First, let us re-state the two statements clearly:

Statement (I): An element in the extreme left of the periodic table forms acidic oxides.

Statement (II): Acid is formed during the reaction between water and oxide of a reactive element present in the extreme right of the periodic table.

Analyzing Statement (I)

The extreme left of the periodic table corresponds to the alkali metals (Group 1) and alkaline earth metals (Group 2).

These metals typically form basic (or occasionally amphoteric, in the case of some Group 2 elements) oxides, not acidic oxides.

For example, Na₂O, K₂O, MgO, CaO, etc., all form basic solutions (e.g., Na₂O + H₂O → 2 NaOH).

Hence, Statement (I)—that an element in the extreme left forms acidic oxides—is false.

Analyzing Statement (II)

The extreme right of the periodic table corresponds to the nonmetals in Groups 15, 16, 17 (and noble gases in Group 18).

Nonmetal oxides (such as those of sulfur, phosphorus, chlorine) are generally acidic.

When these oxides dissolve in water, they typically form acids.

Example: SO₃ + H₂O → H₂SO₄ (sulfuric acid)

Example: P₂O₅ + 3 H₂O → 2 H₃PO₄ (phosphoric acid)

Example: Cl₂O₇ + H₂O → 2 HClO₄ (perchloric acid)

Thus, Statement (II)—that acid is formed when water reacts with an oxide of a reactive element in the extreme right—is true.

Conclusion

Statement (I) is false.

Statement (II) is true.

Therefore, the correct choice is:

(D) Statement (I) is false but Statement (II) is true.