Identify the incorrect statement.a)The transition metals and their co...
Oxidation state of Cr in CrO42− and Cr2O72− is +6 i.e. oxidation states are same.
Identify the incorrect statement.a)The transition metals and their co...
The incorrect statement is option C: The oxidation states of chromium in CrO42− and Cr2O72− are not the same.
Explanation:
Transition metals are known for their ability to adopt multiple oxidation states. These oxidation states are due to the presence of partially filled d orbitals in their electronic configurations. This property allows transition metals to form complexes and exhibit catalytic activity.
a) Catalytic activity of transition metals:
Transition metals and their compounds are known for their catalytic activity. This is because they can undergo oxidation-reduction reactions by changing their oxidation states. The partially filled d orbitals in these metals allow them to accept or donate electrons, making them effective catalysts for various chemical reactions.
b) Interstitial compounds:
Interstitial compounds are formed when small atoms, such as hydrogen (H), carbon (C), or nitrogen (N), are trapped in the interstitial sites within the crystal lattices of metals. These compounds are characterized by the presence of small atoms occupying the spaces between the metal atoms in a crystal structure. This leads to changes in the physical and chemical properties of the metal.
c) Oxidation states of chromium:
The oxidation states of chromium in CrO42− and Cr2O72− are indeed the same. In both compounds, chromium has an oxidation state of +6. In CrO42−, the oxidation state of oxygen is -2. Therefore, to balance the charges, the chromium ion must have an oxidation state of +6. Similarly, in Cr2O72−, the oxidation state of oxygen is -2, and the two chromium ions must have an oxidation state of +6 each to balance the charges.
d) Reducing agent strength of Cr2 (d4) and Fe2 (d6):
In water, the reducing agent strength of a transition metal depends on its ability to donate electrons. The strength of a reducing agent is related to its oxidation state and the stability of its oxidation state. In general, a lower oxidation state is associated with a stronger reducing agent. Therefore, Cr2 (d4), with an oxidation state of +2, is a stronger reducing agent than Fe2 (d6), with an oxidation state of +3.
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