Which of the following is the $CORRECT$ decreasing order of ionisation enthalpy for the given elements?

Given below are two statements:
Statement $I$: The second ionization enthalpy of $B$,$Al$ and $Ga$ is in the order of $B > Al > Ga$.
Statement $II$: The correct order in terms of first ionization enthalpy is $Si < Ge < Pb < Sn$.

Which of the following elements has the highest metallic character?
Element $- IP$

The electronic configurations of elements $A, B$ and $C$ are $[He] 2s^1$,$[Ne] 3s^1$ and $[Ar] 4s^1$ respectively. Which one of the following orders is correct for the first ionization potentials (in $kJ \ mol^{-1}$) of $A, B$ and $C$?

The second ionization enthalpy of an element is always higher than its first ionization enthalpy because

What factors should be considered to understand the trends in ionization enthalpy values? Explain.