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In which complex is the transition metal in zero oxidation state:
- a)[Co(NH3)6Cl2]
- b)[Fe(H2O)6]SO4
- c)H[Co(CO)4]
- d)K4[Ni(CN)4]
Correct answer is option 'D'. Can you explain this answer?
Verified Answer
In which complex is the transition metal in zero oxidation state:a)[Co...
K4[Ni(CN)4] Let O.S of Ni = x
4 + x – 4 = 0
x = 0
(A) Co3+ (B) Fe2+ (C) Co–1
4 + x – 4 = 0
x = 0
(A) Co3+ (B) Fe2+ (C) Co–1
Most Upvoted Answer
In which complex is the transition metal in zero oxidation state:a)[Co...
The answer to the question is option 'D' - K4[Ni(CN)4].
Explanation:
In order to determine the oxidation state of the transition metal in each complex, we need to analyze the ligands and their charge contributions.
a) [Co(NH3)6Cl2]:
- In this complex, we have six ammine (NH3) ligands and two chloride (Cl) ligands.
- Ammine is a neutral ligand, so it does not contribute any charge.
- Chloride is a negatively charged ligand, contributing a charge of -1 each. Since there are two chloride ligands, the total charge contribution is -2.
- Since the overall charge of the complex is 0, the oxidation state of the central transition metal (Co) must be +2 to balance the charge.
- Therefore, the transition metal in this complex is in the +2 oxidation state.
b) [Fe(H2O)6]SO4:
- In this complex, we have six water (H2O) ligands and a sulfate (SO4) ligand.
- Water is a neutral ligand, so it does not contribute any charge.
- Sulfate is a negatively charged ligand, contributing a charge of -2.
- Since the overall charge of the complex is 0, the oxidation state of the central transition metal (Fe) must be +2 to balance the charge.
- Therefore, the transition metal in this complex is in the +2 oxidation state.
c) H[Co(CO)4]:
- In this complex, we have four carbonyl (CO) ligands.
- Carbonyl is a neutral ligand, so it does not contribute any charge.
- Since there is no other ligand or counterion present in the complex, the overall charge of the complex is +1.
- Therefore, the oxidation state of the central transition metal (Co) must be -1 to balance the charge.
- Therefore, the transition metal in this complex is in the -1 oxidation state.
d) K4[Ni(CN)4]:
- In this complex, we have four cyanide (CN) ligands.
- Cyanide is a negatively charged ligand, contributing a charge of -1 each. Since there are four cyanide ligands, the total charge contribution is -4.
- Since the overall charge of the complex is -4 (as indicated by the K4 counterions), the oxidation state of the central transition metal (Ni) must be 0 to balance the charge.
- Therefore, the transition metal in this complex is in the 0 oxidation state.
Conclusion:
The transition metal in the complex K4[Ni(CN)4] is in the zero oxidation state.
Explanation:
In order to determine the oxidation state of the transition metal in each complex, we need to analyze the ligands and their charge contributions.
a) [Co(NH3)6Cl2]:
- In this complex, we have six ammine (NH3) ligands and two chloride (Cl) ligands.
- Ammine is a neutral ligand, so it does not contribute any charge.
- Chloride is a negatively charged ligand, contributing a charge of -1 each. Since there are two chloride ligands, the total charge contribution is -2.
- Since the overall charge of the complex is 0, the oxidation state of the central transition metal (Co) must be +2 to balance the charge.
- Therefore, the transition metal in this complex is in the +2 oxidation state.
b) [Fe(H2O)6]SO4:
- In this complex, we have six water (H2O) ligands and a sulfate (SO4) ligand.
- Water is a neutral ligand, so it does not contribute any charge.
- Sulfate is a negatively charged ligand, contributing a charge of -2.
- Since the overall charge of the complex is 0, the oxidation state of the central transition metal (Fe) must be +2 to balance the charge.
- Therefore, the transition metal in this complex is in the +2 oxidation state.
c) H[Co(CO)4]:
- In this complex, we have four carbonyl (CO) ligands.
- Carbonyl is a neutral ligand, so it does not contribute any charge.
- Since there is no other ligand or counterion present in the complex, the overall charge of the complex is +1.
- Therefore, the oxidation state of the central transition metal (Co) must be -1 to balance the charge.
- Therefore, the transition metal in this complex is in the -1 oxidation state.
d) K4[Ni(CN)4]:
- In this complex, we have four cyanide (CN) ligands.
- Cyanide is a negatively charged ligand, contributing a charge of -1 each. Since there are four cyanide ligands, the total charge contribution is -4.
- Since the overall charge of the complex is -4 (as indicated by the K4 counterions), the oxidation state of the central transition metal (Ni) must be 0 to balance the charge.
- Therefore, the transition metal in this complex is in the 0 oxidation state.
Conclusion:
The transition metal in the complex K4[Ni(CN)4] is in the zero oxidation state.
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In which complex is the transition metal in zero oxidation state:a)[Co(NH3)6Cl2]b)[Fe(H2O)6]SO4c)H[Co(CO)4]d)K4[Ni(CN)4]Correct answer is option 'D'. Can you explain this answer? for Class 12 2026 is part of Class 12 preparation. The Question and answers have been prepared according to the Class 12 exam syllabus. Information about In which complex is the transition metal in zero oxidation state:a)[Co(NH3)6Cl2]b)[Fe(H2O)6]SO4c)H[Co(CO)4]d)K4[Ni(CN)4]Correct answer is option 'D'. Can you explain this answer? covers all topics & solutions for Class 12 2026 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for In which complex is the transition metal in zero oxidation state:a)[Co(NH3)6Cl2]b)[Fe(H2O)6]SO4c)H[Co(CO)4]d)K4[Ni(CN)4]Correct answer is option 'D'. Can you explain this answer?.
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