274342
The number of unpaired electrons in $\left[\mathrm{NiCI}_{4}\right]^{2-}$, $\mathrm{Ni}(\mathrm{CO})_{4}$ and $\left[\mathrm{Cu}\left(\mathrm{NH}_{3}\right)_{4}\right]^{2+}$ respectively are
1 $2,2,1$
2 $2,0,1$
3 $0,2,1$
4 $2,2,0$
Explanation:
(B) : $\mathrm{In}\left[\mathrm{NiCl}_{4}\right]^{2-} \mathrm{Ni}$ is in +2 oxidation state $\mathrm{Cl}^{-}$is a weak field ligand, thus pairing of electrons does not takes place. Unpaired electrons $=2$ $\mathrm{sp}^{3}$ hybridisation In $\mathrm{Ni}(\mathrm{Co})_{4}, \mathrm{Ni}$ is in zero oxidation state. $\mathrm{Ni}=[\mathrm{Ar}] 3 \mathrm{~d}^{8} 4 \mathrm{~s}^{2}$ Co is strong field ligand and cause pairing of electron of $4 \mathrm{~s}$ to $3 \mathrm{~d}$. $\mathrm{Cu}^{2+}:[\mathrm{Ar}] 3 \mathrm{~d}^9 4 \mathrm{~s}^0$
WB-JEE-2017
COORDINATION COMPOUNDS
274343
In the complex, $\mathrm{K}_{2} \mathrm{Fe}\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]$
1 the complex is high spin complex
2 both $\mathrm{Fe}$ atoms are in the same oxidation state
3 the coordination number of iron is 4
4 both $\mathrm{Fe}$ atoms are in different oxidation states
Explanation:
(B) : $\mathrm{K}_{2} \mathrm{Fe}\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]$ Let, $\mathrm{x}$ be the oxidation state of $\mathrm{Fe}$. $2(+1)+\mathrm{x}+\mathrm{x}+6(-1)=0$ $2 \mathrm{x}=+4$ $\mathrm{x}=+2$ (a) The complex will be low spin because $\mathrm{CN}$ is strong filled ligand due to which pairing take place in inner orbital's. (b) Both Fe metal are in same oxidation state i.e. +2 . Thus, statement is true. (c) The co-ordination number of iron is 6 because metal connected with six $\mathrm{CN}$ ligand. (d) Both $\mathrm{Fe}$ is in same oxidation state.
BITSAT-2016
COORDINATION COMPOUNDS
274344
The coordination number and the oxidation state of the central metal ion in the complex ion $\left[\mathrm{CrCl}_{2}(\mathrm{Ox})_{2}\right]^{3-}$ are respectively,
1 4 and $3-$
2 6 and $3+$
3 4 and 3+
4 6 and $3-$
Explanation:
(B) : The complex contains the two bidentate ligand and two chlorine ligand. Thus, the metal connected with the six donor sites. Hence, the coordination number is 6 . Let, $\mathrm{x}$ be the oxidation state of $\mathrm{Cr}$. $\therefore \mathrm{x}+2(-1)+2(-2)=-3$ $\mathrm{x}-2-4=-3$ $\mathrm{x}=+3$ The oxidation state of $\mathrm{Cr}$ is +3
J and K CET-(2016)
COORDINATION COMPOUNDS
274345
In which of the following coordination compounds, the central metal ion is in zero oxidation state?
(C) : The oxidation state of all the central metal ion are- (i) $\left[\mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right] \mathrm{Cl}_{3}$ $\mathrm{x}+6 \times 0+3(-1)=0$ $\mathrm{x}=+3$ Objective Chemistry Volume-II $\text { (ii) } \mathrm{K}_{4}\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]$ $4 \times(+1)+\mathrm{x}+6(-1)=0$ $\mathrm{x}=+2$ (iii) $\mathrm{Fe}(\mathrm{CO})_{5}$ $x+5 \times 0=0$ $\mathrm{x}=0$ (iv) $\left[\mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right] \mathrm{Cl}_{2}$ $\mathrm{x}+6 \times(0)+2(-1)=0$ $x=+2$ So, the $\mathrm{Fe}(\mathrm{CO})_{5}$ has zero oxidation state in central metal.
