Which among the following pairs of halogens forms the interhalogen compound of the type $XX_{7}^{\prime}$?

Which of the following arrangements does not represent the correct trend indicated against it?

Which of the following elements of the halogen family is in a liquid state at room temperature?

Assertion $(A)$: The bond dissociation energy increases from $F_2$ to $Cl_2$ and then decreases to $I_2$.
Reason $(R)$: The low bond energy of fluorine is due to the repulsion between the lone pairs of electrons in two fluorine atoms.
The correct option among the following is

Which of the following statements regarding the properties of halogens are correct?
$(a)$ Due to small size and strong inter-electronic repulsion,the electron gain enthalpy of fluorine is less negative than that of chlorine.
$(b)$ Iodine has a different physical state and colour compared to other members of the group.
$(c)$ Fluorine does not show a positive oxidation state.
$(d)$ In $X_{2(g)} + H_2O(l) \rightarrow HX(aq) + HOX(aq)$ (where $X = Cl$ or $Br$).

Among the following halogens $F_2$,$Cl_2$,$Br_2$ and $I_2$,which can undergo disproportionation reaction?