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Atomic symbol: I |
Atomic number: 53 |
Atomic weight: 126.9045 |
Atomic volume: 25.74 cm3/mol |
Density: 4.93 g/cm3 |
Period Number: 5 |
Group number: 17 |
Group name: Halogen |
Element classification: Non-metal |
Phase at room temperature: Solid |
Melting Point: 386.7 K |
Boiling point: 458.4 K |
Heat of fusion: 7.824 kJ/mol |
Heat of vaporization: 20.752 kJ/mol |
Ionization Energy: 10.451 eV |
1st ionization energy: 1008.4 kJ/mole |
2nd ionization energy: 1845.8 kJ/mole |
3rd ionization energy: 3184 kJ/mole |
Electronegativity: 2.66 |
Electron affinity: 295.16 kJ/mole |
Specific heat: 0.214 J/gK |
Heat atomization: 107 kJ/mole atoms |
Shells: 2,8,18,18,7 |
Electron Shell Configuration: [Kr] 4d10 5s2 5p5 |
Minimum oxidation number: -1 |
Maximum oxidation number: 7 |
Minimum common oxidation number: 0 |
Maximum common oxidation no: 7 |
Appearance & Characteristics |
Structure:: layers of I2 |
Color: bluish-black |
Hardness: mohs |
Toxicity: yes |
Characteristics: diatomic |
Uses: nutrient, antiseptic |
Reaction with air: none |
Reaction with 6M HCl: none |
Reaction with 15M HNO3: mild, =>HIO3 |
Reaction with 6M NaOH: mild, =>OI-, I- |
Number of isotopes: 1 |
Oxide(s): I2O5 I4O9I2O4 |
Hydride(s): HI |
Chloride(s): ICl ICl3 |
Atomic Radius: 133 pm |
Ionic radius (1- ion): 206 pm |
Ionic radius (1+ ion): pm |
Ionic radius (2- ion): pm |
Ionic radius (2+ ion): pm |
Ionic radius (3+ ion): pm |
Thermal conductivity: 0.45 J/m-sec-deg |
Electrical conductivity: 0 1/mohm-cm |
Polarizability: 5 A^3 |
Source: Brines, Chilean nitrate (misc) |
Relative abundance solar system: -0.046 log |
Abundance earth's crust: -0.3 log |
Estimated crustal abundance: 4.5×10-1 milligrams per kilogram |
Estimated oceanic abundance: 6×10-2 milligrams per liter |
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(Gr. iodes: violet) Discovered by Courtois in 1811, Iodine, a halogen, occurs sparingly in the form of iodides in sea water from which it is assimilated by seaweeds, Chilean saltpeter, nitrate-bearing earth (known as caliche), brines from old sea deposits, and in brackish waters from oil and salt wells. |
Ultrapure iodine can be obtained from the reaction of potassium iodide with copper sulfate. Several other methods of isolating the element are known. |
Iodine is a bluish-black, lustrous solid, volatizing at ordinary temperatures into a blue-violet gas with an irritating odor; it forms compounds with many elements, but is less active than the other halogens, which displace it from iodides. Iodine exhibits some metallic-like properties. It dissolves readily in chloroform, carbon tetrachloride, or carbon disulfide to form beautiful purple solutions. It is only slightly soluble in water. |
Iodine compounds are important in organic chemistry and very useful in medicine. Iodides, and thyroxine which contains iodine, are used internally in medicine, and as a solution of KI and iodine in alcohol is used for external wounds. Potassium iodide finds use in photography. The deep blue color with starch solution is characteristic of the free element. |
Thirty isotopes are recognized. Only one stable isotope, 127I is found in nature. The artificial radioisotope 131I, with a half-life of 8 days, has been used in treating the thyroid gland. The most common compounds are the iodides of sodium and potassium (KI) and the iodates (KIO3). Lack of iodine is the cause of goiter. |
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