Iodine: the essentials
Iodine atoms have 53 electrons and the shell structure is 126.96.36.199.7. The ground state electronic configuration of neutral iodine is [Kr].4d10.5s2.5p5 and the term symbol of iodine is 2P3/2.
Iodine is a bluish-black, lustrous solid. It volatilises at ambient temperatures into a pretty blue-violet gas with an irritating odour.
It forms compounds with most elements, but is less reactive than the other halogens, which displace it from iodides. Iodine exhibits some metallic-like properties. It dissolves readily in chloroform, carbon tetrachloride, or carbon disulphide to form beautiful purple solutions. It is only slightly soluble in water. Iodine compounds are important in organic chemistry and very useful in medicine and photography. Lack of iodine is the cause of goitre (Derbyshire neck). The deep blue colour with starch solution is characteristic of the free element. It is assimilated by seaweeds from which it may be recovered, and is found in Chilean saltpetre, caliche, old salt brines, and salt wells.
Iodine: physical properties
Iodine: heat properties
- Melting point: 386.85 [113.7 °C (236.66 °F)] K
- Boiling point: 386.85 [113.7 °C (236.66 °F)] K
- Enthalpy of fusion: 20.5 kJ mol-1
Iodine: atom sizes
- Atomic radius (empirical): 140 pm
- Molecular single bond covalent radius: 133 (coordination number 1) ppm
- van der Waals radius: 204 ppm
- Pauling electronegativity: 2.66 (Pauling units)
- Allred Rochow electronegativity: 2.21 (Pauling units)
- Mulliken-Jaffe electronegativity: 2.74 (14.3% s orbital)
Iodine: orbital properties
- First ionisation energy: 1008.39 kJ mol‑1
- Second ionisation energy: 1845.89 kJ mol‑1
- Third ionisation energy: 2853.1 kJ mol‑1
Iodine: crystal structure
Iodine: biological data
- Human abundance by weight: 200 ppb by weight
In nature, iodine exists as iodide ions, I-, and it is as iodide that it is taken into our bodies. Iodine is an essential component of the human diet and in fact appears to be the heaviest required element in the diet. Iodine compounds are useful in medicine.
Lack of iodine in the diet is a cause of goitre (Derbyshire neck). This condition is rare now as table salt is dosed with a little iodide.
Reactions of iodine as the element with air, water, halogens, acids, and bases where known.
Iodine: binary compounds
Binary compounds with halogens (known as halides), oxygen (known as oxides), hydrogen (known as hydrides), and other compounds of iodine where known.
Iodine: compound properties
Bond strengths; lattice energies of iodine halides, hydrides, oxides (where known); and reduction potentials where known.
Iodine: historyIodine was discovered by Bernard Courtois in 1811 at France. Origin of name: from the Greek word "iodes" meaning "violet".
Isolation: iodine is available commercially so it is not normally necessary to make it in the laboratory. Iodine occurs in seawater but in much smaller quantities than chloride or bromide. As for bromine, with suitable sources of brine, it is recovered commercially through the treatment of brine with chlorine gas and flushing through with air. In this treatment, iodide is oxidized to iodine by the chlorine gas.
2I- + Cl2 → 2Cl- + I2
Small amounts of iodine can be made through the reaction of solid sodium iodide, NaI, with concentrated sulphuric acid, H2SO4. The first stage is formation of HI, which is a gas, but under the reaction conditions some of the HI is oxidized by further H2SO4 to form iodine and sulphur dioxide.
NaI (s) + H2SO4 (l) → HI (g) + NaHSO4 (s)
2HI (g) + H2SO4 (l) → I2 (g) + SO2 (g) + 2H2O (l)