There are 27 electron containing orbitals in an atom of Iodine.
Potassium lose an electron (iodine gain this electron) to form potassium iodide, KI.
Steal an electron from an atom of a different element.
The outer most electron shell of iodine atom contains 7 electrons.
Iodine only needs to gain one electron to become an anion.
Iodine gains one electron to form iodide ion. The size of iodide ion is larger than the size of iodine atom.
Potassium lose an electron (iodine gain this electron) to form potassium iodide, KI.
Steal an electron from an atom of a different element.
Iodine with one extra electron in its atom
The outer most electron shell of iodine atom contains 7 electrons.
Iodine in its natural form is I2, two iodine atoms bonded with a single covalent bond. There are 6 non-bonded valance electrons on each atom, so there are 12 electrons in the electron-dot structure.
Iodine only needs to gain one electron to become an anion.
Iodine gains one electron to form iodide ion. The size of iodide ion is larger than the size of iodine atom.
Aluminum, sulfur, fluorine, phosphorus, iodine, and neon
Ioding when combined in a compound is usually combined as the iodide. Iodide ions are negatively charged (ie each ion has an extra electron compared with an iodine atom). When elemental iodine is liberated, iodine atoms are formed from these ions which in turn pair up to form iodine molecules. When an Iodine ion changes into an atom it must lose the extra electron. From the acronym 'OILRIG' (Oxidation Is Loss of electrons, Reduction Is Gain of electrons) it is clear that as the elemental iodine has formed because of the loss of an electron the process must involve oxidation.
Iodine is reactive because it has 7 valence electrons and is unstable. It needs one more electron to get 8, which would give it a noble gas configuration, and which would make the iodine atom stable. Iodine reacts with other elements in order to gain the needed electron and therefore become stable.
Iodine's electron configuration is 2, 8, 18, 18, 7; bromine's is 2, 8, 18, 7. At the simplest level of modelling there is one more electron shell occupying space in an iodine atom than in one of bromine.
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