Moving from right to left in a periodic table, the atomic size is:

1. Increased                                               

2. Decreased

3. Remains constant                                     

4. None of the above

One element has atomic weight 39. Its electronic configuration is 1s² 2s² 2p⁶ 3s² 3p⁶ 4s¹. The true statement for this element is: 

1. High value of IE                               

2. Transition element

3. Isotone with $18A{}^{}$   $$

4. None of the above

The incorrect statement among the following is:

1. The first ionisation potential of Al is less than the first ionisation potential of Mg

2. The second ionisation potential of Mg is greater than the second ionisation potential of Na

3. The first ionisation potential of Na is less than the first ionisation potential of Mg

4. The third ionisation potential of Mg is greater than the third ionisation potential of Al

The element Z = 114 has been discovered recently. 

It will belong to which of the following family/group and electronic configuration?

1. $\mathrm{Carbon} \mathrm{family}\left[\mathrm{Rn}\right]5 {\mathrm{f}}^{14} 6{\mathrm{d}}^{10}7{\mathrm{s}}^{2}7{\mathrm{p}}^2$

2. $\mathrm{Oxygen} \mathrm{family}\left[\mathrm{Rn}\right]5 {\mathrm{f}}^{14} 6{\mathrm{d}}^{10}7{\mathrm{s}}^{2}7{\mathrm{p}}^4$

3. $\mathrm{Nitrogen} \mathrm{family}\left[\mathrm{Rn}\right]5 {\mathrm{f}}^{14} 6{\mathrm{d}}^{10}7{\mathrm{s}}^{2}7{\mathrm{p}}^6$

4. $\mathrm{Halogen} \mathrm{family}\left[\mathrm{Rn}\right]5 {\mathrm{f}}^{14} 6{\mathrm{d}}^{10}7{\mathrm{s}}^{2}7{\mathrm{p}}^5$

Magnesium reacts with an element (X) to form an ionic compound. If the ground state electronic configuration of (X) is 1s²2s²2p³, the simplest formula for this compound is: 
1. Mg₂X₃
2. MgX₂
3. Mg₂X
4. Mg₃X₂

The species Ar, K⁺ and Ca²⁺ contain the same number of electrons. In which order do their radii increase?

$1. \mathrm{Ar} < {\mathrm{K}}^{+} < {\mathrm{Ca}}^{2+}$
$2. {\mathrm{Ca}}^{2+} < \mathrm{Ar} < {\mathrm{K}}^{+}$
$3. {\mathrm{Ca}}^{2+} < {\mathrm{K}}^{+} < \mathrm{Ar}$
$4. {\mathrm{K}}^{+} <\hspace{0.17em}\mathrm{Ar} < {\mathrm{Ca}}^{2+}$

Which of the following orders of ionic radii is correctly represented?

1. $H^{-}>H^{+}>H$

2. $N{a}^{+}>F^{-}>O^{2-}$

3. $F^{-}>O^{2-}>N{a}^{+}$

4. $N^{3-}>M{g}^{2+}>A{l}^{3+}$

Identify the wrong statement among the following: 

1. Amongst isoelectronic species, the smaller the positive charge on the cation, the smaller the ionic radius.
2. Amongst isoelectronic species, the greater the negative charge on the anion, the larger is the ionic radius.
3. The atomic radius of the elements increases as one moves down the first group of the Periodic Table.
4. The atomic radius of the elements decreases as one moves across from left to right in the 2nd period of the Periodic Table.