifluoride, Interhalogen, Explosive, Hexafluoride, Trigonal Bipyramidal, Covalent Bond, Chlorine Fluoride, Oxidizer, VSEPR Theory
Structure of Chlorine Trifluoride
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The structure of Chlorine Trifluoride in terms of molecular geometry has two long bonds and one short bond and has almost a T-shaped and in the ClF3 molecule, the central chlorine atom has five regional electron densities which consist of two lone pairs and three bonds.
- The structure of Chlorine Trifluoride predicts that the lone pairs of the electrons being present in the two equatorial positions of a say trigonal bipyramid are satisfying the VSEPR Theory and these are arranged at 175 degrees of F(axial)-Cl-F(axial) bond angle and the elongated axial bonds of Cl-F bonds are consistent using hypervalent bonding.
- Along with this, Chlorine Trifluoride is stable to 180 degrees Celsius in a quartz vessel but if we keep it above this temperature, it decomposes to its constituent elements by a free radical mechanism.
Structure of Chlorine Trifluoride
Read More: Covalent Bond
Chemical Data of Chlorine Trifluoride
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Below mentioned is the chemical data of Chlorine Trifluoride.
| Name of the Compound | Chlorine Trifluoride |
| Density | 1.77 g/cm³ |
| Molecular Weight/ Molar Mass | 92.448 g/mol |
| Boiling Point | 11.75 °C |
| Melting Point | −76.34 °C |
| Chemical Formula | ClF3 |
Physical Properties of Chlorine Trifluoride
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The physical properties of chlorine trifluoride are:
- Chlorine Trifluoride is a chemical compound that is not present as a free compound in nature and is precarious and highly combustible. ClF3 has a density of 1.77g/cm3 and a molecular mass of 92.448g/mol and the boiling point of Chlorine Trifluoride is 11.75 degrees Celsius while the melting point of the compound is -76.34 degrees Celsius. There are four heavy atoms present and the molecule of Chlorine Trifluoride has one covalently-bonded unit also. Along with this, Chlorine Trifluoride is surprisingly soluble in water.
- Chlorine Trifluoride in the vapour state may decompose to ClF, ClOF, ClO2F, ClO3F, ClO2, Cl2, and HF, among which the most significant ones are Cl2, ClO2, and HF and all the resultants of the decomposition depend on the availability of water.
| Odour | Pungent odour |
| Appearance | Pale green-yellow colour solid |
| Covalently-Bonded Unit | 1 |
| Heavy Atom Count | 4 |
| Complexity | 8 |
| Solubility | Soluble in water |
Read More: Difference between Molar Mass and Molecular Mass
Preparations of Chlorine Trifluoride
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Chlorine Trifluoride prepares the direct actions of chlorine and fluorine gasses and may also be prepared by the reaction of ClF and Chlorine gasses.
Cl2 + 3F2 → 2ClF3
ClF + F2 → ClF3
ClF3 is one of the most reactive and aggressive compounds which catches fire spontaneously with wood and must build materials- even asbestos. CIF3 was used in incendiary bombs in World War II
Chemical Properties of Chlorine Trifluoride
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Chlorine Trifluoride dissolves in water forming hydrogen fluoride, hydrogen chloride, and oxygen. Below mentioned is the chemical equation of the compound.
ClF3 + 2H2O → 3HF + HCl + O2
Chlorine Trifluoride reacts with uranium forms Uranium hexafluoride and an interhalogen compound chlorine fluoride and the chemical equation is given below.
U + 3ClF3 → UF6 + 3ClF
Chlorine Trifluoride- Highly Combustible Compound
Read More: Writing Chemical Formulae
Uses of Chlorine Trifluoride
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Here are the uses of Chlorine Trifluoride:
- Chlorine trifluoride is used as a fluorinating agent and may be used as an igniter and propellant in rockets.
- Chlorine Trifluoride is also used in etching operations and as a component in plasma less cleaning.
- It is used in nuclear fuel processing and is also used as a fluorinating agent, incendiary, igniter, and propellant for rockets, in nuclear reactor fuel processing, pyrolysis inhibitor for fluorocarbon polymers.
- Chlorine trifluoride is also used in nuclear fuel processing to convert uranium into gaseous hexafluoride uranium but there are several problems regarding the use of ClF3 as a component in the rocket propellant systems as ClF3 is known to be rapidly hypergolic with all other fuels and doesn't make any measurable ignition delay.
- ClF3 is used to clean chemical vapour deposition chambers in the semiconductor industry. Another benefit of using Chlorine Trifluoride is that it can be used to remove the chamber walls' semiconductor material without the need to dismantle and also does not require to be activated by plasma as the heat of the chamber is enough for reaction and decomposition with the semiconductor material.
- Production of Uranium Hexafluoride (UF6) is also one of the primary uses of ClF3 as uranium metal goes under the process of fluorination as part of nuclear fuel processing and reprocessing.
U + 3ClF3 → UF6 + 3ClF
Read More: Transuranium Elements
Facts about Chlorine Trifluoride
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- The reactions of Chlorine Trifluoride with many metals yield chlorides and fluorides and when reacts with Phosphorus (P2), then it produces Phosphorus Trichloride (PCl3) and Phosphorus Pentafluoride (PF5).
- When ClF3 acts with Sulphur (S2), then it yields Sulphur Tetrafluoride (SF4) and Sulphur Dichloride (SCl2).
- Chlorine Trifluoride reacts violently with water by either oxidizing it to provide Oxygen gas or to provide Oxygen Difluoride (OF2) in controlled amounts and also, the reduction will cause Hydrogen Fluoride and Hydrogen Chloride.
