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

The electronic configurations of $4$ atoms are given below:
$P = [Ne] \, 3s^2 3p^3$
$Q = [Ar] \, 3d^{10} 4s^2 4p^3$
$R = [He] \, 2s^2 2p^5$
$S = [Ne] \, 3s^1$
Which of the following statements is incorrect?

Given below are two statements:
Statement $I$: The second ionisation enthalpy of $Na$ is larger than the corresponding ionisation enthalpy of $Mg$.
Statement $II$: The ionic radius of $O^{2-}$ is larger than that of $F^{-}$.
In the light of the above statements, choose the correct answer from the options given below.

In general,the properties that decrease and increase down a group in the periodic table respectively are

Consider the following:
$(I)$ The order of first ionisation enthalpy of the first three elements of the $3^{rd}$ period is $Mg > Al > Na$
$(II)$ The element with an electronegativity of $3.5$ is chlorine
$(III)$ The order of sizes of ions $Mg^{2+}, Na^{+}, F^{-}$ and $O^{2-}$ is $Mg^{2+} < Na^{+} < F^{-} < O^{2-}$
$(IV)$ The $IUPAC$ name of the element with atomic number $106$ is Bohrium.
The correct statements are

Match the following elements,given as hints to their first,second ionization enthalpies and electron gain enthalpies.

List-$I$	List-$II$
$i)$ Most reactive non-metal	$A$. $\Delta H_1=419, \Delta H_2=3051, \Delta_{Eg} H=-48$
$ii)$ Most reactive metal	$B$. $\Delta H_1=1681, \Delta H_2=3374, \Delta_{Eg} H=-328$
$iii)$ Least reactive element	$C$. $\Delta H_1=738, \Delta H_2=1451, \Delta_{Eg} H=-40$
$iv)$ Metal forming binary halide	$D$. $\Delta H_1=3272, \Delta H_2=5251, \Delta_{Eg} H=+48$