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For more information on the Visual Elements image see the Uses and properties section below. < Move to Sulfur Move to Argon > Chlorine  Discovery date1774 Discovered byCarl Wilhelm Scheele Origin of the nameThe name is derived from the Greek 'chloros', meaning greenish yellow. AllotropesCl2 Cl Chlorine 17 35.45
Glossary Group Period Block Atomic number Electron configuration Melting point Boiling point Sublimation Density (g cm−3) Relative atomic mass Isotopes CAS number Fact boxFact boxGroup17 Melting point−101.5°C, −150.7°F, 171.7 K Period3 Boiling point−34.04°C, −29.27°F, 239.11 K Blockp Density (g cm−3)0.002898 Atomic number17 Relative atomic mass35.45 State at 20°CGas Key isotopes35Cl, 37Cl Electron configuration[Ne] 3s23p5 CAS number7782-50-5 ChemSpider ID4514529ChemSpider is a free chemical structure database
Glossary Image explanation Murray Robertson is the artist behind the images which make up Visual Elements. This is where the artist explains his interpretation of the element and the science behind the picture. Appearance The description of the element in its natural form. Biological role The role of the element in humans, animals and plants. Natural abundance Where the element is most commonly found in nature, and how it is sourced commercially. Uses and propertiesUses and propertiesImage explanation The symbol shows a gas mask. This is because chlorine is a toxic gas, and has been used as a chemical weapon. Chlorine is yellowy-green in colour, as is the image. Appearance A yellowy-green dense gas with a choking smell. Uses Chlorine kills bacteria – it is a disinfectant. It is used to treat drinking water and swimming pool water. It is also used to make hundreds of consumer products from paper to paints, and from textiles to insecticides. About 20% of chlorine produced is used to make PVC. This is a very versatile plastic used in window frames, car interiors, electrical wiring insulation, water pipes, blood bags and vinyl flooring. Another major use for chlorine is in organic chemistry. It is used as an oxidising agent and in substitution reactions. 85% of pharmaceuticals use chlorine or its compounds at some stage in their manufacture. In the past chlorine was commonly used to make chloroform (an anaesthetic) and carbon tetrachloride (a dry-cleaning solvent). However, both of these chemicals are now strictly controlled as they can cause liver damage. Chlorine gas is itself very poisonous, and was used as a chemical weapon during the First World War. Biological role The chloride ion is essential to life. It is mostly present in cell fluid as a negative ion to balance the positive (mainly potassium) ions. It is also present in extra-cellular fluid (eg blood) to balance the positive (mainly sodium) ions. We get most of the chloride we need from salt. Typical daily salt intake is about 6 grams, but we could manage with half this amount. Natural abundance Chlorine is not found uncombined in nature. Halite (sodium chloride or ‘common salt’) is the main mineral that is mined for chlorine. Sodium chloride is a very soluble salt that has been leached into the oceans over the lifetime of the Earth. Several salt beds, or ‘lakes’ are found where ancient seas have evaporated, and these can be mined for chloride. Chlorine is also found in the minerals carnallite (magnesium potassium chloride) and sylvite (potassium chloride). 40 million tonnes of chlorine gas are made each year from the electrolysis of brine (sodium chloride solution). This process also produces useful sodium hydroxide. Help text not available for this section currently HistoryHistoryElements and Periodic Table History Hydrochloric acid (HCl) was known to the alchemists. The gaseous element itself was first produced in 1774 by Carl Wilhelm Scheele at Uppsala, Sweden, by heating hydrochloric acid with the mineral pyrolusite which is naturally occuring manganese dioxide, MnO2. A dense, greenish-yellow gas was evolved which he recorded as having a choking smell and which dissolved in water to give an acid solution. He noted that it bleached litmus paper, and decolourised leaves and flowers. Humphry Davy investigated it in 1807 and eventually concluded not only that it was a simple substance, but that it was truly an element. He announced this in 1810 and yet it took another ten years for some chemists finally to accept that chlorine really was an element.