274342
The number of unpaired electrons in $\left[\mathrm{NiCI}_{4}\right]^{2-}$, $\mathrm{Ni}(\mathrm{CO})_{4}$ and $\left[\mathrm{Cu}\left(\mathrm{NH}_{3}\right)_{4}\right]^{2+}$ respectively are
1 $2,2,1$
2 $2,0,1$
3 $0,2,1$
4 $2,2,0$
Explanation:
(B) : $\mathrm{In}\left[\mathrm{NiCl}_{4}\right]^{2-} \mathrm{Ni}$ is in +2 oxidation state $\mathrm{Cl}^{-}$is a weak field ligand, thus pairing of electrons does not takes place. Unpaired electrons $=2$ $\mathrm{sp}^{3}$ hybridisation In $\mathrm{Ni}(\mathrm{Co})_{4}, \mathrm{Ni}$ is in zero oxidation state. $\mathrm{Ni}=[\mathrm{Ar}] 3 \mathrm{~d}^{8} 4 \mathrm{~s}^{2}$ Co is strong field ligand and cause pairing of electron of $4 \mathrm{~s}$ to $3 \mathrm{~d}$. $\mathrm{Cu}^{2+}:[\mathrm{Ar}] 3 \mathrm{~d}^9 4 \mathrm{~s}^0$
WB-JEE-2017
COORDINATION COMPOUNDS
274343
In the complex, $\mathrm{K}_{2} \mathrm{Fe}\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]$
1 the complex is high spin complex
2 both $\mathrm{Fe}$ atoms are in the same oxidation state
3 the coordination number of iron is 4
4 both $\mathrm{Fe}$ atoms are in different oxidation states
Explanation:
(B) : $\mathrm{K}_{2} \mathrm{Fe}\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]$ Let, $\mathrm{x}$ be the oxidation state of $\mathrm{Fe}$. $2(+1)+\mathrm{x}+\mathrm{x}+6(-1)=0$ $2 \mathrm{x}=+4$ $\mathrm{x}=+2$ (a) The complex will be low spin because $\mathrm{CN}$ is strong filled ligand due to which pairing take place in inner orbital's. (b) Both Fe metal are in same oxidation state i.e. +2 . Thus, statement is true. (c) The co-ordination number of iron is 6 because metal connected with six $\mathrm{CN}$ ligand. (d) Both $\mathrm{Fe}$ is in same oxidation state.
BITSAT-2016
COORDINATION COMPOUNDS
274344
The coordination number and the oxidation state of the central metal ion in the complex ion $\left[\mathrm{CrCl}_{2}(\mathrm{Ox})_{2}\right]^{3-}$ are respectively,
1 4 and $3-$
2 6 and $3+$
3 4 and 3+
4 6 and $3-$
Explanation:
(B) : The complex contains the two bidentate ligand and two chlorine ligand. Thus, the metal connected with the six donor sites. Hence, the coordination number is 6 . Let, $\mathrm{x}$ be the oxidation state of $\mathrm{Cr}$. $\therefore \mathrm{x}+2(-1)+2(-2)=-3$ $\mathrm{x}-2-4=-3$ $\mathrm{x}=+3$ The oxidation state of $\mathrm{Cr}$ is +3
J and K CET-(2016)
COORDINATION COMPOUNDS
274345
In which of the following coordination compounds, the central metal ion is in zero oxidation state?
(C) : The oxidation state of all the central metal ion are- (i) $\left[\mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right] \mathrm{Cl}_{3}$ $\mathrm{x}+6 \times 0+3(-1)=0$ $\mathrm{x}=+3$ Objective Chemistry Volume-II $\text { (ii) } \mathrm{K}_{4}\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]$ $4 \times(+1)+\mathrm{x}+6(-1)=0$ $\mathrm{x}=+2$ (iii) $\mathrm{Fe}(\mathrm{CO})_{5}$ $x+5 \times 0=0$ $\mathrm{x}=0$ (iv) $\left[\mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right] \mathrm{Cl}_{2}$ $\mathrm{x}+6 \times(0)+2(-1)=0$ $x=+2$ So, the $\mathrm{Fe}(\mathrm{CO})_{5}$ has zero oxidation state in central metal.
