Fluoromethane (CH3F) is a colorless gas with a faint ethereal odor. It is used in the production of electronics, pharmaceuticals, and as a refrigerant. It has low toxicity but is a potent greenhouse gas.
| IUPAC Name | Fluoromethane |
| Molecular Formula | CH3F |
| CAS Number | 593-53-3 |
| Synonyms | Methyl fluoride, Freon 41, Halocarbon 41, R 41, UN 2452 |
| InChI | InChI=1S/CH3F/c1-2/h1H3 |
Fluoromethane Properties
CH3F Boiling Point
The boiling point of CH3F is -78.4°C, which is relatively low. This makes it an ideal refrigerant for various applications such as refrigeration and air conditioning systems. CH3F is also used as a propellant in aerosol sprays due to its low boiling point.
CH3F Molar Mass
CH3F is a chemical compound with the molecular formula CH3F. It is also known as methyl fluoride and has a molar mass of 34.03 g/mol. CH3F is a colorless gas with a faint ethereal odor and is widely used in various applications due to its unique properties.
CH3F Melting Point
CH3F has a melting point of -141°C, which is also relatively low. Its low melting point makes it easy to handle and transport, making it a popular choice for various industrial applications. The low melting point of CH3F also makes it suitable for use as a refrigerant in low-temperature applications.
CH3F Density
The density of CH3F is 0.89 g/ml, which is relatively low. This makes it less dense than air, which has a density of 1.29 g/ml. As a result, CH3F is often used as a lighter-than-air gas in various applications, including leak detection, gas chromatography, and as a lifting gas for balloons and airships.
CH3F Molecular Weight
The molecular weight of CH3F is 34.03 g/mol, which is relatively low. This makes it a lightweight compound that is easy to handle and transport. CH3F is often used in the production of electronics and pharmaceuticals due to its low molecular weight and unique properties.
CH3F Structure
The structure of CH3F consists of a single carbon atom bonded to three hydrogen atoms and one fluorine atom. The fluorine atom is attached to the carbon atom, replacing one of the hydrogen atoms in methane. The structure of CH3F makes it a stable compound with unique chemical properties.
Fluoromethane Formula
The formula for Fluoromethane is CH3F, which represents the arrangement of atoms in the molecule. The formula shows that Fluoromethane consists of one carbon atom, three hydrogen atoms, and one fluorine atom. The formula is used to describe the chemical composition of Fluoromethane and is important in various applications.
| Appearance | Colorless gas |
| Specific Gravity | 0.89 at 20°C (air = 1) |
| Color | Colorless |
| Odor | Faint ethereal odor |
| Molar Mass | 34.03 g/mol |
| Density | 0.89 g/mL |
| Melting Point | -141°C |
| Boiling Point | -78.4°C |
| Flash Point | Non-flammable |
| Water Solubility | 0.5 g/L at 20°C |
| Solubility | Miscible in organic solvents |
| Vapour Pressure | 4.4 bar at 20°C |
| Vapour Density | 1.43 (air = 1) |
| pKa | 50.9 |
| pH | Not applicable |
Fluoromethane Safety and Hazards
Fluoromethane is generally considered a safe compound to handle and use, with low toxicity and non-flammability. However, like any chemical, it does have potential hazards and safety considerations. Exposure to high concentrations of Fluoromethane can cause dizziness, headaches, and nausea. It is also a potent greenhouse gas, contributing to climate change. Fluoromethane should be handled in a well-ventilated area and protective equipment, such as gloves and goggles, should be worn. It is important to follow proper storage and handling procedures to prevent leaks and accidental release into the environment.
| Hazard Symbols | F+ |
| Safety Description | Highly flammable gas; Toxic if inhaled; Causes skin irritation; Causes serious eye irritation; May cause drowsiness or dizziness; May cause damage to organs |
| UN Ids | UN2452 |
| HS Code | 2903.49.90 |
| Hazard Class | 2.1 |
| Packing Group | II |
| Toxicity | Low toxicity, but can cause health effects if inhaled in high concentrations. |
Fluoromethane Synthesis Methods
Several methods, including direct fluorination of methane and halogen exchange reactions, can synthesize fluoromethane.
One common method is the reaction of methanol with hydrogen fluoride in the presence of a catalyst, such as aluminum oxide or aluminum fluoride.
Another method involves the reaction of chloromethane or bromomethane with hydrogen fluoride gas. Both of these methods produce fluoromethane as a byproduct, which can then be separated and purified using distillation or other methods.
Another method of synthesizing fluoromethane involves the reaction of fluoroform and hydrogen chloride in the presence of a catalyst, such as zinc or copper. This reaction produces a mixture of chlorofluoromethane and fluoromethane, which can be separated and purified using distillation.
Fluoromethane Uses
Fluoromethane has several uses in various industries, including:
- Refrigeration: Used as a refrigerant in industrial and commercial refrigeration systems due to its low boiling point and non-flammability.
- Electronics: Used as a cleaning agent for electronic components and as a plasma etchant in the semiconductor industry.
- Medical applications: Used as an anesthetic in veterinary medicine due to its low toxicity and fast onset of action.
- Pesticide production: Used as a precursor in the production of certain pesticides, including herbicides and insecticides.
- Polymer production: Used as a blowing agent in the production of polymer foams, such as polyurethane foam.
- Laboratory applications: Used as a solvent and reagent in various laboratory applications, including chemical synthesis and analysis.
- Fire suppression: Also used as a fire suppression agent in certain types of fire extinguishers, particularly those used in computer and telecommunications rooms.
Questions:
Q: Is CH3F polar or nonpolar?
A: CH3F is a polar molecule due to the asymmetrical arrangement of the fluorine and hydrogen atoms around the central carbon atom, resulting in a net dipole moment.
Q: Does CH3F have hydrogen bonding?
A: Fluoromethane does not have hydrogen bonding because it does not contain a hydrogen atom bonded to a highly electronegative element such as nitrogen, oxygen, or fluorine.
Q: Which compound has the strongest intermolecular forces: HF, CH3Cl, CH3F, HCl?
A: HF has the strongest intermolecular forces due to its ability to form hydrogen bonds, which are stronger than the dipole-dipole forces in the other compounds.
Q: Which has the smallest dipole-dipole forces: N2, CO, CH3F, HCl?
A: N2 has the smallest dipole-dipole forces because it is a nonpolar molecule and therefore does not have a net dipole moment. CO, CH3F, and HCl are polar molecules and have dipole-dipole forces, but the strength of these forces increases in the order HCl < CH3F < CO due to the increasing polarity of the molecules.