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The transition element ( with few except...

The transition element ( with few exceptions ) show a large number of oxidation states . The various oxidation states are related to the electronic configuration of their atoms. The variable oxidation states of a transition metal is due to the involvement of (n-1)d and outer ns electrons . For the first five elements of 3d transition series , the minimum oxidation state is equal to the number of electrons in 4s shell and the maximum oxidation state is equal to the sum of 4s and 3d electrons. The relative stability of various oxidation states of a given element can be explained on the basis of stability of `d^(0),d^(5) and d^(10)` configuration .
Identify the correct statement

A

(A) The most common oxidation state of 3d series is +2

B

(B) The lowest oxidation state of Cr and Cu is +1 while for other it is +2

C

(C) `Ti^(4+),Mn^(2+)` are stable oxidation states

D

(D) All of these

Text Solution

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The correct Answer is:
To solve the question regarding the oxidation states of transition elements, let's analyze the statements provided and verify their correctness based on the electronic configurations and stability of the oxidation states. ### Step-by-Step Solution: 1. **Understanding Oxidation States**: - Transition metals can exhibit multiple oxidation states due to the involvement of (n-1)d and ns electrons in bonding. - For the first five elements of the 3d transition series (Scandium to Zinc), the minimum oxidation state corresponds to the number of electrons in the 4s subshell, while the maximum oxidation state is the sum of the electrons in the 4s and 3d subshells. 2. **Analyzing Statement A**: - Statement A claims that the most stable oxidation state of the 3d series is +2. - For elements like Scandium (Sc), Titanium (Ti), Vanadium (V), Chromium (Cr), Manganese (Mn), Iron (Fe), Cobalt (Co), Nickel (Ni), Copper (Cu), and Zinc (Zn), the +2 oxidation state is indeed common due to the loss of the 4s electrons. - **Conclusion**: Statement A is correct. 3. **Analyzing Statement B**: - Statement B states that the lowest oxidation state of chromium and copper is +1, while for others it is +2. - Chromium (Cr) has the electronic configuration [Ar] 3d^5 4s^1, allowing it to lose one electron to form Cr^+1. - Copper (Cu) has the configuration [Ar] 3d^10 4s^1, also allowing it to lose one electron to form Cu^+1. - Other transition metals typically have two electrons in the 4s subshell, leading to a minimum oxidation state of +2. - **Conclusion**: Statement B is correct. 4. **Analyzing Statement C**: - Statement C claims that Ti^4+ and Mn^2+ are stable oxidation states. - Titanium (Ti) has an atomic number of 22 and loses four electrons to achieve a noble gas configuration (D^0), which is stable. - Manganese (Mn) has an atomic number of 25 and, when it loses two electrons, achieves a half-filled d-orbital configuration (D^5), which is also stable. - **Conclusion**: Statement C is correct. 5. **Final Conclusion**: - Since all statements A, B, and C are correct, the answer to the question is option D: "All of these." ### Answer: **Option D: All of these.**
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The transition element ( with few exceptions ) show a large number of oxidation states . The various oxidation states are related to the electronic configuration of their atoms. The variable oxidation states of a transition metal is due to the involvement of (n-1)d and outer ns electrons . For the first five elements of 3d transition series , the minimum oxidation state is equal to the number of electrons in 4s shell and the maximum oxidation state is equal to the sum of 4s and 3d electrons. The relative stability of various oxidation states of a given element can be explained on the basis of stability of d^(0),d^(5) and d^(10) configuration . In 3d series, the maximum oxidation state is shown by

The transition element ( with few exceptions ) show a large number of oxidation states . The various oxidation states are related to the electronic configuration of their atoms. The variable oxidation states of a transition metal is due to the involvement of (n-1)d and outer ns electrons . For the first five elements of 3d transition series , the minimum oxidation state is equal to the number of electrons in 4s shell and the maximum oxidation state is equal to the sum of 4s and 3d electrons. The relative stability of various oxidation states of a given element can be explained on the basis of stability of d^(0),d^(5) and d^(10) configuration . In which of the following pairs , the first species is more stable than second one

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