These elements when combining with the more electronegative element, their electrons of nth orbit get promoted to n-‘d’ orbital. Hence, they tend to gain one electron to form the stable electronic configuration of the nearest noble gas atom and exhibit – 1 uniform oxidation state.Ĭhlorine, bromine and Iodine have empty n-‘d’ orbital. The characteristic electronic configuration of the halogens is ns2 np5. It is to be noted that every ion is larger in size than the corresponding atom. Atomic number and number of shell increases.Trend: As we go down in the group atomic radius increases from fluorine to iodine. From fluorine to iodine atomic radius increases because of following reasons. Hence they are monovalent.Ītomic and ionic radius is the distance from the centre of the nucleus to the outermost shell of the atom or ion. Therefore, the common valency of halogen family is 1. They attain the octet either by accepting an electron to form a univalent anion, X-, (F-, Cl-, Br- and I-) by sharing the unpaired electron with the unpaired electron of another atom to form a covalent bond (as in Cl2, Br2, HCI, HF etc). They need one electron to complete their octet. They contain seven electrons in the valence shell. So these elements require only one electron to complete the octet.Īll halogen have shell electronic configuration is ns2 np5. There are seven electrons in the outermost shell.Hence they are kept in group VII-A (17) of a periodic table, before inert gases. All halogens contain seven electrons in their outermost shell.All orbits except the last orbit are completely filled.The last electron during configuration occupies p orbital, hence these elements are p block elements.They have characteristic outer orbit configuration of ns2 np5. Characteristic Electronic Configuration of Halogens:
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