Question

Describe the anomalous behavior of fluorine with the other elements of group 17 with reference to:
Oxidation state

Answer 1

We know that fluorine is a halogen present in group 17 of the periodic table. The other elements present in group 17 of the periodic table are chlorine, bromine, iodine etc. Oxidation state is the number of electrons that an atom loses or gains to form a chemical bond.

Complete step-by-step answer:
Now we will understand the reason for the anomalous behavior of fluorine.

Fluorine shows anomalous behaviour compared to other elements of groups 17 due to its smallest size among all the halogens, high electronegativity and non-availability of d-orbitals. All the halogens except fluorine such as chlorine, bromine, iodine possess positive as well as negative oxidation state. Fluorine possesses only -1 oxidation state. Some of the positive oxidation states of halogens are +1,+3,+5 and +7.

Note: Students might get confused in oxidation state possessed by halogens. They might think that as all the halogen atoms can form an anion of -1 charge, so, their oxidation state is -1 but it is not correct.

1. Oxidation state possessed by chlorine are -1, +1, +3, +5 and +7
2. Oxidation state possessed by bromine are -1, +1, +3, +4 and +5
3. Oxidation state possessed by iodine are-1, +1, +5 and +7
4. Oxidation state possessed by Astatine are -1, +1, +3, +5 and +7
5. Oxidation state possessed by fluorine is -1
   So, we can clearly see that all the halogens except fluorine have both positive and negative oxidation state.