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In which of the following complexes, oxidation state of metal is zero ?
- a)[Pt(NH₃)₂ Cl₂]
- b)[Cr(CO)₆]
- c)[Cr(NH₃)₃ Cl₃]
- d)[Cr(en)₂ Cl₂]
Correct answer is option 'B'. Can you explain this answer?
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In which of the following complexes, oxidation state of metal is zero ...
In metal carbonyls oxidation state is zero since Co is a neutral ligand!
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In which of the following complexes, oxidation state of metal is zero ...
Explanation:
Zero Oxidation State in Metal Complexes:
Metal complexes with a metal in the oxidation state of zero are known as zerovalent complexes. In these complexes, the metal atom or ion has donated all of its valence electrons to the ligands, resulting in a formal oxidation state of zero.
Identifying the Zerovalent Complex:
In the given options, the complex [Cr(CO)₆] is a zerovalent complex where the oxidation state of chromium is zero. This is because each carbon monoxide ligand donates a lone pair of electrons to the chromium atom, resulting in a total of 6 donated pairs, which satisfies the 18-electron rule for a zerovalent complex.
Explanation of Other Options:
a) [Pt(NH₃)₂ Cl₂]: In this complex, the oxidation state of platinum is +2, as it donates two electrons to each of the ammonia ligands.
c) [Cr(NH₃)₃ Cl₃]: In this complex, the oxidation state of chromium is +3, as it donates three electrons to each of the ammonia ligands and three electrons to the chloride ligands.
d) [Cr(en)₂ Cl₂]: In this complex, the oxidation state of chromium is +2, as it donates two electrons to each of the ethylenediamine ligands and two electrons to the chloride ligands.
Therefore, the correct answer is option 'B' [Cr(CO)₆], where the oxidation state of the metal is zero due to the donation of electrons from the ligands.
Zero Oxidation State in Metal Complexes:
Metal complexes with a metal in the oxidation state of zero are known as zerovalent complexes. In these complexes, the metal atom or ion has donated all of its valence electrons to the ligands, resulting in a formal oxidation state of zero.
Identifying the Zerovalent Complex:
In the given options, the complex [Cr(CO)₆] is a zerovalent complex where the oxidation state of chromium is zero. This is because each carbon monoxide ligand donates a lone pair of electrons to the chromium atom, resulting in a total of 6 donated pairs, which satisfies the 18-electron rule for a zerovalent complex.
Explanation of Other Options:
a) [Pt(NH₃)₂ Cl₂]: In this complex, the oxidation state of platinum is +2, as it donates two electrons to each of the ammonia ligands.
c) [Cr(NH₃)₃ Cl₃]: In this complex, the oxidation state of chromium is +3, as it donates three electrons to each of the ammonia ligands and three electrons to the chloride ligands.
d) [Cr(en)₂ Cl₂]: In this complex, the oxidation state of chromium is +2, as it donates two electrons to each of the ethylenediamine ligands and two electrons to the chloride ligands.
Therefore, the correct answer is option 'B' [Cr(CO)₆], where the oxidation state of the metal is zero due to the donation of electrons from the ligands.
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In which of the following complexes, oxidation state of metal is zero ?a)[Pt(NH₃)₂ Cl₂]b)[Cr(CO)₆]c)[Cr(NH₃)₃ Cl₃]d)[Cr(en)₂ Cl₂]Correct answer is option 'B'. Can you explain this answer?
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