Chlorine is a halogen in group 17 and period 3. It is very reactive and is widely used for many purposes, such as as a disinfectant. Due to its high reactivity, it is commonly found in nature bonded to many different elements.
- Chlorine Atomic Number And Atomic Mass
- Chlorine Atomic Number And Mass
- Chlorine Atomic Mass
- How Many Protons Are In Chlorine
Our chlorine page has over 210 facts that span 98 different quantities. Each entry has a full citation identifying its source. Areas covered include atomic structure, physical properties, atomic interaction, thermodynamics, identification, atomic size, crystal structure, history, abundances, and nomenclature. Chlorine is a chemical element with symbol Cl and atomic number 17. Classified as a halogen, Chlorine is a gas at room temperature. Chlorine atom Cl CID 5360523 - structure, chemical names, physical and chemical properties, classification, patents, literature, biological activities, safety.
Chlorine, which is similar to fluorine but not as reactive, was prepared by Sheele in the late 1700's and shown to be an element by Davy in 1810. It is a greenish-yellow gas with a disagreeable odor (you can detect it near poorly balanced swimming pools). Its name comes from the Greek word chloros, meaning greenish-yellow. In high concentration it is quite toxic and was used in World War I as a poison gas.
Properties
Chlorine Atomic Number And Atomic Mass
| Atomic Number | 17 |
| Atomic Weight | 35.457 |
| Electron Configuration | [Na]3s23p5 |
| 1st Ionization Energy | 1251 kJ/mol |
| Ionic Radius | 181 pm |
| Density (Dry Gas) | 3.2 g/L |
| Melting Point | -101°C |
| Boiling Point | -34.05°C |
| Specific Heat | 0.23 g cal/g/°C |
| Heat of Vaporization | 68 g cal/g |
| Heat of Fusion | 22 g cal/g |
| Critical Temperature | 114°C |
Standard Electron Potential (Cl_2 + 2e^- rightarrow 2Cl^-) | 1.358V |
At room temperature, pure chlorine is a yellow-green gas. Chlorine is easily reduced, making it a good oxidation agent. By itself, it is not combustible, but many of its reactions with different compounds are exothermic and produce heat. Because chlorine is so highly reactive, it is found in nature in a combined state with other elements, such as NaCl (common salt) or KCl (sylvite). It forms strong ionic bonds with metal ions.
Like fluorine and the other members of the halogen family, chlorine is diatomic in nature, occurring as (Cl_2) rather than Cl. It forms -1 ions in ionic compounds with most metals. Perhaps the best known compound of that type is sodium chloride, common table salt (NaCl).
Small amounts of chlorine can be produced in the lab by oxidizing (HCl) with (MnO_2). On an industrial scale, chlorine is produced by electrolysis of brines or even sea water. Sodium hydroxide (also in high demand) is a by-product of the process.
In addition to the ionic compounds that chlorine forms with metals, it also forms molecular compounds with non-metals such as sulfur and oxygen. There are four different oxides of the element. Hydrogen chloride gas (from which we get hydrochloric acid) is an important industrial product.
Reactions with Water
Usually, reactions of chlorine with water are for disinfection purposes. Chlorine is only slightly soluble in water, with its maximum solubility occurring at 49° F. After that, its solubility decreases until 212° F. At temperatures below that range, it forms crystalline hydrates (usually (Cl_2)) and becomes insoluble. Between that range, it usually forms hypochlorous acid ((HOCl)). This is the primary reaction used for water/wastewater disinfection and bleaching.
[Cl_2+H_2O rightarrow HOCl + HCl]
At the boiling temperature of water, chlorine decomposes water
[2Cl_2+2H_2O rightarrow 4HCl + O_2]
Reactions with Oxygen
Although chlorine usually has -1 oxidation state, it can have oxidation states of +1, +3, +4, or +7 in certain compounds, such as when it forms Oxoacids with the alkali metals
| Oxidation State | Compound |
| +1 | NaClO |
| +3 | NaClO2 |
| +5 | NaClO3 |
| +7 | NaClO4 |
Reactions with Hydrogen
When H2 and Cl2 are exposed to sunlight or high temperatures, they react quickly and violently in a spontaneous reaction. Otherwise, the reaction proceeds slowly.
[H_2+Cl_2 rightarrow 2HCl]
HCl can also be produced by reacting Chlorine with compounds containing Hydrogen, such as Hydrogen sulfide
Reactions with Halogens
Chlorine, like many of the other halogens, can form interhalogen compounds (examples include BrCl, ICl, ICl2). The heavier elements in one of these compounds acts as the central atom. For Chlorine, this occurs when it is bounded to fluorine in ClF, ClF3, and ClF5
Reactions with Metals
Chlorine reacts with most metals and forms metal chlorides, with most of these compounds being soluble in water. Examples of insoluble compounds include (AgCl) and (PbCl_2). Gaseous or liquid chlorine usually does not have an effect on metals such as iron, copper, platinum, silver, and steel at temperatures below 230°F. At high temperatures, however, it reacts rapidly with many of the metals, especially if the metal is in a form that has a high surface area (such as when powdered or made into wires).
