In which pairs highest oxidation states of transition metals are found? A. Nitrides and Chlorides B. Fluorides and Chlorides C. Fluorides and Oxides D. Nitrides and Oxides
Hint: Oxidation state of an element is related to the number of electrons that an atom gains, loses or appears to use when joining with another atom in the compound.
Complete step by step answer:
- It is also found that oxidation state also determines the ability of an atom to oxidize (that is to lose electrons) or to reduce (that is to gain electrons) the other atoms. Oxidation results in an increase in oxidation state.
- Generally, it is found that metals show the highest oxidation state with fluorides and oxides only.
- Oxygen and Fluorine are having small size, as we go from left to right in periodic table, size decreases. And from top to bottom size decreases. As these are in the right hand side of the periodic table.
- These are electronegative, meaning these attract the lone pairs toward itself. Fluorine is more stable than oxygen. And it will stabilise it.
- Their electron gain enthalpy is also very high, therefore it gets easily reacted. These overcome the ionisation of the metal by giving more energy.
Hence, we can conclude that the correct option is (C), highest oxidation states of transition metals are found in Fluorides and Oxides.
- We can say that oxygen and fluorine has high electronegativity and also small sizes. Hence, these are known to bring out the highest oxidation states from the transition metals. Or we can say transition metals exhibit higher oxidation states in oxides and fluorides.
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