Glossary Atomic radius, non-bonded Covalent radius Electron affinity Electronegativity (Pauling scale) First ionisation energy Atomic dataAtomic dataAtomic radius, non-bonded (Å)1.75Covalent radius (Å)1.00Electron affinity (kJ mol−1)348.575Electronegativity 1st 1251.186 2nd 2297.663 3rd 3821.78 4th 5158.608 5th 6541.7 6th 9361.97 7th 11018.221 8th 33603.91
Glossary Bond enthalpy (kJ mol−1) Bond enthalpiesBond enthalpiesCovalent bondEnthalpy (kJ mol−1)Found inCl–Cl242.1Cl2C–Cl339generalC–Cl327.2CCl4Cl–H431.4HCl
Glossary Common oxidation states The oxidation state of an atom is a measure of the degree of oxidation of an atom. It is defined as being the charge that an atom would have if all bonds were ionic. Uncombined elements have an oxidation state of 0. The sum of the oxidation states within a compound or ion must equal the overall charge. Isotopes Atoms of the same element with different numbers of neutrons. Key for isotopes Half life yyears ddays hhours mminutes ssecondsMode of decay αalpha particle emission βnegative beta (electron) emission β+positron emission ECorbital electron capture sfspontaneous fission ββdouble beta emission ECECdouble orbital electron capture Oxidation states and isotopesOxidation states and isotopesCommon oxidation states7, 5, 3, 1, -1IsotopesIsotopeAtomic massNatural abundance (%)Half lifeMode of decay 35Cl34.96975.76- - 37Cl36.96624.24- -
Glossary Data for this section been provided by the British Geological Survey. Relative supply risk An integrated supply risk index from 1 (very low risk) to 10 (very high risk). This is calculated by combining the scores for crustal abundance, reserve distribution, production concentration, substitutability, recycling rate and political stability scores. Crustal abundance (ppm) The number of atoms of the element per 1 million atoms of the Earth’s crust. Recycling rate The percentage of a commodity which is recycled. A higher recycling rate may reduce risk to supply. Substitutability The availability of suitable substitutes for a given commodity. Production concentration The percentage of an element produced in the top producing country. The higher the value, the larger risk there is to supply. Reserve distribution The percentage of the world reserves located in the country with the largest reserves. The higher the value, the larger risk there is to supply. Political stability of top producer A percentile rank for the political stability of the top producing country, derived from World Bank governance indicators. Political stability of top reserve holder A percentile rank for the political stability of the country with the largest reserves, derived from World Bank governance indicators. Supply riskSupply riskRelative supply risk4Crustal abundance (ppm)145Recycling rate (%)UnknownSubstitutabilityUnknownProduction concentration (%)24.3Reserve distribution (%)UnknownTop 3 producers
Glossary Specific heat capacity (J kg−1 K−1) Specific heat capacity is the amount of energy needed to change the temperature of a kilogram of a substance by 1 K. Young's modulus A measure of the stiffness of a substance. It provides a measure of how difficult it is to extend a material, with a value given by the ratio of tensile strength to tensile strain. Shear modulus A measure of how difficult it is to deform a material. It is given by the ratio of the shear stress to the shear strain. Bulk modulus A measure of how difficult it is to compress a substance. It is given by the ratio of the pressure on a body to the fractional decrease in volume. Vapour pressure A measure of the propensity of a substance to evaporate. It is defined as the equilibrium pressure exerted by the gas produced above a substance in a closed system. Pressure and temperature data – advancedPressure and temperature data – advancedSpecific heat capacity Help text not available for this section currently PodcastsPodcastsListen to Chlorine Podcast Transcript : Chemistry in its element: chlorine(Promo) You're listening to Chemistry in its element brought to you by Chemistry World, the magazine of the Royal Society of Chemistry. (End promo) Chris Smith Hello. What's got three isotopes, keeps swimming pools clean, damages the ozone layer and is used in more chemical synthesis reactions than you can shake a benzene ring at. Well the man with the answer is Tim Harrison. Tim Harrison Chlorine is what you might describe as a Jekyll and Hyde element; it is the friend of the synthetic chemist and has found a use in a number of 'nice' applications such as the disinfecting of drinking water and keeping our swimming pools clean. It also has an unpleasant side, being the first chemical warfare agent and taking some of the blame in the depletion of the Earth's ozone layer. Elemental chlorine is a pale, yellowy green gas at room temperature. It was the Greek word khlôros meaning 'yellowish-green' that was used as inspiration by Sir Humphrey Davy when he named this element in the 19th century. This element was first isolated in 1774 by the Swiss-German chemist Carl Wilhelm Scheele, by reacting hydrochloric acid with manganese (IV) oxide. But he failed to realise his achievement, mistakenly believing it also contained oxygen. It was Davy in 1810 who finally concluded that Scheele had made elemental chlorine. Chlorine is in group 17 of periodic table, also called the halogens, and is not found as the element in nature - only as a compound. The most common of these being salt, or sodium chloride, and the potassium compounds sylvite (or potassium chloride) and carnallite (potassium magnesium chloride hexahydrate). It is also estimated that there are around two thousand organic chlorine compounds. Chlorine has two stable isotopes chlorine-35 and chlorine-37with Chlorine-35 accounting for roughly 