Difference between revisions of "Chlorine"

Revision as of 08:29, 24 August 2021

Chlorine,  ₁₇Cl

Chlorine gas in an ampoule.
General properties
Name, symbol	Chlorine, Cl
Appearance	Greenish gas
Chlorine in the periodic table
F ↑ Cl ↓ Br Sulfur ← Chlorine → Argon
Atomic number	17
Standard atomic weight (Ar)	35.45
Group, block	(halogens); p-block
Period	period 17
Electron configuration	[Ne] 3s2 3p5
per shell	2, 8, 7
Physical properties
Pale green
Phase	Gas
Melting point	171.6 K ​(−101.5 °C, ​−150.7 °F)
Boiling point	239.11 K ​(−34.04 °C, ​​−29.27 °F)
Density at  (0 °C and 101.325 kPa)	3.2 g/L
when liquid, at	1.5625 g/cm3
Critical point	416.9 K, 7.991 MPa
Heat of fusion	6.406 kJ/mol
Heat of	20.41 kJ/mol
Molar heat capacity	33.949 J/(mol·K)
pressure
Atomic properties
Oxidation states	7, 6, 5, 4, 3, 2, 1, −1 ​(a strongly acidic oxide)
Electronegativity	Pauling scale: 3.16
energies	1st: 1251.2 kJ/mol 2nd: 2298 kJ/mol 3rd: 3822 kJ/mol
Covalent radius	102±4 pm
Van der Waals radius	175 pm
Miscellanea
Crystal structure	​Orthorhombic
Thermal conductivity	8.9×10−3 W/(m·K)
Electrical resistivity	>10 Ω·m (at 20 °C)
Magnetic ordering	Diamagnetic
CAS Registry Number	7782-50-5
Discovery and first isolation	Carl Wilhelm Scheele (1774)
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Chlorine is the second-lightest halogen, with the symbol Cl and atomic number 17. It has a sickly green colour and a distinctive smell, recognizable to many at low concentrations as 'the smell of pool centers' due to its compounds use as a water disinfecting agent.

Properties

Chemical

Chlorine is a strong oxidizer with 7 valence electrons. Its unstable electron configuration results in high reactivity. Because of this, chlorine usually exists on earth in the form of a halide salt, and free chlorine is rare. Like fluorine, elemental chlorine forms a highly reactive diatomic gas.^[1] Chlorine, like other halogens, forms many oxoanions, negatively charged ions containing oxygen. Most notably, these are hypochlorite(ClO^-), chlorite(ClO₂^-), chlorate(ClO₃^-), and perchlorate(ClO₄^-).

Unlike hydrochloric acid, elemental chlorine easily corrodes copper, especially in moist air.^[2]

Physical

Chlorine is a yellow-greenish gas, with a powerful odor similar to that of boiling hypochlorite solutions. It is heavier than air, and slightly soluble in water, 3.26 g/L.

Availability

While liquid (as in liquefied, and not aqueous solution) chlorine is sold by gas companies, it is hard to get hold of as it's very toxic and corrosive.

Chlorine is better produced from OTC products.

Production

There are many methods to generating chlorine gas, due to it being such a commonly used ion.

Potassium permanganate will oxidize hydrochloric acid to chlorine gas, as will manganese dioxide. In both cases, manganese(II) chloride will be produced as well.

A hypochlorite and hydrochloric acid will produce chlorine; either a solution of sodium hypochlorite or calcium hypochlorite. A violent reaction with a lot of foam may take place in the case of the latter, and starting small scale is a must to get a sense for the reaction before any large scale chlorine production is attempted.

A popular way of making chlorine on Sciencemadness is using hydrochloric acid and trichloroisocyanuric acid (TCCA). TCCA can be found as slow release chlorine tablets for swimming pools. This reaction is favorable because it not too expensive, produces a large amount of chlorine over an extended period of time (while hypochlorites tend to violently produce all the chlorine right on mixing with the acid), leaves no awful byproducts (such as MnO₂) and the reaction speed at standard concentrations and temperatures is not too fast nor too slow for most applications.

Projects/Experiments

Chlorine can be used to produce anhydrous metal chlorides, such as aluminum(III) chloride, iron(II) or iron(III) chloride, and many others, which cannot be made in solution, due to formation of hydrates which are irreversible, and decompose to the metal oxide and HCl gas upon heating.

2 Al + 3 Cl₂ → 2 AlCl₃

2 Fe + 3 Cl₂ → 2 FeCl₃

Other projects:

• Make hypochlorites
• Make sulfur dichloride
• Make disulfur dichloride
• Make interhalogen compounds
• Alkane halogenation

Handling

Safety

Elemental chlorine is extremely toxic and corrosive to many common metals. Because it is heavier than air, it tends to accumulate at the bottom of poorly ventilated spaces. Chlorine gas is a strong oxidizer, which may react with flammable materials. It is notorious for reacting with iron at high temperatures, in a strong exothermic reaction, known as chlorine-iron fire.

Storage

Liquefied chlorine must be stored in cold places, away from any source of heat. Chlorine can be liquefied at room temperature, at a pressure of 7.4 bar.

Chlorine releasing chemicals, such as bleach and TCCA should be stored in closed bottles, usually covered with a bag or in a box, that must be opened form time to time to release the pressure.

The storage area for both chemicals should not contain any metal parts susceptible to chlorine attack.

Disposal

As it is toxic and has an irritating smell, it is recommended to neutralize chlorine before disposing of it. In gaseous form, elemental chlorine can be neutralized with ammonia, reaction that produces nitrogen gas and ammonium chloride, though chloramines may also be produced as side products.

Aqueous chlorine however, should never be neutralized with ammonia, as it will generate toxic chloramines. Acids should also be avoided. Hydrogen peroxide will neutralize bleach and release oxygen. Ascorbic acid and its salts are also good at neutralizing chlorine. Other good neutralizing agents are certain sulfur compounds, such as bisulfites, metabisulfites, thiosulfites.

Gallery

• 

  A sample of liquid chlorine

References

1. ↑ "Handbook of Toxicology of Chemical Warfare Agents", Academic Press, 2009, p. 313.
2. ↑ Handbook of Corrosion Data, by Bruce D. Craig, David S. Anderson, p. 271

Relevant Sciencemadness threads

• Chlorine gas neutralization