For a general redox reaction

Anode $\quad \operatorname{Red}_1 \rightarrow \mathrm{Ox}_1^{\mathrm{n}_1^{+}}+\mathrm{n}_1 \mathrm{e}^{-}$

Cathode $\mathrm{O} x_2+\mathrm{n}_2 \mathrm{e}^{-} \rightarrow \operatorname{Red}_2^{\mathrm{n}_2-}$

Which of the following statement is incorrect?

In a period, the first ionisation enthalpy of the element at extreme left and the negative electron gain enthalpy of the extreme right element, except noble gases, are respectively.

Given below are two statements :

Statement I : $\mathrm{F}_2 \mathrm{O}<\mathrm{H}_2 \mathrm{O}<\mathrm{Cl}_2 \mathrm{O}$ is the correct trend in terms of bond angle.

Statement II : $\mathrm{SiF}_4, \mathrm{SnF}_4$ and $\mathrm{PbF}_4$ are ionic in nature.

In the light of the above statements, choose the correct answer from the options given below :

The correct order of first $\left(\Delta_i \mathrm{H}_1\right)$ and second $\left(\Delta_i \mathrm{H}_2\right)$ ionisation enthalpy values of Cr and Mn are :

A. $\Delta_i \mathrm{H}_1: \mathrm{Cr}>\mathrm{Mn}$

B. $\Delta_i \mathrm{H}_2: \mathrm{Cr}>\mathrm{Mn}$

C. $\Delta_i \mathrm{H}_1: \mathrm{Mn}>\mathrm{Cr}$

D. $\Delta_i \mathrm{H}_2: \mathrm{Mn}>\mathrm{Cr}$

Choose the correct answer from the options given below :