The correct trend in the first ionization enthalpies of the elements in the $3^{rd}$ period of periodic table is:

The increasing order of the first ionization enthalpies of the elements $B$,$P$,$S$ and $F$ (lowest first) is:

Match List-$I$ with List-$II$:

List-$I$ (Electronic configuration)	List-$II$ ($\Delta_{i}H$ in $kJ\ mol^{-1}$)
$(a)$ $1s^{2} 2s^{2}$	$(i)$ $801$
$(b)$ $1s^{2} 2s^{2} 2p^{4}$	$(ii)$ $899$
$(c)$ $1s^{2} 2s^{2} 2p^{3}$	$(iii)$ $1314$
$(d)$ $1s^{2} 2s^{2} 2p^{1}$	$(iv)$ $1402$

Choose the most appropriate answer from the options given below:

The atomic number of the element from the following with the lowest $1^{st}$ ionisation enthalpy is:

$X_{(g)} \to X^{+}_{(g)} + e^-$,$\Delta H = +720 \ kJ \ mol^{-1}$
Calculate the amount of energy required to convert $110 \ mg$ of $X$ atom in gaseous state into $X^{+}$ ion .................... $kJ$ (Atomic weight for $X = 7 \ g \ mol^{-1}$)

Which elements in a period have the maximum and minimum ionization enthalpy?