(C) : $\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]^{4-}$ $\mathrm{CN}^{-}$is strong field ligand and cause pairing of $\mathrm{d}$ electron. Number of unpaired electron $=0$ $\left[\mathrm{MnCl}_{4}\right]^{2-}, \mathrm{Cl}^{-}$is weak field ligand and causes no pairing of d-electron. No. of unpaired electron $=5$ $\left[\mathrm{CoCl}_{4}\right]^{2-}, \mathrm{Cl}^{-}$is weak field ligand and does not do pairing of d-electron. Number of unpaired electron $=3$ Magnetic moment $\propto$ number of unpaired electron Order:- $\left[\mathrm{MnCl}_{4}\right]^{2-}>\left[\mathrm{CoCl}_{4}\right]^{2-}>\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]^{4-}$
BITSAT-2014
COORDINATION COMPOUNDS
273993
The pair in which both species have same magnetic moment (spin only value) is:
(B) : $\mathrm{H}_{2} \mathrm{O}$ act as weak field ligand and pairing not occurs. ${\left[\mathrm{Cr}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{2+} \Rightarrow \mathrm{Cr}^{2+}}$ $\mathrm{Cr}^{2+}: \mathrm{d}^{4}$ Number of unpaired electron $=4$ No. of unpaired electron $=4$ Both $\left[\mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{2+}$ and $\left[\mathrm{Cr}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{2+}$ having same number of unpaired electrons and that's why there spin only magnetic moment is also same.
JEE Main 2016
COORDINATION COMPOUNDS
273994
Which one of the following cyano complexes would exhibit the lowest value of paramagnetic behavior?
(A) : $\mathrm{CN}^{\ominus}$ act as strong field ligand and cause pairing of metal d-electron. Number of unpaired electron $=0$ Number of unpaired electron $=1$ Number of unpaired electron $=2$ Number of unpaired electron $=3$ Hence, $\left[\mathrm{Co}(\mathrm{CN})_{6}\right]^{3-}$ exhibit the lowest value of paramagnetic behaviour.
BITSAT-2018
COORDINATION COMPOUNDS
273998
The d electron configurations of $\mathrm{Cr}^{2+}, \mathrm{Mn}^{2+}$, $\mathrm{Fe}^{2+}$ and $\mathrm{Ni}^{2+}$ are $3 d^{4}, 3 d^{5}, 3 d^{6}$ and $3 d^{8}$ respectively. Which one of the following aqua complexes will exhibit the minimum paramagnetic behaviour?
273999
The d-electron configurations of $\mathrm{Cr}^{2+}, \mathrm{Mn}^{2+}$, $\mathrm{Fe}^{2+}$ and $\mathrm{Co}^{2+}$ are $d^{4}, d^{5}, d^{6}$ and $d^{7}$ respectively. Which one of the following will exhibit minimum paramagnetic behaviour?
(C) : $\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]^{4-}$ $\mathrm{CN}^{-}$is strong field ligand and cause pairing of $\mathrm{d}$ electron. Number of unpaired electron $=0$ $\left[\mathrm{MnCl}_{4}\right]^{2-}, \mathrm{Cl}^{-}$is weak field ligand and causes no pairing of d-electron. No. of unpaired electron $=5$ $\left[\mathrm{CoCl}_{4}\right]^{2-}, \mathrm{Cl}^{-}$is weak field ligand and does not do pairing of d-electron. Number of unpaired electron $=3$ Magnetic moment $\propto$ number of unpaired electron Order:- $\left[\mathrm{MnCl}_{4}\right]^{2-}>\left[\mathrm{CoCl}_{4}\right]^{2-}>\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]^{4-}$
BITSAT-2014
COORDINATION COMPOUNDS
273993
The pair in which both species have same magnetic moment (spin only value) is:
(B) : $\mathrm{H}_{2} \mathrm{O}$ act as weak field ligand and pairing not occurs. ${\left[\mathrm{Cr}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{2+} \Rightarrow \mathrm{Cr}^{2+}}$ $\mathrm{Cr}^{2+}: \mathrm{d}^{4}$ Number of unpaired electron $=4$ No. of unpaired electron $=4$ Both $\left[\mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{2+}$ and $\left[\mathrm{Cr}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{2+}$ having same number of unpaired electrons and that's why there spin only magnetic moment is also same.
JEE Main 2016
COORDINATION COMPOUNDS
273994
Which one of the following cyano complexes would exhibit the lowest value of paramagnetic behavior?
(A) : $\mathrm{CN}^{\ominus}$ act as strong field ligand and cause pairing of metal d-electron. Number of unpaired electron $=0$ Number of unpaired electron $=1$ Number of unpaired electron $=2$ Number of unpaired electron $=3$ Hence, $\left[\mathrm{Co}(\mathrm{CN})_{6}\right]^{3-}$ exhibit the lowest value of paramagnetic behaviour.