3 out of every 4 naturally occurring chlorine atoms. Chlorine-36 is also known naturally and is a radioactive isotope with a half life of about 30,000 years. Chlorine has a major role to play in synthetic organic chemistry, taking part in three of the most common reaction mechanisms. In the first of these, the photochemical substitution reaction, chlorine reacts with an alkane by replacing one of the hydrogen atoms attached to a carbon forming a chloroalkane. This radical reaction is initiated by the use of sunlight or ultraviolet light to split diatomic chlorine into two radicals. Chlorine can also react with alkenes via the electrophilic addition mechanism. This time two chlorine atoms add to a molecule across the electron-rich carbon-carbon double bond. This reaction has to be carried out in the dark to avoid complications with competing free radical substitutions. A third common mechanism is electrophilic substitution, which occurs when chlorine reacts with a benzene ring by replacing a hydrogen atom forming chlorobenzene and hydrogen chloride. This reaction is most commonly known as the Friedal-Crafts reaction. Chlorine also has a multitude of industrial uses. Including making bulk materials like bleached paper products, plastics such as PVC and the solvents tetrachloromethane, chloroform and dichloromethane. It is also used to make dyes, textiles, medicines, antiseptics, insecticides and paints. It's best known uses however are probably in making bleaches such as 'Domestos' and in treating drinking and swimming pool waters to make them safe to use and of course its role as a chemical warfare agent. The treatment of water with chlorine began in London after a cholera outbreak in 1850 when the physician and pioneering hygienist John Snow identified a well in Soho as the source of the outbreak. Chlorine is still used in most sewage treatment works today. Snow also used a compound of chlorine - chloroform with the formula CHCl3 - as an anesthetic to aid the childbirth of two of Queen Victoria's children. The use of chlorine gas as a chemical weapon was pioneered by German chemist Fritz Haber, who is better known for his work with ammonia. It was first used against the Allied soldiers in the battle of Ypres during the first world war. While it was quickly replaced by the more deadly phosgene and mustard gases, chlorine gas has been used as a weapon as recently as 2007 in Iraq during the second gulf war. Chlorine was also once used to make a series of aerosol solvents and refrigerants called chlorofluorocarbons or CFCs. However their use was stopped once it became apparent that when in the atmosphere these compounds absorb ultraviolet light and cause homolytic bond fission producing a chlorine free radical which in turn reacts with ozone. This has led to a reduction in the concentration of ozone in the so-called ozone layer, and therefore a reduction in the protection for those of us on the surface of the planet making us more susceptible to skin cancers. So, that's chlorine - a Jeckll and Hyde element with an extremely wide range of applications. Chris Smith So slap on your sun screen. Tim Harrison was telling the tale of Element number 17, and that's chlorine. Tim's based at the University of Bristol's ChemLabs. Next week, the stuff that gives itself an x-ray. Brian Clegg This grey metallic element gives off beta particles as it decays. These can cause radioactive damage in their own right, but prometheum is probably most dangerous because those beta particles generate X-rays when they hit heavy nuclei, making a sample of promethium bathe its surroundings in a constant low dosage x-ray beam. It was initially used to replace radium in luminous dials. Promethium chloride was mixed with phosphors that glow yellowy-green or blue when radiation hits them. However, as the dangers of the element's radioactive properties became apparent, this too was dropped from the domestic glow-in-the-dark market, only employed now in specialist applications. Chris Smith And you can hear what some of those applications are when Brian Clegg looks at the story of promethium in next week's Chemistry in its Element. In the meantime more elements are available from the Chemistry in its Element podcast, that's on iTunes or on the web at chemistryworld.org/elements. I'm Chris Smith, thank you very much for listening and goodbye. (Promo) Chemistry in its element is brought to you by the Royal Society of Chemistry and produced by thenakedscientists.com. There's more information and other episodes of Chemistry in its element on our website at chemistryworld.org/elements. (End promo) Help text not available for this section currently VideoVideoClick here to view videos about Chlorine View videos about Help Text ResourcesResourcesLearn Chemistry: Your single route to hundreds of free-to-access chemistry teaching resources.
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What do you call the atoms of the same element that have different atomic mass number due to different numbers of neutrons?Isotopes are atoms of the same element that have different numbers of neutrons but the same number of protons and electrons. The difference in the number of neutrons between the various isotopes of an element means that the various isotopes have different masses.
What is it called there are two atoms of the same element with different atomic masses what on the subatomic level is different between the two atoms?We refer to the atoms of the same element with different numbers of neutrons as "isotopes".
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What do we call atoms of the same element with different mass numbers explain the meaning of each term in the symbol?
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