274072
The coordination number and oxidation number $X$ in the following compound $\left[\mathrm{X}\left(\mathrm{SO}_{4}\right)\left(\mathrm{NH}_{3}\right)_{5}\right] \mathrm{CI}$ will be
1 10 and 3
2 02 and 6
3 06 and 3
4 06 and 4
Explanation:
(C) : In complex $\left[\mathrm{X}\left(\mathrm{SO}_{4}\right)\left(\mathrm{NH}_{3}\right)_{5}\right] \mathrm{Cl}$ or $\left[\mathrm{X}\left(\mathrm{SO}_{4}\right)\left(\mathrm{NH}_{3}\right)_{5}\right]^{+}$ Let, oxidation of metal $=\mathrm{x}$ $x+1 \times(-2)+5 \times 0=+1$ $x-2=1$ $x=+3$ Coordination number is the number of monodentate ligands attach with central metal. Here, coordination number $=6$
CG PET- 2015
COORDINATION COMPOUNDS
274073
What is the value of $x$ on the $\left[\operatorname{Ni}(\mathrm{CN})_{4}\right]^{x}$ complex ion?
1 +2
2 -2
3 0 (zero)
4 +4
Explanation:
(B) : If any complex follows E.A.N. rule then that complex is stable and exist. According to E.A.N. rule, complex having total electron is equal to atomic number of inert gases. E.A.N. $=$ atomic number of metal $+2 \times$ number of ligand - oxidation state $\left[\mathrm{Ni}(\mathrm{CN})_{4}\right]^{\mathrm{x}}$ is a square planar complex and its E.A.N. value is 34 . $34=28+4 \times(-1)-$ Oxidation state Oxidation state $=2$ $2+4(-1)=\mathrm{x}$ $\mathrm{x}=-2$
CG PET- 2015
COORDINATION COMPOUNDS
274075
The compound which does not show paramagnetism, is
(B) : ${\left[\mathrm{Ag}\left(\mathrm{NH}_3\right)_4\right] \mathrm{Cl} } \underset{[\mathrm{Ag}(}{\left.\left(\mathrm{NH}_3\right)_4\right]^{+}+\mathrm{Cl}^{-}}$ $\downarrow$ $\mathrm{x}+4 \times 0=+1$ $\mathrm{x}=+1$ $\mathrm{Ag}=[\mathrm{Kr}] 4 \mathrm{~d}^{10} 5 \mathrm{~s}^1$ $\mathrm{Ag}^{+}=[\mathrm{Kr}] 4 \mathrm{~d}^{10}$ The no. of unpaired electron is zero its show diamagnetic not paramagnetic.
MPPET- 2009
COORDINATION COMPOUNDS
274077
The complex showing a spin-only magnetic moment of 2.82 B.M. is:
274072
The coordination number and oxidation number $X$ in the following compound $\left[\mathrm{X}\left(\mathrm{SO}_{4}\right)\left(\mathrm{NH}_{3}\right)_{5}\right] \mathrm{CI}$ will be
1 10 and 3
2 02 and 6
3 06 and 3
4 06 and 4
Explanation:
(C) : In complex $\left[\mathrm{X}\left(\mathrm{SO}_{4}\right)\left(\mathrm{NH}_{3}\right)_{5}\right] \mathrm{Cl}$ or $\left[\mathrm{X}\left(\mathrm{SO}_{4}\right)\left(\mathrm{NH}_{3}\right)_{5}\right]^{+}$ Let, oxidation of metal $=\mathrm{x}$ $x+1 \times(-2)+5 \times 0=+1$ $x-2=1$ $x=+3$ Coordination number is the number of monodentate ligands attach with central metal. Here, coordination number $=6$
CG PET- 2015
COORDINATION COMPOUNDS
274073
What is the value of $x$ on the $\left[\operatorname{Ni}(\mathrm{CN})_{4}\right]^{x}$ complex ion?
1 +2
2 -2
3 0 (zero)
4 +4
Explanation:
(B) : If any complex follows E.A.N. rule then that complex is stable and exist. According to E.A.N. rule, complex having total electron is equal to atomic number of inert gases. E.A.N. $=$ atomic number of metal $+2 \times$ number of ligand - oxidation state $\left[\mathrm{Ni}(\mathrm{CN})_{4}\right]^{\mathrm{x}}$ is a square planar complex and its E.A.N. value is 34 . $34=28+4 \times(-1)-$ Oxidation state Oxidation state $=2$ $2+4(-1)=\mathrm{x}$ $\mathrm{x}=-2$
CG PET- 2015
COORDINATION COMPOUNDS
274075
The compound which does not show paramagnetism, is
(B) : ${\left[\mathrm{Ag}\left(\mathrm{NH}_3\right)_4\right] \mathrm{Cl} } \underset{[\mathrm{Ag}(}{\left.\left(\mathrm{NH}_3\right)_4\right]^{+}+\mathrm{Cl}^{-}}$ $\downarrow$ $\mathrm{x}+4 \times 0=+1$ $\mathrm{x}=+1$ $\mathrm{Ag}=[\mathrm{Kr}] 4 \mathrm{~d}^{10} 5 \mathrm{~s}^1$ $\mathrm{Ag}^{+}=[\mathrm{Kr}] 4 \mathrm{~d}^{10}$ The no. of unpaired electron is zero its show diamagnetic not paramagnetic.
