Here are the essential concepts you must grasp in order to answer the question correctly.
Transition Metals
Transition metals are elements found in the d-block of the periodic table, characterized by their ability to form variable oxidation states and complex ions. They typically have partially filled d-orbitals, which allow them to engage in bonding and exhibit unique properties such as catalytic activity and colored compounds.
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Electron Configuration
Electron configuration describes the distribution of electrons in an atom's orbitals. For transition metals, the electron configuration can be expressed in terms of the principal quantum number (n) and the d-orbital occupancy. A configuration of nd5 indicates that there are five electrons in the d-orbital, which is significant for understanding the chemical behavior and reactivity of these ions.
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Electron Configuration Example
Oxidation States
Oxidation states refer to the charge of an ion, indicating the number of electrons lost or gained by an atom in a compound. For transition metals, the +3 oxidation state is common and results from the loss of three electrons, often from both the s and d orbitals. This state is crucial for identifying specific transition metal ions with an electron configuration of nd5.
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