Question map
Which one of the following compounds does not exhibit a different oxidation number of the same element?
Explanation
In chemistry, mixed-valence compounds contain the same element in multiple oxidation states. Fe3O4 (magnetite) is a classic mixed-valence oxide consisting of FeO and Fe2O3, where iron exists as both Fe2+ and Fe3+. Similarly, Mn3O4 (hausmannite) is a mixed-valence oxide containing Mn2+ and Mn3+ ions [1]. Pb3O4 (red lead) is another example, composed of Pb2+ and Pb4+. In contrast, Fe2O3 (hematite) is a simple oxide where all iron atoms exhibit a single oxidation state of +3 to balance the -2 charge of the three oxygen atoms. While the question lists Pb2O4, it is likely a typographical error for the common mixed-valence oxide Pb3O4; however, Fe2O3 remains the only compound in the list that strictly represents a single oxidation state (+3) for the metal cation.
Sources
- [1] https://www.sciencedirect.com/science/article/pii/S2772571523000153
SIMILAR QUESTIONS
Which one of the following is an element which never exhibits positive oxidation state in any of its compounds?
Which one among the following oxides has the highest melting point ?
Which of the following salts are insoluble in water?
Match List I (Oxdiation number) with List II (The element) and select the correct answer using the codes given below this lists
(Oxidation number) | (The element)
A. 2 | 1. Oxidation number of Mn in MnO2
B. 3 | 2. Oxidation number of S in H2S2O7
C. 4 | 3. Oxidation number of Ca in CaO2
D. 6 | 4. Oxidation number of Al in NaAIH4