MPPET- 2009
COORDINATION COMPOUNDS
274077
The complex showing a spin-only magnetic moment of 2.82 B.M. is:
274072
The coordination number and oxidation number $X$ in the following compound $\left[\mathrm{X}\left(\mathrm{SO}_{4}\right)\left(\mathrm{NH}_{3}\right)_{5}\right] \mathrm{CI}$ will be
1 10 and 3
2 02 and 6
3 06 and 3
4 06 and 4
Explanation:
(C) : In complex $\left[\mathrm{X}\left(\mathrm{SO}_{4}\right)\left(\mathrm{NH}_{3}\right)_{5}\right] \mathrm{Cl}$ or $\left[\mathrm{X}\left(\mathrm{SO}_{4}\right)\left(\mathrm{NH}_{3}\right)_{5}\right]^{+}$ Let, oxidation of metal $=\mathrm{x}$ $x+1 \times(-2)+5 \times 0=+1$ $x-2=1$ $x=+3$ Coordination number is the number of monodentate ligands attach with central metal. Here, coordination number $=6$
CG PET- 2015
COORDINATION COMPOUNDS
274073
What is the value of $x$ on the $\left[\operatorname{Ni}(\mathrm{CN})_{4}\right]^{x}$ complex ion?
1 +2
2 -2
3 0 (zero)
4 +4
Explanation:
(B) : If any complex follows E.A.N. rule then that complex is stable and exist. According to E.A.N. rule, complex having total electron is equal to atomic number of inert gases. E.A.N. $=$ atomic number of metal $+2 \times$ number of ligand - oxidation state $\left[\mathrm{Ni}(\mathrm{CN})_{4}\right]^{\mathrm{x}}$ is a square planar complex and its E.A.N. value is 34 . $34=28+4 \times(-1)-$ Oxidation state Oxidation state $=2$ $2+4(-1)=\mathrm{x}$ $\mathrm{x}=-2$
CG PET- 2015
COORDINATION COMPOUNDS
274075
The compound which does not show paramagnetism, is
(B) : ${\left[\mathrm{Ag}\left(\mathrm{NH}_3\right)_4\right] \mathrm{Cl} } \underset{[\mathrm{Ag}(}{\left.\left(\mathrm{NH}_3\right)_4\right]^{+}+\mathrm{Cl}^{-}}$ $\downarrow$ $\mathrm{x}+4 \times 0=+1$ $\mathrm{x}=+1$ $\mathrm{Ag}=[\mathrm{Kr}] 4 \mathrm{~d}^{10} 5 \mathrm{~s}^1$ $\mathrm{Ag}^{+}=[\mathrm{Kr}] 4 \mathrm{~d}^{10}$ The no. of unpaired electron is zero its show diamagnetic not paramagnetic.
MPPET- 2009
COORDINATION COMPOUNDS
274077
The complex showing a spin-only magnetic moment of 2.82 B.M. is:
274072
The coordination number and oxidation number $X$ in the following compound $\left[\mathrm{X}\left(\mathrm{SO}_{4}\right)\left(\mathrm{NH}_{3}\right)_{5}\right] \mathrm{CI}$ will be
1 10 and 3
2 02 and 6
3 06 and 3
4 06 and 4
Explanation:
(C) : In complex $\left[\mathrm{X}\left(\mathrm{SO}_{4}\right)\left(\mathrm{NH}_{3}\right)_{5}\right] \mathrm{Cl}$ or $\left[\mathrm{X}\left(\mathrm{SO}_{4}\right)\left(\mathrm{NH}_{3}\right)_{5}\right]^{+}$ Let, oxidation of metal $=\mathrm{x}$ $x+1 \times(-2)+5 \times 0=+1$ $x-2=1$ $x=+3$ Coordination number is the number of monodentate ligands attach with central metal. Here, coordination number $=6$
CG PET- 2015
COORDINATION COMPOUNDS
274073
What is the value of $x$ on the $\left[\operatorname{Ni}(\mathrm{CN})_{4}\right]^{x}$ complex ion?
1 +2
2 -2
3 0 (zero)
4 +4
Explanation:
(B) : If any complex follows E.A.N. rule then that complex is stable and exist. According to E.A.N. rule, complex having total electron is equal to atomic number of inert gases. E.A.N. $=$ atomic number of metal $+2 \times$ number of ligand - oxidation state $\left[\mathrm{Ni}(\mathrm{CN})_{4}\right]^{\mathrm{x}}$ is a square planar complex and its E.A.N. value is 34 . $34=28+4 \times(-1)-$ Oxidation state Oxidation state $=2$ $2+4(-1)=\mathrm{x}$ $\mathrm{x}=-2$
CG PET- 2015
COORDINATION COMPOUNDS
274075
The compound which does not show paramagnetism, is
(B) : ${\left[\mathrm{Ag}\left(\mathrm{NH}_3\right)_4\right] \mathrm{Cl} } \underset{[\mathrm{Ag}(}{\left.\left(\mathrm{NH}_3\right)_4\right]^{+}+\mathrm{Cl}^{-}}$ $\downarrow$ $\mathrm{x}+4 \times 0=+1$ $\mathrm{x}=+1$ $\mathrm{Ag}=[\mathrm{Kr}] 4 \mathrm{~d}^{10} 5 \mathrm{~s}^1$ $\mathrm{Ag}^{+}=[\mathrm{Kr}] 4 \mathrm{~d}^{10}$ The no. of unpaired electron is zero its show diamagnetic not paramagnetic.
MPPET- 2009
COORDINATION COMPOUNDS
274077
The complex showing a spin-only magnetic moment of 2.82 B.M. is:
