274078
Amongst $\mathrm{Ni}(\mathrm{CO})_{4},\left[\mathrm{Ni}(\mathrm{CN})_{4}\right]^{2-}$ and $\left[\mathrm{NiCl}_{4}^{2-}\right]$
1 $\mathrm{Ni}(\mathrm{CO})_{4}$ and $\left[\mathrm{NiCl}_{4}^{2-}\right]$ are diamagnetic but $\left[\mathrm{Ni}(\mathrm{CN})_{4}\right]^{2-}$ is paramagnetic
2 $\mathrm{Ni}(\mathrm{CO})_{4}$ and $\left[\mathrm{Ni}(\mathrm{CN})_{4}\right]^{2-}$ are diamagnetic but $\mathrm{NiCl}_{4}^{2-}$ is paramagnetic
3 $\mathrm{NiCl}_{4}^{2-}$ and $\left[\mathrm{Ni}(\mathrm{CN})_{4}\right]^{2-}$ are diamagnetic but $\mathrm{Ni}(\mathrm{CO})_{4}$ is paramagnetic
4 $\mathrm{Ni}(\mathrm{CO})_{4}$ is diamagnetic but $\mathrm{NiCl}_{4}^{2-}$ and $\left[\mathrm{Ni}(\mathrm{CN})_{4}\right]^{2-}$ is paramagnetic
Explanation:
(B) : Electronic configuration of ${ }_{28} \mathrm{Ni}$ in $\left[\mathrm{Ni}(\mathrm{CO})_{4}\right]$ $=[\mathrm{Ar}] 3 \mathrm{~d}^{8} 4 \mathrm{~s}^{2}$ $=0$ unpaired electron (diamagnetic) Electronic configuration of ${ }_{28} \mathrm{Ni}^{+2}$ in $\left[\mathrm{Ni}(\mathrm{CN})_{4}\right]^{2-}$ $=[\mathrm{Ar}] 3 \mathrm{~d}^{8}$ (square planar) $=0$ unpaired electron (diamagnetic) Electronic configuration of ${ }_{28} \mathrm{Ni}^{+2}$ in $\left[\mathrm{Ni}(\mathrm{Cl})_{4}\right]^{2-}$ $=[\mathrm{Ar}] 3 \mathrm{~d}^{8}$ $=2$ unpaired electron (paramagnetic)
VITEEE-2011
COORDINATION COMPOUNDS
274082
Identify the order in which the spin only magnetic moment (in BM) increases for the following four ions (I) $\mathrm{Fe}^{2+}$ (II) $\mathrm{Ti}^{2+}$ (III) $\mathrm{Cu}^{2+}$ (IV) $\mathrm{V}^{2+}$
1 I, II, IV, III
2 IV, I, II, III
3 III, IV, I, II
4 III, II, IV, I
Explanation:
(D) : (i) Magnetic moment $(\mu)=\sqrt{\mathrm{n}(\mathrm{n}+2)}$ Where $\mathrm{n}=$ no. of unpaired electron $\mu=\sqrt{4(4+2)}=\sqrt{24}=4.90 \mathrm{BM}$ (ii) $\mathrm{n}=2, \mu=2.83 \mathrm{BM}$ (iii) $\mathrm{n}=1, \mu=1.732 \mathrm{BM}$ (iv) $\mathrm{n}=3, \mu=3.87$ BM. Hence, the increasing order of magnetic moment is $\mathrm{Cu}^{2+}<\mathrm{Ti}^{2+}<\mathrm{V}^{2+}<\mathrm{Fe}^{+2}$ Hence, III $<$ II $<$ IV $<$ I
AP EAMCET- (Engg.)-2011
COORDINATION COMPOUNDS
274086
Which among the following is a paramagnetic complex?
