Chlorine (Cl2) is a highly reactive, greenish-yellow gas. It is used in water treatment, as a disinfectant, and in the production of various chemicals, such as PVC and solvents.
| IUPAC Name | Dichlorine |
| Molecular Formula | Cl2 |
| CAS Number | 7782-50-5 |
| Synonyms | Molecular chlorine, Chlore, Cloro, Chlor, Chloor, Cloreto de cloro |
| InChI | InChI=1S/Cl2/c1-2 |
Cl2 Molar Mass
The molar mass of Cl2, or dichlorine, is the sum of the atomic masses of two chlorine atoms, which is 70.906 g/mol. It is important to know the molar mass of Cl2 when calculating the amount of the substance needed for a chemical reaction or when converting between different units of measurement.
Cl2 Lewis Structure
Cl2 has a linear molecular geometry with two chlorine atoms bonded by a single covalent bond. Its Lewis structure consists of two Cl atoms each with three lone pairs and a shared pair of electrons between them.
Cl2 Boiling Point
The boiling point of Cl2 is -34.04°C (-29.27°F) at standard pressure. This is a relatively low boiling point, which makes Cl2 gas at room temperature and pressure. It is important to be cautious when handling Cl2 because it can easily convert to a liquid or solid at low temperatures and pressures.
Cl2 Melting Point
The melting point of Cl2 is -101.5°C (-150.7°F) at standard pressure. This is a relatively low melting point, which makes Cl2 gas at room temperature and pressure. It is important to be cautious when handling Cl2 because it can easily convert to a liquid or solid at low temperatures and pressures.
Cl2 Density g/ml
The density of Cl2 is 0.003214 g/mL at standard temperature and pressure (STP). This means that Cl2 is much less dense than air, and it will rise in the atmosphere. Cl2 can be stored in pressurized cylinders or in tanks with heavier-than-air gas such as nitrogen.
Chlorine Molecular Weight
The molecular weight of Cl2 is 70.906 g/mol. This is the mass of one mole of Cl2, which contains Avogadro’s number of molecules (6.022 x 10^23). The molecular weight of Cl2 is important for stoichiometric calculations in chemistry.
Chlorine Structure
The structure of Cl2 is linear, with two chlorine atoms bonded together by a covalent bond. The bond length between the two chlorine atoms is 1.99 Ångstroms, and the bond energy is 242 kJ/mol. The electron configuration of Cl2 is [Ne]3s23p5, with each chlorine atom contributing one electron to the bonding pair.
Chlorine Formula
The formula for Cl2 is simply two Cl atoms bonded together. This is represented as Cl-Cl or Cl2. The formula is important for identifying the composition of a compound or molecule, and for stoichiometric calculations in chemistry.
| Appearance | Greenish-yellow gas |
| Specific Gravity | 1.56 (liquid) |
| Color | Greenish-yellow |
| Odor | Pungent, suffocating odor |
| Molar Mass | 70.906 g/mol |
| Density | 0.003214 g/mL at STP |
| Melting Point | -101.5°C (-150.7°F) |
| Boiling Point | -34.04°C (-29.27°F) |
| Flash Point | Non-flammable |
| Water Solubility | 0.92 g/100 mL at 20°C |
| Solubility | Soluble in water, ethanol, ether, benzene, and many organic solvents |
| Vapor Pressure | 102.44 kPa at 20°C |
| Vapor Density | 2.49 (air = 1) |
| pKa | – |
| pH | – |
Cl2 Safety and Hazards
Chlorine is a highly reactive gas that can pose serious safety and health hazards if not handled properly. It can cause severe respiratory irritation and damage to the eyes, skin, and mucous membranes. Inhaling high concentrations of Chlorine can cause pulmonary edema, which can be life-threatening. Chlorine is also highly corrosive and can cause damage to metals, plastics, and other materials. To ensure safe handling of Chlorine, appropriate personal protective equipment must be worn, such as goggles, gloves, and a respirator. Chlorine should only be used in well-ventilated areas, and all containers should be properly labeled and stored in a secure location.
| Hazard Symbols | Skull and crossbones |
| Safety Description | Highly toxic and corrosive gas; causes severe respiratory and skin irritation; can be fatal if inhaled at high concentrations |
| UN IDs | UN1017 |
| HS Code | 2801.1 |
| Hazard Class | 2.3 |
| Packing Group | I |
| Toxicity | Highly toxic; inhalation of high concentrations can cause pulmonary edema and be fatal |
Chlorine Synthesis Methods
There are various methods to synthesize chlorine gas, including the electrolysis of brine, the oxidation of HCl, and the thermal decomposition of metal chlorides.
The most common method is the electrolysis of brine, which involves passing an electric current through a solution of sodium chloride (NaCl) and water (H2O). This process generates chlorine gas at the anode and hydrogen gas at the cathode.
Another method for producing chlorine is the oxidation of HCl with an oxidizing agent, such as KMnO4 or MnO2. This reaction produces chlorine gas and water as byproducts.
The thermal decomposition of metal chlorides, such as MgCl2 or FeCl3, is another method for generating chlorine gas. This process involves heating the metal chloride to a high temperature, which causes it to decompose and release chlorine gas.
Overall, the synthesis method used for chlorine depends on the specific application and desired purity of the gas. Regardless of the method used, it is important to handle chlorine with caution due to its highly reactive and toxic nature.
Chlorine Uses
Chlorine gas has a wide range of uses in various industries. One of the primary uses of chlorine is in the production of polyvinyl chloride (PVC), a widely used plastic material. Chlorine is also used in the production of other chlorinated compounds, such as chloroform and carbon tetrachloride, which are used as solvents and in the manufacturing of refrigerants.
In the water treatment industry, chlorine is commonly used as a disinfectant for treating drinking water and wastewater. chlorine gas is effective at killing bacteria and viruses, and it can also oxidize and remove organic compounds and other contaminants from water.
In the pulp and paper industry, chlorine gas is used as a bleaching agent to whiten paper products. It is also used in the production of textiles, such as nylon and polyester, as well as in the manufacturing of dyes and pigments.
Chlorine gas has other applications as well, including in the production of certain pharmaceuticals and in the metalworking industry for etching and cleaning metal surfaces. However, due to its hazardous nature, chlorine must be handled with care and appropriate safety precautions must be taken during its storage, transportation, and use.
Questions:
Q: Is Cl2 polar or nonpolar?
A: Cl2 is a nonpolar molecule.
Q: Is chlorine a metal?
A: No, chlorine is not a metal. It is a halogen and belongs to the nonmetal group of elements.
Q: What soft metal combines with chlorine to make table salt?
A: Sodium (Na) is the soft metal that combines with chlorine (Cl) to make table salt (NaCl).
Q: How to do chlorination of water?
A: Chlorination of water is typically done by adding a measured amount of chlorine gas, sodium hypochlorite, or calcium hypochlorite to the water supply. The amount of chlorine added depends on the quality of the water and the desired level of disinfection. The chlorine reacts with bacteria and other microorganisms in the water, effectively killing them and making the water safe for consumption.
Q: Which of the following is treated with chlorine to obtain bleaching powder?
A: Calcium oxide (CaO) is treated with chlorine (Cl2) to obtain bleaching powder (CaOCl2).