274342
The number of unpaired electrons in $\left[\mathrm{NiCI}_{4}\right]^{2-}$, $\mathrm{Ni}(\mathrm{CO})_{4}$ and $\left[\mathrm{Cu}\left(\mathrm{NH}_{3}\right)_{4}\right]^{2+}$ respectively are
1 $2,2,1$
2 $2,0,1$
3 $0,2,1$
4 $2,2,0$
Explanation:
(B) : $\mathrm{In}\left[\mathrm{NiCl}_{4}\right]^{2-} \mathrm{Ni}$ is in +2 oxidation state $\mathrm{Cl}^{-}$is a weak field ligand, thus pairing of electrons does not takes place. Unpaired electrons $=2$ $\mathrm{sp}^{3}$ hybridisation In $\mathrm{Ni}(\mathrm{Co})_{4}, \mathrm{Ni}$ is in zero oxidation state. $\mathrm{Ni}=[\mathrm{Ar}] 3 \mathrm{~d}^{8} 4 \mathrm{~s}^{2}$ Co is strong field ligand and cause pairing of electron of $4 \mathrm{~s}$ to $3 \mathrm{~d}$. $\mathrm{Cu}^{2+}:[\mathrm{Ar}] 3 \mathrm{~d}^9 4 \mathrm{~s}^0$
WB-JEE-2017
COORDINATION COMPOUNDS
274343
In the complex, $\mathrm{K}_{2} \mathrm{Fe}\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]$
1 the complex is high spin complex
2 both $\mathrm{Fe}$ atoms are in the same oxidation state
3 the coordination number of iron is 4
4 both $\mathrm{Fe}$ atoms are in different oxidation states
Explanation:
(B) : $\mathrm{K}_{2} \mathrm{Fe}\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]$ Let, $\mathrm{x}$ be the oxidation state of $\mathrm{Fe}$. $2(+1)+\mathrm{x}+\mathrm{x}+6(-1)=0$ $2 \mathrm{x}=+4$ $\mathrm{x}=+2$ (a) The complex will be low spin because $\mathrm{CN}$ is strong filled ligand due to which pairing take place in inner orbital's. (b) Both Fe metal are in same oxidation state i.e. +2 . Thus, statement is true. (c) The co-ordination number of iron is 6 because metal connected with six $\mathrm{CN}$ ligand. (d) Both $\mathrm{Fe}$ is in same oxidation state.
BITSAT-2016
COORDINATION COMPOUNDS
274344
The coordination number and the oxidation state of the central metal ion in the complex ion $\left[\mathrm{CrCl}_{2}(\mathrm{Ox})_{2}\right]^{3-}$ are respectively,
1 4 and $3-$
2 6 and $3+$
3 4 and 3+
4 6 and $3-$
Explanation:
(B) : The complex contains the two bidentate ligand and two chlorine ligand. Thus, the metal connected with the six donor sites. Hence, the coordination number is 6 . Let, $\mathrm{x}$ be the oxidation state of $\mathrm{Cr}$. $\therefore \mathrm{x}+2(-1)+2(-2)=-3$ $\mathrm{x}-2-4=-3$ $\mathrm{x}=+3$ The oxidation state of $\mathrm{Cr}$ is +3
J and K CET-(2016)
COORDINATION COMPOUNDS
274345
In which of the following coordination compounds, the central metal ion is in zero oxidation state?
(C) : The oxidation state of all the central metal ion are- (i) $\left[\mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right] \mathrm{Cl}_{3}$ $\mathrm{x}+6 \times 0+3(-1)=0$ $\mathrm{x}=+3$ Objective Chemistry Volume-II $\text { (ii) } \mathrm{K}_{4}\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]$ $4 \times(+1)+\mathrm{x}+6(-1)=0$ $\mathrm{x}=+2$ (iii) $\mathrm{Fe}(\mathrm{CO})_{5}$ $x+5 \times 0=0$ $\mathrm{x}=0$ (iv) $\left[\mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right] \mathrm{Cl}_{2}$ $\mathrm{x}+6 \times(0)+2(-1)=0$ $x=+2$ So, the $\mathrm{Fe}(\mathrm{CO})_{5}$ has zero oxidation state in central metal.