Example: Oxidizing Iron
Chlorine can oxidizing iron
[Cl_2+Fe rightarrow FeCl_2]
Half Reactions:
[Fe rightarrow Fe^{+2} +2e^-]
[Cl_2+2e^- rightarrow 2Cl^-]
Isotopes
(ce{^35}Cl) and (ce{^37}Cl) are the two natural, stable isotopes of Chlorine. (ce{^36}Cl), a radioactive isotope, occurs only in trace amounts as a result of cosmic rays in the atmosphere. Chlorine is usually a mixture of 75% (ce{^35}Cl) and 25% (ce{^37}Cl). Besides these isotopes, the other isotopes must be artificially produced. A table containing some common isotopes is found below:
| Isotope | Atomic Mass | Half-Life |
| (ce{^35}Cl) | 32.986 | 2.8 seconds |
| (ce{^34}Cl) | 33.983 | 33 minutes |
| (ce{^35}Cl) | 34.979 | Stable ((infty)) |
| (ce{^36}Cl) | 35.978 | 400,000 years |
| (ce{^37}Cl) | 35.976 | Stable ((infty)) |
| (ce{^38}Cl) | 37.981 | 39 Minutes |
Production and Uses
Chlorine is a widely used chemical with many applications.
Water Treatment
Chlorine is used in the disinfection (removal of harmful microorganisms) of water and wastewater. In the United States, it is almost exclusively used. Chlorine was first used to disinfect drinking water in 1908, using sodium hypochlorite (NaOCl):
[NaOCl+ H_2O rightarrow HOCl+NaOH]
Following widespread use of sodium hypochlorite to disinfect water, diseases caused by unclean water decreased greatly. Compared to other methods, it is effective at lower concentrations and is inexpensive.
Polyvinyl Chloride (PVC)
Polyvinyl Chloride is a plastic which is widely manufactured throughout the globe, and is responsible for nearly a third of the world’s use of chlorine. It is usually manufactured by first taking EDC (ethylene dichloride) and then making it into a vinyl chloride, the basic unit for PVC. From then on, vinyl chloride monomers are linked together to form a polymer. PVC becomes malleable at high temperatures, making it flexible and ideal for many purposes from pipes to clothing. However, PVC is toxic. When in gaseous form and inhaled, it can cause damage to the lungs, the body’s blood circulation, and nervous system. The production of PVC has many regulations surrounding it due to the many harmful effects that the plastic itself and the intermediates involved have on the environment and on human health.
Paper Bleaching
Paper is one of the most widely consumed products in the world. Before wood is made into a paper product, however, it must be turned into pulp (separated fibrous material). This pulp has a color that ranges from light to dark brown. Chlorine is used to bleach the pulp to turn it into a bright, white color, which makes it desirable for consumers. The process usually involves a number of steps, depending on the nature of the pulp.
Problems
1) Solve and balance the following equations
- (H_2S + Cl_2 + H_2O rightarrow)
- (Sb + Cl_2 +H_2O rightarrow )
2) Write the electron configuration for Chlorine.
3) What is the molecular geometry of the following? (See Valence Bond Theory) Free download microsoft visio 2010 full version product key.
- (ClO_2)
- (ClF_5)
4) What are the naturally occurring Chlorine isotopes?
5) When does Chlorine have an oxidation state of +5?
Answers
1) Solve and balance the following equations:
- H2S + 4Cl2 + 4H20 --> H2S04 + HCl
- 2Sb + 3Cl2 +H20 > 2SbCl3
2) The electron configuration of Chlorine is: 1s22s22p63s23p5
3) What is the molecular geometry of the following?
- (ClO_2) -Bent or angular; ClO2 is bonded to two ligands, has one lone pair and one unpaired electron.
- (ClF_5) -Square pyramid; ClO2 is bonded to five ligands and has one lone pair
4) The naturally occurring Chlorine isotopes are Chlorine-35 and Chlorine-36. While Chlorine-37 does occur naturally, it is radioactive and unstable.
5) Chlorine has an oxidation state of +5 when it reacts with oxoacids with the Alkali Metals.
References
- Sconce, J.S. Chlorine: Its Manufacture, Properties, and Uses. Reinhold Corporation, 1962.
- Stringer, Ruth, and Paul Johnston. Chlorine and the Enviroment. Norwell: Kluwer Academic, 2001.