274089
The spin only magnetic moment value (in B.M. unit) of $\mathrm{Cr}(\mathrm{CO})_{6}$ is
1 Zero
2 2.84
3 4.90
4 5.92
Explanation:
(A) : In $\mathrm{Cr}(\mathrm{CO})_{6}$, the oxidation state of chromium is zero. $\mathrm{Cr}=3 \mathrm{~d}^{5} 4 \mathrm{~s}^{1}$ $\mathrm{CO}$ ligand act as strong field ligand hence pairing of electrons occurs. Therefore, Number of unpaired electron $(\mathrm{n})=0$ Spin magnetic moment $=\sqrt{\mathrm{n}(\mathrm{n}+2)}=0$
274078
Amongst $\mathrm{Ni}(\mathrm{CO})_{4},\left[\mathrm{Ni}(\mathrm{CN})_{4}\right]^{2-}$ and $\left[\mathrm{NiCl}_{4}^{2-}\right]$
1 $\mathrm{Ni}(\mathrm{CO})_{4}$ and $\left[\mathrm{NiCl}_{4}^{2-}\right]$ are diamagnetic but $\left[\mathrm{Ni}(\mathrm{CN})_{4}\right]^{2-}$ is paramagnetic
2 $\mathrm{Ni}(\mathrm{CO})_{4}$ and $\left[\mathrm{Ni}(\mathrm{CN})_{4}\right]^{2-}$ are diamagnetic but $\mathrm{NiCl}_{4}^{2-}$ is paramagnetic
3 $\mathrm{NiCl}_{4}^{2-}$ and $\left[\mathrm{Ni}(\mathrm{CN})_{4}\right]^{2-}$ are diamagnetic but $\mathrm{Ni}(\mathrm{CO})_{4}$ is paramagnetic
4 $\mathrm{Ni}(\mathrm{CO})_{4}$ is diamagnetic but $\mathrm{NiCl}_{4}^{2-}$ and $\left[\mathrm{Ni}(\mathrm{CN})_{4}\right]^{2-}$ is paramagnetic
Explanation:
(B) : Electronic configuration of ${ }_{28} \mathrm{Ni}$ in $\left[\mathrm{Ni}(\mathrm{CO})_{4}\right]$ $=[\mathrm{Ar}] 3 \mathrm{~d}^{8} 4 \mathrm{~s}^{2}$ $=0$ unpaired electron (diamagnetic) Electronic configuration of ${ }_{28} \mathrm{Ni}^{+2}$ in $\left[\mathrm{Ni}(\mathrm{CN})_{4}\right]^{2-}$ $=[\mathrm{Ar}] 3 \mathrm{~d}^{8}$ (square planar) $=0$ unpaired electron (diamagnetic) Electronic configuration of ${ }_{28} \mathrm{Ni}^{+2}$ in $\left[\mathrm{Ni}(\mathrm{Cl})_{4}\right]^{2-}$ $=[\mathrm{Ar}] 3 \mathrm{~d}^{8}$ $=2$ unpaired electron (paramagnetic)
VITEEE-2011
COORDINATION COMPOUNDS
274082
Identify the order in which the spin only magnetic moment (in BM) increases for the following four ions (I) $\mathrm{Fe}^{2+}$ (II) $\mathrm{Ti}^{2+}$ (III) $\mathrm{Cu}^{2+}$ (IV) $\mathrm{V}^{2+}$
1 I, II, IV, III
2 IV, I, II, III
3 III, IV, I, II
4 III, II, IV, I
Explanation:
(D) : (i) Magnetic moment $(\mu)=\sqrt{\mathrm{n}(\mathrm{n}+2)}$ Where $\mathrm{n}=$ no. of unpaired electron $\mu=\sqrt{4(4+2)}=\sqrt{24}=4.90 \mathrm{BM}$ (ii) $\mathrm{n}=2, \mu=2.83 \mathrm{BM}$ (iii) $\mathrm{n}=1, \mu=1.732 \mathrm{BM}$ (iv) $\mathrm{n}=3, \mu=3.87$ BM. Hence, the increasing order of magnetic moment is $\mathrm{Cu}^{2+}<\mathrm{Ti}^{2+}<\mathrm{V}^{2+}<\mathrm{Fe}^{+2}$ Hence, III $<$ II $<$ IV $<$ I
AP EAMCET- (Engg.)-2011
COORDINATION COMPOUNDS
274086
Which among the following is a paramagnetic complex?
