Question:
Arrange the following ions in the decreasing order of covalent double bonds formed by the transition metal with oxygen.
\[
A. = \text{chromate}, \quad B = \text{permanganate}, \quad C = \text{dichromate}
\]
Arrange the following ions in the decreasing order of covalent double bonds formed by the transition metal with oxygen.
\[
A. = \text{chromate}, \quad B = \text{permanganate}, \quad C = \text{dichromate}
\]
Show Hint
The covalent nature of the bond between a transition metal and oxygen increases with the oxidation state of the metal. Higher oxidation states lead to stronger covalent bonds.
Updated On: May 5, 2026
- \( A > B > C \)
- \( B > C > A \)
- \( B > A > C \)
- \( C > B > A \)
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The Correct Option is D
Solution and Explanation
Step 1: Understand the nature of the bonds.
The covalent bonds formed by transition metals with oxygen depend on the oxidation state of the metal and the nature of the ligands (in this case, the oxide anions). Higher oxidation states of the metal result in stronger covalent bonds with oxygen due to the increased electron withdrawal by the metal center, which makes the metal-oxygen bonds more polarized.
Step 2: Analyze the chromate ion (\( \text{CrO}_4^{2-} \)).
Chromate (\( \text{CrO}_4^{2-} \)) has chromium in the +6 oxidation state, which is a high oxidation state, resulting in a strong covalent bond between chromium and oxygen. The nature of the bonding in chromates is characterized by a significant degree of covalent character due to the high oxidation state of chromium.
Step 3: Analyze the permanganate ion (\( \text{MnO}_4^{-} \)).
Permanganate (\( \text{MnO}_4^{-} \)) has manganese in the +7 oxidation state, which is even higher than the +6 oxidation state of chromium in chromate. This leads to stronger covalent bonds between manganese and oxygen. Therefore, permanganate exhibits more covalent bonding than chromate.
Step 4: Analyze the dichromate ion (\( \text{Cr}_2\text{O}_7^{2-} \)).
Dichromate (\( \text{Cr}_2\text{O}_7^{2-} \)) also contains chromium in the +6 oxidation state, but since it involves two chromium centers, the bonding between chromium and oxygen is not as strong as in permanganate, which has a higher oxidation state for manganese.
Step 5: Conclusion.
Based on the analysis, the order of decreasing covalent bonds formed by the transition metal with oxygen is:
\[ C > B > A \]
Thus, the correct answer is option (D).
The covalent bonds formed by transition metals with oxygen depend on the oxidation state of the metal and the nature of the ligands (in this case, the oxide anions). Higher oxidation states of the metal result in stronger covalent bonds with oxygen due to the increased electron withdrawal by the metal center, which makes the metal-oxygen bonds more polarized.
Step 2: Analyze the chromate ion (\( \text{CrO}_4^{2-} \)).
Chromate (\( \text{CrO}_4^{2-} \)) has chromium in the +6 oxidation state, which is a high oxidation state, resulting in a strong covalent bond between chromium and oxygen. The nature of the bonding in chromates is characterized by a significant degree of covalent character due to the high oxidation state of chromium.
Step 3: Analyze the permanganate ion (\( \text{MnO}_4^{-} \)).
Permanganate (\( \text{MnO}_4^{-} \)) has manganese in the +7 oxidation state, which is even higher than the +6 oxidation state of chromium in chromate. This leads to stronger covalent bonds between manganese and oxygen. Therefore, permanganate exhibits more covalent bonding than chromate.
Step 4: Analyze the dichromate ion (\( \text{Cr}_2\text{O}_7^{2-} \)).
Dichromate (\( \text{Cr}_2\text{O}_7^{2-} \)) also contains chromium in the +6 oxidation state, but since it involves two chromium centers, the bonding between chromium and oxygen is not as strong as in permanganate, which has a higher oxidation state for manganese.
Step 5: Conclusion.
Based on the analysis, the order of decreasing covalent bonds formed by the transition metal with oxygen is:
\[ C > B > A \]
Thus, the correct answer is option (D).
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