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d-block elements generally show multiple oxidation states. An exception to this is:
- a)Zinc
- b)Mercury
- c)Copper
- d)None of the mentioned
Correct answer is option 'A'. Can you explain this answer?
Most Upvoted Answer
d-block elements generally show multiple oxidation states. An exceptio...
Introduction:
The d-block elements, also known as transition metals, are characterized by their ability to exhibit multiple oxidation states. This means that they can lose or gain different numbers of electrons, resulting in different charges on the ions they form. However, there are exceptions to this general trend, and one such exception is zinc (Zn).
Explanation:
1. Transition Metals:
Transition metals are located in the d-block of the periodic table and include elements such as iron (Fe), copper (Cu), and zinc (Zn). These elements have partially filled d-orbitals, which allow them to easily gain or lose electrons and form ions with different charges.
2. Multiple Oxidation States:
Transition metals can exhibit multiple oxidation states due to the presence of different oxidation states of their d-orbitals. This is attributed to the fact that the d-orbitals can be easily filled or emptied, allowing the transition metals to have different oxidation states.
3. Zinc (Zn):
Zinc is an exception to the general trend of transition metals exhibiting multiple oxidation states. It mainly exhibits a +2 oxidation state, where it loses two electrons to form Zn2+ ions. The electronic configuration of Zn is [Ar] 3d10 4s2, which means that its d-orbitals are completely filled. This stable electronic configuration makes it difficult for zinc to lose or gain additional electrons.
4. Stability of Zn2+ Ion:
Zinc readily loses its two valence electrons to attain a stable electronic configuration similar to the noble gas configuration of argon ([Ar] 3d10). The resulting Zn2+ ion has a completely filled d-orbital, making it highly stable. Due to this stability, zinc does not readily form ions with different charges, unlike other transition metals.
5. Other Examples:
In contrast to zinc, other transition metals such as copper (Cu) and mercury (Hg) can exhibit multiple oxidation states. Copper, for example, can form Cu+ and Cu2+ ions, while mercury can form Hg2+ and Hg22+ ions.
Conclusion:
In summary, zinc is an exception to the general trend of transition metals showing multiple oxidation states. This is because zinc has a completely filled d-orbital, making it difficult for the element to lose or gain additional electrons. As a result, zinc primarily exhibits a +2 oxidation state, where it loses two electrons to form Zn2+ ions.
The d-block elements, also known as transition metals, are characterized by their ability to exhibit multiple oxidation states. This means that they can lose or gain different numbers of electrons, resulting in different charges on the ions they form. However, there are exceptions to this general trend, and one such exception is zinc (Zn).
Explanation:
1. Transition Metals:
Transition metals are located in the d-block of the periodic table and include elements such as iron (Fe), copper (Cu), and zinc (Zn). These elements have partially filled d-orbitals, which allow them to easily gain or lose electrons and form ions with different charges.
2. Multiple Oxidation States:
Transition metals can exhibit multiple oxidation states due to the presence of different oxidation states of their d-orbitals. This is attributed to the fact that the d-orbitals can be easily filled or emptied, allowing the transition metals to have different oxidation states.
3. Zinc (Zn):
Zinc is an exception to the general trend of transition metals exhibiting multiple oxidation states. It mainly exhibits a +2 oxidation state, where it loses two electrons to form Zn2+ ions. The electronic configuration of Zn is [Ar] 3d10 4s2, which means that its d-orbitals are completely filled. This stable electronic configuration makes it difficult for zinc to lose or gain additional electrons.
4. Stability of Zn2+ Ion:
Zinc readily loses its two valence electrons to attain a stable electronic configuration similar to the noble gas configuration of argon ([Ar] 3d10). The resulting Zn2+ ion has a completely filled d-orbital, making it highly stable. Due to this stability, zinc does not readily form ions with different charges, unlike other transition metals.
5. Other Examples:
In contrast to zinc, other transition metals such as copper (Cu) and mercury (Hg) can exhibit multiple oxidation states. Copper, for example, can form Cu+ and Cu2+ ions, while mercury can form Hg2+ and Hg22+ ions.
Conclusion:
In summary, zinc is an exception to the general trend of transition metals showing multiple oxidation states. This is because zinc has a completely filled d-orbital, making it difficult for the element to lose or gain additional electrons. As a result, zinc primarily exhibits a +2 oxidation state, where it loses two electrons to form Zn2+ ions.
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Community Answer
d-block elements generally show multiple oxidation states. An exceptio...
Due to a small increase in successive ionization enthalpies, most d-block elements exist in multiple oxidation states. However, Zn(I) compounds are very rare and the ion exists in a dimeric form.
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