ClF3 + 2H2O → 3HF + HCl + O2
ClF3 + H2O → HF + HCl +OF2
Hence it is quite impossible to store Fluorine in solutions because Fluoride is the most powerful oxidizing agent of all elements.
- In a laboratory experiment, it has been found that the exposure of 400ppm of Chlorine Trifluoride gas for thirty minutes was lethal to the rats.
- Chlorine Trifluoride (ClF3) has 28 valence electrons in total, and the bonds are between the centre Chlorine atom and the surrounding three Fluorine atoms.
Read More: Ionization Energy Formula
Things to Remember
- Chlorine Trifluoride is an interhalogen compound with the chemical formula ClF3.
- It is a poisonous, corrosive, colourless, and extremely reactive gas with the sweet and suffocating pungent type of colour.
- Chlorine Trifluoride comprises 28 valence electrons having chlorine atoms and the surrounding three fluorine atoms and is almost T-shaped.
- Chlorine Trifluoride is a highly reactive compound that represents a trigonal bipyramidal geometry that satisfies VSEPR theory.
- It is used in nuclear reactor fuel processing and is also used to convert uranium into gaseous Hexafluoride uranium.
- CIF3 doesn't make any measurable ignition delay as it is known to rapidly hypergolic all other fuels.
Sample Questions
Ques How is Chlorine Trifluoride formed? (3 Marks)
Ans. The ClF3 is formed by cation Chloride in the centre which is bound to three Fluoride anions and Chloride atoms have two lone pairs of electrons due to the repulsion caused by the electron over Fluoride atoms, it forms a trigonal bipyramidal structure of the molecule. In this structure, one of the paired electrons of Cl in the 3p subshell remains as a lone pair or unpaired and undergo sp3d hybridization to give a T-shaped structure to the CIF3 molecule.
Ques. How is Chlorine Trifluoride stored? (3 Marks)
Ans. Chlorine Trifluoride uses containers made of steel, iron, copper, and nickel after they've been treated with Fluorine gas for safely storing and sealing. it forms a thin film of insoluble metal fluoride that protects the bulk of the metal just like the invisible coat of oxide on aluminium keeps it from burning up in the atmosphere and the thin Fluoride layer formed inside the container is created by processing the container with Fluorine doesn't disturb the ClF3 and if the coating step is not done right, then an explosion might occur when ClF3 comes into contact with the vessel.
Ques. Explain the geometry of chlorine trifluoride. (3 Marks)
Ans. Chlorine Trifluoride (ClF3) represents a Trigonal bipyramidal geometry where the central atom is chlorine and Valence electrons on the central atom is 7 and in this compound, there are three bond pairs of electrons and two lone pairs of electrons so we can say that a total of five pairs of electrons represent trigonal bipyramidal geometry with a 175 degree F(axial)-Cl(axial) bond angle. These two lone pairs take equatorial positions because they demand more space than the bonds which results in a T-shaped molecule.
Ques. Can chlorine trifluoride burn water? (3 Marks)
Ans. The larger amounts of chlorine trifluoride undergo hydrolysis in presence of water which results in violence and exposure in a thermal burn and exposure of chlorine trifluoride liquid or gas, ignites living tissue. It also ignites water by oxidizing it to give oxygen in the form of chlorine and hydrochloric acid with the release of heat. Not only this, chlorine reacts explosively or forms exclusive compounds with many substances that include ether, ammonia, fuel gas, acetylene, hydrogen, chlorine, and finely divided metals too.
Ques. What is the colour of chlorine trifluoride and explain why candle wax is unreactive to CIF3? (3 Marks)
Ans. Chlorine trifluoride in liquid form appears green with a pungent odour while in gaseous form appears colourless. Chlorine trifluoride is a chemical that should only be handled by professionals and once it turns into a gas, ClF3 is colourless with a sweet and pungent odour. There are only a few chemicals that remain completely unreactive with chlorine trifluoride and Shockingly, one of them is regular candle wax. The compound could react violently which can prove to be fatal without a proper container.
Ques. Explain what makes CIF3 highly reactive or deadly. (5 Marks)
Ans. When ClF3 comes into contact with virtually any element it evaporates into a toxic gas. Though even if it decomposes it still produces hydrofluoric and hydrochloric acid, typically in steam form, and if it ignites (which it does easily), it burns at over 2,400 degrees Celsius. As it turns out, the chemical is more oxidizing than oxygen itself, making it an extremely effective explosive.
Essentially, in layman's terms, chlorine trifluoride can even set fire to inflammable materials including things like sand, glass, or even asbestos. Even compounds that have already been burnt can be reignited, like a pile of ash and upon contact with water, ClF3 reacts explosively. Unfortunately for humans, water is an element humans are mostly composed of, and once in contact with human skin, the mixture quickly ignites.
Ques. Explain briefly the structure of CIF3 based on VSEPR Theory. (5 Marks)
Ans. In chlorine trifluoride, the central atom is chlorine, and valence electrons on central atoms are 7 also there is a contribution of three fluorine atoms of 1 electron each. Hence, there are a total of 10 electrons or we can say five electron pairs. We must know that the highest repulsion is between any two lone electron pairs which result in these moving apart as far as possible.
The next highest repulsion is between one lone pair and a bond pair and the lowest is between two bond pairs and the two lone pairs occupy equatorial positions at an angle of 120 degrees to each other, this gives the lowest energy arrangement of electron pairs in the molecules. Because repulsion involving lone pairs is stronger than bond pairs, F−Cl−F angles are a little less than 180 degrees. Therefore, molecules have a T−shape geometry.
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