The nature of oxides V\(_2\)O\(_3\) and CrO is indexed as 'X' and 'Y' type respectively. The correct set of X and Y is:
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A useful trend to remember for transition metals is the change in oxide character with oxidation state. For chromium: CrO (+2) is basic, Cr\(_2\)O\(_3\) (+3) is amphoteric, and CrO\(_3\) (+6) is acidic. This pattern holds for many transition metals.
Step 1: Understanding the Question:
This question asks to determine the acidic/basic nature of two transition metal oxides, V\(_2\)O\(_3\) and CrO. Step 2: Key Formula or Approach:
The nature of transition metal oxides is generally related to the oxidation state of the metal:
Low oxidation state oxides are typically basic.
Intermediate oxidation state oxides are typically amphoteric.
High oxidation state oxides are typically acidic.
We need to find the oxidation states of Vanadium (V) and Chromium (Cr) in the given oxides. Step 3: Detailed Explanation: For V\(_2\)O\(_3\) (Oxide X):
Let the oxidation state of V be 'x'. Oxygen usually has an oxidation state of -2.
\[ 2(x) + 3(-2) = 0 \]
\[ 2x - 6 = 0 \]
\[ 2x = 6 \implies x = +3 \]
The oxidation state of Vanadium is +3. For Vanadium, which exhibits states from +2 to +5, +3 is a relatively low state. Oxides in lower oxidation states are basic. For example, V\(_2\)O\(_3\) reacts with acids to form V\(^{3+}\) salts. Therefore, V\(_2\)O\(_3\) is a basic oxide. So, X = basic. For CrO (Oxide Y):
Let the oxidation state of Cr be 'y'.
\[ y + (-2) = 0 \]
\[ y = +2 \]
The oxidation state of Chromium is +2. This is a low oxidation state for Chromium (which commonly exists in +2, +3, and +6 states). Therefore, CrO is a basic oxide. For example, CrO reacts with acids to form Cr\(^{2+}\) salts. So, Y = basic. Step 4: Final Answer:
Both V\(_2\)O\(_3\) and CrO are basic oxides. Therefore, the correct set is X = basic and Y = basic.
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