274089
The spin only magnetic moment value (in B.M. unit) of $\mathrm{Cr}(\mathrm{CO})_{6}$ is
1 Zero
2 2.84
3 4.90
4 5.92
Explanation:
(A) : In $\mathrm{Cr}(\mathrm{CO})_{6}$, the oxidation state of chromium is zero. $\mathrm{Cr}=3 \mathrm{~d}^{5} 4 \mathrm{~s}^{1}$ $\mathrm{CO}$ ligand act as strong field ligand hence pairing of electrons occurs. Therefore, Number of unpaired electron $(\mathrm{n})=0$ Spin magnetic moment $=\sqrt{\mathrm{n}(\mathrm{n}+2)}=0$
NEET Test Series from KOTA - 10 Papers In MS WORD
WhatsApp Here
COORDINATION COMPOUNDS
274078
Amongst $\mathrm{Ni}(\mathrm{CO})_{4},\left[\mathrm{Ni}(\mathrm{CN})_{4}\right]^{2-}$ and $\left[\mathrm{NiCl}_{4}^{2-}\right]$
1 $\mathrm{Ni}(\mathrm{CO})_{4}$ and $\left[\mathrm{NiCl}_{4}^{2-}\right]$ are diamagnetic but $\left[\mathrm{Ni}(\mathrm{CN})_{4}\right]^{2-}$ is paramagnetic
2 $\mathrm{Ni}(\mathrm{CO})_{4}$ and $\left[\mathrm{Ni}(\mathrm{CN})_{4}\right]^{2-}$ are diamagnetic but $\mathrm{NiCl}_{4}^{2-}$ is paramagnetic
3 $\mathrm{NiCl}_{4}^{2-}$ and $\left[\mathrm{Ni}(\mathrm{CN})_{4}\right]^{2-}$ are diamagnetic but $\mathrm{Ni}(\mathrm{CO})_{4}$ is paramagnetic
4 $\mathrm{Ni}(\mathrm{CO})_{4}$ is diamagnetic but $\mathrm{NiCl}_{4}^{2-}$ and $\left[\mathrm{Ni}(\mathrm{CN})_{4}\right]^{2-}$ is paramagnetic
Explanation:
(B) : Electronic configuration of ${ }_{28} \mathrm{Ni}$ in $\left[\mathrm{Ni}(\mathrm{CO})_{4}\right]$ $=[\mathrm{Ar}] 3 \mathrm{~d}^{8} 4 \mathrm{~s}^{2}$ $=0$ unpaired electron (diamagnetic) Electronic configuration of ${ }_{28} \mathrm{Ni}^{+2}$ in $\left[\mathrm{Ni}(\mathrm{CN})_{4}\right]^{2-}$ $=[\mathrm{Ar}] 3 \mathrm{~d}^{8}$ (square planar) $=0$ unpaired electron (diamagnetic) Electronic configuration of ${ }_{28} \mathrm{Ni}^{+2}$ in $\left[\mathrm{Ni}(\mathrm{Cl})_{4}\right]^{2-}$ $=[\mathrm{Ar}] 3 \mathrm{~d}^{8}$ $=2$ unpaired electron (paramagnetic)
VITEEE-2011
COORDINATION COMPOUNDS
274082
Identify the order in which the spin only magnetic moment (in BM) increases for the following four ions (I) $\mathrm{Fe}^{2+}$ (II) $\mathrm{Ti}^{2+}$ (III) $\mathrm{Cu}^{2+}$ (IV) $\mathrm{V}^{2+}$
1 I, II, IV, III
2 IV, I, II, III
3 III, IV, I, II
4 III, II, IV, I
Explanation:
(D) : (i) Magnetic moment $(\mu)=\sqrt{\mathrm{n}(\mathrm{n}+2)}$ Where $\mathrm{n}=$ no. of unpaired electron $\mu=\sqrt{4(4+2)}=\sqrt{24}=4.90 \mathrm{BM}$ (ii) $\mathrm{n}=2, \mu=2.83 \mathrm{BM}$ (iii) $\mathrm{n}=1, \mu=1.732 \mathrm{BM}$ (iv) $\mathrm{n}=3, \mu=3.87$ BM. Hence, the increasing order of magnetic moment is $\mathrm{Cu}^{2+}<\mathrm{Ti}^{2+}<\mathrm{V}^{2+}<\mathrm{Fe}^{+2}$ Hence, III $<$ II $<$ IV $<$ I
AP EAMCET- (Engg.)-2011
COORDINATION COMPOUNDS
274086
Which among the following is a paramagnetic complex?