BITSAT-2018
COORDINATION COMPOUNDS
273998
The d electron configurations of $\mathrm{Cr}^{2+}, \mathrm{Mn}^{2+}$, $\mathrm{Fe}^{2+}$ and $\mathrm{Ni}^{2+}$ are $3 d^{4}, 3 d^{5}, 3 d^{6}$ and $3 d^{8}$ respectively. Which one of the following aqua complexes will exhibit the minimum paramagnetic behaviour?
273999
The d-electron configurations of $\mathrm{Cr}^{2+}, \mathrm{Mn}^{2+}$, $\mathrm{Fe}^{2+}$ and $\mathrm{Co}^{2+}$ are $d^{4}, d^{5}, d^{6}$ and $d^{7}$ respectively. Which one of the following will exhibit minimum paramagnetic behaviour?
(C) : $\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]^{4-}$ $\mathrm{CN}^{-}$is strong field ligand and cause pairing of $\mathrm{d}$ electron. Number of unpaired electron $=0$ $\left[\mathrm{MnCl}_{4}\right]^{2-}, \mathrm{Cl}^{-}$is weak field ligand and causes no pairing of d-electron. No. of unpaired electron $=5$ $\left[\mathrm{CoCl}_{4}\right]^{2-}, \mathrm{Cl}^{-}$is weak field ligand and does not do pairing of d-electron. Number of unpaired electron $=3$ Magnetic moment $\propto$ number of unpaired electron Order:- $\left[\mathrm{MnCl}_{4}\right]^{2-}>\left[\mathrm{CoCl}_{4}\right]^{2-}>\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]^{4-}$
BITSAT-2014
COORDINATION COMPOUNDS
273993
The pair in which both species have same magnetic moment (spin only value) is:
(B) : $\mathrm{H}_{2} \mathrm{O}$ act as weak field ligand and pairing not occurs. ${\left[\mathrm{Cr}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{2+} \Rightarrow \mathrm{Cr}^{2+}}$ $\mathrm{Cr}^{2+}: \mathrm{d}^{4}$ Number of unpaired electron $=4$ No. of unpaired electron $=4$ Both $\left[\mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{2+}$ and $\left[\mathrm{Cr}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{2+}$ having same number of unpaired electrons and that's why there spin only magnetic moment is also same.
JEE Main 2016
COORDINATION COMPOUNDS
273994
Which one of the following cyano complexes would exhibit the lowest value of paramagnetic behavior?
(A) : $\mathrm{CN}^{\ominus}$ act as strong field ligand and cause pairing of metal d-electron. Number of unpaired electron $=0$ Number of unpaired electron $=1$ Number of unpaired electron $=2$ Number of unpaired electron $=3$ Hence, $\left[\mathrm{Co}(\mathrm{CN})_{6}\right]^{3-}$ exhibit the lowest value of paramagnetic behaviour.
BITSAT-2018
COORDINATION COMPOUNDS
273998
The d electron configurations of $\mathrm{Cr}^{2+}, \mathrm{Mn}^{2+}$, $\mathrm{Fe}^{2+}$ and $\mathrm{Ni}^{2+}$ are $3 d^{4}, 3 d^{5}, 3 d^{6}$ and $3 d^{8}$ respectively. Which one of the following aqua complexes will exhibit the minimum paramagnetic behaviour?
273999
The d-electron configurations of $\mathrm{Cr}^{2+}, \mathrm{Mn}^{2+}$, $\mathrm{Fe}^{2+}$ and $\mathrm{Co}^{2+}$ are $d^{4}, d^{5}, d^{6}$ and $d^{7}$ respectively. Which one of the following will exhibit minimum paramagnetic behaviour?
(C) : $\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]^{4-}$ $\mathrm{CN}^{-}$is strong field ligand and cause pairing of $\mathrm{d}$ electron. Number of unpaired electron $=0$ $\left[\mathrm{MnCl}_{4}\right]^{2-}, \mathrm{Cl}^{-}$is weak field ligand and causes no pairing of d-electron. No. of unpaired electron $=5$ $\left[\mathrm{CoCl}_{4}\right]^{2-}, \mathrm{Cl}^{-}$is weak field ligand and does not do pairing of d-electron. Number of unpaired electron $=3$ Magnetic moment $\propto$ number of unpaired electron Order:- $\left[\mathrm{MnCl}_{4}\right]^{2-}>\left[\mathrm{CoCl}_{4}\right]^{2-}>\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]^{4-}$
BITSAT-2014
COORDINATION COMPOUNDS
273993
The pair in which both species have same magnetic moment (spin only value) is:
(B) : $\mathrm{H}_{2} \mathrm{O}$ act as weak field ligand and pairing not occurs. ${\left[\mathrm{Cr}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{2+} \Rightarrow \mathrm{Cr}^{2+}}$ $\mathrm{Cr}^{2+}: \mathrm{d}^{4}$ Number of unpaired electron $=4$ No. of unpaired electron $=4$ Both $\left[\mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{2+}$ and $\left[\mathrm{Cr}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{2+}$ having same number of unpaired electrons and that's why there spin only magnetic moment is also same.