- Reynolds, Tom D. Unit Operations and Processes in Environmental Engineering. Brooks/Cole Engineering Division, a Division of Wadsworth Inc, 1982. 523-532
- Davis, Stanley N., DeWayne Cecil, Marek Zreda, and Pankaj Sharma. 'Chlorine-36 and the Initial Value Problem.' Hydrogeology Journal 6.1 (1998): 104-14. SpringerLink. Web. 23 May 2010. <www.springerlink.com/content/3205uburlwx2x48g/>
- Pettrucci, Ralph H. General Chemistry: Principles and Modern Applications. 9th. Upper Saddle River: Pearson Prentice Hall, 2007
Contributors and Attributions
- Judy Hsia (University of California, Davis)
Atomic Number of Chlorine is 17.
Chemical symbol for Chlorine is Cl. Number of protons in Chlorine is 17. Atomic weight of Chlorine is 35.45 u or g/mol. Melting point of Chlorine is -34,6 °C and its the boiling point is -101 °C.
» Boiling Point» Melting Point» Abundant» State at STP» Discovery YearAbout Chlorine
Chlorine is a light green-yellowish gas, with irritating odor and very toxic properties. The name of this gas is derived from a Greek expression meaning yellow-green. It is one of the oldest known disinfectants as it can very effectively destroy a large number of bacteria. It is very reactive and creates a variety of compounds which are widely used in chemical and other industries. Chlorine is important for life, and we usually take it in small doses from salt. It is impossible to find this chemical element in its pure form in nature; it is usually received from minerals known as halites, which are sodium chlorides. Chloride is used for producing bleach and other disinfectants, especially for disinfecting water. It is also widely used in organic chemistry and in pharmacology, to speed up chemical reactions and manufacturing processes. Chlorine is also used for producing PVC with further use in construction, medicine, car parts, and so on.
Uses of Chlorine
Chlorine (Cl), the second lightest element of the halogens, is mostly used as a disinfectant for drinking water and swimming pools. It also is used in the manufacturing of consumer products such as paper, textiles, contact lenses, solar panels, paints, prosthetics, etc. An important percentage of chlorine is used in making PVC (Polyvinyl chloride) which is a widely produced plastic polymer. PVC is extensively used in manufacturing pipes, electrical cables, building construction, sports clothing and medical devices.
Salt (Sodium chloride), a chemical compound with sodium and chloride ions, is preferred for household purposes, but also used in the production of many chemicals too. Besides, sodium chloride is used in the food industry, agriculture, medicine, the pulp and paper industry. Chlorine is also used on planes, boats and automobiles in the manufacturing of safety belts, airbags, bumpers, dashboards, etc.
Compounds with Chlorine
- NaCl: Salt (Sodium chloride)
- C2H3Cl: Vinyl chloride
- (C2H3Cl)n: Polyvinyl chloride (abbreviated PVC)
- Cl2O: Dichlorine monoxide
- NaClO3: Sodium chlorate
- HOCl: Hypochlorous acid
- HCl: Hydrogen chloride
- Ca(ClO)2: Calcium hypochlorite
- MgCl2: Magnesium dichloride
- CaCl2: Calcium chloride
- NH4Cl: Ammonium chloride
Properties of Chlorine Element
| Atomic Number (Z) | 17 |
|---|---|
| Atomic Symbol | Cl |
| Group | 17 |
| Period | 3 |
| Atomic Weight | 35.45 u |
| Density | 0.003214 g/cm3 |
| Melting Point (K) | 171.6 K |
| Melting Point (℃) | -34,6 °C |
| Boiling Point (K) | 239.11 K |
| Boiling Point (℃) | -101 °C |
| Heat Capacity | 0.479 J/g · K |
| Abundance | 145 mg/kg |
| State at STP | Gas |
| Occurrence | Primordial |
| Description | Halogen |
| Electronegativity (Pauling) χ | 3.16 |
| Ionization Energy (eV) | 12.96764 |
| Atomic Radius | 100pm |
| Covalent Radius | 99pm |
| Van der Waals Radius | 175 |
| Valence Electrons | 7 |
| Year of Discovery | 1774 |
| Discoverer | Scheele |
What is the Boiling Point of Chlorine?
Chlorine boiling point is -101 °C. Boiling point of Chlorine in Kelvin is 239.11 K.
What is the Melting Point of Chlorine?
Chlorine melting point is -34,6 °C. Melting point of Chlorine in Kelvin is 171.6 K.
Chlorine Atomic Number And Mass
How Abundant is Chlorine?
Abundant value of Chlorine is 145 mg/kg.
What is the State of Chlorine at Standard Temperature and Pressure (STP)?
Chlorine Atomic Mass
State of Chlorine is Gas at standard temperature and pressure at 0℃ and one atmosphere pressure.
When was Chlorine Discovered?
Chlorine was discovered in 1774.
How Many Protons Are In Chlorine