274089
The spin only magnetic moment value (in B.M. unit) of $\mathrm{Cr}(\mathrm{CO})_{6}$ is
1 Zero
2 2.84
3 4.90
4 5.92
Explanation:
(A) : In $\mathrm{Cr}(\mathrm{CO})_{6}$, the oxidation state of chromium is zero. $\mathrm{Cr}=3 \mathrm{~d}^{5} 4 \mathrm{~s}^{1}$ $\mathrm{CO}$ ligand act as strong field ligand hence pairing of electrons occurs. Therefore, Number of unpaired electron $(\mathrm{n})=0$ Spin magnetic moment $=\sqrt{\mathrm{n}(\mathrm{n}+2)}=0$
274078
Amongst $\mathrm{Ni}(\mathrm{CO})_{4},\left[\mathrm{Ni}(\mathrm{CN})_{4}\right]^{2-}$ and $\left[\mathrm{NiCl}_{4}^{2-}\right]$
1 $\mathrm{Ni}(\mathrm{CO})_{4}$ and $\left[\mathrm{NiCl}_{4}^{2-}\right]$ are diamagnetic but $\left[\mathrm{Ni}(\mathrm{CN})_{4}\right]^{2-}$ is paramagnetic
2 $\mathrm{Ni}(\mathrm{CO})_{4}$ and $\left[\mathrm{Ni}(\mathrm{CN})_{4}\right]^{2-}$ are diamagnetic but $\mathrm{NiCl}_{4}^{2-}$ is paramagnetic
3 $\mathrm{NiCl}_{4}^{2-}$ and $\left[\mathrm{Ni}(\mathrm{CN})_{4}\right]^{2-}$ are diamagnetic but $\mathrm{Ni}(\mathrm{CO})_{4}$ is paramagnetic
4 $\mathrm{Ni}(\mathrm{CO})_{4}$ is diamagnetic but $\mathrm{NiCl}_{4}^{2-}$ and $\left[\mathrm{Ni}(\mathrm{CN})_{4}\right]^{2-}$ is paramagnetic
Explanation:
(B) : Electronic configuration of ${ }_{28} \mathrm{Ni}$ in $\left[\mathrm{Ni}(\mathrm{CO})_{4}\right]$ $=[\mathrm{Ar}] 3 \mathrm{~d}^{8} 4 \mathrm{~s}^{2}$ $=0$ unpaired electron (diamagnetic) Electronic configuration of ${ }_{28} \mathrm{Ni}^{+2}$ in $\left[\mathrm{Ni}(\mathrm{CN})_{4}\right]^{2-}$ $=[\mathrm{Ar}] 3 \mathrm{~d}^{8}$ (square planar) $=0$ unpaired electron (diamagnetic) Electronic configuration of ${ }_{28} \mathrm{Ni}^{+2}$ in $\left[\mathrm{Ni}(\mathrm{Cl})_{4}\right]^{2-}$ $=[\mathrm{Ar}] 3 \mathrm{~d}^{8}$ $=2$ unpaired electron (paramagnetic)
VITEEE-2011
COORDINATION COMPOUNDS
274082
Identify the order in which the spin only magnetic moment (in BM) increases for the following four ions (I) $\mathrm{Fe}^{2+}$ (II) $\mathrm{Ti}^{2+}$ (III) $\mathrm{Cu}^{2+}$ (IV) $\mathrm{V}^{2+}$
1 I, II, IV, III
2 IV, I, II, III
3 III, IV, I, II
4 III, II, IV, I
Explanation:
(D) : (i) Magnetic moment $(\mu)=\sqrt{\mathrm{n}(\mathrm{n}+2)}$ Where $\mathrm{n}=$ no. of unpaired electron $\mu=\sqrt{4(4+2)}=\sqrt{24}=4.90 \mathrm{BM}$ (ii) $\mathrm{n}=2, \mu=2.83 \mathrm{BM}$ (iii) $\mathrm{n}=1, \mu=1.732 \mathrm{BM}$ (iv) $\mathrm{n}=3, \mu=3.87$ BM. Hence, the increasing order of magnetic moment is $\mathrm{Cu}^{2+}<\mathrm{Ti}^{2+}<\mathrm{V}^{2+}<\mathrm{Fe}^{+2}$ Hence, III $<$ II $<$ IV $<$ I
AP EAMCET- (Engg.)-2011
COORDINATION COMPOUNDS
274086
Which among the following is a paramagnetic complex?
