![]() It is also present in extra-cellular fluid (all body fluid outside the cells, eg: blood) to balance the positive ions (mainly sodium, Na). Biological role of ChlorineĬhloride ion is essential for life, and It is mostly present in cell fluid as a negative ‘-‘ ion to balance the positive ‘+’ ions (mainly potassium, K). It is also used in the production of Chloroform (CHCl 3, Sweet-smelling organic compound), Chlorates (ClO 3 –), carbon tetrachloride (a dry-cleaning solvent, CCl 4), & in the bromine extraction.Ĭhlorine gas is very poisonous, and it was used as a war gas (chemical weapon) during the First World War. Most of the chlorine is used in the manufacture of chlorinated compounds for sanitation, pulp bleaching (for paper making & also used in industrially to remove ink from recycle paper), disinfectants, and textile processing.Īnother major use of chlorine is in organic chemistry, where It is used in substitution reactions (single substitution reaction) & as an oxidising agent. It is used to treat drinking & swimming pool water, and also used to make hundreds of consumer products, such as production of paper products, textiles, dyestuffs, petroleum products, medicines, antiseptics, insecticides, solvents, food, plastics, paints, etc…Ībout 20% of chlorine is used to make PVC (polymerization of vinyl chloride), which is very versatile plastic that used in window frames, electrical wiring insulation, water pipes, car interiors, blood bags, & vinyl flooring. In Deacon process, Hydrogen chloride gas is convert to chlorine gas, by oxidation using oxygen:ĤHCl + O 2 → 2 Cl 2 + 2 H 2O Chlorine Historyĭiscovery and first isolation: Carl Wilhelm Scheele (1774) in Uppsala (Sweden) Chlorine UsesĬhlorine is a disinfectant, that kills bacteria. Sulfur reacts with excess Cl 2, and forming sulfur (I) chloride or sulfur (II) chloride:Ĭhlorine is produced by electrolysis of sodium chloride (NaCl) dissolved in water, and gives chlorine with hydrogen gas & sodium hydroxide.Ģ NaCl + 2 H 2O (l) → Cl 2 + H 2 + 2 NaOH Phosphorus reacts with excess Cl 2, and forming phosphorus chloride: Hydrogen reacts with Cl 2, and forming chloride, where the speed of reaction increase with increasing of temperature, even the reaction can be explosive under the right conditions. Reacts with hot aqueous alkali, and forming Chlorate (ClO 3 –).ģ Cl 2 (g) + 6 OH – (aq) → ClO 3 – (aq) + 5 Cl – (aq) + 3 H 2O (l) Iodide reacts with chlorine, and forming ClI:Ĭl 2 (g) + I 2 (g) → 2 ClI (s) (Chlorine iodide) When reacts with water, it forms hypochlorite (ClO –), where the position of equilibrium depends upon the pH of the solution.Ĭl 2 (g) + H 2O (l) ⇌ OCl – (aq) + 2 H + (aq) + Cl – (aq)įluorine Reacts with chlorine at 225 oC, and forming ClF & ClF 3:Ĭl 2 (g) + F 2 (g) → 2 ClF (g) (Chlorine (I) fluoride)Ĭl 2 (g) + 3 F 2 (g) → 2 ClF 3 (g) (Chlorine (III) fluoride)įluorine reacts at 225 oC & 225 Atm pressure, and forms ClF 5:Ĭl 2 (g) + 5 F 2 (g) → 2 ClF 5 (g) (Chlorine (V) fluoride)īromine reacts with chlorine, and forming ClBr:Ĭl 2 (g) + Br 2 (g) → 2 ClBr (g) (Bromine chloride) It doesn’t react with oxygen & nitrogen, but reacts with carbon monoxide (CO), and forming COCl 2: Grid parameters: a=6.29 Å b=4.5 Å c=8.21 ÅĮlectron affinity: 349 kJ/mol Nuclear Properties of Chlorine Ionization energies: 1st: 1251 kJ.mol 2nd: 2298 kJ/mol 3rd: 3822 kJ/mol Sound Speed: 206 m/s Atomic Properties of Chlorine Molar magnetic susceptibility: -0.511×10 -9 m 3/mol Physical Properties of Chlorineĭensity: 3.2 g/cm 3 (In STP) 1.562 g/cm 3 (In Liquid at B.P) Mass magnetic susceptibility: -7.2×10 -9 m 3/kg ![]() Volume magnetic susceptibility: -2.31×10 -8 Magnetic susceptibility (x mol): -40.5×10 -6 cm 3/mol Thermal conductivity: 8.9×10 -3 W/(m∙K) Electrical properties of ChlorineĪ Electrical type: Insulator Magnetic Properties of Chlorine Molar heat capacity: 33.950 J/(mol.K) (Cl 2) Chlorine Electron Configuration Thermal Properties of Chlorine
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