Match List I with List II

Choose the correct answer from the options given below:

List I contains four statements about the periodic properties of some main-group elements, while List II supplies four specific elements. We have to pair every statement with the correct element by using the well-known periodic trends.

List I (statements)
A. Element having the most negative (highest) electron-gain enthalpy
B. Element having the greatest first ionisation enthalpy among the elements listed
C. Element having the highest electronegativity
D. Element whose hydrated cation possesses the highest (most exothermic) hydration enthalpy

List II (elements)
I. $$Li$$     II. $$Cl$$     III. $$F$$     IV. $$Ne$$

Matching the items one by one

A → II ($$Cl$$)
For the halogens, electron-gain enthalpy becomes most negative from $$F$$ to $$Cl$$ because the very small size of $$F$$ leads to strong inter-electronic repulsion in its compact 2p subshell. Hence $$Cl$$, not $$F$$, has the highest (most negative) electron-gain enthalpy in the periodic table.

B → IV ($$Ne$$)
First ionisation enthalpy increases across a period and is highest for the noble gas at the end of the period. Among the four elements listed, $$Ne$$ is the only noble gas, so it possesses the greatest first ionisation enthalpy.

C → III ($$F$$)
Electronegativity rises across a period and drops down a group; the maximum value for any element is for $$F$$ (Pauling value ≈ 4.0). Therefore the element with the highest electronegativity is $$F$$.

D → I ($$Li$$)
Hydration enthalpy of an ion is inversely related to its ionic radius; smaller cations attract water molecules more strongly. Among the alkali-metal cations the smallest (and therefore most strongly hydrated) is $$Li^+$$, giving $$Li$$ the highest hydration enthalpy.

Thus the correct correspondence is:
A → II, B → IV, C → III, D → I,

which matches Option C: A-II, B-IV, C-III, D-I.