274089
The spin only magnetic moment value (in B.M. unit) of $\mathrm{Cr}(\mathrm{CO})_{6}$ is
1 Zero
2 2.84
3 4.90
4 5.92
Explanation:
(A) : In $\mathrm{Cr}(\mathrm{CO})_{6}$, the oxidation state of chromium is zero. $\mathrm{Cr}=3 \mathrm{~d}^{5} 4 \mathrm{~s}^{1}$ $\mathrm{CO}$ ligand act as strong field ligand hence pairing of electrons occurs. Therefore, Number of unpaired electron $(\mathrm{n})=0$ Spin magnetic moment $=\sqrt{\mathrm{n}(\mathrm{n}+2)}=0$
274078
Amongst $\mathrm{Ni}(\mathrm{CO})_{4},\left[\mathrm{Ni}(\mathrm{CN})_{4}\right]^{2-}$ and $\left[\mathrm{NiCl}_{4}^{2-}\right]$
1 $\mathrm{Ni}(\mathrm{CO})_{4}$ and $\left[\mathrm{NiCl}_{4}^{2-}\right]$ are diamagnetic but $\left[\mathrm{Ni}(\mathrm{CN})_{4}\right]^{2-}$ is paramagnetic
2 $\mathrm{Ni}(\mathrm{CO})_{4}$ and $\left[\mathrm{Ni}(\mathrm{CN})_{4}\right]^{2-}$ are diamagnetic but $\mathrm{NiCl}_{4}^{2-}$ is paramagnetic
3 $\mathrm{NiCl}_{4}^{2-}$ and $\left[\mathrm{Ni}(\mathrm{CN})_{4}\right]^{2-}$ are diamagnetic but $\mathrm{Ni}(\mathrm{CO})_{4}$ is paramagnetic
4 $\mathrm{Ni}(\mathrm{CO})_{4}$ is diamagnetic but $\mathrm{NiCl}_{4}^{2-}$ and $\left[\mathrm{Ni}(\mathrm{CN})_{4}\right]^{2-}$ is paramagnetic
Explanation:
(B) : Electronic configuration of ${ }_{28} \mathrm{Ni}$ in $\left[\mathrm{Ni}(\mathrm{CO})_{4}\right]$ $=[\mathrm{Ar}] 3 \mathrm{~d}^{8} 4 \mathrm{~s}^{2}$ $=0$ unpaired electron (diamagnetic) Electronic configuration of ${ }_{28} \mathrm{Ni}^{+2}$ in $\left[\mathrm{Ni}(\mathrm{CN})_{4}\right]^{2-}$ $=[\mathrm{Ar}] 3 \mathrm{~d}^{8}$ (square planar) $=0$ unpaired electron (diamagnetic) Electronic configuration of ${ }_{28} \mathrm{Ni}^{+2}$ in $\left[\mathrm{Ni}(\mathrm{Cl})_{4}\right]^{2-}$ $=[\mathrm{Ar}] 3 \mathrm{~d}^{8}$ $=2$ unpaired electron (paramagnetic)
VITEEE-2011
COORDINATION COMPOUNDS
274082
Identify the order in which the spin only magnetic moment (in BM) increases for the following four ions (I) $\mathrm{Fe}^{2+}$ (II) $\mathrm{Ti}^{2+}$ (III) $\mathrm{Cu}^{2+}$ (IV) $\mathrm{V}^{2+}$
1 I, II, IV, III
2 IV, I, II, III
3 III, IV, I, II
4 III, II, IV, I
Explanation:
(D) : (i) Magnetic moment $(\mu)=\sqrt{\mathrm{n}(\mathrm{n}+2)}$ Where $\mathrm{n}=$ no. of unpaired electron $\mu=\sqrt{4(4+2)}=\sqrt{24}=4.90 \mathrm{BM}$ (ii) $\mathrm{n}=2, \mu=2.83 \mathrm{BM}$ (iii) $\mathrm{n}=1, \mu=1.732 \mathrm{BM}$ (iv) $\mathrm{n}=3, \mu=3.87$ BM. Hence, the increasing order of magnetic moment is $\mathrm{Cu}^{2+}<\mathrm{Ti}^{2+}<\mathrm{V}^{2+}<\mathrm{Fe}^{+2}$ Hence, III $<$ II $<$ IV $<$ I
AP EAMCET- (Engg.)-2011
COORDINATION COMPOUNDS
274086
Which among the following is a paramagnetic complex?
274089
The spin only magnetic moment value (in B.M. unit) of $\mathrm{Cr}(\mathrm{CO})_{6}$ is
1 Zero
2 2.84
3 4.90
4 5.92
Explanation:
(A) : In $\mathrm{Cr}(\mathrm{CO})_{6}$, the oxidation state of chromium is zero. $\mathrm{Cr}=3 \mathrm{~d}^{5} 4 \mathrm{~s}^{1}$ $\mathrm{CO}$ ligand act as strong field ligand hence pairing of electrons occurs. Therefore, Number of unpaired electron $(\mathrm{n})=0$ Spin magnetic moment $=\sqrt{\mathrm{n}(\mathrm{n}+2)}=0$
