Identify the homoleptic complexes with odd number of d-electrons in the central metal:
(A) [FeO4]2− (B) [Fe(CN)6]3−
(C) [Fe(CN)5NO]2− (D) [CoCl4]2−
(E) [Co(H2O)3F3]
Choose the correct answer from the options given below :
(A) [FeO4]2− (B) [Fe(CN)6]3−
(C) [Fe(CN)5NO]2− (D) [CoCl4]2−
(E) [Co(H2O)3F3]
Choose the correct answer from the options given below :
Show Hint
(B) and (D) only
(C) and (E) only
(A), (B) and (D) only
(A), (C) and (E) only
The Correct Option is A
Approach Solution - 1
- (A) \([FeO_4]^{2-}\): Iron in this complex is in the +2 oxidation state, with \( d^6 \) electrons. Since 6 is an even number, this complex does not meet the requirement for an odd number of d-electrons.
- (B) \([Fe(CN)_6]^{3-}\): Iron in this complex is in the +3 oxidation state, with \( d^5 \) electrons. This gives an odd number of d-electrons, so this is a homoleptic complex with odd d-electrons.
- (C) \([Fe(CN)_6]^{2-}\): Iron is in the +2 oxidation state with \( d^6 \) electrons. This complex has an even number of d-electrons.
- (D) \([CoCl_4]^{2-}\): Cobalt in this complex is in the +2 oxidation state, with \( d^7 \) electrons. This gives an odd number of d-electrons, so this is a homoleptic complex with odd d-electrons.
- (E) \([Co(H_2O)_6]^{3+}\): Cobalt in the +3 oxidation state has \( d^6 \) electrons, which is an even number.
Thus, the correct answer is (1) (B) and (D) only.
Approach Solution -2
We are asked to identify the homoleptic complexes (complexes having identical ligands) that contain a central metal atom with an odd number of d-electrons.
Step 2: Analyze each complex.
(A) [FeO₄]²⁻
Oxidation state of Fe: Let it be x.
\[ x + 4(-2) = -2 \Rightarrow x = +6 \] Electronic configuration of Fe (Z = 26): [Ar] 3d⁶ 4s²
Fe⁶⁺ → [Ar] 3d⁰ (no d-electrons)
Therefore, it has 0 d-electrons and is not odd. Also, this complex is homoleptic but does not have an odd number of d-electrons.
(B) [Fe(CN)₆]³⁻
Oxidation state of Fe: Let it be x.
\[ x + 6(-1) = -3 \Rightarrow x = +3 \] Fe³⁺ → [Ar] 3d⁵
Thus, there are 5 d-electrons (odd number). The ligands (CN⁻) are identical, making it a homoleptic complex.
Hence, (B) is correct.
(C) [Fe(CN)₅NO]²⁻
This complex contains two different types of ligands (CN⁻ and NO), so it is heteroleptic and does not qualify as homoleptic. Hence, (C) is incorrect.
(D) [CoCl₄]²⁻
Oxidation state of Co: Let it be x.
\[ x + 4(-1) = -2 \Rightarrow x = +2 \] Co²⁺ → [Ar] 3d⁷
Thus, it has 7 d-electrons (odd number). All ligands are identical (Cl⁻), making it homoleptic.
Hence, (D) is correct.
(E) [Co(H₂O)₃F₃]
Contains two different types of ligands (H₂O and F⁻), making it heteroleptic. Hence, (E) is incorrect.
Step 3: Conclusion.
Homoleptic complexes with an odd number of d-electrons are (B) and (D).
Final Answer:
\[ \boxed{(B) \text{ and } (D) \text{ only}} \]
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