Question

Fluorine exhibits only -1 oxidation state while iodine exhibits oxidation states of -1, + 1, + 3, +5 and + 7. This is due to :

• A. flourine being a gas
• B. available $d$-orbitals in iodine
• C. non-availability of $d$-orbitals in iodine
• D. none of the above.

Answer 1

Answer: (B)

available $d$-orbitals in iodine

Due to absence of d-orbitals, $F$ can not expand its valency but $I$ can expand its valency (as shown in the figure) and therefore, exhibts variable oxidation states.