JEE Main 2016
COORDINATION COMPOUNDS
273994
Which one of the following cyano complexes would exhibit the lowest value of paramagnetic behavior?
(A) : $\mathrm{CN}^{\ominus}$ act as strong field ligand and cause pairing of metal d-electron. Number of unpaired electron $=0$ Number of unpaired electron $=1$ Number of unpaired electron $=2$ Number of unpaired electron $=3$ Hence, $\left[\mathrm{Co}(\mathrm{CN})_{6}\right]^{3-}$ exhibit the lowest value of paramagnetic behaviour.
BITSAT-2018
COORDINATION COMPOUNDS
273998
The d electron configurations of $\mathrm{Cr}^{2+}, \mathrm{Mn}^{2+}$, $\mathrm{Fe}^{2+}$ and $\mathrm{Ni}^{2+}$ are $3 d^{4}, 3 d^{5}, 3 d^{6}$ and $3 d^{8}$ respectively. Which one of the following aqua complexes will exhibit the minimum paramagnetic behaviour?
273999
The d-electron configurations of $\mathrm{Cr}^{2+}, \mathrm{Mn}^{2+}$, $\mathrm{Fe}^{2+}$ and $\mathrm{Co}^{2+}$ are $d^{4}, d^{5}, d^{6}$ and $d^{7}$ respectively. Which one of the following will exhibit minimum paramagnetic behaviour?
(C) : $\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]^{4-}$ $\mathrm{CN}^{-}$is strong field ligand and cause pairing of $\mathrm{d}$ electron. Number of unpaired electron $=0$ $\left[\mathrm{MnCl}_{4}\right]^{2-}, \mathrm{Cl}^{-}$is weak field ligand and causes no pairing of d-electron. No. of unpaired electron $=5$ $\left[\mathrm{CoCl}_{4}\right]^{2-}, \mathrm{Cl}^{-}$is weak field ligand and does not do pairing of d-electron. Number of unpaired electron $=3$ Magnetic moment $\propto$ number of unpaired electron Order:- $\left[\mathrm{MnCl}_{4}\right]^{2-}>\left[\mathrm{CoCl}_{4}\right]^{2-}>\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]^{4-}$
BITSAT-2014
COORDINATION COMPOUNDS
273993
The pair in which both species have same magnetic moment (spin only value) is:
(B) : $\mathrm{H}_{2} \mathrm{O}$ act as weak field ligand and pairing not occurs. ${\left[\mathrm{Cr}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{2+} \Rightarrow \mathrm{Cr}^{2+}}$ $\mathrm{Cr}^{2+}: \mathrm{d}^{4}$ Number of unpaired electron $=4$ No. of unpaired electron $=4$ Both $\left[\mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{2+}$ and $\left[\mathrm{Cr}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{2+}$ having same number of unpaired electrons and that's why there spin only magnetic moment is also same.
JEE Main 2016
COORDINATION COMPOUNDS
273994
Which one of the following cyano complexes would exhibit the lowest value of paramagnetic behavior?
(A) : $\mathrm{CN}^{\ominus}$ act as strong field ligand and cause pairing of metal d-electron. Number of unpaired electron $=0$ Number of unpaired electron $=1$ Number of unpaired electron $=2$ Number of unpaired electron $=3$ Hence, $\left[\mathrm{Co}(\mathrm{CN})_{6}\right]^{3-}$ exhibit the lowest value of paramagnetic behaviour.
BITSAT-2018
COORDINATION COMPOUNDS
273998
The d electron configurations of $\mathrm{Cr}^{2+}, \mathrm{Mn}^{2+}$, $\mathrm{Fe}^{2+}$ and $\mathrm{Ni}^{2+}$ are $3 d^{4}, 3 d^{5}, 3 d^{6}$ and $3 d^{8}$ respectively. Which one of the following aqua complexes will exhibit the minimum paramagnetic behaviour?
273999
The d-electron configurations of $\mathrm{Cr}^{2+}, \mathrm{Mn}^{2+}$, $\mathrm{Fe}^{2+}$ and $\mathrm{Co}^{2+}$ are $d^{4}, d^{5}, d^{6}$ and $d^{7}$ respectively. Which one of the following will exhibit minimum paramagnetic behaviour?