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COORDINATION COMPOUNDS
274342
The number of unpaired electrons in $\left[\mathrm{NiCI}_{4}\right]^{2-}$, $\mathrm{Ni}(\mathrm{CO})_{4}$ and $\left[\mathrm{Cu}\left(\mathrm{NH}_{3}\right)_{4}\right]^{2+}$ respectively are
1 $2,2,1$
2 $2,0,1$
3 $0,2,1$
4 $2,2,0$
Explanation:
(B) : $\mathrm{In}\left[\mathrm{NiCl}_{4}\right]^{2-} \mathrm{Ni}$ is in +2 oxidation state $\mathrm{Cl}^{-}$is a weak field ligand, thus pairing of electrons does not takes place. Unpaired electrons $=2$ $\mathrm{sp}^{3}$ hybridisation In $\mathrm{Ni}(\mathrm{Co})_{4}, \mathrm{Ni}$ is in zero oxidation state. $\mathrm{Ni}=[\mathrm{Ar}] 3 \mathrm{~d}^{8} 4 \mathrm{~s}^{2}$ Co is strong field ligand and cause pairing of electron of $4 \mathrm{~s}$ to $3 \mathrm{~d}$. $\mathrm{Cu}^{2+}:[\mathrm{Ar}] 3 \mathrm{~d}^9 4 \mathrm{~s}^0$
WB-JEE-2017
COORDINATION COMPOUNDS
274343
In the complex, $\mathrm{K}_{2} \mathrm{Fe}\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]$
1 the complex is high spin complex
2 both $\mathrm{Fe}$ atoms are in the same oxidation state
3 the coordination number of iron is 4
4 both $\mathrm{Fe}$ atoms are in different oxidation states
Explanation:
(B) : $\mathrm{K}_{2} \mathrm{Fe}\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]$ Let, $\mathrm{x}$ be the oxidation state of $\mathrm{Fe}$. $2(+1)+\mathrm{x}+\mathrm{x}+6(-1)=0$ $2 \mathrm{x}=+4$ $\mathrm{x}=+2$ (a) The complex will be low spin because $\mathrm{CN}$ is strong filled ligand due to which pairing take place in inner orbital's. (b) Both Fe metal are in same oxidation state i.e. +2 . Thus, statement is true. (c) The co-ordination number of iron is 6 because metal connected with six $\mathrm{CN}$ ligand. (d) Both $\mathrm{Fe}$ is in same oxidation state.
BITSAT-2016
COORDINATION COMPOUNDS
274344
The coordination number and the oxidation state of the central metal ion in the complex ion $\left[\mathrm{CrCl}_{2}(\mathrm{Ox})_{2}\right]^{3-}$ are respectively,
1 4 and $3-$
2 6 and $3+$
3 4 and 3+
4 6 and $3-$
Explanation:
(B) : The complex contains the two bidentate ligand and two chlorine ligand. Thus, the metal connected with the six donor sites. Hence, the coordination number is 6 . Let, $\mathrm{x}$ be the oxidation state of $\mathrm{Cr}$. $\therefore \mathrm{x}+2(-1)+2(-2)=-3$ $\mathrm{x}-2-4=-3$ $\mathrm{x}=+3$ The oxidation state of $\mathrm{Cr}$ is +3
J and K CET-(2016)
COORDINATION COMPOUNDS
274345
In which of the following coordination compounds, the central metal ion is in zero oxidation state?
(C) : The oxidation state of all the central metal ion are- (i) $\left[\mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right] \mathrm{Cl}_{3}$ $\mathrm{x}+6 \times 0+3(-1)=0$ $\mathrm{x}=+3$ Objective Chemistry Volume-II $\text { (ii) } \mathrm{K}_{4}\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]$ $4 \times(+1)+\mathrm{x}+6(-1)=0$ $\mathrm{x}=+2$ (iii) $\mathrm{Fe}(\mathrm{CO})_{5}$ $x+5 \times 0=0$ $\mathrm{x}=0$ (iv) $\left[\mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right] \mathrm{Cl}_{2}$ $\mathrm{x}+6 \times(0)+2(-1)=0$ $x=+2$ So, the $\mathrm{Fe}(\mathrm{CO})_{5}$ has zero oxidation state in central metal.
